Class 11 Chemistry Part I

Introduction to the development of chemistry from ancient India to modern science, the nature of matter and its properties, laws of chemical combination, Dalton's atomic theory, atomic and molecular masses, the mole concept, percentage composition, empirical and molecular formulae, stoichiometric calculations, balancing equations, and expressing concentration of solutions using mass per cent, mole fraction, molarity, and molality

Discovery of sub-atomic particles (electron, proton, neutron) and their properties, Thomson and Rutherford atomic models, atomic number, mass number, isobars and isotopes, Bohr's model of the hydrogen atom, electromagnetic radiation, Planck's quantum theory, photoelectric effect, atomic spectra, de Broglie relation, Heisenberg uncertainty principle, quantum mechanical model, atomic orbitals, quantum numbers, electronic configuration of atoms, and the stability of completely filled and half-filled subshells

Historical development of the Periodic Table from Dobereiner's Triads through Newlands' Octaves to Mendeleev's Periodic Law, the Modern Periodic Law based on atomic number, electronic configuration as the basis for periodic classification, naming of elements with Z > 100, s-p-d-f block classification, and periodic trends in physical and chemical properties including atomic and ionic radii, ionization enthalpy, electron gain enthalpy, electronegativity, valence, and chemical reactivity

Kossel-Lewis approach to ionic and covalent bonding, Lewis dot structures and the octet rule with its limitations, formal charge, ionic and covalent bond formation, lattice enthalpy and Born-Haber cycle, bond parameters including length energy and polarity, VSEPR theory for predicting molecular geometry, valence bond theory and orbital overlap, sigma and pi bonds, hybridisation involving s p and d orbitals, molecular orbital theory applied to homonuclear diatomic molecules, bonding and antibonding orbitals, bond order and magnetic properties, and the concept of hydrogen bonding

Thermodynamic terms including system, surroundings, boundary, and types of systems; internal energy, work, and heat; first law of thermodynamics with mathematical formulation; enthalpy as a state function and the relationship between enthalpy change and internal energy change; measurement of enthalpy changes using calorimetry; standard enthalpy of reactions including formation, combustion, atomisation, sublimation, ionisation, bond dissociation, solution, and dilution; Hess's law of constant heat summation; extensive and intensive properties; spontaneous and non-spontaneous processes; entropy as a thermodynamic state function; Gibbs energy change and its relationship with spontaneity and equilibrium constant; second and third laws of thermodynamics with absolute entropy and standard entropy calculations

Dynamic nature of equilibrium in physical and chemical processes; the law of equilibrium and expressions for equilibrium constants; relationship between Kp and Kc; factors affecting equilibrium and Le Chatelier's principle; Arrhenius, Bronsted-Lowry, and Lewis concepts of acids and bases; ionization constants and degree of ionization; pH scale and hydrogen ion concentration; ionization of water and ionic product; buffer solutions; solubility product constant; common ion effect on solubility and pH-dependent solubility of weak acid salts