PřF:C1601 General and Inorg. Chemistry - Course Information

C1601 General and Inorganic Chemistry

Extent and Intensity

3/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

doc. RNDr. Josef Novosad, CSc. (lecturer)

Guaranteed by

doc. RNDr. Josef Novosad, CSc.
Chemistry Section – Faculty of Science

Prerequisites

NOW( C1620 General and Inorg.Chem.-lab. )
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 20 fields of study the course is directly associated with, display

Course objectives

The course on General and Inorganic Chemistry is targeted to students of biological sciences, and does consist of two major parts. The part on general chemistry examines basic principles underlying chemistry. Topics include electronic structure of atoms, chemical bonding theories, chemical reactions along with the energy changes, and the states of matter, i.e., gases, liquids and solids. The second part (Inorganic Chemistry) provides an introduction into systematic chemistry of elements including their origin, periodicity of their properties, and general features of metals and non-metals. The main block elements are thoroughly examined while transition elements are referred briefly. Important role of selected metals in living systems is emphasized.

Syllabus

• 1. Chemistry and its relation to other disciplines. Matter, its physical and chemical properties, pure substance, chemical purity grades. The common types of compounds. Homogenous and heterogenous mixtures. Basic chemistry concepts. Atomic mass unit, atomic and molecular weights. Avogadro's constant. Relative atomic and molecular masses. Mole, molar mass. 2. 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. 3. 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. 4. Molecular structure. Chemical bonding and its parameters, weak bonding interactions (van der Waals forces, hydrogen bond). Metallic bond. 5. Gas properties, ideal vs. real gas, gas mixtures. Ideal gas equation of state and the other ideal gas laws. 6. General properties of liquids, vapor pressure, boiling point. The phase diagram for water. Polar and non-polar solvents. Solutions, solubility, expressing concentration of solutions, calculation of concentrations. Acids and bases. Water and its dissociation. Acidity and basicity of water solutions. The strength of acids and bases. pH calculations, salt hydrolysis, buffers. 7. Structure and properties of solids, crystal lattice, crystal lattice structures, fundamentals of crystallography, X-Ray diffraction. 8. Chemical reactions, selected examples. Catalysts and their impact on reaction progress. Chemical equations, stoichiometry. 9. Electrochemistry, electrode potential, electrolysis, material corrosion. 10. 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. 11. Carbon and its allotropes, carbides, oxides, carbon acids salts and derivatives. Nitrogen, ammonia, and ammonium salts, azides, oxides, oxoacids and their salts. Phosphorus, phosphines, phosphides, oxides, sulfides, halides, oxoacids and their salts. 12. Oxygen, oxides, water, hydrogen peroxide. Sulfur, sulfane, sulfides and polysulfides, oxides, oxoacids. Selenium and its oxo-compounds. Halogens, hydrogen halides and halides, oxoacids and their salts. 13. Properties of d- and f- block elements, examples of their compounds. 14. Coordination compounds, ligands and their classification, coordination numbers, chelates, isomerism in coordination compounds. Iron, cobalt, chromium, molybdenum, copper, zinc, lithium, sodium, potassium, magnesium and calcium in biological systems.

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
• Hála J.: Pomůcka ke studiu obecné chemie, MU Brno 2000
• 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

Assessment methods (in Czech)

Výuka formou přednášky, ústní zkouška.

Language of instruction

Czech

Further Comments

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

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 2002, recent)
  
• Permalink: https://is.muni.cz/course/sci/autumn2002/C1601