Chemistry syllabus UiTM

1. Faculty of Applied Science
Universiti Teknologi MARA Perlis
July – November 2009 Semester
Course Information
Course Name : Chemistry
Course Code : CHM 105
Programme : Diploma in Planting Industrial Management (AS 110)
Credit Hours :3
Contact Hours :3
Course Outline
1.0 Atom and Molecule
1.1 Definition of atom, ion, molecule, element and compound. Basic structure
of an atom.
1.2 Definition of proton number, nucleon number and isotopes. Calculations
on proton and nucleon numbers and the number of electrons in an atom.
1.3 Definition of atomic mass and relative molecular mass, mole concept and
Avogadro’s number (NA).
1.4 Molar mass, molar volume of gas and ideal gas equation.
1.5 Concentration and molarity of solution.
1.6 Empirical formula and molecular formula.
1.7 Writing and balancing chemical equations. Calculations on mole, mass,
molarity, concentration and volume of gas based on balanced equation.

2. 2.0 Electronic structure of an atom
2.1 Energy levels concept. Calculations on the number of maximum electrons
using the 2n2 formula.
2.2 Relative energy for K, L, M and N levels and for s, p, d and f orbital.
2.3 Electrons configurations based on levels and sublevels.
3.0 Periodic Table
3.1 Properties of modern periodic table: group, periods, valence electrons.
Classification into s, p, d and f blocks and also into metals, non-metals and
metalloids. Special names for Group 1 to 18.
3.2 Changes in physical properties of elements moving down the groups and
across the periods.
3.3 Changes in acidity of oxides across the period 3.
4.0 Chemical Bonding
4.1 Concept on ionic/ electrovalent bonding and covalent bonding. Using
Lewis structure to show the sharing and transferring of electrons in the
following examples: NaCl, MgO, CCl4, O2, N2, CO2 and etc.
4.2 General properties of ionic and covalent bonding.
4.3 Covalent dative bonding, metal bonding, hydrogen bonding and Van der
Waals forces.
5.0 Inorganic Chemistry
5.1 Group 1 (focus more on Na, K and H); physical and chemical properties
including their compounds – nitrates, carbonates, sulphates, chlorides and
oxides.
5.2 Group 2 (focus more on Ca and Mg); physical and chemical properties
including their compounds – nitrates, carbonates, sulphates, chlorides and
oxides.

3. 5.3 Group 15 (focus more on N and P); physical and chemical properties
including their compounds (especially fertilizer) – ammonium sulphate,
ammonium nitrate, urea and phosphoric acid.
5.4 Group 16 (concentrate more on O and S); physical and chemical
properties including their compounds – SO2, SO3, H2SO4 and H2O2.
6.0 Oxidation and Reduction
6.1 Definition of oxidation, reduction, oxidizing agent and reducing agent in
terms of hydrogen, oxygen, electron transfer and oxidation number.
6.2 Determination of oxidation number.
6.3 Balancing redox equation using ion-electron method.
6.4 Balancing redox equation using oxidation number method.
7.0 Acids and Bases
7.1 Definition based on Arrhenius, Brønsted-Lowry and Lewis with simple
examples. General properties of acid and base. Definitions and examples
of strong acid, strong base, weak acid and weak base.
7.2 pH scale: definition and examples on calculation of pH for strong base and
strong acid only (using the pH = - log [H+] and [H+][OH-] = 1.0 X 10-14
formula).
7.3 Calculations on volumetric analysis, neutralization and titration involving
acid and base; oxidizing and reducing agents.
8.0 Organic Chemistry
8.1 Tetravalence organic compound structure for carbon (3 dimensional
structural formula using ball and stick model).
8.2 Classification of organic compound, homologous series and functional
groups for alkanes, alkenes, alcohols, aldehydes and ketones. Molecular
and structural formulas. Examples of each homologous series.
8.3 IUPAC nomenclature for alkanes, alkenes, alcohols, aldehydes and
ketones with examples.

4. Assessment
Tests : 30%
Laboratory work : 10%
Final Examination : 60%
Final Examination Format
Comprising two parts;
Part A (40 marks) : 20 objective questions
Part B (60 marks) : 4 subjective questions (Answer ALL of the questions)
Recommended Textbook
Chang, Raymond. Essential Chemistry. Mc-Graw Hill.
Other Suggested References
1. Fullick, Ann & Patrick. Chemistry. Heinemann.
2. Cherim, S. M. & L. E. Kallan. Chemistry: An Introduction. Saunders Golden
Sunburst Series, Philadelphia.
3. Dickson, T. R. Introduction to Chemistry. John Wiley & Sons, New York.
4. Tan Yin Toon. Kimia Lengkap STPM. Fajar Bakti, Petaling Jaya.
5. Underwood, D. N. & W. E. Webster. Kimia (Edisi Malaysia). Federal
Publications, Kuala Lumpur.
6. Whitten, K. E., K.D. Gailey & R. E. Davis. General Chemistry with Qualitative
Analysis. Saunders Golden Sunburst Series, Philadelphia.