COMPLETE PHYSICAL CHEMISTRY FOR CLASS XI And XII
Subject chemistry Medium ENGLISH
Faculty NV Sir Status AVAILABLE
Category COMPLETE COURSE Lecture 143
Target XI XII XIII Books QUESTION BANK ATTACHED
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Syllabus

Mole concept

Lecture# Description Duration
01 Dalton atomic theory, isotope ,isobar, atomic mass, atomic mass unit amu, molecule, molecular mass 41 Minutes
02 molar mass. Gram atomic mass, gram molecular mass, avogadro law 48 Minutes
03 Relative atomic mass, relative density, vapour density, specific gravity, average atomic mass, average molar mass 44 Minutes
04 Percentage composition, molecular formula, empirical formula, gay-lussac law 30 Minutes
05

Stoichiometry, mole-mole analysis, combustion of hydrocarbon

34 Minutes
06

limiting reagent, percentage yield , consecutive reaction

39 Minutes
07 Principle of atomic conservation POAC 37 Minutes
08 Percentage purity of sample, combustion of carbon, analysis of mixture 29 Minutes
09 Numerical on analysis of mixture, law of mass conservation, law of definite proportions, law of  multiple proportions, law of reciprocal proportions 24 Minutes
10 Solution, solute , solvent, mole fraction, %w/w/, 18 Minutes
11 %w/v, % v/v, strength of solution, molarity, molality, ppm 35 Minutes
12 Interconversion of concentration terms 46 Minutes
13 Molarity of pure water , volume strength of hydrogen peroxide solution, relation between volume strength and molarity 35 Minutes
14 Silver salt method , Eudiometry 38 Minutes
15 examples of eudiometry 27 Minutes
16 Significant figure, rules for counting , rounding off, scientific notation, addition/subtraction, multiplication of significant figure 42 Minutes

 

Equivalent concept

Lecture# Description Duration
01 Oxidation number calculation, average O.N. individual O. N. 44 Minutes
02 Oxidizing agent, reducing agent, disproportion reactions 58 Minutes
03 Balancing of redox and disproportion reaction , balancing of molecular reaction 46 Minutes
04 Equivalent concept. Law of chemical equivalence, relation between mole and equivalent, equivalent mass, valence factor calculation for acid & base 45 Minutes
05 n- factor for salt, n - factor for disproportion reaction 49 Minutes
06 Titration, acid base titration, permanganate titration, dichromate titration 39 Minutes
07 Back titration , double titration 34 Minutes
08 Numerical on double titration, iodometric titration, limitation of equivalent concept 33 Minutes
09 Bleaching powder and calculation of available chlorine from bleaching powder sample 31 Minutes
10 Hardne    ss of water ( temporary & permanent hardness) strength of oleum 35 Minutes
11 Volume strength of hydrogen peroxide solution 20 Minutes

Chemical equilibrium

Lecture# Description Duration
01 Reversible & irreversible reactions, physical and chemical eq, homogeneous and heterogeneous eq, properties of eq, Kp, Kc, Kx, relation between Kp & Kc, relation between Kp and Kx, degree of dissociation 1 hr  13 Minutes
02 Effect of stoichiometry on kp & Kc, examples of homogeneous equilibrium 38 Minutes
03 Numericals of homogeneous eq. 29 Minutes
04 Heterogeneous eq., homogeneous liquid eq., significance of value of k, reaction quotient 53 Minutes
05 Approximation during calculation, relation between vapour density and degree of dissociation 53 Minutes
06 Thermodynamics for chemical eq, factor affecting composition of eq mixture , le-chatelier's principle, effect of concentration , effect of temperature 38 Minutes
07 Effect of change in pressure and volume , effect of catalyst 36 Minutes
08 Addition of inert gas at constant volume and constant pressure, le-chatelier's principle for physical eq, evaporation of water, boiling of water, melting of ice , melting of metal 1 hr
09 Solubility of gas in liquid , allotropic change , simultaneous eq. 42 Minutes

 

Ionic equilibrium

Lecture# Description Duration
01 Strong electrolyte, weak electrolyte, strong acids, weak acids, strong base, weak base , acid base theory, arrhenius concept, bronsted lowry concept , amphiprotic species 31 Minutes
02 Lewis concept , pH scale, properties of water, ionisation constant of water, ionic product of water 45 Minutes
03 pH calculation for strong acid, strong base, mixture of strong acid , mixture of strong acid and base , common ion effect 43 Minutes
04 pH for monobasic weak acid, weak base, ostwald dilution law, pH for very dilute strong acid 41 Minutes
05 Very dilute weak base , mixture of weak acid and strong acid,polyprotic weak acid 40 Minutes
06 Numerical on polyprotic weak acid, mixture of two weak acids 33 Minutes
07 Hydrolysis of salt, salt of strong acid and strong base, salt of weak acid and strong base , salt of weak base and strong acid 52 Minutes
08 Hydrolysis of salt of weak acid and weak base 39 Minutes
09 pH for polyvalent anion, ph for amphiprotic anion , introduction of buffer solution 37 Minutes
10 Acidic buffer and basic buffer 43 Minutes
11 Buffer capacity, titration ( strong acid v/s strong base, strong acid v/s weak base , weak acid v/s strong base) 53 Minutes
12 Titration of H3PO4 v/s NaOH 35 Minutes
13 Indicator, phenolphthalein, methyl orange, pH range for a buffer ,double titration 38 Minutes
14 Solubility of sparingly soluble salt, Ksp, effect of common ion on solubility, simultaneous solubility 44 Minutes
15 Ionic product v/s solubility product,selective precipitation, 41 Minutes
16 solubility of salt in buffer solution, complex formation by salt 37 Minutes
17 Solubility of amphoteric insoluble hydroxide, solubility of salt if cation is hydrolyzed , solubility of salt if anion is hydrolyzed 43 Minutes

Thermodynamics & thermochemistry

Lecture# Description Duration
01 System ,surrounding,open system, closed system, isolated system, thermodynamic variable, process, open cycle ,closed cycle,intensive prop. Extensive prop., state function, path function, heat, work, heat capacity, molar heat capacity, specific heat capacity ,IUPAC , types of process, isothermal, isobaric, isochoric, adiabatic process,convention for heat and work 41 Minutes
02 Reversible and irreversible process, reversible isothermal compression, single step isothermal compression, two stage isothermal compression 56 Minutes
03 Reversible isothermal expansion, single stage isothermal expansion, two stage isothermal expansion, internal energy, degree of freedom, first law of thermodynamics 50 Minutes
04 Enthalpy change , phase transformation 46 Minutes
05 Free expansion, reversible adiabatic process, work calculation for reversible Adiabatic and irreversible  Adiabatic processes 43 Minutes
06 comparison between reversible adiabatic and irreversible adiabatic processes, comparison between reversible adiabatic and reversible isothermal processes 42 Minutes
07 Spontaneous and nonspontaneous process, entropy, second law of thermodynamics , entropy change for system and surrounding 55 Minutes
08 Numerical on entropy change , entropy change during free expansion 40 Minutes
09 Gibbs energy change, heat pump, carnot cycle 56 Minutes
10 Thermochemistry, enthalpy of formation, enthalpy of combustion 48 Minutes
11 Enthalpy of fusion, vaporization,sublimation,bomb calorimeter, enthalpy of neutralisation, enthalpy of ionisation 57 Minutes
12 Bond enthalpy, hess law, resonance energy. Lattice energy , hydration energy, enthalpy of formation of ion, kirchhoff equation, integral enthalpy of solution, calculation of lattice energy using born haber cycle 1 hr 7 Minutes

Gaseous State

Lecture# Description Duration
01 State of matter (solid, Liq, gas) ideal gas equation, Boyle’s law. 32 Minutes
02 Barometer, faulty Barometer 33 Minutes
03 Problems on barometer, Charles law 40 Minutes
04 Gay-lussac’s law, Avogadro's law, ideal gas equation 21 Minutes
05 Numerical 45 Minutes
06 Graham’s law for diffusion. 36 Minutes
07 Kinetic theory of gas, root mean square velocity 40 Minutes
08 Compressibility factor (Z) pressure correction factor, volume correction factor, excluded volume, van der waal gas equation 50 Minutes
09 Virial equation, liquification of gas, critical temperature (Tc) Critical pressure (Pc) Critical volume (Vc) Boyle’s temperature 46 Minutes
10 Liquification of gas manometer
    (Open end, Closed end, reduced equation of state), Collision diameter, Collision frequency
52 Minutes

Atomic structure

Lecture# Description Duration
01 Cathode tube experiment anode rays, radioactive decay. 33 Minutes
02 Thomson plum pudding model. Rutherford model, Nearest distance of approach. 51 Minutes
03 Electromagnetic theory, Planck Quantum Theory, Blackbody radiation, electron volt. 50 Minutes
04 Photoelectric effect, Work function, Threshold frequency stopping potential. 41 Minutes
05 Photo current photo intensity, Bohr model, Bohr Radius 34 Minutes
06 Velocity, Kinetic Energy, Total energy, Potential energy of electron in Bohr orbit 29 Minutes
07 Time period, frequency, ionisation energy, ionisation potential, Excitation energy, excitation potential Binding energy. 35 Minutes
08 Spectrum, emission, line spectrum, band spectrum , H-spectrum, lyman series. 45 Minutes
09 Balmer series, Paschen, Brackett, Pfund, humphrey series, maximum number of spectral lines. 50 Minutes
10 Limitations of bohr model, dual nature of particle, de broglie's equation 41 Minutes
11 Heisenberg’s uncertainty principle Difference between orbit & orbital 39 Minutes
12 Types of orbitals {s, p, d, f}, quantum numbers, (principal, azimuthal, magnetic, spin) 37 Minutes
13 Electron filling rule, Aufbau principle, Hund’s rule, pauli’s exclusion principle, magnetic nature, magnetic moment 47 Minutes
14 Wave quantum theory, schrodinger wave equation, radial node, angular node. 42 Minutes

 

Solution & colligative properties

Lecture# Description Duration
01 Introduction
    Different concentration terms interconversion, colligative properties, van’t hoff factor calculation, osmotic pressure.
33 Minutes
02 Osmosis , Osmotic pressure (different cases) 47 Minutes
03 Numericals on osmotic pressure 46 Minutes
04 Vapour pressure, relative lowering of vapour pressure, 41 Minutes
05 Numericals on RLVP, Ostwald walker method 40 Minutes
06 Elevation in boiling point, calculation of Kb (molal elevation boiling point constant) . Depression in freezing point, Calculation of Kf, 54 Minutes
07 Numericals on elevation in boiling point and depression in freezing point 36 Minutes
08 Thermodynamic explanation of 𝝙Tb & 𝝙Tf 6 Minutes
09 Raoult’s law when two volatile liquids are mixed 49 Minutes
10 Ideal and nonideal solution 34 Minutes
11 Azeotropes, mixture of two immiscible liquids, solubility of gas in liquid, henry law 58 Minutes

Solid state

Lecture# Description Duration
01 Types of solid, Crystal, Amorphous, unit cell, 2D, 3D, space,lattice. 42 Minutes
02 Primitive, body centred, face centered contribution of atoms in cubic unit cell. Packing fraction of square packing and hexagonal packing 47 Minutes
03 Coordination Number, packing fraction, density of solid.,Simple cubic, BCC, FCC, CCP 44 Minutes
04 Closed packing in 3D HCP packing,
    Linear void, Triangular void, Tetrahedral void, octahedral void, Cubical void Types of void in FCC
57 Minutes
05 Voids in FCC,Different radius ratio for ionic compounds. 47 Minutes
06 Calculation of nearest, next nearest and next to next nearest atoms in SC, BCC, FCC. 29 Minutes
07 Structure of NaCl type, Zns type, CaF2 type, Na2O type, CSCl type, Diamond 50 Minutes
08 Spinal structure, perovskite corundum structure, packing fraction of NaCl, Defect In crystal, Schottky, Frenkel, Interstitial 39 Minutes
09 Non stoichiometric defect, cation excess defect cation deficiency defect, Paramagnetic, Diamagnetic Ferromagnetic, Ferrimagnetic, Antiferromagnetic compound 31 Minutes

 

Chemical kinetics

Lecture# Description Duration
01 Fast reaction , slow reaction, moderate reaction, average rate of reaction, instantaneous rate of reaction, relation of rate of reaction between various reagents , order 57 Minutes
02 Order law, zero order reaction 35 Minutes
03 First order reaction 28 Minutes
04 Half life period for first order reaction 27 Minutes
05 Average life period for first order, generation time , first order bacterial growth, second order reaction 24 Minutes
06 nth order reaction, pseudo first order reaction 35 Minutes
07 Rate of reaction of two or reactant are taken, calculation of order by half life method 32 Minutes
08 Initial rate method , integrated rate law, ostwald isolation method to determine order 40 Minutes
09 Monitoring of first order reaction using pressure measurement 30 Minutes
10 Monitoring of first order reaction using titration and optical rotation 42 Minutes
11 Arrhenius transition state theory 29 Minutes
12 Arrhenius equation 32 Minutes
13 Effect of catalyst on rate constant, temperature coefficient for reaction 39 Minutes
14 Simple and complex reaction, molecularity, rate determining step RDS 29 Minutes
15 Determination of rate if RDS is given , steady state approximation,complexity in first order reaction, parallel first order reactions 48 Minutes
16 Reversible first order reaction 29 Minutes
17 Consecutive first order reaction 19 Minutes

Radioactivity

Lecture# Description Duration
01 Cause of radioactivity belt of stability , comparison between alpha particle, beta particle and gamma rays 15 Minutes
02 Group displacement law soddy fajan rule,, k– electron capture ,first order decay. 28 Minutes
03 Radioactive decay 28 Minutes
04 Carbon dating, Age of rock using U & Pb,Age of rock using U & He 53 Minutes
05 Mass defect ,Binding energy, Binding energy per nucleon. Nuclear fission and fusion. 51 Minutes

 

Surface chemistry

Lecture# Description Duration
01 Adsorption, Adsorbate, Adsorbent, Thermodynamics of Adsorption, Adsorption v/s Absorption, Physical Adsorption. 47 Minutes
02 Freundlich & Langmuir isotherm, catalytic action of Homogeneous catalyst & Heterogeneous catalyst, Positive & negative catalyst, Homogeneous catalyst, Promoters, Catalytic poison, zeolites, enzyme catalyst, Types of solution, Dispersed phase & Dispersion medium. 48 Minutes
03 Types of colloidal solution, Lyophobic, Lyophilic, macromolecular, micromolecular, Associated colloid/ micelle, cleansing action of soap, Bredig’s arc method,Peptization 43 Minutes
04 Chemical method to prepare colloidal solution, Tyndall effect, Brownian motion, Electrophoresis, coagulation, protection of colloid. 53 Minutes
05 Gold number, Helmholtz double layer theory ,emulsion. 22 Minutes

 

Electrochemistry

Lecture# Description Duration
01 Electrochemical cell, Oxidation half cell, Reduction half cell, Galvanic cell 1 hr 05 Minutes
02 Salt bridge, Daniel cell net cell reaction reaction Quotient cell representation relation between DG & E properties of DG & E,nernst equation 44 Minutes
03 Spontaneity of reaction in cell, nernst equation cell at equilibrium, concentration cell. Hydrogen electrode and standard hydrogen electrode 44 Minutes
045 Metal + insoluble salt + soluble anion type half cell
            Eg.   Ag + AgCl + Cl–
1 hr 15 Minutes
05 Calomel electrode, electrochemical series, thermodynamics for electrochemical cell, 𝝙G, 𝝙H, 𝝙S 59 Minutes
06 Electrolysis & electrolytic cell, electrolysis of nacl, nabr, H2SO4,H2O, first law of electrolysis Faraday law 1 hr 11 Minutes
07 Examples of first law of faraday, second law of faraday 51 Minutes
08 Primary cell ,leclanche cell, secondary cell, lead storage battery , Ni-Cd cell , H2-O2 fuel cell, electrolytic conduction 50 Minutes
09 Molar conductivity, equivalent conductivity , relation between molar cond. And equv. Cond., kohlrausch law, calculation of molar cond using wheatstone bridge , relation between molar cond. And concentration for weak electrolyte and strong electrolyte ,huckel onsager equation 54 Minutes
10 Ionic mobility, conductometric titration for strong acid V/s strong base , strong acid v/s weak base and other examples 51 Minutes

 

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