PřF:C1601 General and Inorg. Chemistry - Course Information

C1601 General and Inorganic Chemistry

Extent and Intensity

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

Teacher(s)

doc. Mgr. Marek Nečas, Ph.D. (lecturer)
Mgr. Martin Sojka, Ph.D. (seminar tutor)

Guaranteed by

doc. Mgr. Marek Nečas, Ph.D.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Wed 15:00–16:50 B11/132

Prerequisites

! C1020 General Chemistry && ! C1021 General Chemistry
Knowledge of chemistry on secondary school level.

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 17 fields of study the course is directly associated with, display

Course objectives

At the end of this course, students should be able to: explain basic chemical principles; interpret electronic structure of atoms and chemical bonding theories; describe chemical reactions along with energy changes; discuss the states of matter and phase transitions. They should also be able to describe the elements and their common compounds.

Syllabus

• 1. Matter, compounds and mixtures. Basic chemistry concepts. Atomic mass unit, atomic and molecular weights. Avogadro's constant. Relative atomic and molecular masses. Mole, molar mass. Atoms, molecules, ions, elements, nuclides, and isotopes. Atomic nucleus, mass defect (nuclear binding energy), nuclear stability, alpha, beta, gamma - emission, natural and artificial radioactivity, Fajans-Soddy rules, nuclear reactions. Usage of isotopes. 2. Structure of atom, electromagnetic emission. Wave-particle dualistic character of matter. Atomic orbitals, quantum numbers, energy levels, electronic configuration, valence electrons. Periodic law and the system of elements. Periodic trends. 3. Molecular structure. Chemical bonding and its parameters, weak bonding interactions (van der Waals forces, hydrogen bond). Molecular geometry. 4. Gas properties, ideal vs. real gas, gas mixtures. Ideal gas equation of state and the other ideal gas laws. General properties of liquids, vapor pressure, boiling point. Structure and properties of solids, fundamental structure types. Phase transitions. The phase diagram for water. 5. Solutions, solubility, expressing concentration of solutions, calculation of concentrations. Polar and non-polar solvents. Two-component phase diagrams. Separation methods. 6. Thermodynamic and kinetic aspects of chemical reactions. Elementary concepts in chemical thermodynamics, thermochemistry. Chemical equilibrium, Gibbs free energy, spontaneous reactions. Reaction rates and catalysis. 7. Acids and bases. Water and its dissociation. Acidity and basicity of water solutions. The strength of acids and bases. pH calculations, salt hydrolysis, buffers. 8. Oxidation and reduction. Electrochemistry, electrode potential, galvanic and electrolytic cells, material corrosion. 9. Introduction into systematic inorganic chemistry. General properties of transition and non-transition metals, non-metals, and metalloids, daltonides and berthollides. Hydrogen. Alkaline metals and alkaline earths. Boron and aluminium. 10. Carbon and its allotropes, carbides, oxides, carbon acids salts and derivatives. Silicon, silicon dioxide, silicates and their importance. 11. Elementary nitrogen and phosphorus. Ammonia and Haber-Bosch process, azides, oxides, and oxoacids of nitrogen. Oxides and oxoacids of phosphorus, industrial production of phosphoric acid. Oxygen, oxides, water, hydrogen peroxide. Sulfur, Frasch process, sulfane, oxides, oxoacids, catenation of sulfur. Sulfuric acid production. 12. Halogens, hydrogen halides and halides, oxoacids of halogens. 13. General properties of d-block elements. Coordination compounds, ligands and their classification, coordination numbers, chelates, isomerism in coordination compounds. Importance of transition metals.

Literature

• VACÍK, Jiří. Obecná chemie. 1. vyd. Praha: Státní pedagogické nakladatelství, 1986, 303 s. info
• Atkins P.W., Beran J. A.: General Chemistry, Scientific American Books, New York 1992
• Růžička A., Toužín J.: Příklady a problémy z obecné chemie, Brno 2000
• Toužín J.: Stručný přehled chemie prvků, MU Brno 2001
• KLIKORKA, Jiří, Bohumil HÁJEK and Jiří VOTINSKÝ. Obecná a anorganická chemie. 2., nezměn. vyd. Praha: SNTL - Nakladatelství technické literatury, 1989, 592 s. info
• GREENWOOD, N. N. and A. EARNSHAW. Chemistry of the elements (Orig.) : Chemie prvků. Sv. 1 : Chemie prvků. Sv. 2. info

Teaching methods

Lectures.

Assessment methods

Final written exam covering the syllabus. A final score of 50 % or higher is required to pass the test successfully.

Language of instruction

Czech

Further Comments

The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C2021 Organic Chemistry I
  (C1020 || C1601) && !NOW(C2700)  
• C2700 Principles of Organic Chemistry
  (C1601||C1601bf||C1020) && !C2021 && !C3022 && !C3050 && !NOWANY(C2021,C3022,C3050)  
• C3181 Biochemistry I
  C1601 || C1020  
• C4221 Introductory Biochemistry Laboratory
  C7777 && C1601 && C4222  
• C5040 Nuclear Chemistry
  (C1020||C1601||C1601bf)  

• Enrolment Statistics (Autumn 2013, recent)
  
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