General and Physical Chemistry (I)

Unit 1: Language of Chemistry (Review Lecturers) - 3 teaching hours

1 Chemical equations, their significances and limitations

2 Balancing chemical equations by :

i. hit and trail method ii. Partial equation method

3 Types of chemical reaction

Unit 2: Chemical Arithmetic - 17 teaching hours

2.1 Dalton's atomic theory and Laws of Stoichiometry:

1 Postulates of Dalton's atomic theory

2 Law of conservation of mass

3 Law of constant proportions

4 Law of multiple proportions

5 Law of reciprocal proportions

6 Law of gaseous volumes

7 Chemical calculations based on stoichiometry

2.2. Atomic Mass and Molecular Mass:

Definition of atomic mass and molecular mass

1 Mole concept

2 Mole in term of mass, volume number and ions

3 Calculation based on mole concept

2.3. Empirical, Molecular Formula and Limiting Reactants:

1 Percentage compositions

2 Derivation of empirical and molecular formula from percentage composition

3 Chemical calculation based on following chemical equation

- Limiting reactants

- Mass-mass relationship

- Volume – volume relationship

- Mass volume relationship

(Solving reacted numerical problems)

2.4. Avogadro's Hypothesis and Its Applications:

1 Development of Avogardro's hypothesis

2 Definition of Avogadro's hypothesis

3 Application of Avogadro's hypothesis

i. Deduction of atomicity of elementary gas

ii. Deduction of relationship between molecular mass and vapour density

iii. Deduction of molar volume of gases

iv. Deduction of molecular formula from its volumetric composition

(Solving related numerical problems)

2.5. Equivalent Mass:

1 Concept of equivalent mass

2 Equivalent weight of elements, and compounds (Salt, acid , base, oxidising agents,

reducing agents)

3 Gram equivalent weight (GEW)

4 Relation between equivalent weight, valency and atomic weight

5 Determination of equivalent weight of metal by

i. Hydrogen displacement method ii. Oxide formation method

(Solving related numerical problems)

Unit 3: State of Matter - 14 teaching hours

3.1. Gaseous State:

1 Boyle's law

2 Charle's law and Kelvin scale of temperature

3 Application of Charle's law and Boyle's law

4 Combined gas law, ideal gas equation and universal gas constant

5 Dalton's law of partial pressure

6 Mathematical derivation of Dalton's law and their applications

7 Graham's law of diffusion and its applications

8 Kinetic model of gas and its postulates

9 Ideal and real gases

10 Deviation of gas from ideal behaviour

(Solving related numerical problems)

3.2 Liquid State:

1 Physical properties of liquid

i. Evaporation and condensation

ii. Vapour pressure of liquid and boiling

iii. Surface tension

iv. Viscosity

2 Solution and solubility:

i. Equilibrium in saturated solution

ii. Solubility and solubility curve and its applications.

(Solving related numerical problems)

3.3. Solid State:

1 Crystalline and amorphous solids

2 Water of crystallization

3 Effloresences

4 Deliquesces

5 Hygroscopic

6 Seven types of crystal system

7 Simple cubic, face centered and body centered

Unit 4: Atomic Structure - 10 teaching hours

1 Discovery of fundamental particles of atom (electron, proton and neutron)

2 Concept of atomic number, mass number, fractional atomic mass, isotopes, isobars

3 Rutherford's α ray scattering experiment and nuclear model of atom; limitation

4 Bohr's model of atom and explanation of hydrogen spectra

5 Limitation of Bohr's model of atom

6 Elementary idea of quantum mechanical model

i. Dual nature of electron (de-Broglie equation)

ii. Heisenberg's uncertainty principle

iii. Probability concept

7 Shape of atomic orbital (s and p orbitals only)

8 Quantum numbers

9 Pauli's exclustion principle

10 Hund's rule of maximum multiplicity

11 Aufbau principle and Bohr Bury rule

12 Electronic configuration of the atoms and ions(Z = 1 to 30)

Unit 5: Nuclear Chemistry - 3 Teaching hours

1 Concept radioactivity

2 Radioactive rays (alpha ray, beta ray & gamma ray)

3 Meaning of natural and artificial radioactivity

4 Nuclear reactions, Nuclear energy (fission and fusion)

5 Nuclear isotopes and uses

Unit 6: Electronic Theory of Valency and Bonding - 8 teaching hours

1 Basic assumption of electronic theory of valency

2 Octet rule

3 Ionic bonds, ionic compounds and characteristics of ionic compounds. Lewis symbol to represent the formation of ionic compounds

4 Covalent bonds, covalent compounds and characteristics of covalent compounds – Lewis structure of some typical covalent compounds

5 Co-ordinate covalent bonds. Lewis structures of some typical co-ordinate covalent compounds

6 Exception of the octet rule

7 Partial ionic characters of covalent compounds. Non-polar and polar covalent molecules

8 Dipole moments and its application

9 Some special types of bonds: hydrogen bond and its types, metallic bond, vander Waal's bond, Resonance and resonance hybrid structures of O3, SO3, SO2, CO3-2, SO4-2, PO4-2,NO3-

10 Classification of crystalline solids

i. Ionic solid

ii. Covalent solid

iii. Molecular solid

iv. Metallic solid

Unit 7: Periodic Classification of Elements - 6 teaching hours

1. Introduction

2. Mendeleev's periodic law and periodic table

3. Anamolies of Mendeleev's periodic table

4. Modern periodic law, and modern periodic table

5. Advantages of modern Periodic table

6. Division of elements into s,p, d and f blocks

7. Periodicity of physical properties: valency , atomic radii, ionic radii, ionisation energy, electron affinity and electronegativity (general trends only)

Unit 8: Oxidation and Reduction - 6 teaching hours

1 Classical concept of oxidation and reduction

2 Electronic interpretation of oxidation and reduction

3 Oxidation number and rules for the assignment of oxidation number

4 Differentiate between oxidation number and valency

5 Oxidising and reducing agent

6 Redox reaction

7 Balancing redox reactions by

i. oxidation number method

ii. ion-electron method

Unit 9: Equilibria - 5 teaching hours

1. Introduction

2. Equilibrium involving in physical change

3. Chemical equilibrium

- Reversible and irreversible reactions

- Dynamic nature of chemical equilibrium and its characteristics

- Law of mass action

- Equilibrium constant (Kc) and its characteristics

- Homogenous and heterogeneous equilibrium

- Relation between Kp and Kc (derivation)

- Le-chatelier's principle and its application

(No numerical is required)

General and Physical Chemistry (i)   Inorganic chemistry (i) 

Organic chemistry (i)   General and Physical Chemistry(ii) 

Organic chemistry (ii)   Inorganic chemistry(ii)