C1800 Chemistry for Physicists

Faculty of Science
Spring 2024
Extent and Intensity
3/1/0. 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)
Guaranteed by
doc. Mgr. Markéta Munzarová, Dr. rer. nat.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Mon 19. 2. to Sun 26. 5. Tue 8:00–9:50 F3,03015, Thu 8:00–9:50 C12/311
Prerequisites
Finalization of basic physical courses in the extent of the recommended study plan for the first three semesters of study field Nanotechnology.
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
Course objectives
The goal of the course is to equip students with an insight in chemical thinking in the fields of general, physical, inorganic, and organic chemistry.
Learning outcomes
A solid foundation in general, physical, organic, and inorganic chemistry. A deepening of the understanding of the structure of substances obtained in physics subjects, enriched with an insight into reactivity. Skills necessary for understanding chemical literature in the field of a bachelor's or diploma project.
Syllabus
  • 1. The Hydrogen Atom: The Quantum World
  • 1.1 Particle in a potential well. 1.2 Atomic spectrum of hydrogen. 1.3 Principal quantum number. 1.4 Atomic orbitals and other quantum numbers.
  • 2. Multi-electron atoms and periodicity
  • 2.1 Electron spin. 2.2 Orbital energy. 2.3 Construction principle. 2.4 Effective charge and Slater's rules. 2.5 Atomic and ionic hemispheres. 2.6 Ionization energy and electron affinity. 2.7 Inert couple effect and diagonal relationships.
  • 3. Chemical bonds
  • 3.1 Ionic bonds and interactions between ions. 3.2 Electron configurations of ions and Lewis symbols. 3.3 Nature of covalent bond and Lewis structure. 3.4 Polyatomic Lewis structures and resonances. 3.5 Formal charge. 3.6 Exceptions to the Octet Rule. 3.7 Ionic vs. covalent bonds: Electronegativity and polarizability. 3.8 Chemical bond strengths and lengths, rotational levels and vibrational spectra.
  • 4. Molecular shape and structure
  • 4.1 Basic VSEPR model and molecules with lone pairs on the central atom. 4.2 Polar molecules. 4.3 Sigma and pi bonds, hybridization of orbitals. 4.4 Bonds in hydrocarbons and characteristics of double bonds. 4.5 Molecular orbitals for diatomic molecules A2 and electron configurations. 4.6 Pi molecular orbitals of planar hydrocarbons.
  • 5. Chemical applications of the 1st and 2nd laws of thermodynamics
  • 5.1 Heat transfers at constant pressure and enthalpy of physical transformations. 5.2 Reaction enthalpy and relation to internal energy change. 5.3 Hess's law and heat outputs of selected types of reactions. 5.4 Born-Haber cycle. 5.5 Global entropy changes: System, environment, and total entropy change. 5.6 Gibbs energy and non-expansion work.
  • 6. Description of mixtures and chemical balance
  • 6.1 Solubility of a gas in a liquid and Henry's law. 6.2 Molarity and molality of a solution. 6.3 Raoult's law. An increase in the boiling point and a decrease in the melting point. Osmosis. 6.4 Reactions in equilibrium: reversibility, equilibrium and the law of mass action. 6.5 Equilibrium constant expressed in terms of partial pressures. 6.6 Equilibrium influence: Change in amount of reactants/products, effect of pressure and effect of temperature. 6.7 Catalysts and Haber's contribution.
  • 7. Acids and bases, oxidation and reduction.
  • 7.1 Broensted and Lewis acids and bases. 7.2 Proton exchange between water molecules and the pH scale. 7.3 Weak and strong acids and bases. 7.4 Structure of molecules and strength of acids. 7.5 Writing and balancing redox reactions. 7.6 Galvanic cells. 7.7 Standard potentials and electrochemical series. 7.8 Nernst equation. 7.9 Electrolysis and its applications, corrosion.
  • 8. The first four main groups of the periodic table.
  • 8.1 Hydrogen as an element and hydrogen compounds. 8.2 Group 1 - alkali metals. Elements. Chemical properties. Li, Na and K compounds. 8.3 Elements of the 2nd group. Compounds of beryllium, magnesium and calcium. 8.4 Group 13/III elements. 8.5 Oxides and halides of group 13/III. 8.6 Boranes and boron hydrides. 8.7 Elements of group 14/IV. 8.8 Oxides of carbon and silicon. 8.9 Other important compounds of group 14/IV.
  • 9. The last four groups of the periodic table.
  • 9.1 Elements of group 15/V. 9.2 Compounds with hydrogen and halogens. 9.3 Nitrogen and sulfur oxides and acids. 9.4 Group 16/VI elements and their compounds with hydrogen. 9.5 Sulfur oxides and acids. 9.6 Group 17/VII elements and their compounds. 9.7 Group 18/VIII elements, noble gas compounds.
Literature
    recommended literature
  • ATKINS, P. W. and Loretta JONES. Chemical principles : the quest for insight. 4th ed. New York: W.H. Freeman and Company, 2008, xxv, [1026. ISBN 9780716773559. info
Teaching methods
Lectures and exercies with the employment of a whiteboard.
Assessment methods
Written test with a maximum score of 60 points with a following oral discussion. For a mastering of the course, a minimum score of 30 points for the written part is required.
Language of instruction
Czech
Further comments (probably available only in Czech)
Study Materials
The course can also be completed outside the examination period.
The course is taught annually.
The course is also listed under the following terms Spring 2017, spring 2018, Spring 2019, Spring 2020, Spring 2021, Spring 2022, Spring 2023, Spring 2025.
  • Enrolment Statistics (Spring 2024, recent)
  • Permalink: https://is.muni.cz/course/sci/spring2024/C1800