NEET (UG) 2026–27
Chemistry — Volume 4
Full Revision • Formula & Reaction Maps • Original MCQs • Mock Practice
Note: This volume is an original revision/practice resource aligned to recurring NEET Chemistry concepts. It does not
reproduce NCERT or copyrighted question-bank text.
,Physical Chemistry — Rapid Revision
• Mole concept: n = m/M = N/NA; molarity = moles of solute/L solution; molality = moles/kg solvent.
• Thermodynamics: ∆G = ∆H − T∆S; spontaneous at constant T,P when ∆G < 0. Hess law allows enthalpy changes to be
added algebraically.
• Equilibrium: K relates equilibrium concentrations/activities. Le Chatelier: a system responds to a disturbance in a way that
opposes it.
• Electrochemistry: Ecell = Ecathode − Eanode; ∆G = −nFE. Oxidation at anode, reduction at cathode.
• Kinetics: rate law determines reaction order; for first order, t1/2 = 0.693/k and ln([A]0/[A]) = kt.
• Solutions: Raoult-type relations connect vapour pressure with mole fraction; colligative properties depend on number of
solute particles.
Inorganic Chemistry — High-Yield Map
• Periodic trends: atomic radius generally decreases across a period and increases down a group; ionisation enthalpy
generally shows the reverse trend with known exceptions.
• Chemical bonding: VSEPR predicts molecular geometry from electron-pair repulsions; hybridisation is a useful bonding
model.
• Coordination chemistry: coordination number counts directly attached donor atoms; ligand denticity counts donor sites used
by a ligand.
• Redox: oxidation is loss of electrons/increase in oxidation number; reduction is gain of electrons/decrease in oxidation
number.
• p-block and d/f-block questions often test oxidation states, trends, colours, magnetic behaviour and characteristic
compounds.
Organic Chemistry — Reaction Map
• Core tools: inductive effect, resonance, hyperconjugation and steric effects help explain stability and reactivity.
• Hydrocarbons: electrophilic addition is central for many alkenes/alkynes; aromatic substitution preserves aromaticity.
• Alcohols/phenols/ethers: compare acidity, substitution and oxidation using structure and reaction conditions.
• Carbonyls: aldehydes and ketones undergo nucleophilic addition; carboxylic acids show characteristic acidity and derivative
chemistry.
• Amines: basicity depends on electron density, solvation and structural environment; diazonium chemistry is high-yield.
• Biomolecules: distinguish carbohydrates, amino acids/proteins, nucleic acids and vitamins by structure and function.
, Formula & Reaction Checklist
Topic Must-remember
Mole n=m/M; N=nNA
Gas equation PV=nRT
Thermodynamics ∆G=∆H−T∆S
Electrochemistry ∆G=−nFE
First-order kinetics t1/2=0.693/k
pH pH=−log[H+]
Ideal solution Raoult-type vapour-pressure relation
Organic oxidation Primary alcohol → aldehyde → acid
Carbonyl Aldehyde/ketone + nucleophile → addition product
Amines Basicity depends on electron density + solvation + structure
Chemistry — Volume 4
Full Revision • Formula & Reaction Maps • Original MCQs • Mock Practice
Note: This volume is an original revision/practice resource aligned to recurring NEET Chemistry concepts. It does not
reproduce NCERT or copyrighted question-bank text.
,Physical Chemistry — Rapid Revision
• Mole concept: n = m/M = N/NA; molarity = moles of solute/L solution; molality = moles/kg solvent.
• Thermodynamics: ∆G = ∆H − T∆S; spontaneous at constant T,P when ∆G < 0. Hess law allows enthalpy changes to be
added algebraically.
• Equilibrium: K relates equilibrium concentrations/activities. Le Chatelier: a system responds to a disturbance in a way that
opposes it.
• Electrochemistry: Ecell = Ecathode − Eanode; ∆G = −nFE. Oxidation at anode, reduction at cathode.
• Kinetics: rate law determines reaction order; for first order, t1/2 = 0.693/k and ln([A]0/[A]) = kt.
• Solutions: Raoult-type relations connect vapour pressure with mole fraction; colligative properties depend on number of
solute particles.
Inorganic Chemistry — High-Yield Map
• Periodic trends: atomic radius generally decreases across a period and increases down a group; ionisation enthalpy
generally shows the reverse trend with known exceptions.
• Chemical bonding: VSEPR predicts molecular geometry from electron-pair repulsions; hybridisation is a useful bonding
model.
• Coordination chemistry: coordination number counts directly attached donor atoms; ligand denticity counts donor sites used
by a ligand.
• Redox: oxidation is loss of electrons/increase in oxidation number; reduction is gain of electrons/decrease in oxidation
number.
• p-block and d/f-block questions often test oxidation states, trends, colours, magnetic behaviour and characteristic
compounds.
Organic Chemistry — Reaction Map
• Core tools: inductive effect, resonance, hyperconjugation and steric effects help explain stability and reactivity.
• Hydrocarbons: electrophilic addition is central for many alkenes/alkynes; aromatic substitution preserves aromaticity.
• Alcohols/phenols/ethers: compare acidity, substitution and oxidation using structure and reaction conditions.
• Carbonyls: aldehydes and ketones undergo nucleophilic addition; carboxylic acids show characteristic acidity and derivative
chemistry.
• Amines: basicity depends on electron density, solvation and structural environment; diazonium chemistry is high-yield.
• Biomolecules: distinguish carbohydrates, amino acids/proteins, nucleic acids and vitamins by structure and function.
, Formula & Reaction Checklist
Topic Must-remember
Mole n=m/M; N=nNA
Gas equation PV=nRT
Thermodynamics ∆G=∆H−T∆S
Electrochemistry ∆G=−nFE
First-order kinetics t1/2=0.693/k
pH pH=−log[H+]
Ideal solution Raoult-type vapour-pressure relation
Organic oxidation Primary alcohol → aldehyde → acid
Carbonyl Aldehyde/ketone + nucleophile → addition product
Amines Basicity depends on electron density + solvation + structure
