NEET CHEMISTRY
MASTER FORMULA & REACTION BOOK
Physical Chemistry • Organic Chemistry • Inorganic Chemistry
SCORING USE:
Memorise the formula → understand what each symbol means → solve a NEET-style question immediately. For
Organic/Inorganic, revise reactions, trends and exceptions repeatedly.
Coverage: Mole Concept • Atomic Structure • Solutions • Thermodynamics • Equilibrium • Electrochemistry • Kinetics • Solid State •
Coordination • Periodic Trends • p-block • d/f-block • Metallurgy • GOC • Hydrocarbons • Haloalkanes • Alcohols • Carbonyls • Amines •
Biomolecules & more
NEET Chemistry • Formula & Reaction Revision Page 1
, PART A — PHYSICAL CHEMISTRY
1. Mole Concept & Stoichiometry
• Number of moles: n = given mass / molar mass.
• Number of particles: N = nNA.
• Gas at STP (use the value specified in the question): 1 mol ideal gas ≈ 22.4 L at 273 K, 1 atm.
• Molarity M = moles of solute / volume of solution in L.
• Molality m = moles of solute / mass of solvent in kg.
• Mole fraction xi = ni/Σn.
• Mass % = (mass of solute / mass of solution) × 100.
• Empirical formula: divide all mole values by the smallest; multiply to obtain whole-number ratios.
• Limiting reagent: compare available moles with stoichiometric requirement.
2. Atomic Structure
• E = hν = hc/λ.
• Photon momentum p = h/λ.
• de Broglie: λ = h/mv.
• Bohr: mvr = nh/(2π).
• Hydrogen-like energy: E = −13.6Z²/n² eV.
n
• Radius: r = 0.529(n²/Z) Å.
n
• Rydberg: 1/λ = RZ²(1/n ² − 1/n ²), n > n .
1 2 2 1
• Maximum electrons in shell n = 2n²; orbitals in shell = n²; electrons per orbital = 2.
3. States of Matter / Gas Laws
• Boyle: PV = constant at constant T.
• Charles: V/T = constant at constant P.
• Avogadro: V/n = constant.
• Ideal gas: PV = nRT.
• Density d = PM/RT.
• Dalton: Ptotal = ΣPi; Pi = xiPtotal.
• RMS speed urms = √(3RT/M).
• Average kinetic energy per molecule = 3RT/(2NA) = 3kT/2.
4. Thermodynamics
• First law: ∆U = q + w (chemistry convention; w is work done on system).
• Expansion work: w = −Pext∆V.
• At constant volume: qv = ∆U.
• At constant pressure: qp = ∆H.
• ∆H = ∆U + ∆ngRT.
• Hess law: total enthalpy change = sum of enthalpy changes of steps.
• ∆G = ∆H − T∆S.
• Spontaneous at given T,P: ∆G < 0; equilibrium: ∆G = 0.
• ∆G° = −RT ln K = −2.303RT log K.
5. Chemical Equilibrium
• Kc = product concentrations / reactant concentrations, each raised to stoichiometric coefficient.
NEET Chemistry • Formula & Reaction Revision Page 2
MASTER FORMULA & REACTION BOOK
Physical Chemistry • Organic Chemistry • Inorganic Chemistry
SCORING USE:
Memorise the formula → understand what each symbol means → solve a NEET-style question immediately. For
Organic/Inorganic, revise reactions, trends and exceptions repeatedly.
Coverage: Mole Concept • Atomic Structure • Solutions • Thermodynamics • Equilibrium • Electrochemistry • Kinetics • Solid State •
Coordination • Periodic Trends • p-block • d/f-block • Metallurgy • GOC • Hydrocarbons • Haloalkanes • Alcohols • Carbonyls • Amines •
Biomolecules & more
NEET Chemistry • Formula & Reaction Revision Page 1
, PART A — PHYSICAL CHEMISTRY
1. Mole Concept & Stoichiometry
• Number of moles: n = given mass / molar mass.
• Number of particles: N = nNA.
• Gas at STP (use the value specified in the question): 1 mol ideal gas ≈ 22.4 L at 273 K, 1 atm.
• Molarity M = moles of solute / volume of solution in L.
• Molality m = moles of solute / mass of solvent in kg.
• Mole fraction xi = ni/Σn.
• Mass % = (mass of solute / mass of solution) × 100.
• Empirical formula: divide all mole values by the smallest; multiply to obtain whole-number ratios.
• Limiting reagent: compare available moles with stoichiometric requirement.
2. Atomic Structure
• E = hν = hc/λ.
• Photon momentum p = h/λ.
• de Broglie: λ = h/mv.
• Bohr: mvr = nh/(2π).
• Hydrogen-like energy: E = −13.6Z²/n² eV.
n
• Radius: r = 0.529(n²/Z) Å.
n
• Rydberg: 1/λ = RZ²(1/n ² − 1/n ²), n > n .
1 2 2 1
• Maximum electrons in shell n = 2n²; orbitals in shell = n²; electrons per orbital = 2.
3. States of Matter / Gas Laws
• Boyle: PV = constant at constant T.
• Charles: V/T = constant at constant P.
• Avogadro: V/n = constant.
• Ideal gas: PV = nRT.
• Density d = PM/RT.
• Dalton: Ptotal = ΣPi; Pi = xiPtotal.
• RMS speed urms = √(3RT/M).
• Average kinetic energy per molecule = 3RT/(2NA) = 3kT/2.
4. Thermodynamics
• First law: ∆U = q + w (chemistry convention; w is work done on system).
• Expansion work: w = −Pext∆V.
• At constant volume: qv = ∆U.
• At constant pressure: qp = ∆H.
• ∆H = ∆U + ∆ngRT.
• Hess law: total enthalpy change = sum of enthalpy changes of steps.
• ∆G = ∆H − T∆S.
• Spontaneous at given T,P: ∆G < 0; equilibrium: ∆G = 0.
• ∆G° = −RT ln K = −2.303RT log K.
5. Chemical Equilibrium
• Kc = product concentrations / reactant concentrations, each raised to stoichiometric coefficient.
NEET Chemistry • Formula & Reaction Revision Page 2
