Page 172 - FULL FINAL HANDBOOK 20232024

Faculty of Science Handbook, Academic Session 2023/2024

COURSE SYNOPSIS

SIC1006 Computer Programming for the Sciences
SIC1001 PRINCIPLES OF CHEMISTRY
This course aims to arm science students with the basics of programming
Part A: computers using Python. This course covers the basics of how one constructs a
Atoms, Molecules, Ions and Mass Relationship in Chemical program from a series of simple instructions in Python. This course has no pre-
Reaction requisites and avoids all but the simplest mathematics. Anyone with some
The atomic theory, the structure of the atom, atomic number, mass computer experience should be able to master the materials in this course. At the
number and isotopes, molecules and ions, chemical formulas, naming end of this course students should be able to:
compounds, Avogadro’s number and the molar mass of an element,
percent composition of compounds, empirical formulas, chemical Map scientific problems into computational frameworks. Read, write and debug
reactions and chemical equations, stoichiometry calculations, Python codes for these scientific problems.
amounts of reactants and products, limiting reagents, percentage of Describe the advantages and limitations of a computer language in solving these
yield. problems.
Students who successfully completed this course will be prepared for more
Reactions in Aqueous Solution advanced concepts of programming and effectively use external modules related
General properties of aqueous solutions, precipitation reactions, acid- to the various fields of science in solving more sophisticated problems.
base reactions, oxidation-reduction reactions, concentration of
solutions. Assessment Weightage:
Continuous assessment: 40%
Periodic Relationships Among the Elements Final examination: 60%
History of the periodic table, classification of the elements, trends in
periodic table (atomic radius, ionization energy, electronegativity, SIC1007 INORGANIC CHEMISTRY I
electron affinity, bond energy, lattice energy).
Non-aqueous media:
Chemical Bonding Introduction to non-aqueous media
Ionic bond, covalent bond, dative/coordinate bond, metallic bond, Acid–base behaviour in non-aqueous solvent, self-ionizing and non-ionizing non-
hydrogen bond, Van der Waals interaction, dipole moment, Lewis aqueous solvent, liquid: ammonia, hydrogen fluoride, sulfuric, fluorosulfonic acid,
structure (formal charge and resonance), exceptions to the octet rule, supercritical fluid, ionic liquid.
molecular geometry, valence bond theory, hybridization of atomic Types of solids: Description of the structures of solid, Structure of metals and
orbitals, hybridization in molecules containing double and riple bonds, alloys, Ionic solids.
t
molecular orbital theory, molecular orbital configurations, delocalized
molecular orbitals. Chemistry of s and p-block elements: Occurrence and abundance, extraction,
physical properties and chemical properties.
Chemical Equilibrium
The Equilibrium Law of reactions, relationship between Kp and Kc, Le Acid and base: Arrhenius and Ostwald Theory, Bronsted acidity, Bronsted
Chatelier’s Principle, equilibrium calculations. equilibrium, periodic trend in Bronsted acidity, Lux concept oxoacids,
polyoxoacids, Pauling’s rule, Lewis acids and bases, relative strength of Lewis
Part B: acids and bases, Hard-soft theory for acids and bases, thermodynamic parameter
Atomic Structure for acids and bases, Drago- Wayland equation.
Models of atomic structure (Dalton, Rutherford, Bohr, quantum
theory), wavefunction (quantization, atomic orbitals), particle-wave Oxidation and reduction reactions: definition and types of redox reactions;
duality, many-electron atoms (Heisenberg uncertainty principle, Pauli oxidizing and reducing agents, oxidation number (O.N.) and its importance,
exclusion principle, Hund’s rule, Aufbau principle, electronic procedure for calculating O.N., elements with more than one O.N. Half redox
configuration). reactions and balancing of redox reaction equations, standard electrode potential
and electrochemical series, Frost diagrams, Pourbaix Diagram and its
Gas interpretation, Ellingham diagram.
Ideal gases (states of gases, gas laws, ideal gas law, gas
stoichiometry, Dalton’s law of partial pressures, kinetic molecular Assessment Weightage:
theory of gases, mean free path and collision diameter), molecular Continuous assessment: 40%
speed distribution, Boltzmann distribution law, effusion, diffusion and Final examination: 60%
viscosity, real gases (molecular interactions, Van der Waals equation,
behaviour of real gases, the critical state, the law of corresponding SIC1008 ORGANIC CHEMISTRY I
states).
Free radical substitution, electrophilic addition, electrophilic aromatic substitution
Electrolyte and elimination. Conformational analysis of acyclic and cyclic hydrocarbons.
Properties of electrolyte solutions (Kohlrausch's Law, ionic Stereochemistry: Isomerism in organic compounds: constitutional and
conductivity). stereoisomers; chirality and optical activity; enantiomers, diastereomers,
racemates and resolution; molecules with two (or more) chiral centres, meso-
Assessment Weightage: compounds; configuration and labelling of chiral centres: Cahn–Ingold–Prelog
Continuous assessment: 40% priority rules.
Final examination: 60%

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