Course code:
1102A		 Course name:
Inorganic Chemistry

Academic year:

2012/2013.

Attendance requirements:

There are no requirements.

ECTS:

10

Study level:

basic academic studies

Study programs:

Chemistry: 1. year, summer semester, compulsory course

Chemistry Teacher: 1. year, summer semester, compulsory course

Teachers:

Sofija P. Sovilj, Ph.D.

Tamara R. Todoroviц, Ph.D.
full professor, Faculty of Chemistry, Studentski trg 12-16, Beograd

Assistants:

Jelena M. Poljareviц, Ph.D.
assistant professor, Faculty of Chemistry, Studentski trg 12-16, Beograd

Aleksandar R. Saviц, Ph.D.
assistant professor, Faculty of Chemistry, Studentski trg 12-16, Beograd

Milica R. Milenkoviц, Ph.D.
associate professor, Faculty of Chemistry, Studentski trg 12-16, Beograd

Hours of instruction:

Weekly: four hours of lectures + two hours of exercises + four hours of labwork (4+2+4)

Goals:
  • The concept of Inorganic chemistry 1 systematically offers an elementary knowledge in the field of elements as well as their compounds.
  • There are included a plenty of problems that will challenge the student, including problems applying chemistry to a wide variety of other fields.
  • The number of facts and details presented does not exceed the possibilities of a student on the first class studying.

Outcome:
  • Researching common properties of the elements and their compounds according to the groups and periods of Periodic Table helps student to get an increasing awareness of the importance of descriptive inorganic chemistry in the general chemistry curriculum.
  • Application of general chemistry principles helps student as much as possible to recognize how the pieces can fit together and study inorganic chemistry on a higher level in further years.

Teaching methods:

Lectures, demonstration experiments ex cathedra, experimental and theoretical exercises.

Extracurricular activities:

—

Coursebooks:

Main coursebooks:

  • Дејан Полети: Општа хемија, II део, Хемија елемената, ТМФ, Београд, 2000.
  • Иван Филиповић и Стјепан Липановић: Опћа и анорганска кемија, II део, Кемија елемената, Школска књига, Загреб, 1996.
  • Љ. Богуновић, Д. Васовић, Д. Полети, М. Поповић, С. Стевић: Практикум опште хемије, II део, ТМФ, Београд, 2004.
  • Ненад Јуранић: Збирка задатака из опште хемије, Студентски трг, Београд, 2004.
  • М. Поповић, Д. Васовић, Љ. Богуновић, Д. Полети, О. Ћуковић: Збирка задатака из опште хемије, ТМФ, Београд, 1996.
  • С. Нешић и Ј. Вучетић: Неорганска препаративна хемија, Грађевинска књига, Београд, 1969.

Supplementary coursebooks:

  • Alan G. Sharpe: Inorganic Chemistry, Longman, London and New York, 1981.

Additional material:

—

  Course activities and grading method

Lectures:

0 points (4 hours a week)

Syllabus:

Introduction:

  • Periodic Table of Elements. Nomenclature of inorganic compounds. Chemistry of the Elements. Introduction to the chemistry of the s- and p-elements. Hydrogen.

The Halogens:

  • Overview of the elements and their compounds.
  • Fluorine, chlorine, bromine and iodine.

The Elements of Oxygen:

  • Overview of the elements and their compounds. Oxygen.
  • Sulphur, selenium, tellurium and polonium.

The Elements of Nitrogen:

  • Overview of the elements and their compounds.
  • Nitrogen, phosphorus, arsenic, antimony and bismuth.

The Elements of Carbon:

  • Overview of the elements and their compounds. Carbon.
  • Silicon. Germanium, tin and lead.

The Elements of Boron:

  • Overview of the elements and their compounds. Boron, aluminium, gallium, indium and thallium.

The Alkaline Earth and Alkali Metals:

  • Overview of the elements and their compounds. Beryllium, magnesium, calcium, strontium and barium. Lithium, sodium, potassium, rubidium and cesium. The Noble Gases.

Overview of d- and f-elements:

  • The Transition Elements. Electronic configurations and chemical properties. Coordination compounds.
  • Scandium, yttrium, lanthanum and actinium. Lanthanides and actinides. Titanium, zirconium and hafnium. Vanadium, niobium and tantalum. Chromium, molybdenum and tungsten.
  • Manganese, technetium and rhenium. Iron, cobalt and nickel. Ruthenium, rhodium, palladium, osmium, iridium and platinum.
  • Copper, silver and gold. Zinc, cadmium and mercury.

Occurrences, preparation, properties and uses are points out for all the elements and their compounds. The basic chemical parameters, like as ionization energy, electron affinities, ionic bonding, geometries, hybridization and VSEPR model, sizes of atoms and ions as well as bond energy are interspersed throughout the course. All reactions are explained in terms of thermodynamic state functions, especially the Gibbs free energy that combines enthalpy and entropy. Standard electrode potentials are used to determine whether certain reactions are possible.

Exercises:

0 points (2 hours a week)

Labwork:

10 points (4 hours a week)

Colloquia:

30 points

Written exam:

60 points