C1601 General and Inorganic Chemistry

Faculty of Science
Autumn 2009
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)
RNDr. Valerie Richterová, Ph.D. (assistant)
Guaranteed by
doc. Mgr. Marek Nečas, Ph.D.
Department of Chemistry – Chemistry Section – Faculty of Science
Timetable
Wed 15:00–16:50 A,01026
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
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.
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
The course is also listed under the following terms Autumn 2007 - for the purpose of the accreditation, Autumn 2010 - only for the accreditation, Autumn 2000, Autumn 2001, Autumn 2002, Autumn 2003, Autumn 2004, Autumn 2005, Autumn 2006, Autumn 2007, Autumn 2008, Autumn 2010, Autumn 2011, Autumn 2011 - acreditation, Autumn 2012, Autumn 2013, Autumn 2014, Autumn 2015, Autumn 2016, autumn 2017, Autumn 2018, Autumn 2019, Autumn 2020, autumn 2021, Autumn 2022, Autumn 2023, Autumn 2024.
  • Enrolment Statistics (Autumn 2009, recent)
  • Permalink: https://is.muni.cz/course/sci/autumn2009/C1601