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Faculty of Science Handbook, Session 2017/2018

Balance, Capillary Electrophoresis (CE), Ion
Chromatography, X-ray Fluorescence Spectrometer References:
(XRF), Electroanalytical System and Gel Imager. TOC 1. J. E. Brady, F. A. Senese and N. D. Jespersen,
th
analyser, densitometer, colour spectrometer, light Chemistry, 5 ed., John Wiley & Sons, 2009.
scattering GPC, thermoconductivity meter, particle size 2. T. L. Brown, H. E. LeMay, B. E. Bursten, C. J. Murphy
analyser+ FESEM. and P. Woodward, Chemistry: The Central Science,
th
12 ed., Pearson Education, Prentice Hall, 2011.
JOB OPPORTUNITIES 3. M. S. Silberberg, Chemistry: The Molecular Nature of
Matter and Change, .6 ed., McGraw-Hill, 2011.
th
Courses offered by the Department meet the current 4. L. Pauling, General Chemistry, 3 rd ed., Dover
requirements to accommodate job and career Publications, 1988.
advancement. Chemistry is recognised as a professional 5. P. W. Atkins and J. de Paula, Physical Chemistry, 9 th
field by Malaysian Institute of Chemistry and to date, our ed., Oxford University Press, 2010.
chemistry graduates have filled the job market in both 6. P. Atkins, T. Overton, J. Rourke, M. Weller and F.
public and private sectors. Job opportunities are available Armstrong, Shriver & Atkins' Inorganic Chemistry, 5 th
in basic research and development areas in research ed., Oxford University Press, 2010.
institutions such as FRIM, SIRIM, MARDI, Petronas,
MPOB and IMR. In addition, graduates are employed in
the teaching profession in schools, colleges and SIC1002 INORGANIC CHEMISTRY I
universities. Career opportunities are also available in the
chemical and manufacturing industries, oil and gas Chemical Bonding: Ionic, covalent and metallic bonding,
industries, petrochemicals, energy and fuel industries, bond polarity and electronegativity
polymer and materials, electronics, sales and marketing, Intermolecular forces: Metallic bonding, the hydrogen
and new growth areas of green and sustainable bonds and dipole-dipole forces.
technologies.
Lewis structures and geometry, hybridization, VSEPR and
COURSE SYNOPSIS resonance
Molecular orbital theory, valence bond theory
Note: All level 1 students are required to attend a
practical safety class before commencing their practical Types of solids: Closest packing, different types of crystal
class. Time of class will be announced on the first week of structures (molecular, ionic, covalent and metallic);
the teaching session. relationship between structure and properties, packing
efficiency, density calculation for metallic structures, radius
ratio for ionic solids.
SIC1001 PRINCIPLES OF CHEMISTRY
Chemistry of s and p-block elements: Occurrence and
Stoichiometry abundance, extraction, physical properties and chemical
The mole concept, chemical formulas (empirical and properties.
molecular), balanced chemical equations (molecular and Arrhenius and Ostwald Theory, Bronsted acidity, Bronsted
redox), percentage yield, chemical reactions in aqueous equilibrium, , periodic trend in Bronsted acidity, Lux
solution, molarity, and analytical chemistry (gravimetric concept oxoacids, polyoxoacids, Pauling’s rule, Lewis
and volumetric). acids and bases, relative strength of Lewis acids and
bases, Hard-soft theory for acids and bases,
Atomic structure Thermodynamic parameter for acids and bases, Drago-
Models of atomic structure (Dalton, Bohr, Quantum Wayland equation.
Theory)
Wavefunction (quantisation, atomic orbitals) Oxidation and reduction reactions; definition and types of
Many-electron atoms (Heisenberg uncertainty principle, redox reactions; oxidizing and reducing agents, oxidation
Pauli exclusion principle, Hund’s rule, Aufbau principle, number (O.N.) and its importance, procedure for
electronic configuration) calculating O.N., elements with more than one O.N. Half
redox reactions and balancing of redox reaction equations,
Periodic Table Standard electrode potential and electrochemical series,
Trends in physical and chemical properties of elements in Frost diagrams, Pourbaix Diagram and its interpretation,
relation to electronic configuration (atomic size, ionic Ellingham diagram.
radius, ionization energy, electron affinity, electronegativity
and metallic properties, acid-base and redox). Assessment Methods:
Practical: 25%
Introduction to chemical bonding Continuous assessment: 15%
Ionic versus covalent bonding, nature of the covalent Final examination: 60%
bond, valence bond theory (hybridization), molecular
orbital theory. Medium of instruction:
English
Gas
The kinetic theory of gas and equation of state for ideal Soft skills:
and real gases. CT1-3
Assessment Methods: References:
Continuous assessment: 30% 1.J. Mcmurray and R.C. Fay, Chemistry, 5 ed., Prentice
th
Final examination: 70% Hall International, 2008.
2.J. E. Brady, F.A. Senese and N.D. Jesperson,
th
Medium of instruction: Chemistry, 5 ed., John Wiley, 2009.
English 3.D. F. Shriver and P. W. Atkins, Inorganic Chemistry, 5 th
ed., Oxford University Press, 2010.
Soft skills: 4.Catherine E. Housecroft and Alan G. Sharpe, Inorganic
CT1-3 Chemistry, 4th ed., Pearson Prentice Hall, 2012.

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