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Welcome page > Faculty of Nuclear Sciences and Physical Engineering > Department of Nuclear Chemistry > General Chemistry 1

General Chemistry 1

The course is not on the list Without time-table
Code Completion Credits Range
15CH1 Z 3 2+1
Vztahy:
In order to register for the course 15CH2, the student must have received credit for the course 15CH1 in a previous semester.
Garant předmětu:
Lecturer:
Tutor:
Supervisor:
Department of Nuclear Chemistry
Synopsis:

The most important concepts, quantities and units used in chemistry are introduced in the course General Chemistry I. Their significance and practical use are illustrated by examples solved in exercises.

Requirements:

Chemistry knowledge at secondary school level.

Syllabus of lectures:

1.Chemistry and its disciplines in natural sciences system, the change of the state of a system (process) as the result of energy/mass transfer, the change of the quality of substance resulting from chemical process (chemical reaction), the classification of substances, elements, compounds.

2.Elementary structural units of substances, atoms, molecules, proportional mass (weight) of atoms and molecules, molar amount of matter and its unit mole, associated molar quantities and their use in stoichiometric calculations.

3.Chemical nomenclature, empirical (stoichiometric), molecular, structural and structural-electronic (Lewis) formulas.

4.Electronegativity and its connection with chemical properties of elements, oxidation state (oxidation number) and the formal charge of an atom, their significance.

5.The composition of material systems, concentrations and units, calculations with concentration data.

6.Chemical reactions classification, chemical equations, balancing chemical equations, the work with chemical equations, stoichiometric calculations using chemical equations.

7.The structure of atoms I: Quantum and wave - mechanical model of atom, the types of atomic orbitals and their characterisation.

8.The structure of atoms II: The arrangement of electron shell (aufbau principle), valence shell, valence electrons.

9.The structure of molecules I: The substance of chemical bond, classification of chemical bonds, the order of bond (multiplied bonds), bond energy and bond length.

10.The structure of molecules II: The wave - mechanical concept of chemical binding, molecular orbitals as the combination of valence atomic orbitals, binding, antibinding and non-effective molecular orbitals, application on diatomic molecules.

11.Ideal gas, ideal-gas equation of state, the mixtures of ideal gases, partial pressures and partial volumes of individual components, Ostwald's law, applications on gaseous systems calculations.

12.Real gases, Van der Waals equation of state, the critical state of matter, the connection between gaseous and liquid state of matter.

13.Periodical system of elements.

Syllabus of tutorials:

1.Chemical calculations involving basic quantities (molar mass, molar amount of matter, molar volume).

2.Electronegativity, oxidation number determination.

3.Chemical nomenclature, types of chemical formulas, their development.

4.Concentration quantities, concentration calculations.

5.Chemical equations balancing, the use in stoichiometric calculations, chemical equations combining.

6.Electron configuration of free atoms of elements, periodic system of elements, group trends of chemical properties of elements.

7.Chemical bonds sigma, pi, delta, the development of structural electronic formulas of diatomic molecule using molecular orbital (MO) theory, application of MO theory onto polyatomic molecules.

8.Gas phase, application of the state equation of ideal gas, mixtures of gases, partial pressure, partial volume, using in calculations.

Study Objective:

The course General Chemistry I provides sufficient information in basic chemical concepts, quantities and units for the students of non-chemical specializations.

Study materials:

Key references:

1.Chang, R.: Chemistry, ninth edition, McGraw-Hill, New York, 2007

2.Zumdahl, S.: Chemical Principles, D. C. Heath and Company, Canada, USA,1992

Recommended references:

1.Dickerson, R., Gray, H., Haight, G.: Chemical Principles, 3.vydání, The Benjamin Cummings Publishing Company, Inc., Menlo Park, California, 1979

2.Campbell, J.: Chemical Systems, W. H. Freeman and Company, San Francisco, 1970

Note:
Further information:
No time-table has been prepared for this course
The course is a part of the following study plans:
Data valid to 2024-06-16
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