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COURSE SYNOPSIS

SIC1006 Computer Programming for the Sciences

SIC1001 PRINCIPLES OF CHEMISTRY This course aims to arm science students with the basics of
programming computers using Python. This course covers the
Part A: basics of how one constructs a program from a series of simple
Atoms, Molecules, Ions and Mass Relationship in Chemical instructions in Python. This course has no pre- requisites and avoids
Reaction all but the simplest mathematics. Anyone with some computer
The atomic theory, the structure of the atom, atomic number, experience should be able to master the materials in this course. At
mass number and isotopes, molecules and ions, chemical the end of this course students should be able to:
formulas, naming compounds, Avogadro’s number and the molar
mass of an element, percent composition of compounds, Map scientific problems into computational frameworks. Read, write
empirical formulas, chemical reactions and chemical equations, and debug Python codes for these scientific problems.
stoichiometry calculations, amounts of reactants and products, Describe the advantages and limitations of a computer language in
limiting reagents, percentage of yield. solving these problems.
Students who successfully completed this course will be prepared
Reactions in Aqueous Solution for more advanced concepts of programming and effectively use
General properties of aqueous solutions, precipitation reactions, external modules related to the various fields of science in solving
acid-base reactions, oxidation-reduction reactions, concentration more sophisticated problems.
of solutions.
Assessment Weightage:
Periodic Relationships Among the Elements Continuous assessment: 40%
History of the periodic table, classification of the elements, trends Final examination: 60%
in periodic table (atomic radius, ionization energy,
electronegativity, electron affinity, bond energy, lattice energy).
SIC1007 INORGANIC CHEMISTRY I
Chemical Bonding
Ionic bond, covalent bond, dative/coordinate bond, metallic bond, Non-aqueous media:
hydrogen bond, Van der Waals interaction, dipole moment, Lewis Introduction to non-aqueous media
structure (formal charge and resonance), exceptions to the octet Acid–base behaviour in non-aqueous solvent, self-ionizing and
rule, molecular geometry, valence bond theory, hybridization of non-ionizing non-aqueous solvent, liquid: ammonia, hydrogen
atomic orbitals, hybridization in molecules containing double and fluoride, sulfuric, fluorosulfonic acid, supercritical fluid, ionic liquid.
triple bonds, molecular orbital theory, molecular orbital Types of solids: Description of the structures of solid, Structure of
configurations, delocalized molecular orbitals. metals and alloys, Ionic solids.

Chemical Equilibrium Chemistry of s and p-block elements: Occurrence and
The Equilibrium Law of reactions, relationship between Kp and abundance, extraction, physical properties and chemical properties.
Kc, Le Chatelier’s Principle, equilibrium calculations.
Acid and base: Arrhenius and Ostwald Theory, Bronsted acidity,
Part B: Bronsted equilibrium, periodic trend in Bronsted acidity, Lux
Atomic Structure concept oxoacids, polyoxoacids, Pauling’s rule, Lewis acids and
Models of atomic structure (Dalton, Rutherford, Bohr, quantum bases, relative strength of Lewis acids and bases, Hard-soft theory
theory), wavefunction (quantization, atomic orbitals), particle- for acids and bases, thermodynamic parameter for acids and bases,
wave duality, many-electron atoms (Heisenberg uncertainty Drago- Wayland equation.
principle, Pauli exclusion principle, Hund’s rule, Aufbau principle,
electronic configuration). Oxidation and reduction reactions: definition and types of redox
reactions; oxidizing and reducing agents, oxidation number (O.N.)
Gas and its importance, procedure for calculating O.N., elements with
Ideal gases (states of gases, gas laws, ideal gas law, gas more than one O.N. Half redox reactions and balancing of redox
stoichiometry, Dalton’s law of partial pressures, kinetic molecular reaction equations, standard electrode potential and
theory of gases, mean free path and collision diameter), electrochemical series, Frost diagrams, Pourbaix Diagram and its
molecular speed distribution, Boltzmann distribution law, effusion, interpretation, Ellingham diagram.
diffusion and viscosity, real gases (molecular interactions, Van
der Waals equation, behaviour of real gases, the critical state, the Assessment Weightage:
law of corresponding states). Continuous assessment: 40%
Final examination: 60%
Electrolyte
Properties of electrolyte solutions (Kohlrausch's Law, ionic
conductivity). SIC1008 ORGANIC CHEMISTRY I

Assessment Weightage: Free radical substitution, electrophilic addition, electrophilic
Continuous assessment: 40% aromatic substitution and elimination.
Final examination: 60%
Conformational analysis of acyclic and cyclic hydrocarbons.