NUCLEON Complete Chemistry Class 11+12 (Physical Chemistry & Inorganic Chemistry) for IIT JEE/NEET by NV Sir [ FREE ]

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NUCLEON Complete Chemistry Class 11+12 (Physical Chemistry & Inorganic Chemistry) for IIT JEE/NEET by NV Sir 

  IIT-JEE NUCLEON CHEMISTRY 

• Specially designed for the students preparing for IIT JEE (Main and Advanced), NEET, 11th and 12th Board Exams & Other Engineering or Medical Entrance Examinations by the team of experienced IITians faculties from KOTA.
• Easily Download and play (PC, Laptop: Windows Operating System)
• Course Language: Bilingual (Mix of both English &Hindi)
• No Internet connection required
• Long Term Validity

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PERIODIC TABLE 

Lecture#

Description

1. Dobereiner's triad, Newland’s octave law, lother meyer curve, Mendeleev's periodic table. Moseley's periodic table

2. Periodicity, blocks in periodic table, diagonal relationship, naming of element z > 100, Determination of period & block, Ionic radius

3. Covalent radius, vanderwaal radius, effective nuclear charge, shielding effect/screening effect, slater’s law

4. Factor affecting atomic radius. trend of atomic radius exception of atomic radius, lanthanide contraction.

5. Ionisation energy, Factors affective IE, Trend in I.E.

6. Exceptions in ionisation energy,Comparison of IE1 & IE2,Application of IE ionisation energy

7. Electron affinity, electron gain enthalpy, factor affecting electron affinity,

8. Second electron gain enthalpy,Electronegativity, Pauling scale, mulliken scale, Hanny smith of formula.

9. Nature of XOH-

   Acidic, basic, neutral and amphoteric oxide, Nature of oxide, Hydroxide and oxyacids, Inert pair effect 

Chemical Bonding

Lecture#

Description

1. Chemical bond, ionic bond, lattice energy, born haber cycle, Hess law

2. Properties of ionic compound, Hydration & Hydration energy. Solubility in water.

3. Factors affecting Hydration Energy, Solubility order, Covalent bond, Lewis concept.

4. Lewis structure, Exception of Lewis rule, Hypovalent, Hypervalent, odd electron species, coordinate bond formation, lewis acid & base.

5. Formal charge, Resonance

6. Valence bond theory (VBT) ,axial & Lateral overlapping,𝞂 bond, Π bond, 𝛅 bond

7. Hybridisation-sp, sp2, sp3, sp3d, sp3d2, sp3d3

8. Steric number rule for hybridisation, Valence shell electron pair repulsion theory VSEPR

9. Examples of sp & sp2 Hybridisation

10. Fullerenes, diamond, Compounds of phosphorus & sulphur.

11. Compounds of silicon,Silica, orthosilicate, pyrosilicate, chain silicate, cyclic silicate, double chain silicate

12. Silicons, equivalent and nonequivalent hybrid orbitals bent rule

13. Examples of sp3d, sp3d2 & sp3d3 Hybridisation, Drago’s rule.

14. Molecular orbital theory (MOT),  linear combination of atomic orbital (LCAO)

15. MOT examples , s-p mixing ,O2, F2, H2, N2, Ne2

16. HOMO & LUMO,GERADE & UNGERADE,Dipole moment & ionic character in ionic compound

17. Application of dipole moment % ionic character by dipole moment fazan, rule, covalent character in ionic compound

18. Application of fajan's rule, Banana bonding in diborane.

19. Back bonding in BF3 examples of back bonding

20. Bond angle comparison bond length & bond strength comparison.

21. p𝚷 - d𝚷 bonding, p𝚷 - p𝚷 bonding

22. Solubility due to hydrolysis of BF3, SiCl4, PCl3, compound, Interhalogen

23. Metallic bonding, H bonding, intermolecular H-bonding Intramolecular H bonding

24. Examples of h-bonding, van der waal forces( ion-dipole, dipole-dipole , ion-induced dipole, dipole induced dipole, london dispersion forces)

25. Factors affecting van der waal forces , existence and nonexistence of molecules

Boron & Carbon Family Group 13 & 14

Lecture#

Description

1. Member of boron family. Physical properties  (radius, oxidation state, ionisation energy, electronegativity, density) Chemical properties (reactivity with air) Anomalous behaviour of B Diagonal relationship between B & Si.

2. Formation of boron, compounds of boron, B3O3, boric acid, borax bead test.

3. Diborane, borazine,  boron nitride, back bonding in BF3.

4. Aluminium, Compounds, Al2O3, Al(OH)3, AlCl3 ,Carbon family, Inert Pair effect, order of ionisation energy, electronegativity, Atomic radius, Anomalous behaviour of carbon.

5. Allotropes of carbon, diamond, graphite, fullerene, reactivity with O2., H2O & X2.

6. Compound of carbon,Carbon monoxide,Carbon dioxide,Carbonic acid,Compounds of silicon,Silica.

7. Ortho silicate,Pyrosilicate ,Cyclic silicate,Chain silicate,Double chain silicate,Sheet silicate,3D silicate,Silicates,Compounds of tin & & Lead.

S-Block 

Lecture#

Description

1. Physical and chemical properties of alkali metal( ionisation energy, atomic radius , physical appearance, b.p. And m.p.)

2. Reaction of alkali metal with O2, h2O, halogen, carbon, reducing nature of alkali metal , solution in liquid ammonia, anomalous behaviour of lithium

3. Diagonal relationship between lithium and magnesium, compounds of sodium Na2O2, formation of NaOH

4. Properties of NaOH, , Na2CO3, sovay process , NaHCO3

5. Microcosmic salt, compounds of potassium, solution in liq. Ammonia 

6. Physical and chemical properties of alkaline earth metal( ionisation energy, atomic radius , physical appearance, b.p. And m.p.)

7. Hydride , hydroxide, oxide , nitride of alkaline earth metal

8. anomalous behaviour of berylium,Diagonal relationship between berylium and aluminium, compounds of Mg and Ca, gypsum and plaster of paris

Metallurgy

Lecture#

Description

1. Types of ore, Methods of metallurgy, crushing grinding, concentration, gravity separation, magnetic separation, froth floatation.

2. Leaching, calcination, roasting, flux, slag, reduction with carbon, carbon monoxide, self reduction. Electrolytic reduction is fused / aqueous solution.

3. Reduction with Al, Mg, H2, Thermal decomposition, metal displacement reduction, metallurgy of Aq & Au, Macarthur forrest cyanide method, copper extraction.

4. Extraction of Pb, Zn, Hg, Sn, Fe, Al, bayer methode, Hall, serpeck, Hall-Heroult method.

5. Extraction of Mg, Dow process, Extraction of sodium purification method Liquidation, Distillation Vapour phase refining, poling process, Mond process, Van Arkel method, Electrolytic refining.

6. Parting with Cl2, concentrated H2So4, Parke process, Thermodynamic of metallurgy Ellingham diagram.

Coordination Compound

Lecture#

Description

1. Simple salt, mixed salt, double salt, coordination compound, central atom, ligand, coordination number, oxidation number :-

2. Denticity, flexidentate, Ambidentate liquid

3. Coordination polyhedron, Naming of central atom, cationic ligand, neutral ligand, anionic ligand.

4. Naming of anionic ligand , rules for naming of complex salt, formula of complex , naming of complex having bridging ligand

5. Name of complex containing bridging ligand, reaction with AgNO3, reaction with BaCl2 electrical conductivity.

6. Reaction with conc. H2SO4, Werner’s theory, Sidgwick EAN rule.

7. Valence bond Theory (VBT)

8. Crystal field theory for octahedral complex.

9. Crystal field theory (octahedral complex Examples)

10. Crystal field theory (octahedral complex Examples), CFT for square planar complex, CFT for tetrahedral complex, structural isomerism, ionisation, hydrate, ligand , linkage, coordination isomerism.

11. Examples of tetrahedral complex, factors affecting crystal field splitting energy

12. Stereoisomerism, geometrical & optical isomerism.

13. Optical isomerism in octahedral complex & factors affecting splitting.

14. Properties of coordination compound stability, magnetic nature, colour, d-d transition.

15. Charge transfer in brown ring, sodium nitroprusside, back bonding in metal carbonyl, Delta bond, synergic bonding, bonded organometallic compound,ferrocene, zeise salt.

Nitrogen & oxygen family Group 15 & 16

Lecture#

Description

1. Physical properties of nitrogen family (atomic radius, Ionisation energy, Electronegativity, Oxidation state), Chemical properties (Hydride, Oxide, Halide)

2. Compounds of Nitrogen,N2, NH3, N2O, NO

3. Compounds of Nitrogen:-N2O3, N2O4, N2O5, HNO2, HNO3 allotropes of phosphorus (white, red, black)

4. Compounds of phosphorus, PH3, P4O6, P4O10, PCl3, PCl5

5. Physical properties of oxygen family (atomic radius, Ionisation energy, Electronegativity, Oxidation state), Chemical properties (Hydride, Oxide, Halide), dioxygen, types of oxid (acidic,basic,neutral,amphoteric,mixed oxide), ozone ,hydrogen peroxide

6. Allotropes of sulphur, H2S, SO2, SO3, Hypo solution Na2S2O3

Halogen Family & Noble Gas Family Group 17 & 18

Lecture#

Description

1. Properties of Halogen family members, Atomic radius,Ionisation,enthalpy,Electronegativity, Bond energy,Anomalous behaviour of fluorine

2. Properties of F2, Cl2, Br2, I2 Haloger acid HCl, HBr, HI

3. Properties of HF, CaOCl2, HOCl, HClO2, HClO3. Bleaching powder CaOCl2

4. HClO4, Interhalogen Compounds & their Hydrolysis, Pseudo halide, Pseudo Halogen Noble gas.

5. Properties (atomic radius, Mp, b.p. ionisation energy) of noble gas family Reaction with xenon with F2 & H2, addition compound, Hydrolysis reaction.

D Block Element

Lecture#

Description

1. Transition metal, general configuration atomic radius, ionization energy.

2. Density, melting point, oxidation state, standard electrode potential, colour, magnetic properties, nature of oxide, interstitial compound, catalytic properties, alloy formation.

3. Potassium dichromate, Potassium permanganate ,AgBr photography.

Qualitative Analysis

Lecture#

Description

1. Preliminary test, Dry Heating test, Flame test, Borax bead test, Charcoal cavity test. Cobalt nitrate test.

2. Group A anion, radial

3. s2-

4. starch / iodide test, Brown ring test, CH3 COO-

5. Iodometry test

6. Cl- , F- , Br- , I-

7. Nitrate,oxalate, borate ion

8. Group B anion Sulphate,phosphate,permanganate,chromate anion

9. Cation (basic radical) Zero group- Ist group- Pb+2

10. Ist group - Ag+ , Hg+2

11. II A group - IIA & IIB IIA - Cu+2 , Bi+3 , Pb+2 , Cd+2 , Hg+2

12. III group - Al+3 , Fe+3 , Cr+3 IV group - Mn+2

13. V group - Ba+2 , Sr+2 , Ca+2 VI group - Mg+2

MOLE CONCEPT 

Lecture#

Description

1. Dalton atomic theory, isotope ,isobar, atomic mass, atomic mass unit amu, molecule, molecular mass.

2. molar mass. Gram atomic mass, gram molecular mass, avogadro law.

3. Relative atomic mass, relative density, vapour density, specific gravity, average atomic mass, average molar mass.

4. Percentage composition, molecular formula, empirical formula, gay-lussac law.

5. Stoichiometry, mole-mole analysis, combustion of hydrocarbon.

6. limiting reagent, percentage yield , consecutive reaction

7. Principle of atomic conservation POAC.

8. Percentage purity of sample, combustion of carbon, analysis of mixture.

9. Numerical on analysis of mixture, law of mass conservation, law of definite proportions, law of  multiple proportions, law of reciprocal proportions .

10. Solution, solute , solvent, mole fraction, %w/w/,

11. %w/v, % v/v, strength of solution, molarity, molality, ppm.

12. Interconversion of concentration terms.

13. Molarity of pure water , volume strength of hydrogen peroxide solution, relation between volume strength and molarity.

14. Silver salt method , Eudiometry.

15. examples of eudiometry.

16. Significant figure, rules for counting , rounding off, scientific notation, addition/subtraction, multiplication of significant figure

Equivalent Concept

Lecture#

Description

1. Oxidation number calculation, average O.N. individual O. N.

2. Oxidizing agent, reducing agent, disproportion reactions

3. Balancing of redox and disproportion reaction , balancing of molecular reaction.

4. Equivalent concept. Law of chemical equivalence, relation between mole and equivalent, equivalent mass, valence factor calculation for acid & base.

5. n- factor for salt, n - factor for disproportion reaction.

6. Titration, acid base titration, permanganate titration, dichromate titration.

7. Back titration , double titration.

8. Numerical on double titration, iodometric titration, limitation of equivalent concept.

9. Bleaching powder and calculation of available chlorine from bleaching powder sample.

10. Hardne ss of water ( temporary & permanent hardness) strength of oleum

11. Volume strength of hydrogen peroxide solution.

Chemical Equilibrium

Lecture#

Description

1. 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.

2. Effect of stoichiometry on kp & Kc, examples of homogeneous equilibrium.

3. Numericals of homogeneous eq.

4. Heterogeneous eq., homogeneous liquid eq., significance of value of k, reaction quotie.

5. Approximation during calculation, relation between vapour density and degree of dissociation.

6. Thermodynamics for chemical eq, factor affecting composition of eq mixture , le-chatelier's principle, effect of concentration , effect of temperature.

7. Effect of change in pressure and volume , effect of catalyst.

8. 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.

9. Solubility of gas in liquid , allotropic change , simultaneous eq.

Ionic Equilibrium

Lecture#

Description

1. Strong electrolyte, weak electrolyte, strong acids, weak acids, strong base, weak base , acid base theory, arrhenius concept, bronsted lowry concept , amphiprotic species.

2. Lewis concept , pH scale, properties of water, ionisation constant of water, ionic product of water.

3. pH calculation for strong acid, strong base, mixture of strong acid , mixture of strong acid and base ,common ion effect.

4. pH for monobasic weak acid, weak base, ostwald dilution law, pH for very dilute strong acid.

5. Very dilute weak base , mixture of weak acid and strong acid,polyprotic weak acid.

6. Numerical on polyprotic weak acid, mixture of two weak acids.

7. Hydrolysis of salt, salt of strong acid and strong base, salt of weak acid and strong base , salt of weak base and strong acid.

8. Hydrolysis of salt of weak acid and weak base.

9. pH for polyvalent anion, ph for amphiprotic anion , introduction of buffer solution.

10. Acidic buffer and basic buffer.

11. Buffer capacity, titration ( strong acid v/s strong base, strong acid v/s weak base , weak acid v/s strong base).

12. Titration of H3PO4 v/s NaOH.

13. Indicator, phenolphthalein, methyl orange, pH range for a buffer ,double titration.

14. Solubility of sparingly soluble salt, Ksp, effect of common ion on solubility, simultaneous solubility.

15. Ionic product v/s solubility product,selective precipitation,

16. solubility of salt in buffer solution, complex formation by salt.

17. Solubility of amphoteric insoluble hydroxide, solubility of salt if cation is hydrolyzed , solubility of salt if anion is hydrolyzed  

Thermodynamics & Thermochemistry

Lecture#

Description

1. 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.

2. Reversible and irreversible process, reversible isothermal compression, single step isothermal compression, two stage isothermal compression.

3. Reversible isothermal expansion, single stage isothermal expansion, two stage isothermal expansion, internal energy, degree of freedom, first law of thermodynamics.

4. Enthalpy change , phase transformation.

5. Free expansion, reversible adiabatic process, work calculation for reversible Adiabatic and irreversible  Adiabatic processes.

6. comparison between reversible adiabatic and irreversible adiabatic processes, comparison between reversible adiabatic and reversible isothermal processes.

7. Spontaneous and nonspontaneous process, entropy, second law of thermodynamics , entropy change for system and surrounding.

8. Numerical on entropy change , entropy change during free expansion.

9. Gibbs energy change, heat pump, carnot cycle.

10. Thermochemistry, enthalpy of formation, enthalpy of combustion.

11. Enthalpy of fusion, vaporization,sublimation,bomb calorimeter, enthalpy of neutralisation, enthalpy of ionisation.

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.

Gaseous State

Lecture#

Description

1. State of matter (solid, Liq, gas) ideal gas equation, Boyle’s law.  

2. Barometer, faulty Barometer

3. Problems on barometer, Charles law  

4. Gay-lussac’s law, Avogadro's law, ideal gas equation  

5. Numerical  

6. Graham’s law for diffusion.  

7. Kinetic theory of gas, root mean square velocity  

8. Compressibility factor (Z) pressure correction factor, volume correction factor, excluded volume, van der waal gas equation  

9. Virial equation, liquification of gas, critical temperature (Tc) Critical pressure (Pc) Critical volume (Vc) Boyle’s temperature  

10. Liquification of gas manometer (Open end, Closed end, reduced equation of state), Collision diameter, Collision frequency

                                                      

Atomic Structure

Lecture#

Description

1. Cathode tube experiment anode rays, radioactive decay.

2. Thomson plum pudding model. Rutherford model, Nearest distance of approach.

3. Electromagnetic theory, Planck Quantum Theory, Blackbody radiation, electron volt.

4. Photoelectric effect, Work function, Threshold frequency stopping potential.

5. Photo current photo intensity, Bohr model, Bohr Radius.

6. Velocity, Kinetic Energy, Total energy, Potential energy of electron in Bohr orbit.

7. Time period, frequency, ionisation energy, ionisation potential, Excitation energy, excitation potential Binding energy.

8. Spectrum, emission, line spectrum, band spectrum , H-spectrum, lyman series.

9. Balmer series, Paschen, Brackett, Pfund, humphrey series, maximum number of spectral lines.

10. Limitations of bohr model, dual nature of particle, de broglie's equation.

11. Heisenberg’s uncertainty principle Difference between orbit & orbital.

12. Types of orbitals {s, p, d, f}, quantum numbers, (principal, azimuthal, magnetic, spin)

13. Electron filling rule, Aufbau principle, Hund’s rule, pauli’s exclusion principle, magnetic nature, magnetic moment.

14. Wave quantum theory, schrodinger wave equation, radial node, angular node.

Solution & Colligative Properties

Lecture#

Description

1. Introduction Different concentration terms interconversion, colligative properties, van’t hoff factor calculation, osmotic pressure.

2. Osmosis , Osmotic pressure (different cases)

3. Numericals on osmotic pressure.

4. Vapour pressure, relative lowering of vapour pressure,

5. Numericals on RLVP, Ostwald walker method

6. Elevation in boiling point, calculation of Kb (molal elevation boiling point constant) . Depression in freezing point, Calculation of Kf,

7. Numericals on elevation in boiling point and depression in freezing point.

8. Thermodynamic explanation of 𝝙Tb & 𝝙Tf

9. Raoult’s law when two volatile liquids are mixed.

10. Ideal and nonideal solution.

11. Azeotropes, mixture of two immiscible liquids, solubility of gas in liquid, henry law

Solid State

Lecture#

Description

1. Types of solid, Crystal, Amorphous, unit cell, 2D, 3D, space,lattice.

2. Primitive, body centred, face centered contribution of atoms in cubic unit cell. Packing fraction of square packing and hexagonal packing.

3. Coordination Number, packing fraction, density of solid.,Simple cubic, BCC, FCC, CCP.

4. Closed packing in 3D HCP packing,Linear void, Triangular void, Tetrahedral void, octahedral void, Cubical void Types of void in FCC.

5. Voids in FCC,Different radius ratio for ionic compounds.

6. Calculation of nearest, next nearest and next to next nearest atoms in SC, BCC, FCC.

7. Structure of NaCl type, Zns type, CaF2 type, Na2O type, CSCl type, Diamond.

8. Spinal structure, perovskite corundum structure, packing fraction of NaCl, Defect In crystal, Schottky,Frenkel, Interstitial.

9. Non stoichiometric defect, cation excess defect cation deficiency defect, Paramagnetic, Diamagnetic Ferromagnetic, Ferrimagnetic, Antiferromagnetic compound  

Chemical Kinetics

Lecture#

Description

1. Fast reaction , slow reaction, moderate reaction, average rate of reaction, instantaneous rate of reaction,relation of rate of reaction between various reagents , order

2. Order law, zero order reaction.

3. First order reaction.

4. Half life period for first order reaction.

5. Average life period for first order, generation time , first order bacterial growth, second order reaction 06nth order reaction, pseudo first order reaction.

6. Rate of reaction of two or reactant are taken, calculation of order by half life method.

7. Initial rate method , integrated rate law, ostwald isolation method to determine order.

8. Monitoring of first order reaction using pressure measurement.

9. Monitoring of first order reaction using titration and optical rotation.

10. Arrhenius transition state theory.

11. Arrhenius equation.

12. Effect of catalyst on rate constant, temperature coefficient for reaction.

13. Simple and complex reaction, molecularity, rate determining step RDS.

14. Determination of rate if RDS is given , steady state approximation,complexity in first order reaction, parallel first order reactions.

15. Reversible first order reaction.

16. Consecutive first order reaction

Radioactivity

Lecture#

Description

• Cause of radioactivity belt of stability , comparison between alpha particle, beta particle and gamma rays.

• Group displacement law soddy fajan rule,, k– electron capture ,first order decay.

• Radioactive decay.

• Carbon dating, Age of rock using U & Pb,Age of rock using U & He.

• Mass defect ,Binding energy, Binding energy per nucleon. Nuclear fission and fusion.

Surface Chemistry

Lecture#

Description

1. Adsorption, Adsorbate, Adsorbent, Thermodynamics of Adsorption, Adsorption v/s Absorption, Physical Adsorption.

2. 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.

3. Types of colloidal solution, Lyophobic, Lyophilic, macromolecular, micromolecular, Associated colloid/ micelle, cleansing action of soap, Bredig’s arc method,Peptization.

4. Chemical method to prepare colloidal solution, Tyndall effect, Brownian motion, Electrophoresis, coagulation, protection of colloid.

5. Gold number, Helmholtz double layer theory ,emulsion.

Electrochemistry

Lecture#

Description

1. Electrochemical cell, Oxidation half cell, Reduction half cell, Galvanic cell.

2. Salt bridge, Daniel cell net cell reaction reaction Quotient cell representation relation between DG & E properties of DG & E,nernst equation.

3. Spontaneity of reaction in cell, nernst equation cell at equilibrium, concentration cell. Hydrogen electrode and standard hydrogen electrode.

4. Metal + insoluble salt + soluble anion type half cell Eg.   Ag + AgCl + Cl–

5. Calomel electrode, electrochemical series, thermodynamics for electrochemical cell, 𝝙G, 𝝙H, 𝝙S

6. Electrolysis & electrolytic cell, electrolysis of nacl, nabr, H2SO4,H2O, first law of electrolysis Faraday law.

7. Examples of first law of faraday, second law of faraday.

8. Primary cell ,leclanche cell, secondary cell, lead storage battery , Ni-Cd cell , H2-O2 fuel cell, electrolytic conduction.

9. 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.

10. Ionic mobility, conductometric titration for strong acid V/s strong base , strong acid v/s weak base and other examples