Page 179 - handbook 20162017

Faculty of Science Handbook, Session 2016/2017

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

173