| Unit 1 Some Basic Concepts of Chemistry |
- Dalton's atomic theory, the idea of the atom, molecule, element, and compound, and the nature of matter
- Physical quantities and measurements in chemistry, precision and accuracy, significant figures, SI units, and dimensional analysis
- Chemical mixing laws.
- Atomic and molecular masses, the mole concept, molar mass, percentage composition, and empirical and molecular equations are all covered.
- Stoichiometry and chemical equations
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| Unit 2 States of Matter |
- Matter is classified into three states: solid, liquid, and gaseous.
Gas laws — Boyle's law, Charles' law, Graham's law of diffusion, Avogadro's law, Dalton's law of partial pressure.
The concept of the absolute temperature scale; the ideal gas equation; and the kinetic theory of gases (only postulates).
The average, root mean square, and most likely velocities concepts.
Real gases, deviance from ideal behaviour, compressibility factor, van der Waals equation, gas liquefaction, critical constants
Liquid State: Liquid properties such as vapour pressure, viscosity, and surface tension, as well as the effect of temperature on them (qualitative treatment only).
Solid State: Solids are classified as molecular, ionic, covalent, and metallic solids, as well as amorphous and crystalline solids (elementary idea).
Bragg's Law and its ramifications
- Unit cell and lattices, packing in solids (fcc, bcc and hcp lattices), voids, calculations involving unit cell parameters, Imperfections in solids.
- Electrical, magnetic and dielectric properties.
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| Unit 3 Atomic Structure |
- Subatomic particle discovery (electron, proton, and neutron).
- The limits of the Thomson and Rutherford atomic models
- The characteristics of electromagnetic radiation, The photoelectric effect
- The spectrum of the hydrogen atom, the Bohr model of the hydrogen atom – its postulates, the derivation of the relationships for the energy of the electron and the radii of the various orbits, the limitations of Bohr's model
- Matter's dual nature, the de-Broglie connection, and the Heisenberg uncertainty principle
- The fundamental concepts of quantum mechanics, the quantum mechanical model of an atom, its key properties, and the concept of atomic orbitals as one-electron wave functions.
- Variation of 1 and 2 with r for 1s and 2s orbitals; importance of various quantum numbers (principal, angular momentum, and magnetic quantum numbers).
- Shapes of s, p and d – orbitals, electron spin and spin quantum number.
- Rules for filling electrons in orbitals – Aufbau principle, Pauli exclusion principle and Hund’s rule, electronic configuration of elements, the extra stability of half-filled and completely filled orbitals.
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| Unit 4 Chemical Bonding and Molecular Structure |
- The Kossel – Lewis approach to chemical bond formation, as well as the concept of ionic and covalent bonds
- Ionic Bonding: Formation of ionic bonds, variables influencing ionic bond formation, computation of lattice enthalpy
- Electronegativity, Fajan's rule, and the dipole moment are all concepts in covalent bonding. The theory of Shell Electron Pair Repulsion (VSEPR) and the morphologies of simple molecules
- Valence bond theory is a quantum mechanical approach to covalent bonding. Its key aspects include the concept of hybridization involving s, p, and d orbitals, as well as resonance.
- Molecular Orbital Theory: Its key elements include LCAOs, several forms of molecular orbitals (bonding and antibonding), sigma and pi-bonds, molecular orbital electronic configurations of homonuclear diatomic molecules, and the concepts of bond order, bond length, and bond energy.
- The fundamental concept of metallic bonding, hydrogen bonding, and its applications
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| Unit 5 Chemical Thermodynamics |
- The fundamentals of thermodynamics are as follows: system and surroundings, extensive and intense properties, state functions, and process types.
- The concept of work, heat internal energy, and enthalpy, as well as heat capacity and molar heat capacity, are all part of the first law of thermodynamics.
- Hess's constant heat summation law.
- Bond dissociation enthalpies, combustion enthalpies, formation enthalpies, atomization enthalpies, sublimation enthalpies, phase transition enthalpies, hydration ionisation enthalpies, and solution enthalpies
- Spontaneity of processes; Delta S of the universe and Delta G of the system as criterion for spontaneity, Delta Go (Standard Gibbs energy change) and equilibrium constant.
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| Unit 6 Solutions |
- There are several ways to express the concentration of a solution: molality, molarity, mole fraction, percentage (by volume and mass), solution vapour pressure, and Raoult's Law.
- Ideal and non-ideal solutions, vapour pressure – composition, ideal and non-ideal solution charts
- Dilute solution colligative qualities, relative decrease in vapour pressure, decrease in freezing point, increase in boiling point, and osmotic pressure
- Using colligative properties to calculate molecular mass.
- Molar mass with an abnormal value, the Hoff factor, and its importance
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| Unit 7 Equilibrium |
- The definition of equilibrium, as well as the concept of dynamic equilibrium.
- Equilibria involving physical processes include solid-liquid, liquid-gas, and solid-gas equilibria, as well as Henry's law, which is a general feature of equilibrium involving physical processes.
- Chemochemical process equilibria: Chemical equilibrium law, equilibrium constants (Kp and Kc) and their relevance, Delta G and Delta Go in chemical equilibria, factors affecting equilibrium concentration, pressure, temperature, and the impact of the catalyst
- The principle of Le Chatelier.
- Weak and strong electrolytes, ionisation of electrolytes, different concepts of acids and bases (Arrhenius, Bronsted-Lowry, and Lewis) and their ionisation, acid-base equilibria (including multistage ionisation) and ionisation constants, ionisation of water, pH scale, common ion effect, hydrolysis of salts and pH of their solutions, solubility of sparingly soluble salts and so
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| Unit 8 Redox Reactions and Electrochemistry |
- Electronic concepts of oxidation and reduction, redox reactions, oxidation number, oxidation number assignment methods, and redox reaction balancing
- Conduction in electrolytic and metallic solutions, specific and molar conductivities, and their fluctuation with concentration
- The law of Kohlrausch and its applications
- Electrochemical cells include electrolytic and galvanic cells, various types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions, and the measurement of the emf of a Galvanic cell.
- The Nernst equation and its applications; the relationship between cell potential and the Gibbs energy change.
- Fuel cells, dry cell and lead accumulator
- Corrosion and its control.
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| Unit 9 Chemical Kinetics |
- The rate of a chemical reaction, as well as the elements influencing reaction rates: concentration, temperature, pressure, and catalyst.
- Elementary and complicated reactions, reaction order and molecularity, rate law, rate constant and its units, differential and integral forms of zero and first-order reactions, their properties and half-lives, and the effect of temperature on reaction rate
- Arrhenius theory, activation energy and its computation, bimolecular gaseous collision theory (no derivation).
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| Unit 10 Surface Chemistry |
- Adsorption: Physisorption and chemisorption and their properties, variables influencing gas adsorption on solids: Adsorption isotherms of Freundlich and Langmuir, as well as adsorption from solutions
- Catalysis: Homogeneous and heterogeneous, solid catalyst activity and selectivity, enzyme catalysis, and its mechanism
- Colloidal state: distinction between real solutions, colloids, and suspensions; colloidal classification: lyophilic, lyophobic.
- Preparation and properties of colloids: Tyndall effect, Brownian movement, electrophoresis, dialysis, coagulation, and flocculation of multimolecular, macromolecular, and linked colloids (micelles).
- Emulsions and their properties
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