Physical Chemistry basic to Adv by AD in 25hr

Explain the transition from Thomson's plum pudding model to a nucleus-centered atom, illustrated by alpha particle scattering in gold foil that reveals a tiny nucleus and mostly empty space.

Examine how electromagnetic radiation drives electron emission in the photoelectric effect, linking photon energy, work function, and kinetic energy to stopping potential and frequency-dependent thresholds.

Explore the Bohr model of the atom, linking electron orbits, energy levels, and radius calculations for hydrogen, and derive kinetic, potential, and ionization energies.

Explore how atomic spectra arise from electronic transitions, focusing on line spectra and emission processes, and how energy differences between levels create distinct spectral lines in the visible range.

Explore the wave mechanical model of the atom, explaining how energy levels, sublevels, and de Broglie wavelengths account for spectral lines and how Heisenberg’s uncertainty principle limits orbital descriptions.

Explore the wave mechanical model of the electron, grounded in Heisenberg's uncertainty principle, Schrödinger's equation, and the wavefunction's radial and angular parts, revealing quantum numbers and orbital probabilities.

Explains how the four quantum numbers n, l, m_l, and m_s define electron location, orbital shape, orientation, and spin, and how pauli exclusion shapes electronic configurations.

Explore the ideal gas concept and gas laws, including Boyle's law, Charles's law, Avogadro's law, and Dalton's partial pressures, with discussions on diffusion, effusion, density, and molar volume.

Explore how real gases deviate from ideal behavior due to intermolecular forces and molecular volume. Learn about van der Waals corrections, critical constants, and reduced properties.

Explore fundamentals of thermodynamics, defining systems and boundaries, distinguishing open, closed, and isolated systems; examine state functions, intensive and extensive properties, heat capacity, and reversible versus irreversible processes.

Explore how to apply the first law to calculate work for expansion, contraction, and isothermal processes, relate changes in internal energy to degrees of freedom, kinetic energy, and Boltzmann's constant.

Explore the first law details: energy conservation, internal energy as a state function, and heat–work exchange under constant volume and constant pressure, including adiabatic and isothermal processes.

Explore how entropy governs spontaneity in the second law by comparing reversible and irreversible processes and the roles of system, surroundings, and universe.

Explore the second law in detail by deriving system entropy changes for reversible and irreversible processes, and comparing isothermal and adiabatic scenarios with system and surroundings.

Explore thermochemistry by defining enthalpy as heat at constant pressure, and learn standard enthalpy of formation from elements in standard states, with internal combustion and Hess's law.

Explore enthalpy in physical chemistry, including enthalpy of fusion, enthalpy of sublimation, enthalpy of formation, enthalpy of neutralisation, enthalpy of ionisation, and bomb calorimetry to quantify heat changes.

Explore how bond enthalpy and formation enthalpy determine reaction heat by counting bonds broken and formed, using examples like sublimation, lattice energy, and dissolution through Born-Haber cycles.

Explore reversible reactions, chemical equilibrium, and the balance of forward and backward rates in a closed system, with mass-action concepts and physical versus chemical, homogeneous versus heterogeneous equilibria.

Explore how rate law and equilibrium concepts shape reaction direction, using the reaction quotient Q, equilibrium constant K, temperature effects, and degree of dissociation.

Explore how concentration, pressure, volume, and temperature shifts drive equilibria via Le Chatelier's principle, with gas and solid examples like graphite–diamond, ice–water, and inert gas effects.

Explore the oxidation state concept, rules, and exceptions, learn to determine individual and average oxidation states from structure and electronegativity differences, with practical sodium, oxygen, hydrogen, and peroxide examples.

Explain how to assign oxidation states in diverse structures using electronegativity and coordinated bonds, including mixed oxides and carbon dioxide, and define oxidising and reducing agents.

Identify oxidation states, distinguish oxidation and reduction, and balance redox reactions using half-reaction methods, including balancing atoms, oxygen, hydrogen, and electrons.

Balance redox reactions in acidic medium by identifying oxidation states and using half-reactions with water and H+, ensuring electron transfer and charge balance.

Explore balancing redox reactions by converting molecular formulas to ionic forms, removing unchanged oxidation-state ions, balancing electrons and hydrogens with water and H+, and converting back to molecular equations.

Explore the law of chemical equivalence and the concept of equivalent mass, showing how to balance and apply equivalents in redox and oxidation-reduction problems.

Explore the equivalent concept in redox chemistry by calculating oxidation and reduction changes, applying balancing and equivalent factors, and solving disproportionation and redox balancing problems.