JEE Main Chemistry Formula Sheet 2026: Chapter-wise PDF & Revision Notes

The JEE Main Chemistry Formula Sheet 2026 is a complete and easy-to-use study resource created to help students revise Chemistry quickly and effectively. Chemistry is one of the most scoring subjects in JEE Main, and with the right jee mains chemistry formula sheet, students can save time and improve accuracy in the exam. This chapter-wise PDF includes all important formulas, reactions, and key points from Physical, Organic, and Inorganic Chemistry, strictly based on the latest JEE Main syllabus. It works as a one-stop chemistry jee formula sheet for regular revision and last-minute preparation.

In Physical Chemistry, formulas play a major role in solving numerical questions. This jee chemistry formula sheet covers all essential equations from topics like mole concept, atomic structure, thermodynamics, equilibrium, electrochemistry, solutions, and chemical kinetics. Having a well-organized jee mains formula sheet helps students revise faster and practice questions with confidence. Many students prefer a jee mains chemistry all formulas pdf download so they can revise anytime, anywhere.

For Organic Chemistry, the formula sheet focuses on important reactions, reagents, name reactions, mechanisms, and stability orders. Chapters such as GOC, hydrocarbons, alcohols, carbonyl compounds, amines, and biomolecules are explained in a simple format. This jee main chemistry formula sheet helps students remember reactions easily and reduces confusion during exams.

In Inorganic Chemistry, the chemistry formula sheet jee highlights important trends, reactions, exceptions, and factual points from chapters like the periodic table, p-block, d- and f-block elements, and coordination compounds. Since Inorganic Chemistry depends a lot on memory, short revision notes are very useful.

Overall, this jee formula sheet is perfect for daily revision, mock test preparation, and final revision before JEE Main 2026, helping students boost confidence and score better in Chemistry.

JEE Main 2026 Chemistry Syllabus

The JEE Main 2026 Chemistry syllabus covers three main parts: Physical, Organic, and Inorganic Chemistry. 

• Physical Chemistry mostly includes numerical problems and formulas, with important topics like mole concept, atomic structure, thermodynamics, equilibrium, electrochemistry, and chemical kinetics.
• Organic Chemistry focuses on reactions, mechanisms, reagents, and functional groups, including chapters such as GOC, hydrocarbons, alcohols, carbonyl compounds, amines, and biomolecules.
• Inorganic Chemistry is mainly theory-based and requires learning facts, trends, and properties from topics like the periodic table, p-block, d- and f-block elements, and coordination compounds. 

To do well in JEE Main 2026 Chemistry, students should clearly understand concepts, practice regularly, and revise NCERT-based points and formulas often.

Physical Chemistry Syllabus for JEE Mains

Physical Chemistry usually gives good scoring chances if your formulas and calculation practice are strong. Commonly important chapters include: Stoichiometry, Atomic Structure, Thermodynamics, Equilibrium, Kinetics, and Electrochemistry.

Practical tip: For Physical Chemistry, keep a formula sheet and solve mixed numericals daily.

Organic Chemistry Syllabus for JEE Mains

Organic Chemistry is mostly about understanding how reactions happen (mechanism), which reagent does what, and how functional groups behave. Frequently important chapters include: Hydrocarbons, Haloalkanes & Haloarenes, Alcohols/Phenols/Ethers, Carbonyls & Acids, Amines, and Biomolecules.

Practical tip: Organic becomes easy when you make a “reaction map” (reagent → change → product) and revise it often.

Inorganic Chemistry Syllabus for JEE Mains

Inorganic Chemistry is mainly about the periodic table, trends, key properties, and standard reactions. High-value areas usually include P-block, d- & f-block, Coordination compounds, and periodic trends.

Practical tip: For Inorganic, revise from short notes + NCERT-style points, and do frequent quick tests.

Download JEE Main 2026 Chemistry Formulas

Download the JEE Main 2026 Chemistry Formulas PDF to get a clear, chapter-wise collection of the most important formulas and reactions from Physical, Organic, and Inorganic Chemistry. This concise formula sheet is designed for quick revision, helping you save time while covering high-weightage topics as per the latest NTA syllabus. Ideal for last-minute practice and daily revision, it simplifies complex concepts and boosts confidence before the exam.

Download Most Important Chemistry Formulas for JEE Main PDF

Chapter Wise Most Important Chemistry Formuals for JEE Mains 2026

Chapter-wise most important Chemistry formulas for JEE Main 2026 are designed to help students revise efficiently and focus on high-scoring concepts. This collection covers all key formulas from Physical, Organic, and Inorganic Chemistry, arranged topic-wise as per the latest NTA syllabus. It is especially useful for quick revision before exams, strengthening numerical problem-solving in Physical Chemistry, recalling reactions and mechanisms in Organic Chemistry, and memorizing trends and facts in Inorganic Chemistry. Regular practice and revision of these formulas can significantly improve speed, accuracy, and overall performance in JEE Main 2026.

Physical Chemistry Formulas for JEE Mains 2026

Chapter – Some Basic Concepts in Chemistry

• Number of Moles: n = w / M
• Molarity: M = (moles of solute) / (volume (L))
• Molality: m = (moles of solute) / (kg of solvent)
• Mole fraction: X_A = n_A / (n_A + n_B)
• Density relation: Density = M / V_m
• Gas volume at STP: 1 mol gas = 22.4 L

Chapter – Atomic Structure

Bohr’s model of the hydrogen atom

• Radius of nth orbit: r_n = (n^2 h^2)/(4π^2 m e^2) · (1/Z) = (n^2 a₀)/Z, a₀ = 0.529 Å
• Velocity of electron in nth orbit: v_n = 2.18 × 10^6 · (Z/n) m/s
• Energy of nth orbit (Hydrogen-like atom): E_n = −13.6 · (Z^2 / n^2) eV
• Energy difference between levels (photon emitted/observed): ΔE = E_i − E_f = hν
• Rydberg formula (spectral lines): 1/λ = R_H (1/n₁² − 1/n₂²), n₂ > n₁, R_H = 1.097 × 10^7 m⁻¹
• De Broglie wavelength: λ = h/(mv), also λ = h/√(2mE)
• Heisenberg uncertainty principle: Δx · Δp ≥ h/(4π)
• Energy of electron in terms of wavenumber: E = −(R_H h c)/n²
• Effective nuclear charge (Slater’s rule approximation): Z_eff = Z − S, S = shielding constant
• Quantum numbers

1. Principal (n): energy level
2. Azimuthal (l): 0 → s, 1 → p, 2 → d, 3 → f
3. Magnetic (m_l): −l to +l
4. Spin (m_s): +1/2, −1/2

• Ionisation energy (Hydrogen atom): E_ion = 13.6 eV
• Velocity of electron (Bohr’s model): v_n = 2.18 × 10^6 · (Z/n) m s⁻¹

Chapter – Chemical Bonding and Molecular Structure

• Bond Order (Molecular Orbital Theory): Bond Order = 1/2 (No. of bonding e⁻ − No. of antibonding e⁻)
• Dipole Moment: μ = q · d (Unit: Debye, D)
• Percentage ionic character: % Ionic Character = (μ_observed / μ_theoretical) × 100
• Formal Charge: FC = V − N − (B/2, where V = valence electrons, N = non-bonded electrons, B = bonded electrons.
• Lattice Enthalpy (Born–Landé Equation): U = (N_A A Z⁺ Z⁻ e²)/(4π ε₀ r₀) (1 − 1/n), where N_A = Avogadro’s number, A = Madelung constant, Z± = ionic charges, r₀ = nearest neighbour distance, n = Born exponent.
• Steric Number (Hybridisation): Steric number = σ-bonds + lone pairs

• Relation Between Bond Length and Bond Order: Higher bond order ⇒ shorter bond length and higher bond energy
• Electronegativity Difference & Type of Bond

1. Δχ < 0.4 ⇒ Covalent
2. 0.4 < Δχ < 1.7 ⇒ Polar covalent
3. Δχ > 1.7 ⇒ Ionic

• Radius relation in ionic solids: r⁺ + r⁻ = r₀, where r₀ is the interionic distance (used in lattice energy formulas).
• Resonance Energy (concept): Resonance Energy = E_actual − E_most stable contributing structure
• VSEPR Lone Pair–Bond Pair Repulsion Order: LP–LP > LP–BP > BP–BP
• Relation Between Dipole Moment & Geometry: μ⃗_net = Σ μ⃗_i

Do Check: JEE Mains Subject Wise Formula Sheet

Chapter – Chemical Thermodynamics

• First Law of Thermodynamics: ΔU = q + w
• Enthalpy Change: ΔH = ΔU + Δn_g RT
• Gibbs Free Energy: ΔG = ΔH − TΔS
• Gibbs Free Energy at equilibrium: ΔG° = −RT ln K
• Heat at constant pressure: q_p = n C_p ΔT
• Relation between C_p and C_v: C_p − C_v = R

Chapter – Solutions

• Raoult’s Law: P_A = X_A P°_A
• Elevation in boiling point: ΔT_b = K_b m
• Depression in freezing point: ΔT_f = K_f m
• Van’t Hoff factor: i = (observed value) / (calculated value)
• Osmotic Pressure: π = C R T

Chapter – Chemical Equilibrium

• Law of Mass Action: K_c = [C]^c [D]^d / ([A]^a [B]^b)
• Relation between K_p and K_c: K_p = K_c (RT)^{Δn}
• Degree of dissociation: α = (moles dissociated) / (initial moles)
• Relation with equilibrium constant (weak electrolyte): K = (α² C) / (1 − α)

Chapter – Ionic Equilibrium

• pH definition: pH = −log[H⁺]
• pOH: pOH = −log[OH⁻]
• Relationship between pH and pOH: pH + pOH = 14
• Ionic Product of Water: K_w = [H⁺][OH⁻]
• Henderson–Hasselbalch Equation: pH = pK_a + log( (salt)/(acid) )

Chapter – Redox Reactions and Electrochemistry

• Nernst equation: E = E° − (0.0591/n) log Q
• Faraday’s first law of electrolysis: m = Z I t
• Faraday’s second law of electrolysis: m₁/m₂ = E₁/E₂
• Gibbs free energy relation: ΔG = −n F E
• Kohlrausch law of independent migration of ions: Λ°_m = ν⁺ λ°_+ + ν⁻ λ°_−

Chapter – Chemical Kinetics

• Rate Law: Rate = k [A]^n
• First Order Rate Constant: k = (2.303/t) log( [A]₀/[A] )
• Half-life for First Order Reaction: t_1/2 = 0.693/k
• Arrhenius Equation: k = A e^{−E_a/(RT)}
• Log form of Arrhenius: log k = log A − E_a/(2.303 RT)

Organic Chemistry Formulas for JEE Main 2026

Chapter – Purification and Characterisation of Organic Compounds

• Percentage of Element: %Element = (Mass of element / Molar mass) × 100
• Empirical formula: Empirical Mass = Σ(atomic masses)
• Molecular mass: Molecular Mass = n × Empirical Mass
• Vapour density relation: M = 2 × V.D.

Key Reactions / Tests

Lassaigne’s Test (Detection)

Chapter – Some Basic Principles of Organic Chemistry (GOC)

• Inductive Effect: +I, −I
  Order: −NO₂ > −CN > −COOH > −F > −Cl
• Hyperconjugation: Stability ∝ Number of α-Hydrogens
• Index of Hydrogen Deficiency (IHD): IHD = (2C + 2 + N − H − X)/2

Key Reactions

• Heterolytic bond fission

1. Definition: Bond breaks unequally → ions form
2. Reaction: CH₃–Cl → CH₃⁺ + Cl⁻
3. Use: SN1, E1 reactions

• Homolytic bond fission

1. Definition: Bond breaks equally → free radicals form
2. Reaction: Cl₂ →[hν] 2Cl·
3. Use: Free radical substitution

• Formation of carbanion (example): HC≡CH + OH⁻ ⟶ HC≡C⁻ + H₂O

1. Carbanion stability: CH₃⁻ > 1° > 2° > 3°
2. Formation of free radical (example): CH₃–CH₃ →[hν] CH₃· + CH₃·
3. Free radical stability: 3° > 2° > 1°

Must-Know Stability Orders

1. Carbocation: 3° > 2° > 1° > CH₃⁺
2. Carbanion: CH₃⁻ > 1° > 2° > 3°
3. Free Radical: 3° > 2° > 1°

Chapter – Hydrocarbons

Most Important Reactions

• Wurtz Reaction (Alkane Formation): 2R–X + 2Na →(dry ether) R–R + 2NaX

Mechanism: Free radical coupling

• Ozonolysis of Alkenes: RCH=CHR′ → O₃ → RCHO + R′CHO Via ozonide formation and cleavage
• Friedel–Crafts Alkylation / Acylation: C₆H₆ + RCl →(AlCl₃) C₆H₅R + HCl

Mechanism: Electrophilic Aromatic Substitution

• Baeyer’s Test: Alkene + KMnO₄ ⟶ Vicinal Diol

Chapter – Organic Compounds Containing Halogens

• Finkelstein Reaction: R–Cl + NaI →(acetone) R–I + NaCl

Mechanism: SN2

• Swarts Reaction: R–Cl + AgF ⟶ R–F + AgCl
• Dow’s Process: C₆H₅Cl →(NaOH, 623 K) C₆H₅OH

Mechanism: Nucleophilic Aromatic Substitution

• Sandmeyer Reaction: ArN₂⁺Cl⁻ + CuCl ⟶ ArCl + N₂

Chapter – Organic Compounds Containing Oxygen

• Lucas Test: R–OH + HCl →(ZnCl₂) R–Cl
• Williamson Ether Synthesis (SN2): R–O⁻Na⁺ + R′X ⟶ R–O–R′ + NaX
• Aldol Condensation: 2CH₃CHO →(NaOH) CH₃CH(OH)CH₂CHO
• Cannizzaro Reaction: 2HCHO + NaOH ⟶ HCOONa + CH₃OH
• Clemmensen Reduction: RCOR′ →(Zn/Hg, HCl) RCH₂R′
• Wolff–Kishner Reduction: RCOR′ →(NH₂NH₂, KOH) RCH₂R′
• HVZ Reaction: RCH₂COOH + Br₂ + P ⟶ RCHBrCOOH
• Esterification: RCOOH + ROH →(H₂SO₄) RCOOR + H₂O

Chapter – Organic Compounds Containing Nitrogen

• Hoffmann Bromamide Reaction: RCONH₂ + Br₂ + 4KOH ⟶ RNH₂ + K₂CO₃ + 2KBr + 2H₂O
• Carbylamine Test: RNH₂ + CHCl₃ + 3KOH ⟶ RNC + 3KCl + 3H₂O
• Diazotization: Aniline + NaNO₂ + HCl ⟶ ArN₂⁺Cl⁻ + 2H₂O
• Coupling Reaction: ArN₂⁺ + Phenol ⟶ Azo Dye

Chapter – Biomolecules

• Peptide Bond Formation: Amino Acid + Amino Acid ⟶ Dipeptide + H₂O
• Glucose Open Chain: CHO–(CHOH)₄–CH₂OH
• Sucrose Hydrolysis: Sucrose + H₂O ⟶ Glucose + Fructose

Chapter – Principles Related to Practical Chemistry

Inorganic Chemistry Formulas for JEE Main 2026

Chapter – Classification Of Elements And Periodicity In Properties

• Effective nuclear charge: Z_eff = Z − S, where Z = atomic number, S = shielding constant.
• Ionisation Energy (IE) Relation: Higher Z_eff ⇒ higher ionisation energy
• Electronegativity (Pauling scale approximate relation): Δχ = 0.208 √( E_AB − (E_AA + E_BB)/2 , where Δχ = |χ_A − χ_B|, E_AB = bond energy of A–B, E_AA, E_BB = bond energies of A–A and B–B.

Important Concepts / Reactions

• Alkali metals reacting with water: 2M + 2H₂O ⟶ 2MOH + H₂↑

(M = Li, Na, K, Rb, Cs)

• Halogen displacement reactions:X₂ + 2Y⁻ ⟶ 2X⁻ + Y₂

More reactive halogen displaces less reactive halogen.

Chapter – p-Block Elements

Group 13 (Boron Family)

• Bond energy trend: B–B > B–Al > Al–Al
• Lewis acidity of BX₃: BF₃ < BCl₃ < BBr₃ < BI₃
• Hydrolysis of boron halides: BCl₃ + 3H₂O ⟶ B(OH)₃ + 3HCl

Group 14 (Carbon Family)

• Oxidation states: +2 and +4 (stability of +2 increases down the group)
• Important reaction (Fischer–Tropsch mention): CO + H₂ ⟶ CH₄

Group 15 (Nitrogen Family)

• Oxidation states: −3 to +5
• Formation of ammonium chloride: NH₃ + HCl ⟶ NH₄Cl
• Haber process (ammonia synthesis): N₂ + 3H₂ ⟶(Fe catalyst, 500°C) 2NH₃

Group 16 (Oxygen Family)

• Oxidation states: −2 to +6
• Ozone formation: 3O₂ ⟶(UV) 2O₃
• Oxidation reaction (example): H₂S + Cl₂ ⟶ S + 2HCl

Group 17 (Halogens)

• Displacement reactions: X₂ + Y⁻ ⟶ Y₂ + X⁻
• Interhalogen formation (examples): ClF₃, BrF₅

Group 18 (Noble Gases)

• Oxidation reaction (example): Xe + F₂ ⟶ XeF₂
• Important compounds: XeF₂, XeF₄, XeF₆

Chapter – d-Block Elements

• Electronic configuration: (n−1)d¹–¹⁰ ns¹–²
• Coordination number & geometry

1. CN = 4 → tetrahedral / square planar
2. CN = 6 → octahedral

Important Reactions

• Formation of complexes: [Fe(H₂O)₆]³⁺ + SCN⁻ ⟶ [Fe(H₂O)₅(SCN)]²⁺ + H₂O
• Redox reaction: Fe²⁺ ⟶ Fe³⁺ + e⁻
• Ligand substitution: [Cu(NH₃)₄]²⁺ + 4Cl⁻ ⟶ [CuCl₄]²⁻ + 4NH₃
• Stability of complexes (CFSE concept): Δ_oct = crystal field splitting energy (octahedral)

High-spin vs low-spin determination is based on Δ and pairing energy.

Chapter – f-Block Elements

• Lanthanide contraction: Affects ionic radius, density, and chemistry of subsequent elements
• Oxidation states

1. Lanthanides: mostly +3
2. Actinides: +3, +4, +5, +6 (depends on element)

Key Reactions

• Reduction of lanthanides (some Ln): Ln³⁺ + e⁻ ⟶ Ln²⁺
• Complex formation with water: Ln³⁺ + 6H₂O ⟶ [Ln(H₂O)₆]³⁺

Chapter – Coordination Compounds

• Oxidation number of metal: Ox. no. of M = (charge on complex) − (charge on ligands)
• Substitution reaction: [Co(NH₃)₆]³⁺ + Cl⁻ ⟶ [Co(NH₃)₅Cl]²⁺ + NH₃
• Chelation with EDTA: [Ni(H₂O)₆]²⁺ + EDTA⁴⁻ ⟶ [Ni(EDTA)]²⁻ + 6H₂O
• Formation constant: K_f = [MLⁿ] / ( [M][L]^n )