Chemistry for IMU-CET 2026: Complete Preparation Guide

Chemistry in IMU-CET carries 25 marks and is often considered tricky due to its breadth. However, with focused preparation on high-weightage topics, you can easily score 20+ marks. This guide covers the complete strategy.

Chemistry Section Overview

Exam Pattern

Aspect	Detail
Total Questions	25
Marks per Question	1
Negative Marking	-0.25 per wrong answer
Time Allocation	15-20 minutes
Difficulty Level	Class 11-12 CBSE

Topic-wise Distribution

Topic	Expected Questions	Weightage
Organic Chemistry	8-10	32-40%
Physical Chemistry	8-10	32-40%
Inorganic Chemistry	5-8	20-32%

Physical Chemistry

1. Atomic Structure

Key Concepts:

• Bohr’s model
• Quantum numbers
• Electronic configuration
• Periodic properties

Quantum Numbers:

Symbol	Name	Values
n	Principal	1, 2, 3…
l	Azimuthal	0 to (n-1)
m	Magnetic	-l to +l
s	Spin	+½ or -½

Electronic Configuration Rules:

1. Aufbau principle: Fill lowest energy first
2. Pauli exclusion: Max 2 electrons per orbital
3. Hund’s rule: Maximum multiplicity

2. Chemical Bonding

Types of Bonds:

Bond Type	Examples	Properties
Ionic	NaCl, KBr	High MP, conducts in solution
Covalent	H₂O, CH₄	Low MP, poor conductor
Metallic	Fe, Cu	Malleable, conducts
Hydrogen	H₂O molecules	Affects BP, MP

VSEPR Theory:

Electron Pairs	Shape	Example
2	Linear	BeCl₂
3	Trigonal planar	BF₃
4	Tetrahedral	CH₄
5	Trigonal bipyramidal	PCl₅
6	Octahedral	SF₆

Hybridization:

Hybridization	Geometry	Bond Angle
sp	Linear	180°
sp²	Trigonal planar	120°
sp³	Tetrahedral	109.5°
sp³d	Trigonal bipyramidal	90°, 120°
sp³d²	Octahedral	90°

3. Chemical Equilibrium

Key Formulas:

Concept	Formula
Equilibrium Constant (Kc)	[Products]/[Reactants]
Relationship	Kp = Kc(RT)^Δn
Degree of dissociation	α = √(Kc/C) for weak acids

Le Chatelier’s Principle:

Change	System Response
Increase concentration	Shifts away
Increase pressure	Shifts to fewer moles
Increase temperature	Shifts toward endothermic

4. Chemical Kinetics

Rate Laws:

Order	Rate Law	Half-life
Zero	Rate = k	t½ = [A]₀/2k
First	Rate = k[A]	t½ = 0.693/k
Second	Rate = k[A]²	t½ = 1/k[A]₀

Arrhenius Equation: k = Ae^(-Ea/RT)

ln(k₂/k₁) = (Ea/R)(1/T₁ - 1/T₂)

5. Thermodynamics

Important Equations:

Law/Concept	Equation
First Law	ΔU = q + w
Enthalpy	ΔH = ΔU + PΔV
Hess’s Law	ΔH = ΣΔH(products) - ΣΔH(reactants)
Gibbs Energy	ΔG = ΔH - TΔS

Spontaneity Criteria:

ΔH	ΔS	ΔG	Spontaneity
-	+	-	Always
+	-	+	Never
-	-	Depends	Low T
+	+	Depends	High T

6. Electrochemistry

Key Equations:

Concept	Formula
Nernst Equation	E = E° - (0.059/n)log Q
Faraday’s Laws	m = (M × I × t)/(n × F)
Cell EMF	E°cell = E°cathode - E°anode

Electrochemical Series (Important): Li > K > Na > Mg > Al > Zn > Fe > Ni > Sn > H > Cu > Ag > Au

7. Solutions

Colligative Properties:

Property	Formula
Relative lowering of VP	(P° - P)/P° = n₂/n₁
Elevation in BP	ΔTb = Kb × m
Depression in FP	ΔTf = Kf × m
Osmotic Pressure	π = CRT

Molarity vs Molality:

Measure	Formula
Molarity (M)	moles/liters of solution
Molality (m)	moles/kg of solvent
Mole fraction	n₁/(n₁ + n₂)

Organic Chemistry

1. Basic Concepts

IUPAC Nomenclature:

Functional Group	Suffix
Alkane	-ane
Alkene	-ene
Alkyne	-yne
Alcohol	-ol
Aldehyde	-al
Ketone	-one
Carboxylic acid	-oic acid
Amine	-amine

Isomerism:

Type	Definition
Structural	Different connectivity
Geometrical	cis-trans about double bond
Optical	Mirror images (enantiomers)
Conformational	Rotation about single bond

2. Hydrocarbons

Alkanes:

• General formula: CₙH₂ₙ₊₂
• Reactions: Substitution (halogenation), combustion

Alkenes:

• General formula: CₙH₂ₙ
• Reactions: Addition (Markovnikov’s rule)

Alkynes:

• General formula: CₙH₂ₙ₋₂
• Reactions: Addition, acidic hydrogen reactions

Markovnikov’s Rule: In addition reactions, H adds to C with more H atoms.

Anti-Markovnikov (Peroxide Effect): HBr with peroxide gives opposite addition.

3. Alcohols and Ethers

Alcohol Reactions:

Reaction	Product
Oxidation (1°)	Aldehyde → Acid
Oxidation (2°)	Ketone
Oxidation (3°)	No reaction (ordinary)
Dehydration	Alkene
With Na	Alkoxide + H₂

Acidity Order: CH₃OH > 1° > 2° > 3° alcohol

4. Aldehydes and Ketones

Important Reactions:

Reaction	Reagent	Product
Reduction	NaBH₄, LiAlH₄	Alcohol
Oxidation	KMnO₄, K₂Cr₂O₇	Acid (aldehyde only)
Aldol condensation	Base	β-hydroxy aldehyde
Cannizzaro	Conc. NaOH	Acid + Alcohol

Tests:

Test	Positive For
Tollen’s (Silver mirror)	Aldehydes
Fehling’s (Red ppt)	Aldehydes
Iodoform	CH₃CO- group

5. Carboxylic Acids

Reactions:

Reaction	Product
With alcohol	Ester
With PCl₅	Acyl chloride
With NH₃	Amide
Reduction (LiAlH₄)	Alcohol

Acidity Order: HCOOH > CH₃COOH > C₂H₅COOH

Electron-withdrawing groups increase acidity.

6. Amines

Classification:

• Primary (1°): R-NH₂
• Secondary (2°): R₂NH
• Tertiary (3°): R₃N

Basicity Order: R₂NH > RNH₂ > R₃N > NH₃

Important Reactions:

• Diazotization (1° aromatic amines)
• Carbylamine test (1° amines)
• Hinsberg test (distinguish 1°, 2°, 3°)

Inorganic Chemistry

1. Periodic Table

Periodic Trends:

Property	Across Period	Down Group
Atomic radius	Decreases	Increases
Ionization energy	Increases	Decreases
Electronegativity	Increases	Decreases
Metallic character	Decreases	Increases

2. s-Block Elements

Alkali Metals (Group 1):

• Reactivity increases down group
• Form ionic compounds
• Strong reducing agents

Alkaline Earth Metals (Group 2):

• Less reactive than Group 1
• Form stable compounds
• Important: Ca, Mg compounds

3. p-Block Elements

Group 15 (Nitrogen Family):

Property	N	P	As	Sb	Bi
Oxidation states	-3 to +5	-3 to +5	-3 to +5	-3 to +5	+3, +5

Group 16 (Oxygen Family):

• Oxygen: Strong oxidizer
• Sulfur: Allotropy, acids

Group 17 (Halogens):

• Reactivity: F > Cl > Br > I
• Oxidizing power decreases down

4. d-Block Elements

General Properties:

• Variable oxidation states
• Form colored compounds
• Catalytic activity
• Form complex compounds

Important Compounds:

Compound	Formula	Use
Potassium dichromate	K₂Cr₂O₇	Oxidizing agent
Potassium permanganate	KMnO₄	Oxidizing agent
Copper sulfate	CuSO₄	Blue vitriol

5. Coordination Compounds

Terminology:

Term	Definition
Ligand	Ion/molecule bonded to central metal
Coordination number	Number of ligand bonds
Denticity	Number of donor atoms in ligand

Common Ligands:

Ligand	Denticity	Examples
Monodentate	1	H₂O, NH₃, Cl⁻
Bidentate	2	Ethylenediamine, oxalate
Polydentate	>2	EDTA (6)

Preparation Strategy

3-Month Plan

Month 1: Physical Chemistry

Week	Topics
Week 1	Atomic structure, Bonding
Week 2	Thermodynamics, Equilibrium
Week 3	Kinetics, Electrochemistry
Week 4	Solutions, Practice

Month 2: Organic Chemistry

Week	Topics
Week 1	Basic concepts, Hydrocarbons
Week 2	Alcohols, Aldehydes, Ketones
Week 3	Acids, Amines
Week 4	Reactions practice

Month 3: Inorganic + Revision

Week	Topics
Week 1	Periodic table, s-block
Week 2	p-block, d-block
Week 3	Coordination compounds
Week 4	Full revision, Mock tests

High-Yield Topics

Priority	Topics
Very High	Organic reactions, Equilibrium
High	Electrochemistry, Coordination
Medium	Thermodynamics, Kinetics
Lower	Inorganic details

Common Mistakes

Organic Chemistry

Mistake	Correct Approach
Wrong mechanism	Identify reaction type first
Nomenclature errors	Follow IUPAC rules systematically
Missing stereochemistry	Consider 3D structure

Physical Chemistry

Mistake	Correct Approach
Unit conversion	Always convert to SI
Sign convention	Follow thermodynamic signs
Equilibrium direction	Apply Le Chatelier correctly

Exam Tips

Time Management

Section	Questions	Time
Organic	8-10	8 minutes
Physical	8-10	8 minutes
Inorganic	5-8	4 minutes

Answering Strategy

1. Start with familiar topics
2. Organic reactions - identify patterns
3. Physical chemistry - apply formulas
4. Inorganic - recall facts

Quick Revision Points

Must-Remember Reactions

1. Aldol condensation
2. Cannizzaro reaction
3. Friedel-Crafts reaction
4. Grignard synthesis
5. Diazotization

Must-Remember Formulas

1. Nernst equation
2. Rate laws
3. Gibbs free energy
4. Colligative properties
5. pH calculations

Conclusion

Chemistry in IMU-CET rewards focused preparation. Prioritize organic reactions and physical chemistry calculations. Inorganic chemistry requires memorization but carries fewer marks.

With 2-3 hours daily for 3 months, scoring 20+ marks is achievable.

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