Course Information

C9920 Introduction to Quantum Chemistry

Extent and Intensity

2/1/0. 3 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).
Taught in person.

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)
Mgr. Hugo Semrád, Ph.D. (seminar tutor)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Contact Person: doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Prerequisites

Any of the university introductory classes on mathematics. Sufficient is any of mathematics courses for students of chemistry, biochemistry, or chemistry with teaching specialization.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 7 fields of study the course is directly associated with, display

Course objectives

The course represents a one-semestre introduction into the foundations of quantum chemistry and its applications to the reproduction, interpretation, and prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. The main goal of this course is the understanding of basic concepts of quantum mechanics.

Learning outcomes

At the end of the course students will possess the following skills: understanding the basic quantum mechanics concepts on simple yet real chemical systems; grasp the principles of computational quantum chemistry; the creation of orbital-interaction diagrams for simple real molecules.

Syllabus

• 1. Basic notions of quantum mechanics. The notion of the wavefunction, the wavefunction postulate. Stationary Schrodinger equation. The notion of an operator, an eigenfunction of an operator, an eigenvalue corresponding to an operator and an eigenfunction. Hermitian operator: definition and properties. The coordinate operator, momentum operator, operator of the square of angular momentum, operator of the projection of the angular momentum in the z axis, energy operator - Hamiltonian. Commuting operators and common set of eigenfunctions. 2. Hydrogen atom. Hamiltonian for the fixed H atom and with the introduction of the reduced mass. Coordinate set for a spherically symmetrical system. Eigenstates for negative and positive eigenvalues. The notion of degeneracy, eigenfunctions. Radial factors, radial distribution function. Angular factors as eigenfunctions of momentum operators. Complex and real angular functions. Means of plotting atomic orbitals, the notion of orthogonality. 3. Many-electron atoms. Atomic units. Hamiltonian for the He atom. The meaning of the "orbital" notion. Total wavefunction in relation to one-electron wavefunctions. Total energy in relation to one-electron energies. Exchange symmetry of the wavefunction, electron spin, antisymmetry. Electron configuration of Li, Pauli principle. Slater determinant. Slater orbital. Aufbau principle, Klechowsky and Hund's rules. The evolution of atomic properties in the periodical system. 4. H2+ molecule. Three-particle Hamiltonian. Born-Oppenheimer approximation of the wavefunction. The method of molecular orbitals (MO) as linear combination of atomic orbitals (LCAO). Solution (a) employing symmetry and (b) using the variational method. Overlap integral, interaction integral as functions of internuclear distance. Secular equation, resulting energies and wavefunctions. MO graphical representations, symmetry properties, bonding and antibonding MO. Interaction diagram. 5. Simple Hückel method. Approximation of independent pi-electrons. Hückel determinant, values alpha and beta. Eigenfunctions and eigenvalues. Diagrams for energy levels. Charge densities, pi electron densities, HMO energies: the relation to experimental observables. The principle of extended Hückel method, bases, overlap and interaction integrals, parameter K, eigenfunctions and eigenvalues. Electronic structure of planar hydrocarbons. 6. Molecular symmetry. Symmetry groups. Matrices and their multiplication. Matrix representation of symmetry group. Reducible and irreducible representations. Symbols used for irreducible representations. Symmetry-adapted linear combinations. The use of character tables: zero and non-zero overlap integrals. Symmetry driven orbital interaction. 7. Two-orbital interaction: Molecules A2 and AB. The interaction of two identical and two different AOs. Level occupation, total energy. Overlap and symmetry. Four-AO interaction. Diatomic molecules A2 and AB: basis functions, pi and sigma MOs, s-p interaction, interaction diagrams, electron configurations, bond lengths and energies. 8. Interaction between two fragment orbitals. Linear and bent molecules AH2: The notion of a fragment orbital, symmetry elements, MOs, correlation diagram for linear and bent geometry, geometries of AH2 molecules. Application to BeH2. 9. AH3 and AH4 molecules. MOs of trigonal planar AH3. Orbital correlation diagram for trigonal planar and pyramidal AH3. Planar of pyramidal geometries? Tetrahedral molecules AH4. Shapes of AH4 systems.

Literature

recommended literature
• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• JEAN, Yves and François VOLATRON. An introduction to molecular orbitals. Edited by Jeremy K. Burdett. New York: Oxford University Press, 1993, xiv, 337. ISBN 0195069188. info

Teaching methods

Lectures, exercises, consultations.

Assessment methods

Written exam based 75% on practical skills practiced in the seminar, 25% on lectured theory. The theoretical questions will be motivated by the "Multiple-choice questions" tasks at the end of the Lowe textbook chapters from the areas we will cover. Students have the option of voluntarily taking an oral retest, during which the grade from the written part can be improved or unchanged, it cannot be worsened.

Language of instruction

Czech

Further comments (probably available only in Czech)

The course is taught annually.
The course is taught: every week.

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

C9920 Introduction to Quantum Chemistry

Extent and Intensity

2/1/0. 3 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).
Taught in person.

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)
Mgr. Hugo Semrád, Ph.D. (seminar tutor)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Contact Person: doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Thu 12:00–13:50 B11/305

• Timetable of Seminar Groups:

C9920/01: Tue 16:00–16:50 A08/309, H. Semrád
C9920/02: Tue 17:00–17:50 A08/309, H. Semrád

Prerequisites

Any of the university introductory classes on mathematics. Sufficient is any of mathematics courses for students of chemistry, biochemistry, or chemistry with teaching specialization.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 7 fields of study the course is directly associated with, display

Course objectives

The course represents a one-semestre introduction into the foundations of quantum chemistry and its applications to the reproduction, interpretation, and prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. The main goal of this course is the understanding of basic concepts of quantum mechanics.

Learning outcomes

At the end of the course students will possess the following skills: understanding the basic quantum mechanics concepts on simple yet real chemical systems; grasp the principles of computational quantum chemistry; the creation of orbital-interaction diagrams for simple real molecules.

Syllabus

• 1. Basic notions of quantum mechanics. The notion of the wavefunction, the wavefunction postulate. Stationary Schrodinger equation. The notion of an operator, an eigenfunction of an operator, an eigenvalue corresponding to an operator and an eigenfunction. Hermitian operator: definition and properties. The coordinate operator, momentum operator, operator of the square of angular momentum, operator of the projection of the angular momentum in the z axis, energy operator - Hamiltonian. Commuting operators and common set of eigenfunctions. 2. Hydrogen atom. Hamiltonian for the fixed H atom and with the introduction of the reduced mass. Coordinate set for a spherically symmetrical system. Eigenstates for negative and positive eigenvalues. The notion of degeneracy, eigenfunctions. Radial factors, radial distribution function. Angular factors as eigenfunctions of momentum operators. Complex and real angular functions. Means of plotting atomic orbitals, the notion of orthogonality. 3. Many-electron atoms. Atomic units. Hamiltonian for the He atom. The meaning of the "orbital" notion. Total wavefunction in relation to one-electron wavefunctions. Total energy in relation to one-electron energies. Exchange symmetry of the wavefunction, electron spin, antisymmetry. Electron configuration of Li, Pauli principle. Slater determinant. Slater orbital. Aufbau principle, Klechowsky and Hund's rules. The evolution of atomic properties in the periodical system. 4. H2+ molecule. Three-particle Hamiltonian. Born-Oppenheimer approximation of the wavefunction. The method of molecular orbitals (MO) as linear combination of atomic orbitals (LCAO). Solution (a) employing symmetry and (b) using the variational method. Overlap integral, interaction integral as functions of internuclear distance. Secular equation, resulting energies and wavefunctions. MO graphical representations, symmetry properties, bonding and antibonding MO. Interaction diagram. 5. Simple Hückel method. Approximation of independent pi-electrons. Hückel determinant, values alpha and beta. Eigenfunctions and eigenvalues. Diagrams for energy levels. Charge densities, pi electron densities, HMO energies: the relation to experimental observables. The principle of extended Hückel method, bases, overlap and interaction integrals, parameter K, eigenfunctions and eigenvalues. Electronic structure of planar hydrocarbons. 6. Molecular symmetry. Symmetry groups. Matrices and their multiplication. Matrix representation of symmetry group. Reducible and irreducible representations. Symbols used for irreducible representations. Symmetry-adapted linear combinations. The use of character tables: zero and non-zero overlap integrals. Symmetry driven orbital interaction. 7. Two-orbital interaction: Molecules A2 and AB. The interaction of two identical and two different AOs. Level occupation, total energy. Overlap and symmetry. Four-AO interaction. Diatomic molecules A2 and AB: basis functions, pi and sigma MOs, s-p interaction, interaction diagrams, electron configurations, bond lengths and energies. 8. Interaction between two fragment orbitals. Linear and bent molecules AH2: The notion of a fragment orbital, symmetry elements, MOs, correlation diagram for linear and bent geometry, geometries of AH2 molecules. Application to BeH2. 9. AH3 and AH4 molecules. MOs of trigonal planar AH3. Orbital correlation diagram for trigonal planar and pyramidal AH3. Planar of pyramidal geometries? Tetrahedral molecules AH4. Shapes of AH4 systems.

Literature

recommended literature
• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• JEAN, Yves and François VOLATRON. An introduction to molecular orbitals. Edited by Jeremy K. Burdett. New York: Oxford University Press, 1993, xiv, 337. ISBN 0195069188. info

Teaching methods

Lectures, exercises, consultations.

Assessment methods

Written exam based 75% on practical skills practiced in the seminar, 25% on lectured theory. The theoretical questions will be motivated by the "Multiple-choice questions" tasks at the end of the Lowe textbook chapters from the areas we will cover. Students have the option of voluntarily taking an oral retest, during which the grade from the written part can be improved or unchanged, it cannot be worsened.

Language of instruction

Czech

Further comments (probably available only in Czech)

Study Materials
The course is taught annually.

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

C9920 Introduction to Quantum Chemistry

Extent and Intensity

2/1/0. 3 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).
Taught in person.

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)
Mgr. Hugo Semrád, Ph.D. (seminar tutor)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Contact Person: doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Tue 15:00–16:50 B11/305

• Timetable of Seminar Groups:

C9920/01: Tue 14:00–14:50 C12/311, H. Semrád
C9920/02: Tue 17:00–17:50 C12/311, H. Semrád

Prerequisites

Any of the university introductory classes on mathematics. Sufficient is any of mathematics courses for students of chemistry, biochemistry, or chemistry with teaching specialization.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 7 fields of study the course is directly associated with, display

Course objectives

The course represents a one-semestre introduction into the foundations of quantum chemistry and its applications to the reproduction, interpretation, and prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. The main goal of this course is the understanding of basic concepts of quantum mechanics.

Learning outcomes

At the end of the course students will possess the following skills: understanding the basic quantum mechanics concepts on simple yet real chemical systems; grasp the principles of computational quantum chemistry; the creation of orbital-interaction diagrams for simple real molecules.

Syllabus

• 1. Basic notions of quantum mechanics. The notion of the wavefunction, the wavefunction postulate. Stationary Schrodinger equation. The notion of an operator, an eigenfunction of an operator, an eigenvalue corresponding to an operator and an eigenfunction. Hermitian operator: definition and properties. The coordinate operator, momentum operator, operator of the square of angular momentum, operator of the projection of the angular momentum in the z axis, energy operator - Hamiltonian. Commuting operators and common set of eigenfunctions. 2. Hydrogen atom. Hamiltonian for the fixed H atom and with the introduction of the reduced mass. Coordinate set for a spherically symmetrical system. Eigenstates for negative and positive eigenvalues. The notion of degeneracy, eigenfunctions. Radial factors, radial distribution function. Angular factors as eigenfunctions of momentum operators. Complex and real angular functions. Means of plotting atomic orbitals, the notion of orthogonality. 3. Many-electron atoms. Atomic units. Hamiltonian for the He atom. The meaning of the "orbital" notion. Total wavefunction in relation to one-electron wavefunctions. Total energy in relation to one-electron energies. Exchange symmetry of the wavefunction, electron spin, antisymmetry. Electron configuration of Li, Pauli principle. Slater determinant. Slater orbital. Aufbau principle, Klechowsky and Hund's rules. The evolution of atomic properties in the periodical system. 4. H2+ molecule. Three-particle Hamiltonian. Born-Oppenheimer approximation of the wavefunction. The method of molecular orbitals (MO) as linear combination of atomic orbitals (LCAO). Solution (a) employing symmetry and (b) using the variational method. Overlap integral, interaction integral as functions of internuclear distance. Secular equation, resulting energies and wavefunctions. MO graphical representations, symmetry properties, bonding and antibonding MO. Interaction diagram. 5. Simple Hückel method. Approximation of independent pi-electrons. Hückel determinant, values alpha and beta. Eigenfunctions and eigenvalues. Diagrams for energy levels. Charge densities, pi electron densities, HMO energies: the relation to experimental observables. The principle of extended Hückel method, bases, overlap and interaction integrals, parameter K, eigenfunctions and eigenvalues. Electronic structure of planar hydrocarbons. 6. Molecular symmetry. Symmetry groups. Matrices and their multiplication. Matrix representation of symmetry group. Reducible and irreducible representations. Symbols used for irreducible representations. Symmetry-adapted linear combinations. The use of character tables: zero and non-zero overlap integrals. Symmetry driven orbital interaction. 7. Two-orbital interaction: Molecules A2 and AB. The interaction of two identical and two different AOs. Level occupation, total energy. Overlap and symmetry. Four-AO interaction. Diatomic molecules A2 and AB: basis functions, pi and sigma MOs, s-p interaction, interaction diagrams, electron configurations, bond lengths and energies. 8. Interaction between two fragment orbitals. Linear and bent molecules AH2: The notion of a fragment orbital, symmetry elements, MOs, correlation diagram for linear and bent geometry, geometries of AH2 molecules. Application to BeH2. 9. AH3 and AH4 molecules. MOs of trigonal planar AH3. Orbital correlation diagram for trigonal planar and pyramidal AH3. Planar of pyramidal geometries? Tetrahedral molecules AH4. Shapes of AH4 systems.

Literature

recommended literature
• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• JEAN, Yves and François VOLATRON. An introduction to molecular orbitals. Edited by Jeremy K. Burdett. New York: Oxford University Press, 1993, xiv, 337. ISBN 0195069188. info

Teaching methods

Lectures, exercises, consultations.

Assessment methods

Written exam (requiring in a major part the formulation of answers, in a minor part a choice from several possibilities) and oral exam (2 items from the syllabus by the teacher's choice, 20 minute time for preparation). Examples of examination tests can be found in the information system.

Language of instruction

Czech

Further comments (probably available only in Czech)

The course is taught annually.

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

C9920 Introduction to Quantum Chemistry

Extent and Intensity

2/1/0. 3 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).
Taught in person.

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Contact Person: doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Tue 8:00–9:50 C12/311, Tue 15:00–15:50 C12/311

Prerequisites

Any of the university introductory classes on mathematics. Sufficient is any of mathematics courses for students of chemistry, biochemistry, or chemistry with teaching specialization.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 7 fields of study the course is directly associated with, display

Course objectives

The course represents a one-semestre introduction into the foundations of quantum chemistry and its applications to the reproduction, interpretation, and prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. The main goal of this course is the understanding of basic concepts of quantum mechanics.

Learning outcomes

At the end of the course students will possess the following skills: understanding the basic quantum mechanics concepts on simple yet real chemical systems; grasp the principles of computational quantum chemistry; the creation of orbital-interaction diagrams for simple real molecules.

Syllabus

• 1. Basic notions of quantum mechanics. The notion of the wavefunction, the wavefunction postulate. Stationary Schrodinger equation. The notion of an operator, an eigenfunction of an operator, an eigenvalue corresponding to an operator and an eigenfunction. Hermitian operator: definition and properties. The coordinate operator, momentum operator, operator of the square of angular momentum, operator of the projection of the angular momentum in the z axis, energy operator - Hamiltonian. Commuting operators and common set of eigenfunctions. 2. Hydrogen atom. Hamiltonian for the fixed H atom and with the introduction of the reduced mass. Coordinate set for a spherically symmetrical system. Eigenstates for negative and positive eigenvalues. The notion of degeneracy, eigenfunctions. Radial factors, radial distribution function. Angular factors as eigenfunctions of momentum operators. Complex and real angular functions. Means of plotting atomic orbitals, the notion of orthogonality. 3. Many-electron atoms. Atomic units. Hamiltonian for the He atom. The meaning of the "orbital" notion. Total wavefunction in relation to one-electron wavefunctions. Total energy in relation to one-electron energies. Exchange symmetry of the wavefunction, electron spin, antisymmetry. Electron configuration of Li, Pauli principle. Slater determinant. Slater orbital. Aufbau principle, Klechowsky and Hund's rules. The evolution of atomic properties in the periodical system. 4. H2+ molecule. Three-particle Hamiltonian. Born-Oppenheimer approximation of the wavefunction. The method of molecular orbitals (MO) as linear combination of atomic orbitals (LCAO). Solution (a) employing symmetry and (b) using the variational method. Overlap integral, interaction integral as functions of internuclear distance. Secular equation, resulting energies and wavefunctions. MO graphical representations, symmetry properties, bonding and antibonding MO. Interaction diagram. 5. Simple Hückel method. Approximation of independent pi-electrons. Hückel determinant, values alpha and beta. Eigenfunctions and eigenvalues. Diagrams for energy levels. Charge densities, pi electron densities, HMO energies: the relation to experimental observables. The principle of extended Hückel method, bases, overlap and interaction integrals, parameter K, eigenfunctions and eigenvalues. Electronic structure of planar hydrocarbons. 6. Molecular symmetry. Symmetry groups. Matrices and their multiplication. Matrix representation of symmetry group. Reducible and irreducible representations. Symbols used for irreducible representations. Symmetry-adapted linear combinations. The use of character tables: zero and non-zero overlap integrals. Symmetry driven orbital interaction. 7. Two-orbital interaction: Molecules A2 and AB. The interaction of two identical and two different AOs. Level occupation, total energy. Overlap and symmetry. Four-AO interaction. Diatomic molecules A2 and AB: basis functions, pi and sigma MOs, s-p interaction, interaction diagrams, electron configurations, bond lengths and energies. 8. Interaction between two fragment orbitals. Linear and bent molecules AH2: The notion of a fragment orbital, symmetry elements, MOs, correlation diagram for linear and bent geometry, geometries of AH2 molecules. Application to BeH2. 9. AH3 and AH4 molecules. MOs of trigonal planar AH3. Orbital correlation diagram for trigonal planar and pyramidal AH3. Planar of pyramidal geometries? Tetrahedral molecules AH4. Shapes of AH4 systems.

Literature

recommended literature
• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• JEAN, Yves and François VOLATRON. An introduction to molecular orbitals. Edited by Jeremy K. Burdett. New York: Oxford University Press, 1993, xiv, 337. ISBN 0195069188. info

Teaching methods

Lectures, exercises, consultations.

Assessment methods

Written exam (requiring in a major part the formulation of answers, in a minor part a choice from several possibilities) and oral exam (2 items from the syllabus by the teacher's choice, 20 minute time for preparation). Examples of examination tests can be found in the information system.

Language of instruction

Czech

Further comments (probably available only in Czech)

The course is taught annually.

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

C9920 Introduction to Quantum Chemistry

Extent and Intensity

2/1/0. 3 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).
Taught partially online.

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)
Mgr. Hugo Semrád, Ph.D. (seminar tutor)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Contact Person: doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Tue 12:00–13:50 B11/335

• Timetable of Seminar Groups:

C9920/01: Thu 16:00–16:50 B11/205, M. Munzarová
C9920/02: Thu 17:00–17:50 B11/205, M. Munzarová

Prerequisites

Any of the university introductory classes on mathematics. Sufficient is any of mathematics courses for students of chemistry, biochemistry, or chemistry with teaching specialization.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 7 fields of study the course is directly associated with, display

Course objectives

The course represents a one-semestre introduction into the foundations of quantum chemistry and its applications to the reproduction, interpretation, and prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. The main goal of this course is the understanding of basic concepts of quantum mechanics.

Learning outcomes

At the end of the course students will possess the following skills: understanding the basic quantum mechanics concepts on simple yet real chemical systems; grasp the principles of computational quantum chemistry; the creation of orbital-interaction diagrams for simple real molecules.

Syllabus

• 1. Basic notions of quantum mechanics. The notion of the wavefunction, the wavefunction postulate. Stationary Schrodinger equation. The notion of an operator, an eigenfunction of an operator, an eigenvalue corresponding to an operator and an eigenfunction. Hermitian operator: definition and properties. The coordinate operator, momentum operator, operator of the square of angular momentum, operator of the projection of the angular momentum in the z axis, energy operator - Hamiltonian. Commuting operators and common set of eigenfunctions. 2. Hydrogen atom. Hamiltonian for the fixed H atom and with the introduction of the reduced mass. Coordinate set for a spherically symmetrical system. Eigenstates for negative and positive eigenvalues. The notion of degeneracy, eigenfunctions. Radial factors, radial distribution function. Angular factors as eigenfunctions of momentum operators. Complex and real angular functions. Means of plotting atomic orbitals, the notion of orthogonality. 3. Many-electron atoms. Atomic units. Hamiltonian for the He atom. The meaning of the "orbital" notion. Total wavefunction in relation to one-electron wavefunctions. Total energy in relation to one-electron energies. Exchange symmetry of the wavefunction, electron spin, antisymmetry. Electron configuration of Li, Pauli principle. Slater determinant. Slater orbital. Aufbau principle, Klechowsky and Hund's rules. The evolution of atomic properties in the periodical system. 4. H2+ molecule. Three-particle Hamiltonian. Born-Oppenheimer approximation of the wavefunction. The method of molecular orbitals (MO) as linear combination of atomic orbitals (LCAO). Solution (a) employing symmetry and (b) using the variational method. Overlap integral, interaction integral as functions of internuclear distance. Secular equation, resulting energies and wavefunctions. MO graphical representations, symmetry properties, bonding and antibonding MO. Interaction diagram. 5. Simple Hückel method. Approximation of independent pi-electrons. Hückel determinant, values alpha and beta. Eigenfunctions and eigenvalues. Diagrams for energy levels. Charge densities, pi electron densities, HMO energies: the relation to experimental observables. The principle of extended Hückel method, bases, overlap and interaction integrals, parameter K, eigenfunctions and eigenvalues. Electronic structure of planar hydrocarbons. 6. Molecular symmetry. Symmetry groups. Matrices and their multiplication. Matrix representation of symmetry group. Reducible and irreducible representations. Symbols used for irreducible representations. Symmetry-adapted linear combinations. The use of character tables: zero and non-zero overlap integrals. Symmetry driven orbital interaction. 7. Two-orbital interaction: Molecules A2 and AB. The interaction of two identical and two different AOs. Level occupation, total energy. Overlap and symmetry. Four-AO interaction. Diatomic molecules A2 and AB: basis functions, pi and sigma MOs, s-p interaction, interaction diagrams, electron configurations, bond lengths and energies. 8. Interaction between two fragment orbitals. Linear and bent molecules AH2: The notion of a fragment orbital, symmetry elements, MOs, correlation diagram for linear and bent geometry, geometries of AH2 molecules. Application to BeH2. 9. AH3 and AH4 molecules. MOs of trigonal planar AH3. Orbital correlation diagram for trigonal planar and pyramidal AH3. Planar of pyramidal geometries? Tetrahedral molecules AH4. Shapes of AH4 systems.

Literature

recommended literature
• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• JEAN, Yves and François VOLATRON. An introduction to molecular orbitals. Edited by Jeremy K. Burdett. New York: Oxford University Press, 1993, xiv, 337. ISBN 0195069188. info

Teaching methods

Lectures, exercises, consultations.

Assessment methods

Written exam (requiring in a major part the formulation of answers, in a minor part a choice from several possibilities) and oral exam (2 items from the syllabus by the teacher's choice, 20 minute time for preparation). Examples of examination tests can be found in the information system.

Language of instruction

Czech

Further comments (probably available only in Czech)

Study Materials
The course is taught annually.

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

C9920 Introduction to Quantum Chemistry and Electronic Structure of Molecules

Extent and Intensity

2/1/0. 3 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)
Mgr. Hugo Semrád, Ph.D. (seminar tutor)
Mgr. Jakub Stošek, Ph.D. (assistant)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Contact Person: doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Mon 13:00–14:50 B11/335

• Timetable of Seminar Groups:

C9920/01: Thu 16:00–16:50 C12/311, M. Munzarová
C9920/02: Thu 17:00–17:50 C12/311, M. Munzarová

Prerequisites

Any of the university introductory classes on mathematics. Sufficient is any of mathematics courses for students of chemistry, biochemistry, or chemistry with teaching specialization.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 7 fields of study the course is directly associated with, display

Course objectives

The course represents a one-semestre introduction into the foundations of quantum chemistry and its applications to the reproduction, interpretation, and prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. The main goal of this course is the understanding of basic concepts of quantum mechanics.

Learning outcomes

At the end of the course students will possess the following skills: understanding the basic quantum mechanics concepts on simple yet real chemical systems; grasp the principles of computational quantum chemistry; the creation of orbital-interaction diagrams for simple real molecules.

Syllabus

• 1. Basic notions of quantum mechanics. The notion of the wavefunction, the wavefunction postulate. Stationary Schrodinger equation. The notion of an operator, an eigenfunction of an operator, an eigenvalue corresponding to an operator and an eigenfunction. Hermitian operator: definition and properties. The coordinate operator, momentum operator, operator of the square of angular momentum, operator of the projection of the angular momentum in the z axis, energy operator - Hamiltonian. Commuting operators and common set of eigenfunctions. 2. Hydrogen atom. Hamiltonian for the fixed H atom and with the introduction of the reduced mass. Coordinate set for a spherically symmetrical system. Eigenstates for negative and positive eigenvalues. The notion of degeneracy, eigenfunctions. Radial factors, radial distribution function. Angular factors as eigenfunctions of momentum operators. Complex and real angular functions. Means of plotting atomic orbitals, the notion of orthogonality. 3. Many-electron atoms. Atomic units. Hamiltonian for the He atom. The meaning of the "orbital" notion. Total wavefunction in relation to one-electron wavefunctions. Total energy in relation to one-electron energies. Exchange symmetry of the wavefunction, electron spin, antisymmetry. Electron configuration of Li, Pauli principle. Slater determinant. Slater orbital. Aufbau principle, Klechowsky and Hund's rules. The evolution of atomic properties in the periodical system. 4. H2+ molecule. Three-particle Hamiltonian. Born-Oppenheimer approximation of the wavefunction. The method of molecular orbitals (MO) as linear combination of atomic orbitals (LCAO). Solution (a) employing symmetry and (b) using the variational method. Overlap integral, interaction integral as functions of internuclear distance. Secular equation, resulting energies and wavefunctions. MO graphical representations, symmetry properties, bonding and antibonding MO. Interaction diagram. 5. Simple Hückel method. Approximation of independent pi-electrons. Hückel determinant, values alpha and beta. Eigenfunctions and eigenvalues. Diagrams for energy levels. Charge densities, pi electron densities, HMO energies: the relation to experimental observables. The principle of extended Hückel method, bases, overlap and interaction integrals, parameter K, eigenfunctions and eigenvalues. Electronic structure of planar hydrocarbons. 6. Molecular symmetry. Symmetry groups. Matrices and their multiplication. Matrix representation of symmetry group. Reducible and irreducible representations. Symbols used for irreducible representations. Symmetry-adapted linear combinations. The use of character tables: zero and non-zero overlap integrals. Symmetry driven orbital interaction. 7. Two-orbital interaction: Molecules A2 and AB. The interaction of two identical and two different AOs. Level occupation, total energy. Overlap and symmetry. Four-AO interaction. Diatomic molecules A2 and AB: basis functions, pi and sigma MOs, s-p interaction, interaction diagrams, electron configurations, bond lengths and energies. 8. Interaction between two fragment orbitals. Linear and bent molecules AH2: The notion of a fragment orbital, symmetry elements, MOs, correlation diagram for linear and bent geometry, geometries of AH2 molecules. Application to BeH2. 9. AH3 and AH4 molecules. MOs of trigonal planar AH3. Orbital correlation diagram for trigonal planar and pyramidal AH3. Planar of pyramidal geometries? Tetrahedral molecules AH4. Shapes of AH4 systems.

Literature

recommended literature
• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• JEAN, Yves and François VOLATRON. An introduction to molecular orbitals. Edited by Jeremy K. Burdett. New York: Oxford University Press, 1993, xiv, 337. ISBN 0195069188. info

Teaching methods

Lectures, exercises, consultations.

Assessment methods

Written exam (requiring in a major part the formulation of answers, in a minor part a choice from several possibilities) and oral exam (2 items from the syllabus by the teacher's choice, 20 minute time for preparation). Examples of examination tests can be found in the information system.

Language of instruction

Czech

Further comments (probably available only in Czech)

Study Materials
The course is taught annually.

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

C9920 Introduction to Quantum Chemistry and Electronic Structure of Molecules

Extent and Intensity

2/1/0. 3 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Contact Person: doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Mon 1. 10. to Fri 14. 12. Tue 12:00–13:50 B11/335

• Timetable of Seminar Groups:

C9920/01: Mon 17. 9. to Fri 14. 12. Wed 16:00–16:50 C12/311, M. Munzarová
C9920/02: Mon 17. 9. to Fri 14. 12. Wed 15:00–15:50 C12/311, M. Munzarová

Prerequisites

Any of the university introductory classes on mathematics. Sufficient is any of mathematics courses for students of chemistry, biochemistry, or chemistry with teaching specialization.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 8 fields of study the course is directly associated with, display

Course objectives

Characterization of the course: It is a one-semestral introduction to the foundations of quantum chemistry and its applications to the reproduction, the interpretation, and the prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. At the end of the course students should be able to understand the basic quantum mechanics concepts on simple yet real chemical systems; grasp the principles of computational quantum chemistry; be able to use basic rules of the qualitative MO theory that (1) enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Learning outcomes

The skill to create simple orbital-interaction diagrams for simple compounds, understanding of basic quantum chemistry concepts.

Syllabus

• 1. Basic notions of quantum mechanics. The notion of the wavefunction, the wavefunction postulate. Stationary Schrodinger equation. The notion of an operator, an eigenfunction of an operator, an eigenvalue corresponding to an operator and an eigenfunction. Hermitian operator: definition and properties. The coordinate operator, momentum operator, operator of the square of angular momentum, operator of the projection of the angular momentum in the z axis, energy operator - Hamiltonian. Commuting operators and common set of eigenfunctions. 2. Hydrogen atom. Hamiltonian for the fixed H atom and with the introduction of the reduced mass. Coordinate set for a spherically symmetrical system. Eigenstates for negative and positive eigenvalues. The notion of degeneracy, eigenfunctions. Radial factors, radial distribution function. Angular factors as eigenfunctions of momentum operators. Complex and real angular functions. Means of plotting atomic orbitals, the notion of orthogonality. 3. Many-electron atoms. Atomic units. Hamiltonian for the He atom. The meaning of the "orbital" notion. Total wavefunction in relation to one-electron wavefunctions. Total energy in relation to one-electron energies. Exchange symmetry of the wavefunction, electron spin, antisymmetry. Electron configuration of Li, Pauli principle. Slater determinant. Slater orbital. Aufbau principle, Klechowsky and Hund's rules. The evolution of atomic properties in the periodical system. 4. H2+ molecule. Three-particle Hamiltonian. Born-Oppenheimer approximation of the wavefunction. The method of molecular orbitals (MO) as linear combination of atomic orbitals (LCAO). Solution (a) employing symmetry and (b) using the variational method. Overlap integral, interaction integral as functions of internuclear distance. Secular equation, resulting energies and wavefunctions. MO graphical representations, symmetry properties, bonding and antibonding MO. Interaction diagram. 5. Simple Hückel method. Approximation of independent pi-electrons. Hückel determinant, values alpha and beta. Eigenfunctions and eigenvalues. Diagrams for energy levels. Charge densities, pi electron densities, HMO energies: the relation to experimental observables. The principle of extended Hückel method, bases, overlap and interaction integrals, parameter K, eigenfunctions and eigenvalues. Electronic structure of planar hydrocarbons. 6. Molecular symmetry. Symmetry groups. Matrices and their multiplication. Matrix representation of symmetry group. Reducible and irreducible representations. Symbols used for irreducible representations. Symmetry-adapted linear combinations. The use of character tables: zero and non-zero overlap integrals. Symmetry driven orbital interaction. 7. Two-orbital interaction: Molecules A2 and AB. The interaction of two identical and two different AOs. Level occupation, total energy. Overlap and symmetry. Four-AO interaction. Diatomic molecules A2 and AB: basis functions, pi and sigma MOs, s-p interaction, interaction diagrams, electron configurations, bond lengths and energies. 8. Interaction between two fragment orbitals. Linear and bent molecules AH2: The notion of a fragment orbital, symmetry elements, MOs, correlation diagram for linear and bent geometry, geometries of AH2 molecules. Application to BeH2. 9. AH3 and AH4 molecules. MOs of trigonal planar AH3. Orbital correlation diagram for trigonal planar and pyramidal AH3. Planar of pyramidal geometries? Tetrahedral molecules AH4. Shapes of AH4 systems.

Literature

recommended literature
• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• LEVINE, Ira N. Quantum chemistry. 5th ed. Upper Saddle River: Prentice Hall, 1999, x, 739. ISBN 0136855121. info
• JEAN, Yves and François VOLATRON. An introduction to molecular orbitals. Edited by Jeremy K. Burdett. New York: Oxford University Press, 1993, xiv, 337. ISBN 0195069188. info
• ALBRIGHT, Thomas A., Jeremy K. BURDETT and Myung-Hwan WHANGBO. Orbital interactions in chemistry. New York: Wiley, 1985, xv, 447. ISBN 0471873934. URL info

Teaching methods

Lectures, exercises, consultations.

Assessment methods

Written exam (requiring in a major part the formulation of answers, in a minor part a choice from several possibilities) and oral exam (2 items from the syllabus by the teacher's choice, 20 minute time for preparation). Examples of examination tests can be found in the information system.

Language of instruction

Czech

Further comments (probably available only in Czech)

Study Materials
The course is taught annually.

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

C9920 Introduction to Quantum Chemistry and Electronic Structure of Molecules

Extent and Intensity

2/1/0. 3 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Contact Person: doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Mon 18. 9. to Fri 15. 12. Tue 14:00–16:50 C12/311

Prerequisites

Any of the university introductory classes on mathematics. Sufficient is any of mathematics courses for students of chemistry, biochemistry, or chemistry with teaching specialization.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 8 fields of study the course is directly associated with, display

Course objectives

Characterization of the course: It is a one-semestral introduction to the foundations of quantum chemistry and its applications to the reproduction, the interpretation, and the prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. At the end of the course students should be able to understand the basic quantum mechanics concepts on simple yet real chemical systems; grasp the principles of computational quantum chemistry; be able to use basic rules of the qualitative MO theory that (1) enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Learning outcomes

The skill to create simple orbital-interaction diagrams for simple compounds, understanding of basic quantum chemistry concepts.

Syllabus

• 1. Basic notions of quantum mechanics. The notion of the wavefunction, the wavefunction postulate. Stationary Schrodinger equation. The notion of an operator, an eigenfunction of an operator, an eigenvalue corresponding to an operator and an eigenfunction. Hermitian operator: definition and properties. The coordinate operator, momentum operator, operator of the square of angular momentum, operator of the projection of the angular momentum in the z axis, energy operator - Hamiltonian. Commuting operators and common set of eigenfunctions. 2. Hydrogen atom. Hamiltonian for the fixed H atom and with the introduction of the reduced mass. Coordinate set for a spherically symmetrical system. Eigenstates for negative and positive eigenvalues. The notion of degeneracy, eigenfunctions. Radial factors, radial distribution function. Angular factors as eigenfunctions of momentum operators. Complex and real angular functions. Means of plotting atomic orbitals, the notion of orthogonality. 3. Many-electron atoms. Atomic units. Hamiltonian for the He atom. The meaning of the "orbital" notion. Total wavefunction in relation to one-electron wavefunctions. Total energy in relation to one-electron energies. Exchange symmetry of the wavefunction, electron spin, antisymmetry. Electron configuration of Li, Pauli principle. Slater determinant. Slater orbital. Aufbau principle, Klechowsky and Hund's rules. The evolution of atomic properties in the periodical system. 4. H2+ molecule. Three-particle Hamiltonian. Born-Oppenheimer approximation of the wavefunction. The method of molecular orbitals (MO) as linear combination of atomic orbitals (LCAO). Solution (a) employing symmetry and (b) using the variational method. Overlap integral, interaction integral as functions of internuclear distance. Secular equation, resulting energies and wavefunctions. MO graphical representations, symmetry properties, bonding and antibonding MO. Interaction diagram. 5. Simple Hückel method. Approximation of independent pi-electrons. Hückel determinant, values alpha and beta. Eigenfunctions and eigenvalues. Diagrams for energy levels. Charge densities, pi electron densities, HMO energies: the relation to experimental observables. The principle of extended Hückel method, bases, overlap and interaction integrals, parameter K, eigenfunctions and eigenvalues. Electronic structure of planar hydrocarbons. 6. Molecular symmetry. Symmetry groups. Matrices and their multiplication. Matrix representation of symmetry group. Reducible and irreducible representations. Symbols used for irreducible representations. Symmetry-adapted linear combinations. The use of character tables: zero and non-zero overlap integrals. Symmetry driven orbital interaction. 7. Two-orbital interaction: Molecules A2 and AB. The interaction of two identical and two different AOs. Level occupation, total energy. Overlap and symmetry. Four-AO interaction. Diatomic molecules A2 and AB: basis functions, pi and sigma MOs, s-p interaction, interaction diagrams, electron configurations, bond lengths and energies. 8. Interaction between two fragment orbitals. Linear and bent molecules AH2: The notion of a fragment orbital, symmetry elements, MOs, correlation diagram for linear and bent geometry, geometries of AH2 molecules. Application to BeH2. 9. AH3 and AH4 molecules. MOs of trigonal planar AH3. Orbital correlation diagram for trigonal planar and pyramidal AH3. Planar of pyramidal geometries? Tetrahedral molecules AH4. Shapes of AH4 systems.

Literature

recommended literature
• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• LEVINE, Ira N. Quantum chemistry. 5th ed. Upper Saddle River: Prentice Hall, 1999, x, 739. ISBN 0136855121. info
• JEAN, Yves and François VOLATRON. An introduction to molecular orbitals. Edited by Jeremy K. Burdett. New York: Oxford University Press, 1993, xiv, 337. ISBN 0195069188. info
• ALBRIGHT, Thomas A., Jeremy K. BURDETT and Myung-Hwan WHANGBO. Orbital interactions in chemistry. New York: Wiley, 1985, xv, 447. ISBN 0471873934. URL info

Teaching methods

Lectures, exercises, consultations.

Assessment methods

Written exam (requiring in a major part the formulation of answers, in a minor part a choice from several possibilities) and oral exam (2 items from the syllabus by the teacher's choice, 20 minute time for preparation). Examples of examination tests can be found in the information system.

Language of instruction

Czech

Further comments (probably available only in Czech)

Study Materials
The course is taught annually.

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

C9920 Introduction to Quantum Chemistry and Electronic Structure of Molecules

Extent and Intensity

2/1/0. 3 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)
Mgr. Hugo Semrád, Ph.D. (seminar tutor)
doc. Mgr. Jana Pavlů, Ph.D. (assistant)
Mgr. Jakub Stošek, Ph.D. (assistant)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Contact Person: doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Mon 19. 9. to Sun 18. 12. Wed 8:00–10:50 C12/311

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 8 fields of study the course is directly associated with, display

Course objectives

Characterization of the course: It is a one-semestral introduction to the foundations of quantum chemistry and its applications to the reproduction, the interpretation, and the prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. At the end of the course students should be able to understand the basic quantum mechanics concepts on simple yet real chemical systems; grasp the principles of computational quantum chemistry; be able to use basic rules of the qualitative MO theory that (1) enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Syllabus

• 1. Basic notions of quantum mechanics. The notion of the wavefunction, the wavefunction postulate. Stationary Schrodinger equation. The notion of an operator, an eigenfunction of an operator, an eigenvalue corresponding to an operator and an eigenfunction. Hermitian operator: definition and properties. The coordinate operator, momentum operator, operator of the square of angular momentum, operator of the projection of the angular momentum in the z axis, energy operator - Hamiltonian. Commuting operators and common set of eigenfunctions. 2. Hydrogen atom. Hamiltonian for the fixed H atom and with the introduction of the reduced mass. Coordinate set for a spherically symmetrical system. Eigenstates for negative and positive eigenvalues. The notion of degeneracy, eigenfunctions. Radial factors, radial distribution function. Angular factors as eigenfunctions of momentum operators. Complex and real angular functions. Means of plotting atomic orbitals, the notion of orthogonality. 3. Many-electron atoms. Atomic units. Hamiltonian for the He atom. The meaning of the "orbital" notion. Total wavefunction in relation to one-electron wavefunctions. Total energy in relation to one-electron energies. Exchange symmetry of the wavefunction, electron spin, antisymmetry. Electron configuration of Li, Pauli principle. Slater determinant. Slater orbital. Aufbau principle, Klechowsky and Hund's rules. The evolution of atomic properties in the periodical system. 4. H2+ molecule. Three-particle Hamiltonian. Born-Oppenheimer approximation of the wavefunction. The method of molecular orbitals (MO) as linear combination of atomic orbitals (LCAO). Solution (a) employing symmetry and (b) using the variational method. Overlap integral, interaction integral as functions of internuclear distance. Secular equation, resulting energies and wavefunctions. MO graphical representations, symmetry properties, bonding and antibonding MO. Interaction diagram. 5. Simple Hückel method. Approximation of independent pi-electrons. Hückel determinant, values alpha and beta. Eigenfunctions and eigenvalues. Diagrams for energy levels. Charge densities, pi electron densities, HMO energies: the relation to experimental observables. The principle of extended Hückel method, bases, overlap and interaction integrals, parameter K, eigenfunctions and eigenvalues. Electronic structure of planar hydrocarbons. 6. Molecular symmetry. Symmetry groups. Matrices and their multiplication. Matrix representation of symmetry group. Reducible and irreducible representations. Symbols used for irreducible representations. Symmetry-adapted linear combinations. The use of character tables: zero and non-zero overlap integrals. Symmetry driven orbital interaction. 7. Two-orbital interaction: Molecules A2 and AB. The interaction of two identical and two different AOs. Level occupation, total energy. Overlap and symmetry. Four-AO interaction. Diatomic molecules A2 and AB: basis functions, pi and sigma MOs, s-p interaction, interaction diagrams, electron configurations, bond lengths and energies. 8. Interaction between two fragment orbitals. Linear and bent molecules AH2: The notion of a fragment orbital, symmetry elements, MOs, correlation diagram for linear and bent geometry, geometries of AH2 molecules. Application to BeH2. 9. AH3 and AH4 molecules. MOs of trigonal planar AH3. Orbital correlation diagram for trigonal planar and pyramidal AH3. Planar of pyramidal geometries? Tetrahedral molecules AH4. Shapes of AH4 systems. 10. Solids. Orbitals and bands in one dimension. Bloch functions, k, band structures. How does the band run? Density of states. Distorsion of simple systems. Two and three dimensional systems. High-spin and low-spin considerations.

Literature

recommended literature
• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• LEVINE, Ira N. Quantum chemistry. 5th ed. Upper Saddle River: Prentice Hall, 1999, x, 739. ISBN 0136855121. info
• JEAN, Yves and François VOLATRON. An introduction to molecular orbitals. Edited by Jeremy K. Burdett. New York: Oxford University Press, 1993, xiv, 337. ISBN 0195069188. info
• ALBRIGHT, Thomas A., Jeremy K. BURDETT and Myung-Hwan WHANGBO. Orbital interactions in chemistry. New York: Wiley, 1985, xv, 447. ISBN 0471873934. URL info

Teaching methods

Lectures, exercises, consultations.

Assessment methods

Written exam (requiring in a major part the formulation of answers, in a minor part a choice from several possibilities) and oral exam (2 items from the syllabus by the teacher's choice, 20 minute time for preparation)

Language of instruction

Czech

Further Comments

Study Materials
The course is taught annually.

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

C9920 Introduction to Quantum Chemistry and Electronic Structure of Molecules

Extent and Intensity

2/1/0. 3 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)
Cina Foroutannejad, Ph.D. (assistant)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Contact Person: doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Wed 11:00–13:50 C12/311

Prerequisites

A successful examination in C1020 "General chemistry".

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 8 fields of study the course is directly associated with, display

Course objectives

Characterization of the course: It is a one-semestral introduction to the foundations of quantum chemistry and its applications to the reproduction, the interpretation, and the prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. At the end of the course students should be able to understand the basic quantum mechanics concepts on simple yet real chemical systems; grasp the principles of computational quantum chemistry; be able to use basic rules of the qualitative MO theory that (1) enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Syllabus

• 1. Basic notions of quantum mechanics. The notion of the wavefunction, the wavefunction postulate. Stationary Schrodinger equation. The notion of an operator, an eigenfunction of an operator, an eigenvalue corresponding to an operator and an eigenfunction. Hermitian operator: definition and properties. The coordinate operator, momentum operator, operator of the square of angular momentum, operator of the projection of the angular momentum in the z axis, energy operator - Hamiltonian. Commuting operators and common set of eigenfunctions. 2. Hydrogen atom. Hamiltonian for the fixed H atom and with the introduction of the reduced mass. Coordinate set for a spherically symmetrical system. Eigenstates for negative and positive eigenvalues. The notion of degeneracy, eigenfunctions. Radial factors, radial distribution function. Angular factors as eigenfunctions of momentum operators. Complex and real angular functions. Means of plotting atomic orbitals, the notion of orthogonality. 3. Many-electron atoms. Atomic units. Hamiltonian for the He atom. The meaning of the "orbital" notion. Total wavefunction in relation to one-electron wavefunctions. Total energy in relation to one-electron energies. Exchange symmetry of the wavefunction, electron spin, antisymmetry. Electron configuration of Li, Pauli principle. Slater determinant. Slater orbital. Aufbau principle, Klechowsky and Hund's rules. The evolution of atomic properties in the periodical system. 4. H2+ molecule. Three-particle Hamiltonian. Born-Oppenheimer approximation of the wavefunction. The method of molecular orbitals (MO) as linear combination of atomic orbitals (LCAO). Solution (a) employing symmetry and (b) using the variational method. Overlap integral, interaction integral as functions of internuclear distance. Secular equation, resulting energies and wavefunctions. MO graphical representations, symmetry properties, bonding and antibonding MO. Interaction diagram. 5. Simple Hückel method. Approximation of independent pi-electrons. Hückel determinant, values alpha and beta. Eigenfunctions and eigenvalues. Diagrams for energy levels. Charge densities, pi electron densities, HMO energies: the relation to experimental observables. The principle of extended Hückel method, bases, overlap and interaction integrals, parameter K, eigenfunctions and eigenvalues. Electronic structure of planar hydrocarbons. 6. Molecular symmetry. Symmetry groups. Matrices and their multiplication. Matrix representation of symmetry group. Reducible and irreducible representations. Symbols used for irreducible representations. Symmetry-adapted linear combinations. The use of character tables: zero and non-zero overlap integrals. Symmetry driven orbital interaction. 7. Two-orbital interaction: Molecules A2 and AB. The interaction of two identical and two different AOs. Level occupation, total energy. Overlap and symmetry. Four-AO interaction. Diatomic molecules A2 and AB: basis functions, pi and sigma MOs, s-p interaction, interaction diagrams, electron configurations, bond lengths and energies. 8. Interaction between two fragment orbitals. Linear and bent molecules AH2: The notion of a fragment orbital, symmetry elements, MOs, correlation diagram for linear and bent geometry, geometries of AH2 molecules. Application to BeH2. 9. AH3 and AH4 molecules. MOs of trigonal planar AH3. Orbital correlation diagram for trigonal planar and pyramidal AH3. Planar of pyramidal geometries? Tetrahedral molecules AH4. Shapes of AH4 systems. 10. Solids. Orbitals and bands in one dimension. Bloch functions, k, band structures. How does the band run? Density of states. Distorsion of simple systems. Two and three dimensional systems. High-spin and low-spin considerations.

Literature

recommended literature
• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• LEVINE, Ira N. Quantum chemistry. 5th ed. Upper Saddle River: Prentice Hall, 1999, x, 739. ISBN 0136855121. info
• JEAN, Yves and François VOLATRON. An introduction to molecular orbitals. Edited by Jeremy K. Burdett. New York: Oxford University Press, 1993, xiv, 337. ISBN 0195069188. info
• ALBRIGHT, Thomas A., Jeremy K. BURDETT and Myung-Hwan WHANGBO. Orbital interactions in chemistry. New York: Wiley, 1985, xv, 447. ISBN 0471873934. URL info

Teaching methods

Lectures, exercises, consultations.

Assessment methods

Written exam (requiring in a major part the formulation of answers, in a minor part a choice from several possibilities) and oral exam (2 items from the syllabus by the teacher's choice, 20 minute time for preparation)

Language of instruction

Czech

Further Comments

Study Materials
The course is taught annually.

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

C9920 Introduction to Quantum Chemistry and Electronic Structure of Molecules

Extent and Intensity

2/1/0. 3 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)
Cina Foroutannejad, Ph.D. (assistant)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Contact Person: doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Thu 16:00–18:50 C12/311

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 7 fields of study the course is directly associated with, display

Course objectives

Characterization of the course: It is a one-semestral introduction to the foundations of quantum chemistry and its applications to the reproduction, the interpretation, and the prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. At the end of the course students should be able to understand the basic quantum mechanics concepts on simple yet real chemical systems; grasp the principles of computational quantum chemistry; be able to use basic rules of the qualitative MO theory that (1) enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Syllabus

• 1. Basic notions of quantum mechanics. The notion of the wavefunction, the wavefunction postulate. Stationary Schrodinger equation. The notion of an operator, an eigenfunction of an operator, an eigenvalue corresponding to an operator and an eigenfunction. Hermitian operator: definition and properties. The coordinate operator, momentum operator, operator of the square of angular momentum, operator of the projection of the angular momentum in the z axis, energy operator - Hamiltonian. Commuting operators and common set of eigenfunctions. 2. Hydrogen atom. Hamiltonian for the fixed H atom and with the introduction of the reduced mass. Coordinate set for a spherically symmetrical system. Eigenstates for negative and positive eigenvalues. The notion of degeneracy, eigenfunctions. Radial factors, radial distribution function. Angular factors as eigenfunctions of momentum operators. Complex and real angular functions. Means of plotting atomic orbitals, the notion of orthogonality. 3. Many-electron atoms. Atomic units. Hamiltonian for the He atom. The meaning of the "orbital" notion. Total wavefunction in relation to one-electron wavefunctions. Total energy in relation to one-electron energies. Exchange symmetry of the wavefunction, electron spin, antisymmetry. Electron configuration of Li, Pauli principle. Slater determinant. Slater orbital. Aufbau principle, Klechowsky and Hund's rules. The evolution of atomic properties in the periodical system. 4. H2+ molecule. Three-particle Hamiltonian. Born-Oppenheimer approximation of the wavefunction. The method of molecular orbitals (MO) as linear combination of atomic orbitals (LCAO). Solution (a) employing symmetry and (b) using the variational method. Overlap integral, interaction integral as functions of internuclear distance. Secular equation, resulting energies and wavefunctions. MO graphical representations, symmetry properties, bonding and antibonding MO. Interaction diagram. 5. Simple Hückel method. Approximation of independent pi-electrons. Hückel determinant, values alpha and beta. Eigenfunctions and eigenvalues. Diagrams for energy levels. Charge densities, pi electron densities, HMO energies: the relation to experimental observables. The principle of extended Hückel method, bases, overlap and interaction integrals, parameter K, eigenfunctions and eigenvalues. Electronic structure of planar hydrocarbons. 6. Molecular symmetry. Symmetry groups. Matrices and their multiplication. Matrix representation of symmetry group. Reducible and irreducible representations. Symbols used for irreducible representations. Symmetry-adapted linear combinations. The use of character tables: zero and non-zero overlap integrals. Symmetry driven orbital interaction. 7. Two-orbital interaction: Molecules A2 and AB. The interaction of two identical and two different AOs. Level occupation, total energy. Overlap and symmetry. Four-AO interaction. Diatomic molecules A2 and AB: basis functions, pi and sigma MOs, s-p interaction, interaction diagrams, electron configurations, bond lengths and energies. 8. Interaction between two fragment orbitals. Linear and bent molecules AH2: The notion of a fragment orbital, symmetry elements, MOs, correlation diagram for linear and bent geometry, geometries of AH2 molecules. Application to BeH2. 9. AH3 and AH4 molecules. MOs of trigonal planar AH3. Orbital correlation diagram for trigonal planar and pyramidal AH3. Planar of pyramidal geometries? Tetrahedral molecules AH4. Shapes of AH4 systems. 10. Solids. Orbitals and bands in one dimension. Bloch functions, k, band structures. How does the band run? Density of states. Distorsion of simple systems. Two and three dimensional systems. High-spin and low-spin considerations.

Literature

recommended literature
• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• LEVINE, Ira N. Quantum chemistry. 5th ed. Upper Saddle River: Prentice Hall, 1999, x, 739. ISBN 0136855121. info
• JEAN, Yves and François VOLATRON. An introduction to molecular orbitals. Edited by Jeremy K. Burdett. New York: Oxford University Press, 1993, xiv, 337. ISBN 0195069188. info
• ALBRIGHT, Thomas A., Jeremy K. BURDETT and Myung-Hwan WHANGBO. Orbital interactions in chemistry. New York: Wiley, 1985, xv, 447. ISBN 0471873934. URL info

Teaching methods

Lectures, exercises, consultations.

Assessment methods

Written exam (requiring in a major part the formulation of answers, in a minor part a choice from several possibilities) and oral exam (2 items from the syllabus by the teacher's choice, 20 minute time for preparation)

Language of instruction

Czech

Further Comments

Study Materials
The course is taught annually.

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

C9920 Introduction to Quantum Chemistry and Electronic Structure of Molecules

Extent and Intensity

2/1/0. 3 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Contact Person: doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Tue 7:00–9:50 C12/311

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 13 fields of study the course is directly associated with, display

Course objectives

Characterization of the course: It is a one-semestral introduction to the foundations of quantum chemistry and its applications to the reproduction, the interpretation, and the prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. At the end of the course students should be able to understand the basic quantum mechanics concepts on simple yet real chemical systems; grasp the principles of computational quantum chemistry; be able to use basic rules of the qualitative MO theory that (1) enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Syllabus

• 1. Basic notions of quantum mechanics. The notion of the wavefunction, the wavefunction postulate. Stationary Schrodinger equation. The notion of an operator, an eigenfunction of an operator, an eigenvalue corresponding to an operator and an eigenfunction. Hermitian operator: definition and properties. The coordinate operator, momentum operator, operator of the square of angular momentum, operator of the projection of the angular momentum in the z axis, energy operator - Hamiltonian. Commuting operators and common set of eigenfunctions. 2. Hydrogen atom. Hamiltonian for the fixed H atom and with the introduction of the reduced mass. Coordinate set for a spherically symmetrical system. Eigenstates for negative and positive eigenvalues. The notion of degeneracy, eigenfunctions. Radial factors, radial distribution function. Angular factors as eigenfunctions of momentum operators. Complex and real angular functions. Means of plotting atomic orbitals, the notion of orthogonality. 3. Many-electron atoms. Atomic units. Hamiltonian for the He atom. The meaning of the "orbital" notion. Total wavefunction in relation to one-electron wavefunctions. Total energy in relation to one-electron energies. Exchange symmetry of the wavefunction, electron spin, antisymmetry. Electron configuration of Li, Pauli principle. Slater determinant. Slater orbital. Aufbau principle, Klechowsky and Hund's rules. The evolution of atomic properties in the periodical system. 4. H2+ molecule. Three-particle Hamiltonian. Born-Oppenheimer approximation of the wavefunction. The method of molecular orbitals (MO) as linear combination of atomic orbitals (LCAO). Solution (a) employing symmetry and (b) using the variational method. Overlap integral, interaction integral as functions of internuclear distance. Secular equation, resulting energies and wavefunctions. MO graphical representations, symmetry properties, bonding and antibonding MO. Interaction diagram. 5. Simple Hückel method. Approximation of independent pi-electrons. Hückel determinant, values alpha and beta. Eigenfunctions and eigenvalues. Diagrams for energy levels. Charge densities, pi electron densities, HMO energies: the relation to experimental observables. The principle of extended Hückel method, bases, overlap and interaction integrals, parameter K, eigenfunctions and eigenvalues. Electronic structure of planar hydrocarbons. 6. Molecular symmetry. Symmetry groups. Matrices and their multiplication. Matrix representation of symmetry group. Reducible and irreducible representations. Symbols used for irreducible representations. Symmetry-adapted linear combinations. The use of character tables: zero and non-zero overlap integrals. Symmetry driven orbital interaction. 7. Two-orbital interaction: Molecules A2 and AB. The interaction of two identical and two different AOs. Level occupation, total energy. Overlap and symmetry. Four-AO interaction. Diatomic molecules A2 and AB: basis functions, pi and sigma MOs, s-p interaction, interaction diagrams, electron configurations, bond lengths and energies. 8. Interaction between two fragment orbitals. Linear and bent molecules AH2: The notion of a fragment orbital, symmetry elements, MOs, correlation diagram for linear and bent geometry, geometries of AH2 molecules. Application to BeH2. 9. AH3 and AH4 molecules. MOs of trigonal planar AH3. Orbital correlation diagram for trigonal planar and pyramidal AH3. Planar of pyramidal geometries? Tetrahedral molecules AH4. Shapes of AH4 systems. 10. Solids. Orbitals and bands in one dimension. Bloch functions, k, band structures. How does the band run? Density of states. Distorsion of simple systems. Two and three dimensional systems. High-spin and low-spin considerations.

Literature

recommended literature
• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• LEVINE, Ira N. Quantum chemistry. 5th ed. Upper Saddle River: Prentice Hall, 1999, x, 739. ISBN 0136855121. info
• JEAN, Yves and François VOLATRON. An introduction to molecular orbitals. Edited by Jeremy K. Burdett. New York: Oxford University Press, 1993, xiv, 337. ISBN 0195069188. info
• ALBRIGHT, Thomas A., Jeremy K. BURDETT and Myung-Hwan WHANGBO. Orbital interactions in chemistry. New York: Wiley, 1985, xv, 447. ISBN 0471873934. URL info

Teaching methods

Lectures, exercises, consultations.

Assessment methods

Written exam (requiring in a major part the formulation of answers, in a minor part a choice from several possibilities) and oral exam (2 items from the syllabus by the teacher's choice, 20 minute time for preparation)

Language of instruction

Czech

Further Comments

Study Materials
The course is taught annually.

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

C9920 Introduction to Quantum Chemistry and Electronic Structure of Molecules

Extent and Intensity

2/1/0. 3 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Contact Person: doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Wed 12:00–14:50 C12/311

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 13 fields of study the course is directly associated with, display

Course objectives

Characterization of the course: It is a one-semestral introduction to the foundations of quantum chemistry and its applications to the reproduction, the interpretation, and the prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. At the end of the course students should be able to understand of basic quantum mechanics concepts on simple yet real chemical systems; grasping of principles of computational quantum chemistry; learning of basic rules of the qualitative MO theory that (1)enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Syllabus

• 1. Basic notions of quantum mechanics. The notion of the wavefunction, the wavefunction postulate. Stationary Schroedinger equation. The notion of an operator, an eigenfunction of an operator, an eigenvalue corresponding to an operator and an eigenfunction. Hermitian operator: definition and properties. The coordinate operator, momentum operator, operator of the square of angular momentum, operator of the projection of the angular momentum in the z axis, energy operator - Hamiltonian. Commuting operators and common set of eigenfunctions. 2. Hydrogen atom. Hamiltonian for the fixed H atom and with the introduciton of the reduced mass. Coordinate set for a spherically symmetrical system. Eigenstates for negative and positive eigenvalues. The notion of degeneracy, eigenfunctions. Radial factors, radial distribution function. Angular factors as eigenfunctions of momentum operators. Complex and real angular functions. Means of plotting atomic orbitals, the notion of orthogonality. 3. Many-electron atoms. Atomic units. Hamiltonian for the He atom. The meaning of the "orbital" notion. Total wavefunction in relation to one-electron wavefunctions. Total energy in relation to one-electron energies. Exchange symmetry of the wavefunction, electron spin, antisymmetry. Electron configuration of Li, Pauli principle. Slater determinant. Slater orbital. Aufbau principle, Klechowsky and Hund's rules. The evolution of atomic properties in the periodical system. 4. H2+ molecule. Three-particle Hamiltonian. Born-Oppenheimer approximation of the wavefunction. The method of molecular orbitals (MO) as linear combination of atomic orbitals (LCAO). Solution (a) employing symmetry and (b) using the variational method. Overlap integral, interaction integral as functions of inetrnuclear distance. Secular equation, resulting energies and wavefunctions. MO graphical representations, symmetry properties, bonding and antibonding MO. Interaction diagram. 5. Simple Hückel method. Approximation of independent pi-electrons. Hückel determinant, values alpha and beta. Eigenfunctions and eigenvalues. Diagrams for energy levels. Charge densities, pi electron densities, HMO energies: the relation to experimental observables. The principle of extended Hückel method, bases, overlap and interaction integrals, parameter K, eigenfunctions and eigenvalues. Electronic structure of planar hydrocarbons. 6. Molecular symmetry. Symmetry groups. Matrices and their multiplication. Matrix representation of symmetry group. Reducible and irreducible representations. Symbols used for irreducible representations. Symmetry-adapted linear combinations. The use of character tables: zero and non-zero overlap integrals. Symmetry driven orbital interaction. 7. Two-orbital interaction: Molecules A2 and AB. The interaction of two identical and two different AOs. Level occupation, total energy. Overlap and symmetry. Four-AO interaction. Diatomic molecules A2 and AB: basis functions, pi and sigma MOs, s-p interaction, interaction diagrams, electron configurations, bond lengths and energies. 8. Interaction between two fragment orbitals. Linear and bent molecules AH2: The notion of a fragment orbital, symmetry elements, MOs, correlation diagram for linear and bent geometry, geometries of AH2 molecules. Application to BeH2. 9. AH3 and AH4 molecules. MOs of trigonaly planar AH3. Orbital correlation diagram for trigonaly planar and pyramidal AH3. Planar of pyramidal geometries? Tetrahedral molecules AH4. Shapes of AH4 systems. 10. Solids. Orbitals and bands in one dimension. Bloch functions, k, band structures. How does the band run? Density of states. Distorsion of simple systems. Two and three dimensional systems. High-spin and low-spin considerations.

Literature

recommended literature
• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• LEVINE, Ira N. Quantum chemistry. 5th ed. Upper Saddle River: Prentice Hall, 1999, x, 739. ISBN 0136855121. info
• JEAN, Yves and François VOLATRON. An introduction to molecular orbitals. Edited by Jeremy K. Burdett. New York: Oxford University Press, 1993, xiv, 337. ISBN 0195069188. info
• ALBRIGHT, Thomas A., Jeremy K. BURDETT and Myung-Hwan WHANGBO. Orbital interactions in chemistry. New York: Wiley, 1985, xv, 447. ISBN 0471873934. URL info

Teaching methods

Lectures, exercises, consultations.

Assessment methods

Written test.

Language of instruction

Czech

Further Comments

Study Materials
The course is taught annually.

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

C9920 Introduction to Quantum Chemistry

Extent and Intensity

2/1/0. 3 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
National Centre for Biomolecular Research – Faculty of Science

Timetable

Tue 11:00–12:50 C04/211, Tue 13:00–13:50 C04/211

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

• Chemoinformatics and Bioinformatics (programme PřF, B-BCH)

Course objectives

Characterization of the course: It is a one-semestral introduction to the foundations of quantum chemistry and its applications to the reproduction, the interpretation, and the prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. At the end of the course students should be able to understand of basic quantum mechanics concepts on simple yet real chemical systems; grasping of principles of computational quantum chemistry; learning of basic rules of the qualitative MO theory that (1)enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Syllabus

• 1. Basic concepts of quantum mechanics. History and state-of-the-art of quantum chemistry (QCH). 2. Hydrogen atom. 3. Many-electron atoms. 4. Molecular ion H2+ : The MO-LCAO method. 5. Many-electron molecules: The simple and extended Hueckel Molecular Orbital Methods(HMO a EHT). 6. A qualitative description of electronic structure. Molecular symmetry. Orbital interactions. 7. Interaction andf correlation diagrams of small molecules. 8. "Ab initio" quantum chemistry: The Hartree-Fock (HF) method. 9. Post-HF methods: Configuration Interaction (CI), Moeller-Plesset perturbation theory (MP), The Coupled Cluster method (CC). 10. Density Functional Theory (DFT). 11. The hierarchy of ab initio methods, their relationship to the classical and quantum molecular dynamics (MD). 12. Strategies of ab inito methods application to the problems of chemical interest. Main objectives: Understanding of basic quantum mechanics concepts on simple yet real chemical systems; grasping of principles of computational quantum chemistry; learning of basic rules of the qualitative MO theory that (1)enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Literature

• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• LEVINE, Ira N. Quantum chemistry. 5th ed. Upper Saddle River: Prentice Hall, 1999, x, 739. ISBN 0136855121. info
• PILAR, Frank L. Elementary quantum chemistry. 2nd ed. New York: McGraw-Hill Publishing Company, 1990, xvi, 599 s. ISBN 0-07-050093-2. info
• KOCH, Wolfram and Max C. HOLTHAUSEN. A chemist's guide to density functional theory. 2nd ed. Weinheim: Wiley-VCH, 2001, xiii, 300. ISBN 3527304223. info

Teaching methods

Lectures including discussion, consultations.

Assessment methods

Oral exam.

Language of instruction

Czech

Further Comments

Study Materials

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

C9920 Introduction to Quantum Chemistry

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
National Centre for Biomolecular Research – Faculty of Science

Timetable

Wed 8:00–9:50 C12/311

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

• Chemoinformatics and Bioinformatics (programme PřF, B-BCH)

Course objectives

Characterization of the course: It is a one-semestral introduction to the foundations of quantum chemistry and its applications to the reproduction, the interpretation, and the prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. At the end of the course students should be able to understand of basic quantum mechanics concepts on simple yet real chemical systems; grasping of principles of computational quantum chemistry; learning of basic rules of the qualitative MO theory that (1)enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Syllabus

• 1. Basic concepts of quantum mechanics. History and state-of-the-art of quantum chemistry (QCH). 2. Hydrogen atom. 3. Many-electron atoms. 4. Molecular ion H2+ : The MO-LCAO method. 5. Many-electron molecules: The simple and extended Hueckel Molecular Orbital Methods(HMO a EHT). 6. A qualitative description of electronic structure. Molecular symmetry. Orbital interactions. 7. Interaction andf correlation diagrams of small molecules. 8. "Ab initio" quantum chemistry: The Hartree-Fock (HF) method. 9. Post-HF methods: Configuration Interaction (CI), Moeller-Plesset perturbation theory (MP), The Coupled Cluster method (CC). 10. Density Functional Theory (DFT). 11. The hierarchy of ab initio methods, their relationship to the classical and quantum molecular dynamics (MD). 12. Strategies of ab inito methods application to the problems of chemical interest. Main objectives: Understanding of basic quantum mechanics concepts on simple yet real chemical systems; grasping of principles of computational quantum chemistry; learning of basic rules of the qualitative MO theory that (1)enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Literature

• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• LEVINE, Ira N. Quantum chemistry. 5th ed. Upper Saddle River: Prentice Hall, 1999, x, 739. ISBN 0136855121. info
• PILAR, Frank L. Elementary quantum chemistry. 2nd ed. New York: McGraw-Hill Publishing Company, 1990, xvi, 599 s. ISBN 0-07-050093-2. info
• KOCH, Wolfram and Max C. HOLTHAUSEN. A chemist's guide to density functional theory. 2nd ed. Weinheim: Wiley-VCH, 2001, xiii, 300. ISBN 3527304223. info

Teaching methods

Lectures including discussion, consultations.

Assessment methods

Oral exam.

Language of instruction

Czech

Further Comments

Study Materials

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

C9920 Introduction to Quantum Chemistry

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
National Centre for Biomolecular Research – Faculty of Science

Timetable

Thu 8:00–9:50 C04/211

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

• Chemoinformatics and Bioinformatics (programme PřF, B-BCH)

Course objectives

Characterization of the course: It is a one-semestral introduction to the foundations of quantum chemistry and its applications to the reproduction, the interpretation, and the prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. At the end of the course students should be able to understand of basic quantum mechanics concepts on simple yet real chemical systems; grasping of principles of computational quantum chemistry; learning of basic rules of the qualitative MO theory that (1)enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Syllabus

• 1. Basic concepts of quantum mechanics. History and state-of-the-art of quantum chemistry (QCH). 2. Hydrogen atom. 3. Many-electron atoms. 4. Molecular ion H2+ : The MO-LCAO method. 5. Many-electron molecules: The simple and extended Hueckel Molecular Orbital Methods(HMO a EHT). 6. A qualitative description of electronic structure. Molecular symmetry. Orbital interactions. 7. Interaction andf correlation diagrams of small molecules. 8. "Ab initio" quantum chemistry: The Hartree-Fock (HF) method. 9. Post-HF methods: Configuration Interaction (CI), Moeller-Plesset perturbation theory (MP), The Coupled Cluster method (CC). 10. Density Functional Theory (DFT). 11. The hierarchy of ab initio methods, their relationship to the classical and quantum molecular dynamics (MD). 12. Strategies of ab inito methods application to the problems of chemical interest. Main objectives: Understanding of basic quantum mechanics concepts on simple yet real chemical systems; grasping of principles of computational quantum chemistry; learning of basic rules of the qualitative MO theory that (1)enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Literature

• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• LEVINE, Ira N. Quantum chemistry. 5th ed. Upper Saddle River: Prentice Hall, 1999, x, 739. ISBN 0136855121. info
• PILAR, Frank L. Elementary quantum chemistry. 2nd ed. New York: McGraw-Hill Publishing Company, 1990, xvi, 599 s. ISBN 0-07-050093-2. info
• KOCH, Wolfram and Max C. HOLTHAUSEN. A chemist's guide to density functional theory. 2nd ed. Weinheim: Wiley-VCH, 2001, xiii, 300. ISBN 3527304223. info

Teaching methods

Lectures including discussion, consultations.

Assessment methods

Oral exam.

Language of instruction

Czech

Further Comments

Study Materials

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

C9920 Introduction to Quantum Chemistry

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
National Centre for Biomolecular Research – Faculty of Science

Timetable

Tue 9:00–10:50 C04/211

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

• Chemoinformatics and Bioinformatics (programme PřF, B-BCH)

Course objectives

Characterization of the course: It is a one-semestral introduction to the foundations of quantum chemistry and its applications to the reproduction, the interpretation, and the prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. Main objectives: Understanding of basic quantum mechanics concepts on simple yet real chemical systems; grasping of principles of computational quantum chemistry; learning of basic rules of the qualitative MO theory that (1)enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Syllabus

• 1. Basic concepts of quantum mechanics. History and state-of-the-art of quantum chemistry (QCH). 2. Hydrogen atom. 3. Many-electron atoms. 4. Molecular ion H2+ : The MO-LCAO method. 5. Many-electron molecules: The simple and extended Hueckel Molecular Orbital Methods(HMO a EHT). 6. A qualitative description of electronic structure. Molecular symmetry. Orbital interactions. 7. Interaction andf correlation diagrams of small molecules. 8. "Ab initio" quantum chemistry: The Hartree-Fock (HF) method. 9. Post-HF methods: Configuration Interaction (CI), Moeller-Plesset perturbation theory (MP), The Coupled Cluster method (CC). 10. Density Functional Theory (DFT). 11. The hierarchy of ab initio methods, their relationship to the classical and quantum molecular dynamics (MD). 12. Strategies of ab inito methods application to the problems of chemical interest. Main objectives: Understanding of basic quantum mechanics concepts on simple yet real chemical systems; grasping of principles of computational quantum chemistry; learning of basic rules of the qualitative MO theory that (1)enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Literature

• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• LEVINE, Ira N. Quantum chemistry. 5th ed. Upper Saddle River: Prentice Hall, 1999, x, 739. ISBN 0136855121. info
• PILAR, Frank L. Elementary quantum chemistry. 2nd ed. New York: McGraw-Hill Publishing Company, 1990, xvi, 599 s. ISBN 0-07-050093-2. info
• KOCH, Wolfram and Max C. HOLTHAUSEN. A chemist's guide to density functional theory. 2nd ed. Weinheim: Wiley-VCH, 2001, xiii, 300. ISBN 3527304223. info

Assessment methods

Teaching methods used: lectures, class discussion, presentation of lecturer's scientific results and corresponding discussion, homeworks, reading from recommended literature. Finalization demands: oral exam.

Language of instruction

Czech

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

C9920 Introduction to Quantum Chemistry

The information about the term Autumn 2011 - acreditation is not made public

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
National Centre for Biomolecular Research – Faculty of Science

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

• Chemoinformatics and Bioinformatics (programme PřF, B-BCH)

Course objectives

Characterization of the course: It is a one-semestral introduction to the foundations of quantum chemistry and its applications to the reproduction, the interpretation, and the prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. At the end of the course students should be able to understand of basic quantum mechanics concepts on simple yet real chemical systems; grasping of principles of computational quantum chemistry; learning of basic rules of the qualitative MO theory that (1)enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Syllabus

• 1. Basic concepts of quantum mechanics. History and state-of-the-art of quantum chemistry (QCH). 2. Hydrogen atom. 3. Many-electron atoms. 4. Molecular ion H2+ : The MO-LCAO method. 5. Many-electron molecules: The simple and extended Hueckel Molecular Orbital Methods(HMO a EHT). 6. A qualitative description of electronic structure. Molecular symmetry. Orbital interactions. 7. Interaction andf correlation diagrams of small molecules. 8. "Ab initio" quantum chemistry: The Hartree-Fock (HF) method. 9. Post-HF methods: Configuration Interaction (CI), Moeller-Plesset perturbation theory (MP), The Coupled Cluster method (CC). 10. Density Functional Theory (DFT). 11. The hierarchy of ab initio methods, their relationship to the classical and quantum molecular dynamics (MD). 12. Strategies of ab inito methods application to the problems of chemical interest. Main objectives: Understanding of basic quantum mechanics concepts on simple yet real chemical systems; grasping of principles of computational quantum chemistry; learning of basic rules of the qualitative MO theory that (1)enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Literature

• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• LEVINE, Ira N. Quantum chemistry. 5th ed. Upper Saddle River: Prentice Hall, 1999, x, 739. ISBN 0136855121. info
• PILAR, Frank L. Elementary quantum chemistry. 2nd ed. New York: McGraw-Hill Publishing Company, 1990, xvi, 599 s. ISBN 0-07-050093-2. info
• KOCH, Wolfram and Max C. HOLTHAUSEN. A chemist's guide to density functional theory. 2nd ed. Weinheim: Wiley-VCH, 2001, xiii, 300. ISBN 3527304223. info

Teaching methods

Lectures including discussion, consultations.

Assessment methods

Oral exam.

Language of instruction

Czech

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

C9920 Introduction to Quantum Chemistry

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

doc. Mgr. Markéta Munzarová, Dr. rer. nat. (lecturer)

Guaranteed by

doc. Mgr. Markéta Munzarová, Dr. rer. nat.
National Centre for Biomolecular Research – Faculty of Science

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

• Chemoinformatics and Bioinformatics (programme PřF, B-BCH)

Course objectives

Characterization of the course: It is a one-semestral introduction to the foundations of quantum chemistry and its applications to the reproduction, the interpretation, and the prediction of experimental data for systems of chemical interest. The course is intended for putting a theoretical foundation needed by students, who consider using methods of quantum chemistry in their own scientific work or those who already started doing so. The mathematical formalism used is reduced to a minimum, and the basic quantum-mechanics concepts are introduced within the course using given examples. At the end of the course students should be able to understand of basic quantum mechanics concepts on simple yet real chemical systems; grasping of principles of computational quantum chemistry; learning of basic rules of the qualitative MO theory that (1)enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Syllabus

• 1. Basic concepts of quantum mechanics. History and state-of-the-art of quantum chemistry (QCH). 2. Hydrogen atom. 3. Many-electron atoms. 4. Molecular ion H2+ : The MO-LCAO method. 5. Many-electron molecules: The simple and extended Hueckel Molecular Orbital Methods(HMO a EHT). 6. A qualitative description of electronic structure. Molecular symmetry. Orbital interactions. 7. Interaction andf correlation diagrams of small molecules. 8. "Ab initio" quantum chemistry: The Hartree-Fock (HF) method. 9. Post-HF methods: Configuration Interaction (CI), Moeller-Plesset perturbation theory (MP), The Coupled Cluster method (CC). 10. Density Functional Theory (DFT). 11. The hierarchy of ab initio methods, their relationship to the classical and quantum molecular dynamics (MD). 12. Strategies of ab inito methods application to the problems of chemical interest. Main objectives: Understanding of basic quantum mechanics concepts on simple yet real chemical systems; grasping of principles of computational quantum chemistry; learning of basic rules of the qualitative MO theory that (1)enable an orientation in computed data and (2) make a link towards concepts used by experimentalists.

Literature

• LOWE, John P. Quantum chemistry. 2nd ed. San Diego: Academic Press, 1993, xx, 711. ISBN 0124575552. info
• LEVINE, Ira N. Quantum chemistry. 5th ed. Upper Saddle River: Prentice Hall, 1999, x, 739. ISBN 0136855121. info
• PILAR, Frank L. Elementary quantum chemistry. 2nd ed. New York: McGraw-Hill Publishing Company, 1990, xvi, 599 s. ISBN 0-07-050093-2. info
• KOCH, Wolfram and Max C. HOLTHAUSEN. A chemist's guide to density functional theory. 2nd ed. Weinheim: Wiley-VCH, 2001, xiii, 300. ISBN 3527304223. info

Teaching methods

Lectures including discussion, consultations.

Assessment methods

Oral exam.

Language of instruction

Czech

Listed among pre-requisites of other courses

• C9930 Methods of Quantum Chemistry
  C9920  

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