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Course syllabus N419A3_4B - Inorganic Chemistry I (FCFT - WS 2019/2020)

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University: Slovak University of Technology in Bratislava
Faculty: Faculty of Chemical and Food Technology
Course unit code: N419A3_4B
Course unit title: Inorganic Chemistry I
Mode of delivery, planned learning activities and teaching methods:
lecture3 hours weekly (on-site method)
seminar2 hours weekly (on-site method)

Credits allocated: 6
Recommended semester/trimester: Chemistry, Medical Chemistry and Chemical Materials - bachelor (compulsory), 1. semester
Chemistry, Medical Chemistry and Chemical Materials - bachelor (compulsory), 1. semester
Chemistry, Medical Chemistry and Chemical Materials (Remedial) - bachelor (compulsory), 3. semester
Level of study: 1.
Prerequisites for registration: none
Assesment methods:
Two knowledge tests - S1 (10 points) and S2 (30 points) during the semester. The student must obtain 56% of the points (22 points).
Written exam S3 (40 points). Oral examination (20 points). The student must obtain 56% of the points (22 and 12 points, respectively).

Learning outcomes of the course unit:
During the lectures, the seminar and tests the student will learn:

a)Students will be able determine the electron configuration and binding assumptions atoms of the elements in the periodic system. They can evaluate the binding of atoms in molecules and ions with respect to their shape and interactions between specific molecules or ions.

b) The student is able to identify trends in properties of elements in groups of elements in the periodic system.

c) The student is able to classify the types of compounds, their occurrence and representation in the groups of the periodic system.

d) The student is able to identify trends in acid-base and redox properties of compounds in groups of elements in the periodic system.

e) Student will manage the theory and concepts, types of compounds and substances that significantly advance and extend the boundaries of knowledge Inorganic Chemistry forward.

f) The student gains knowledge of the chemical processes in the atmosphere and hydrosphere.

Course contents:
1.Definition of basic terms. Chemicals and systems. Chemical reactions. Quantity of substances and composition of systems. Solutions. (allowance 3/2)
a.Mass particles, electron, proton, neutron, atomic nucleus, atom, ion, molecule, molecular ion, macromolecule, biomolecule.
b.Element, compound, pure substance. Homogeneous and heterogeneous system. Gas, liquid, solid. Molecular and ionic compounds.
c.The stoichiometric formula, the molecular formula, the functional formula, the structural formula, and the electron structural formula.
d.Classification of chemical reactions, determination of stoichiometric coefficients in chemical equation.
e.Quantity of chemical and composition of systems. Solutions: Substance, molar weight, weight fraction and substance concentration.

2.Electronic orbitals. Electron configuration of elements and ions. Periodic system of elements. (allowance 3/2)
a.Atomic orbitals. Quantum numbers and the relationships between them. The rules for the creation of electron configurations of atoms and ions.
b.Electron configuration of elements and ions - multiplicity and magnetic properties.
c.Periodic law and the periodic system of elements (PSE). Classification of elements according to electron configuration. PSE and electron configuration of elements of each group - possible oxidation numbers.
d.Effective nuclear charge, ionization energy, electron affinity, and electronegativity.

3.Covalent bond. MO theory. Electronegativity. (allowance 3/2)
a.Construction and classification of molecular orbitals. Electron configuration homonuclear binuclear particles. Bonding energy. Bonding order and length of a bond.
b.Electron configuration of hetero binuclear particles.
c.Electronegativity values. Dipole moment of polar binulear molecules.

4.Electron structural formulas. (allowance 3/2)
a.Octet rule.
b.Rules for writing of electron structural formulas.
c.Formal charge. Donor-acceptor (coordination) covalent bond.
d.Resonance structures, partial bonding order.

5.Shape of molecules and their names. Valence bond theory. Ionic bond. Ionic crystal structures. Intermolecular interactions. (allowance 3/2)
a.Shape of particles and their names (VSEPR). Valence bond theory: Hybridization of atomic orbitals. Dipole moment and molecular structure. Intermolecular interactions: Hydrogen bonding and intermolecular interactions.
b.Ionic bond: ion pattern and ion size - ionic radius trends and melting temperature trends. Polarizability and covalence - Fayans rules. Bonding triangular diagram of elements and compounds. The covalent character of the ionic bond.
c.Ionic crystal structures.

6.Formation of inorganic compounds. The spontaneity of chemical process. Energy balance. Chemical equilibrium. Activation energy of inorganic reactions. (allowance 3/2)
a.Formation of inorganic compounds, the spontaneity of reactions - extent of reaction, reaction Gibbs energy. Standard enthalpy, grid energy. Thermochemistry laws.
b.Energy balance - dissolution, solvation quantities (enthalpy, entropy), solubility.
c.Chemical equilibrium - equilibrium constant (Kc, Ka, Kp). The influence of temperature and pressure on chemical balance. Van't Hoff's relationship. Direction of the chemical reaction (reaction quotient).
d.Activation energy of inorganic reactions - kinetics, catalysed and non-catalyzed reaction. Activating energy, Arrhenius' relationship.

7.Acid-base reactions. Brønsted and Lewis theory of acids and bases. Protolytic reactions. Complex-forming reactions. Pearson's theory of soft and hard acids and bases. Precipitation reactions. (allowance 3/2)
a.Solvents. Definitions of acids and bases. Amphiprotic and amphoteric substances. Protolytic reactions (autoprotolysis, neutralization, pH, ionization of acids and bases, hydrolysis). pH of solutions of strong acids, bases and hydrolysable salts.
b.Lewis theory of acids and bases. Complexing equilibria.
c.Pearson's theory of soft and hard acids and bases (HSAB).
d.Precitipation reactions. Balance of weakly soluble electrolytes - Solubility Products. Impact of a common ion on solubility, the effect of hydrolytic and complexing reactions on solubility.

8.Oxidation and reduction. Standard electrode potentials. Potential diagrams. Electrolysis. (allowance 3/2)
a.Redox reactions. Reactions of metals with water, in solutions of oxidizing and non-oxidizing acids and hydroxides. Recording of the redox reaction by means of half-reactions.
b.Standard electrode potentials E° and relationships between E°, G° and K. Nernst-Peters equation.
c.Latimer and Frost diagrams.
d.Faraday's laws and electrolysis.

9.Periodic trends in the properties of elements and compounds. (allowance 3/2)
a.Physical and chemical properties of main group elements and their compounds - trends in groups and periods.
b.Trends in the acid-base properties of oxides of the 2nd and 3rd periods (with the maximum number of oxygen atoms), the oxides of the 15th group (with the maximum number of oxygen atoms), the molecular hydrides of the 2nd and 3rd period.
c.Differences in properties of elements of the 2nd period compared to elements of other periods.
d.Current Topic: Chemistry as the Science of the 21st Century?

10.Noble gases. Hydrogen. (allowance 3/2)
a.Noble gases - the properties of the noble gases. Noble gases as simple substances. The unique properties of helium. Occurrence, production and use of noble gases. Compounds of noble gases - fluorides and oxides of xenon.
b.Hydrogen: The location of hydrogen in a periodic table, the way of bonding, the occurrence of hydrogen. Isotopes of hydrogen. Properties and laboratory preparation of hydrogen. Production and use of hydrogen.
c.Hydrids - molecular (covalent) hydrides, ionic hydrides and metal hydrides. Water and hydrogen bonding. Hydrates (clatrates) of noble gases, methane and carbon dioxide. Biological aspects of hydrogen bonding.
d.Current topic: Energy sources of the future based on hydrogen ("hydrogen economy").

11.Halogens. (allowance 3/2)
a.Halogens: Properties of halogen atoms. Trends in the group. Properties of halogens as simple substances, occurrence, production and use of halogens. Reactions of halogens.
b.Halides. Classification of halides. The stability of halides depending on the oxidation state of the less electronegative element. Preparation of halides. Cyanide anion as a pseudohalogenide anion.
c.Intermolecular compounds of halogens. Hydrogen halides and their acids. Preparation and properties of hydrogen halides. Hydrofluoric acid. Hydrochloric acid. Oxyacids of halogens. Oxyacids and oxaniones of chlorine.
d.Current topics: Fluoridation of water. Ammonium chlorate as rocket fuel.

12.Oxygen and sulfur. Selenium, tellurium and polonium. (allowance 3/2)
a.Trends in the group. Opposities in oxygen and sulfur chemistry. Oxygen. Bonds in covalent oxygen compounds. Trends in Oxidation properties. Ternar metal oxides. Water. Hydrogen peroxide. Hydroxides. Hydroxyl radical.
b.Introduction to sulfur chemistry. Sulfur. Hydrogen sulfide. Sulphides. Sulfur oxides. Sulphites. Sulfuric acid. Sulphates and hydrogens. Other sulfur oxanones. Sulfur halides. Sulfur and nitrogen containing compounds. Bonding or oligomerization of inorganic molecules. Biological aspects.
c.Selenium, tellurium and polonium. Biological aspects.
d.Current topics: Atmospheric chemistry, ozone layer protection, acid rain. Disinfection of water using oxidants (chlorine and its compounds, hydrogen peroxide, ozone).

13.Consultation. (allowance 3/2)
a.Organization of the exam period.

Recommended or required reading:
Anorganická chémia. Bratislava : Alfa, 1993. 598 p. ISBN 80-05-01142-3.
ŠIMA, J. -- SEGĽA, P. -- KOMAN, M. Anorganická chémia. Bratislva: STU, 2009. 480 p. ISBN 978-80-227-3087-7.
SIROTA, A. -- ADAMKOVIČ, E. Názvoslovie anorganických látok. Bratislava : Metodické centrum, 2002. 107 p. ISBN 80-8052-152-2.
KOHOUT, J. -- MELNÍK, M. Anorganická chémia 1: Základy anorganickej chémie. Bratislava : STU v Bratislave, 1997. 365 p. ISBN 80-227-0972-7.
OVERTON, T. -- RAYNER-CANHAM, G. Descriptive Inorganic Chemistry. New York: Clancy Marshall, 2010. 651 p. ISBN 978-1-4292-2434-5.

Language of instruction: slovak or english
Courses evaluation:
Assessed students in total: 886

7,9 %12,9 %22,5 %26,3 %23,7 %6,7 %
Name of lecturer(s): doc. Ing. Vladimír Jorík, CSc. (examiner, instructor, lecturer) - slovak
Ing. Ján Pavlik, PhD. (examiner, instructor, lecturer)
prof. Ing. Peter Segľa, DrSc. (examiner, instructor, lecturer, person responsible for course) - slovak, english
Ing. Jozef Švorec, PhD. (examiner, instructor, lecturer)
Ing. Miroslav Tatarko, PhD. (examiner, instructor, lecturer) - slovak
Last modification: 29. 1. 2019
Supervisor: prof. Ing. Peter Segľa, DrSc. and programme supervisor

Last modification made by Ing. Tomáš Molnár on 01/29/2019.

Type of output: