NEET Chemistry Video Lectures For Class 11

Nature of electromagnetic radiation, photoelectric effect; Spectrum of the hydrogen atom.

Bohr model of a hydrogen atom - its postulates, derivation of the relations for the energy of the electron and radii of the different orbits, limitations of Bohr's model; Dual nature of r,latter, de Broglie's relationship.

Heisenberg uncertainty principle.

Elementary ideas of quantum mechanics, quantum mechanics, the quantum mechanical model of the atom, its important features.

Concept of atomic orbitals as one-electron wave functions:
Variation ofY and Y2 with r for ls and 2s orbitals: various quantum numbers (principal, angular momentum, and magnetic quantum numbers) and their significance; shapes of s, p, and d - orbitals, electron spin and spin quantum number: Rules for filling electrons in orbitals - Aufbau principle.

Pauli's exclusion principle and Hund's rule, electronic configuration of elements, extra stability of half-filled and completely filled orbitals'

Kossel - Lewis approach to chemical bond formation, the concept of ionic and covalent bonds.

Ionic Bonding: Formation of ionic bonds, factors affecting the formation of ionic bonds; calculation of lattice enthalPY.

Covalent Bonding: concept of electronegativity. Fajan's rule, dipole moment: valence Shell Electron Pair Repulsion(VSEPR) theory and shapes of simple molecules.

Quantum mechanical approach to covalent bonding: Valence bond theory - its important features. the concept of hybridization involving s, p, and d orbitals; Resonance

Molecular orbital Theory - Its important features. LCAOs, 'types of molecular orbitals (bonding, antibonding), sigma and pi-bonds, molecular orbital electronic configuration of homonuclear diatomic molecules, the concept of bond order, bond length, and bond energy.

Elementary idea of metallic bonding.

Hydrogen bonding and its applications.

Fundamentals of thermodynamics: system and surroundings, extensive and intensive properties' state functions, types of processes.

The first law of thermodynamics: concept of work, heat internal energy and enthalpy, heat capacity,molar heat capacity;Hess’s law of constant heat summation;Enthalpies of bond dissociation, combustion' formation, atomization. sublimation. phase transition, hydration. ionization. and solution.

The second law of thermodynamics - Spontaneity of processes

Meaning of equilibrium, the concept of dynamic equilibrium.

Equilibria involving physical processes: Solid-liquid, liquid - gas and solid-gas equilibria, Henry's law. General characteristics of equilibrium involving physical processes.

Equilibrium involving chemical processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance, the significance of ΔG and ΔG° in chemical equilibrium, factors affecting equilibrium concentration, pressure, temperature, the effect of catalyst; Le Chatelier's principle.

Ionic equilibrium: weak. and strong electrolytes, ionization of electrolytes, various concepts of acids and bases (Arrhenious and Bronsted - Lowry and Lewis) and their ionization, acid-base equilibria (including multi stage ionization) and ionization constants, ionization of water. PH scale, common ion effect, hydrolysis of salts and PH of their solutions, the solubility of sparingly soluble salts and solubility products, buffer solutions.

Group 13 and 14 elements

General Introduction: Electronic configuration and general trends in physical and chemical properties of elements across the periods and down the groups; unique behaviour of the first element in each group.

Tetravalency of carbon: Shapes of simple molecules - hybridization (s and p): classification of organic compounds based on functional groups: and those containing halogens, oxygen, nitrogen and sulphur; Homologous series: Isomerism - structural and stereoisomerism.

Nomenclature (Trivial and IUPAC)

Covalent bond fission - Homolytic and heterolytic: free radicals. carbocations. and carbanions: stability of carbocations and free radicals. electiophires. and nucleophiles.

Electronic displacement in a covalent bond

Inductive effect, electromeric effect. resonance and hyperconjugation.

Common types of organic reactions- Substitution. addition. elimination, and rearrangement.

Classification' isomerism. IUPAC nomenclature, general methods of preparation, properties, and reactions.

Alkanes - Conformations: Sawhorse and Newman projections (of ethane): Mechanism of halogenation of alkanes, projections (of ethane).

Alkenes - Geometrical isomerism: Mechanism of electrophilic addition: addition of hydrogen. halogens, water. hydrogen halides (Markownikoffs and peroxide effect): Ozonolysis and polymerization.

Alkynes - Acidic character: Addition of hydrogen, halogens, water, and hydrogen halides: Polymerization.

Aromatic hydrocarbons - Nomenclature. benzene - structure and aromaticity: Mechanism of substitution: halogenation, nitration.

Friedel- Craft's alkylation and acylation, directive influence of the functional group in mono-substituted benzene.