Most Important Chemistry Formulas for JEE Main

Knowing the most important chemistry formulas for JEE Main is a game-changer in chemistry preparation. It can make a difference in improving the score from 60+ to 90+ marks out of 100 in chemistry. An interesting analysis observed is that toppers who mastered the most important chemistry formulas and reactions solve questions twice as fast as others. These cover periodic table trends from the p-block, d-block, and f-block elements, the most important organic reactions and a strong foundation in formulas from physical chemistry, organic chemistry and inorganic chemistry.

This blog provides a complete list of JEE Main chemistry chapter-wise high-scoring formulas and organic reactions. The formula list is ideal for beginners and repeaters. Aspirants can also use the list to revise regularly, just like Matrix JEE Academy toppers. By being thorough with these formulas, one can maximise their speed and accuracy while solving chemistry questions. Hence, turn chemistry into a high-scoring section by using this list and applying Matrix topper strategies shared in this blog.

Complete Overview of the JEE Main Chemistry Syllabus (NTA Updated)

The JEE Main chemistry syllabus is divided into three sections – physical chemistry, organic chemistry and inorganic chemistry. Matrix chemistry faculty analysed the chemistry paper and syllabus. They identified that physical chemistry has more emphasis on numerical questions, whereas organic chemistry focuses on reaction mechanisms and reagents. Inorganic chemistry includes memorizing periodic trends and coordination chemistry. Hence, matrix chemistry teachers recommend understanding the syllabus thoroughly before moving to smart study strategies and an important formulas list.

Download Most Important Chemistry Formulas for JEE Main PDF

Physical Chemistry Syllabus for JEE Main

As per Matrix JEE Academy mentors and toppers, the most important chapters of physical chemistry include stoichiometry, atomic structure, chemical thermodynamics, equilibrium, chemical kinetics and electrochemistry. Here is the complete physical chemistry syllabus updated by NTA with topic weightage in the JEE Main paper.

UNIT	CHAPTER NAME	SUB-TOPIC	JEE Main Weightage	Formula Density
1	Some basic concepts in chemistry	Matter types, atomic & molecular mass calculations, Laws of chemical combination, mole concept, molar mass, percentage composition, empirical & molecular formula, stoichiometry, limiting reagent.	High (2-3 questions)	High
2	Atomic structure	Photoelectric effect, Bohr model, quantum numbers, de Broglie wavelength, Heisenberg uncertainty principle, orbitals, electronic configuration	Medium (1-2 questions)	Medium
3	Chemical bonding and molecular structure	Ionic & covalent bonding, lattice enthalpy, electronegativity, VSEPR, hybridisation, resonance, MO theory, bond order, hydrogen bonding	High (2-3 questions)	Medium
4	Chemical thermodynamics	First & second laws, enthalpy changes, Hess’s law, entropy, Gibbs free energy, spontaneity, equilibrium constant relation	High (2-3 questions)	High
5	Solutions	Molarity, molality, mole fraction, Raoult’s law, colligative properties, osmotic pressure, van’t Hoff factor, abnormal molar mass	Medium (1-2 questions)	High
6	Equilibrium	Chemical equilibrium, Kp & Kc, Le Chatelier’s principle, acids–bases, pH, buffer solutions, solubility product, common ion effect	High (2-3 questions)	High
7	Redox reactions and electrochemistry	Oxidation number, redox balancing, conductance, Kohlrausch’s law, electrochemical cells, Nernst equation, Gibbs–EMF relation, fuel cells	High (2-3 questions)	High
8	Chemical kinetics	Rate law, order & molecularity, integrated rate equations, half-life, Arrhenius equation, activation energy, collision theory	Medium (1-2 questions)	High

Organic Chemistry Syllabus for JEE Main

Organic chemistry is all about reaction mechanisms, reagents and functional groups. As analysed by the Matrix JEE faculty, the key topics based on past year JEE Main papers are: Hydrocarbons, Haloalkanes & Haloarenes, Alcohols, Phenols, Ethers, Aldehydes, Ketones, Carboxylic Acids, Amines, and Biomolecules. Below is the complete syllabus of organic chemistry updated by NTA with topic weightage in the JEE Main paper:

UNIT	CHAPTER NAME	SUB-TOPIC	JEE Main Weightage	Formula/Reaction Density
1	Purification and characterisation of organic compounds	Crystallisation, sublimation, distillation, chromatography, qualitative tests (N, S, Halogens), quantitative analysis, empirical & molecular formula calculations.	Low (1-2 questions)	Low
2	Some basic principles of organic chemistry (GOC)	Hybridisation, isomerism, IUPAC nomenclature, carbocations/free radicals, inductive, resonance & hyperconjugation effects, electrophiles & nucleophiles, reaction types.	High (2-3 questions)	High
3	Hydrocarbons	Alkanes (conformations, halogenation), alkenes (addition reactions, ozonolysis), alkynes (acidic nature), aromatic hydrocarbons, electrophilic substitution, Friedel–Crafts reactions.	High (2-3 questions)	High
4	Organic compounds containing halogens	C–X bond nature, SN1 & SN2 mechanisms, nucleophilic substitution reactions, preparation & properties, environmental effects (DDT, freons).	Medium (1-2 questions)	Medium
5	Organic compounds containing oxygen	Alcohols, phenols, ethers, aldehydes, ketones & carboxylic acids – preparation, properties, acidity, oxidation–reduction, aldol, Cannizzaro, haloform, Grignard reactions, tests.	High (2-3 questions)	High
6	Organic compounds containing nitrogen	Amines – basicity, preparation, reactions, diazonium salts & their synthetic importance.	Medium (1-2 questions)	High
7	Biomolecules	Carbohydrates (glucose, fructose), proteins (amino acids, structure), vitamins, nucleic acids (DNA, RNA), and hormones.	Medium (1-2 questions)	Medium
8	Principles related to practical chemistry	Detection of functional groups & extra elements, salt analysis principles, preparation of key compounds, titration chemistry, thermochemistry & kinetics experiments	Low (0-1 questions)	Low

Inorganic Chemistry Syllabus for JEE Main

Inorganic is known for the periodic table and trends, properties of elements and reactions. The important chapters from this sub-section of chemistry include: P-block, D-block, F-block elements, Coordination Compounds, and periodic table trends. Below is the complete inorganic chemistry syllabus updated by NTA with topic weightage in the JEE Main paper:

UNIT	CHAPTER NAME	SUB-TOPIC	JEE Main Weightage	Formula/Reaction Density
1	Classification of elements and periodicity in properties	Modern periodic law, periodic table, s-, p-, d-, f-block classification, periodic trends in atomic radius, ionisation enthalpy, electron gain enthalpy, oxidation states, chemical reactivity.	Medium (1-2 questions)	Medium
2	p-block elements	Electronic configuration, periodic trends, anomalous behaviour of first elements, physical & chemical properties of p-block elements across groups.	High (2-3 questions)	High
3	d- and f- block elements	Transition elements – general properties, oxidation states, magnetic & catalytic behaviour, K₂Cr₂O₇ & KMnO₄ preparation and reactions; lanthanoids & actinoids – configuration & oxidation states.	Medium (1-2 questions)	High
4	Coordination compounds	Werner’s theory, ligands, coordination number, nomenclature, isomerism, VBT & CFT, colour & magnetic properties, applications in metallurgy, biology & qualitative analysis.	High (2-3 questions)	High

Chapter-Wise Most Important Chemistry Formulas For JEE Main

As observed at Matrix JEE Faculty, every matrix focuses on preparing a list of important chemistry formulas for JEE Main and mastering them. These formulas can help answer the majority of chemistry questions if the relevant concepts are studied thoroughly. Below is a chapter-wise list of all important formulas from physical chemistry, organic chemistry and inorganic chemistry. The list is made by the Matrix JEE chemistry faculty based on JEE Main previous year trends.

Most Important Physical Chemistry Formulas For JEE Main

Chapter – Some Basic Concepts in Chemistry

1. \[\text{Number of Moles}: n = \frac{w}{M}\]
2. \[\text{Molarity}: M = \frac{\text{moles of solute}}{\text{volume (L)}}\]
3. \[\text{Molality}: m = \frac{\text{moles of solute}}{\text{kg of solvent}}\]
4. \[\text{Mole fraction}: X_A = \frac{n_A}{n_A + n_B}\]
5. \[\text{Density relation}: \text{Density} = \frac{M}{V_m}\]
6. \[\text{Gas volume at STP}: 1~\text{mol gas} = 22.4~\text{L}\]

Chapter – Atomic Structure

1. \[\text{Bohr’s model of the hydrogen atom:}\]
   • \[\text{Radius of nth orbit : } r_n = \frac{n^2 h^2}{4\pi^2 m e^2} \cdot \frac{1}{Z} = \frac{n^2 a_0}{Z}, a_0 = 0.529\,\text{\AA}\]
   • \[\text{Velocity of electron in nth orbit: } v_n = 2.18 \times 10^6 \, \frac{Z}{n} \ \text{m/s}\]
   • \[\text{Energy of nth orbit (Hydrogen-like atom): }E_n = -\frac{13.6\, Z^2}{n^2} \ \text{eV}\]
   • \[\text{Energy difference between levels (photon emitted/observed): }\Delta E = E_i – E_f = h\nu\]
2. \[\text{Rydberg formula (spectral lines): }\frac{1}{\lambda} = R_H \left( \frac{1}{n_1^2} – \frac{1}{n_2^2} \right), \quad n_2 > n_1\
   R_H = 1.097 \times 10^7 \ \text{m}^{-1}\]
3. \[\text{De broglie wavelength: }\lambda = \frac{h}{mv}, \lambda = \frac{h}{\sqrt{2mE}}\]
4. \[\text{Heisenberg uncertainty principle: }\Delta x \cdot \Delta p \geq \frac{h}{4\pi}\]
5. \[\text{Energy of electron in terms of wavenumber: }E = -\frac{R_H h c}{n^2}\]
6. \[\text{Effective nuclear charge (Slater’s rule approximation): }Z_{\text{eff}} = Z – S
   S = \text{shielding constant}\]
7. \[\text{Quantum numbers:}\]
   • \[\text{Principal (n): energy level}\]
   • \[\text{Azimuthal (l): 0 → s, 1 → p, 2 → d, 3 → f}\]
   • \[\text{Magnetic }(m_l) : m_l = -l \text{ to } +l\]
   • \[\text{Spin } (m_s) : m_s = +\frac{1}{2}, -\frac{1}{2}\]
8. \[\text{Ionisation energy (Hydrogen atom): }E_{\text{ion}} = 13.6 \, \text{eV}\]
9. \[\text{Velocity of electron (Bohr’s model): }v_n = \frac{2.18 \times 10^6 \, Z}{n} \; \text{m s}^{-1}\]

Chapter – Chemical Bonding and Molecular Structure

1. \[\text{Bond Order (Molecular Orbital Theory)}: \text{Bond Order} \;=\; \frac{1}{2}\big(\text{Number of bonding electrons} – \text{Number of antibonding electrons}\big)\]
2. \[\text{Dipole Moment: μ=d}\]\[\text{where,}\]\[\text{μ = dipole moment}\]\[\text{q = charge}\]\[\text{d = distance between charges, Unit: Debye (D)}\]
3. \[\text{Percentage ionic character:} \%\text{ Ionic Character} \;=\; \frac{\mu_{\text{observed}}}{\mu_{\text{theoretical}}}\times 100\]
4. \[\text{Formal Charge}: \text{Formal Charge (FC)} \;=\; V – N – \frac{B}{2}\]\[\text{where: V = valence electrons}\]\[\text{N = non-bonded electrons}\]\[\text{B = bonded electrons}\]\[\text{(Used heavily in resonance & structure stability questions.)}\]
5. \[\text{Lattice Enthalpy (Born–Landé Equation) }: U \;=\; \frac{N_A A Z^+ Z^- e^2}{4\pi \varepsilon_0 r_0}\left(1-\frac{1}{n}\right)\]\[\text{where }N_A = \text{Avogadro’s number }, A = \text{Madelung constant }, Z^\pm = \text{ionic charges }, r_0 = \text{nearest neighbour distance} n = \text{Born exponent}.\]
6. \[\text{Steric Number (Hybridisation Formula): } \text{Steric number} \;=\; \sigma\text{-bonds} + \text{lone pairs}\]

Steric No.	Hybridisation	Shape
2	sp	Linear
3	sp²	Trigonal planar
4	sp³	Tetrahedral
5	sp³d	Trigonal bipyramidal
6	sp³d²	Octahedral

7. \[\text{Relation Between Bond Length and Bond Order}: \text{Higher Bond Order} \;\Longrightarrow\; \text{Shorter bond length and higher bond energy}\]\[\text{(Higher BO → shorter and stronger bond)}\]
8. \[\text{Electronegativity Difference & Type of Bond }:
   \begin{aligned}
   \Delta\chi < 0.4 &\Rightarrow \text{Covalent} \\
   0.4 < \Delta\chi < 1.7 &\Rightarrow \text{Polar covalent} \\
   \Delta\chi > 1.7 &\Rightarrow \text{Ionic}
   \end{aligned}\]
9. \[\text{Radius relation in ionic solids : } r_+ + r_- = r_0\] \[\text{(where r_0 is the interionic distance used in lattice energy formulas)}\] \[\text{Used with Born–Landé equation.}\]
10. \[\text{Resonance Energy Concept (Indirect Formula Use)}: \text{Resonance Energy} \;=\; E_{\text{actual}} – E_{\text{most stable contributing structure}}\]\[\text{(Used in conceptual stability comparison.)}\]
11. \[\text{VSEPR Lone Pair–Bond Pair Repulsion Order: }\text{LP–LP} > \text{LP–BP} > \text{BP–BP}\]\[\text{(Used for shape prediction & bond angle distortion.)}\]
12. \[\text{Relation Between Dipole Moment & Geometry}: \vec{\mu}_{\text{net}} \;=\; \sum_i \vec{\mu}_i\]

Chapter – Chemical Thermodynamics

1. \[\text{First Law of thermodynamics}: \Delta U = q + w\]
2. \[\text{Enthalpy Change}: \Delta H = \Delta U + \Delta n_g RT\]
3. \[\text{Gibbs Free Energy}: \Delta G = \Delta H – T\Delta S\]
4. \[\text{Gibbs Free Energy at equilibrium }: \Delta G^\circ = -RT \ln K\]
5. \[\text{Heat at constant pressure }: q_p = nC_p \Delta T\]
6. \[\text{Relation between } C_p \text{ and } C_v\textbf{:} C_p – C_v = R\]

Chapter – Solutions

1. \[\text{Raoult’s Law}: P_A = X_A P_A^0\]
2. \[\text{Elevation in boiling point}: \Delta T_b = K_b m\]
3. \[\text{Depression in freezing point}: \Delta T_f = K_f m\]
4. \[\text{Van’t Hoff factor}: i = \frac{\text{observed value}}{\text{calculated value}}\]
5. \[\text{Osmotic Pressure}: \pi = C R T\]

Chapter – Chemical Equilibrium

1. \[\text{Law of Mass Action}: K_c = \frac{[C]^c [D]^d}{[A]^a [B]^b}\]
2. \[\text{Relation between} K_p \text{ and } K_c: K_p = K_c (RT)^{\Delta n}\]
3. \[\text{Degree of dissociation}: \alpha = \frac{\text{moles dissociated}}{\text{initial moles}}\]
4. \[\text{Relation with equilibrium constant (weak electrolyte)}: K = \frac{\alpha^2 C}{1 – \alpha}\]

Chapter – Ionic Equilibrium

1. \[\text{pH definition: }pH = -\log [H^+]\]
2. \[\text{pOH: }pOH = -\log [OH^-]\]
3. \[\text{Relationship between pH and pOH: }pH + pOH = 14\]
4. \[\text{Ionic Product of Water: }K_w = [H^+][OH^-]\]
5. \[\text{Henderson–Hasselbalch Equation: }pH = pK_a + \log \frac{\text{salt}}{\text{acid}}\]

Chapter – Redox Reactions and Electrochemistry

1. \[\text{Nernst equation: }E = E^\circ – \frac{0.0591}{n}\log Q\]
2. \[\text{Faraday’s first law of electrolysis: }m = ZIt\]
3. \[\text{Faraday’s second of electrolysis: }\frac{m_1}{m_2} = \frac{E_1}{E_2}\]
4. \[\text{Gibb’s free energy relation: }\Delta G = -nFE\]
5. \[\text{Kohlrausch law of independent migration of ions: }\Lambda_m^\circ = \nu_+ \lambda_+^\circ + \nu_- \lambda_-^\circ\]

Chapter – Chemical Kinetics

1. \[\text{Rate Law: }\text{Rate} = k[A]^n\]
2. \[\text{First Order Rate Constant: }k = \frac{2.303}{t} \log \frac{[A]_0}{[A]}\]
3. \[\text{Half-life for First Order Reaction: }t_{1/2} = \frac{0.693}{k}\]
4. \[\text{Arrhenius Equation: }k = A e^{-\frac{E_a}{RT}}\]
5. \[\text{Log form of Arrhenius: }\log k = \log A – \frac{E_a}{2.303RT}\]

Most Important Organic Chemistry Formulas For JEE Main

Chapter – Purification and Characterisation of Organic Compounds

• \[\text{Percentage of Element: }\%\,\text{Element} = \frac{\text{Mass of element}}{\text{Molar mass}} \times 100\]
• \[\text{Empirical formula: Empirical Mass = ∑(atomic masses)}\]
• \[\text{Molecular mass: Molecular Mass = n × Empirical Mass}\]
• \[\text{Vapour density relation: M = 2 × V.D.}\]

Key Reactions / Tests

 Lassaigne’s Test (Detection):

Element	Reagent	Observation
N	FeSO₄ + HCl	Prussian Blue
S	Lead Acetate	Black ppt
Halogen	AgNO₃	White/Yellow ppt

Chapter – Some Basic Principles of Organic Chemistry (GOC)

• \[\text{Inductive Effect: }+I,−I+I , -I+I,−I: Order: −NO2​>−CN>−COOH>−F>−Cl\]
• \[\text{Hyperconjugation: Stability ∝ No. of α-Hydrogens }\]
• \[\text{Index of Hydrogen Deficiency (IHD): } \text{IHD} = \frac{2C + 2 + N – H – X}{2}\]

Key Reactions:

• Heterolytic bond fission:\[\text{Definition: A covalent bond breaks unequally, then ions form.}\]\[\text{Reaction: } {CH3-Cl -> CH3^+ + Cl^-}\]\[\text{Use: SN1, E1 reactions}\]
• Homolytic bond fission:
  \[\text{Definition: Covalent bond breaks equally → free radicals form.}\]\[\text{Reaction: }{Cl2 ->[h\nu] 2 Cl^.}\]\[\text{Use: Free radical substitution.}\]
• \[\text{Formation of carbocation: }\text{HC} \equiv \text{CH} + \text{OH}^- \longrightarrow \text{HC} \equiv \text{C}^- + H_2O\]
• \[\text{Carbanion stability: }\text{Stability: } CH_3^- > 1^\circ > 2^\circ > 3^\circ\]
• \[\text{Formation of free radical: }CH_3-CH_3 \xrightarrow{h\nu} CH_3\cdot + CH_3\cdot\]
• \[\text{Free radical stability: }\text{Stability: } 3^\circ > 2^\circ > 1^\circ\]

Must-Know Stability Orders:

• \[\text{Carbocation: }3^\circ > 2^\circ > 1^\circ > CH_3^+\]
• \[\text{Carbanion: }CH_3^- > 1^\circ > 2^\circ > 3^\circ\]
• \[\text{Free Radical: }3^\circ > 2^\circ > 1^\circ\]

Chapter – Hydrocarbons

Most Important Reactions-

• \[\text{Wurtz Reaction (Alkane Formation): }2R – X + 2Na \xrightarrow{\text{dry ether}} R – R + 2NaX\quad \text{(Mechanism: Free radical coupling)}\]
• \[\text{Ozonolysis of Alkenes: }RCH = CHR’ \xrightarrow{O_3} RCHO + R’CHO
  \quad \text{(Via ozonide formation and cleavage)}\]
• \[\text{Friedel–Crafts Alkylation & Acylation: }C_6H_6 + RCl \xrightarrow{AlCl_3} C_6H_5R + HCl
  \quad \text{(Mechanism: Electrophilic Aromatic Substitution)}\]
• \[\text{Baeyer’s Test: Alkene } + KMnO_4 \longrightarrow \text{Vicinal Diol}\]

Chapter – Organic Compounds Containing Halogens

• \[\text{Finkelstein Reaction: }R – Cl + NaI \xrightarrow{\text{acetone}} R – I + NaCl
  \quad \text{(Mechanism: } S_N2 \text{)}\]
• \[\text{Swarts Reaction: }R – Cl + AgF \longrightarrow R – F + AgCl\]
• \[\text{Dow’s Process – Mechanism: Nucleophilic Aromatic Substitution: }C_6H_5Cl \xrightarrow[\;623\,K\;]{NaOH} C_6H_5OH\]\[\quad \text{(Mechanism: Nucleophilic Aromatic Substitution)}\]
• \[\text{Sandmeyer Reaction: }ArN_2^+Cl^- + CuCl \longrightarrow ArCl + N_2\]

Chapter – Organic Compounds Containing Oxygen

• \[\text{Lucas Test : } R – OH + HCl \xrightarrow{ZnCl_2} R – Cl\]
• \[\text{Williamson Ether Synthesis (SN2): } R – O^- Na^+ + R’X \longrightarrow R – O – R’ + NaX
  \quad \text{(Mechanism: } S_N2 \text{)}\]
• \[\text{Aldol Condensation: } 2CH_3CHO \xrightarrow{NaOH} CH_3CH(OH)CH_2CHO\]
• \[\text{Cannizzaro Reaction: } 2HCHO + NaOH \longrightarrow HCOONa + CH_3OH\]
• \[\text{Clemmensen Reduction: }RCOR’ \xrightarrow{Zn/Hg,\;HCl} RCH_2R’\]
• \[\text{Wolff–Kishner Reduction: }RCOR’ \xrightarrow{NH_2NH_2,\;KOH} RCH_2R’\]
• \[\text{HVZ Reaction: }RCH_2COOH + Br_2 + P \longrightarrow RCHBrCOOH\]
• \[\text{Esterification: }RCOOH + ROH \xrightarrow{H_2SO_4} RCOOR + H_2O\]

Chapter – Organic Compounds Containing Nitrogen

• \[\text{Hoffmann Bromamide Reaction: }RCONH_2 + Br_2 + 4KOH \longrightarrow RNH_2 + K_2CO_3 + 2KBr + 2H_2O\]
• \[\text{Carbylamine Test: }RNH_2 + CHCl_3 + 3KOH \longrightarrow RNC + 3KCl + 3H_2O\]
• \[\text{Diazotization: }\text{Aniline} + NaNO_2 + HCl \longrightarrow ArN_2^+Cl^- + 2H_2O\]
• \[\text{Coupling Reaction: }ArN_2^+ + \text{Phenol} \longrightarrow \text{Azo Dye}\]

Chapter – Biomolecules

• \[\text{Peptide Bond Formation: }\text{Amino Acid} + \text{Amino Acid} \longrightarrow \text{Dipeptide} + H_2O\]
• \[\text{Glucose Open Chain: }CHO – (CHOH)_4 – CH_2OH\]
• \[\text{Sucrose Hydrolysis: }\text{Sucrose} + H_2O \longrightarrow \text{Glucose} + \text{Fructose}\]

Chapter – Principles Related to Practical Chemistry

Test	Observation
Tollens	Silver mirror
Fehling	Brick-red ppt
Lucas	Cloudiness
Bromine water	Decolourization
Baeyer	Purple – colourless
Carbylamine	Foul smell

Most Important Inorganic Chemistry Formulas For JEE Main

Chapter – Classification Of Elements And Periodicity In Properties

• \[\text{Effective nuclear charge (Z_eff):}\]\[\text{Where Z = atomic number, S = shielding constant}\]
• \[\text{Ionisation Energy (IE) Relation:}\]\[\text{Higher Z_eff → higher ionisation energy}\]
• \[\text{Electronegativity (Pauling scale approximate relation) : } \Delta \chi = 0.208 \sqrt{E_{AB} – \frac{E_{AA} + E_{BB}}{2}}\]\[\text{Where:}\]\[\Delta \chi=∣\chi_A−\chi_B∣\]\[E_{AB}​ = \text{bond energy of A–B}\]\[E_{AA}, E_{BB}​ = \text{bond energies of A–A and B–B}\]

Important Concepts / Reactions:

• \[\text{Alkali metals reacting with water: }2M + 2H_2O \longrightarrow 2MOH + H_2 \uparrow\]
• \[\quad (M = \text{Li, Na, K, Rb, Cs})\]
• \[\text{Halogen displacement reactions: }X_2 + 2Y^- \longrightarrow 2X^- + Y_2\]
• \[\quad (\text{More reactive halogen displaces less reactive halogen})\]

Chapter – p-Block Elements

Group 13 (Boron Family):

• \[\text{Bond energy trend: B–B > B–Al > Al–Al}\]
• \[\text{Lewis acidity of } BX_3: \text{BF}_3 < \text{BCl}_3 < \text{BBr}_3 < \text{BI}_3\]
• \[\text{Hydrolysis of Boron halides: } \text{BCl}_3 + 3 H_2O \longrightarrow B(OH)_3 + 3 HCl\]

Group 14 (Carbon Family):

• \[\text{Oxidation states: +2 and +4, the stability of +2 increases down the group}\]
• \[\text{Important reaction: CO + H₂ → CH₄ (Fischer-Tropsch reaction)}\]

Group 15 (Nitrogen Family)

• \[\text{Oxidation states: -3 to +5}\]
• \[\text{Important reactions: % Formation of Ammonium Chloride}\]\[\text{NH}_3 + HCl \longrightarrow NH_4Cl\]\[\text{% Haber Process for Ammonia Synthesis}\]\[N_2 + 3 H_2 \xrightarrow[\text{500 °C}]{\text{Fe catalyst}} 2 NH_3\]

Group 16 (Oxygen Family)

• \[\text{Oxidation states: } -2 to +6\]
• \[\text{Ozone formation: % Ozone Formation }
  3 O_2 \xrightarrow{UV} 2 O_3\]
• \[\text{Oxidation reactions: } H_2S + Cl_2 \longrightarrow S + 2 HCl\]

Group 17 (Halogens)

• \[\text{Displacement reactions: X₂ + Y⁻ → Y₂ + X⁻}\]
• \[\text{Interhalogen formation: ClF₃, BrF₅}\]

Group 18 (Noble Gases)

• \[\text{Oxidation reaction: Xe + F₂ → XeF₂}\]
• \[\text{Important compounds: XeF₂, XeF₄, XeF₆}\]

Chapter – d- Block Elements

Key Formulas & Concepts:

1. \[\text{Electronic configuration: (n-1)d¹⁻¹⁰ ns¹⁻²}\]
2. \[\text{Coordination number & geometry:}\]
   • \[\text{CN = 4 → tetrahedral/square planar}\]
   • \[\text{CN = 6 → octahedral}\]

Important Reactions:

• \[\text{Formation of complexes: } [Fe(H_2O)_6]^{3+} + SCN^- \longrightarrow [Fe(H_2O)_5(SCN)]^{2+} + H_2O\]
• \[\text{Redox reactions: }Fe^{2+} \longrightarrow Fe^{3+} + e^-\]
• \[\text{Ligand substitution: }[Cu(NH_3)_4]^{2+} + 4 Cl^- \longrightarrow [CuCl_4]^{2-} + 4 NH_3\]

Stability of complexes (CFSE concept):

• \[\text{Δ_oct= crystal field splitting energy in octahedral complexes}\]
• \[\text{High-spin vs low-spin determination}\]

Chapter – f- Block Elements

Important Concepts:

• \[\text{Lanthanide contraction → affects ionic radius, density, and chemistry of subsequent elements}\]
• \[\text{Oxidation state: +3 mostly}\]
• \[\text{Actinides → show +3, +4, +5, +6 depending on element}\]

Key Reactions:

• \[\text{Reduction of Lathanides: } \text{Ln}^{3+} + e^- \longrightarrow \text{Ln}^{2+} \quad (\text{for some Ln})\]
• \[\text{Complex formation with water: }\text{Ln}^{3+} + 6 H_2O \longrightarrow [\text{Ln}(H_2O)_6]^{3+}\]

Chapter – Coordination Compounds

• \[\text{Oxidation number of metal:
  Ox. no. of M-charge on complex−charge on ligands}\]
• \[\text{Substitution reaction: }[Co(NH_3)_6]^{3+} + Cl^- \longrightarrow [Co(NH_3)_5Cl]^{2+} + NH_3\]
• \[\text{Chelation with EDTA: }[Ni(H_2O)_6]^{2+} + EDTA^{4-} \longrightarrow [Ni(EDTA)]^{2-} + 6 H_2O\]
• \[\text{Formation constant: } K_f = \frac{[ML_n]}{[M][L]^n}\]
• \[\text{Crystal field splitting (Octahedral): } \Delta_\text{oct} \quad \text{(Determines color and magnetic properties of the complex)}\]

Matrix Topper’s Tricks to Ace Chemistry Formulas

A simple strategy followed by Matrix JEE toppers for chemistry is to focus on NCERT chemistry and master all important formulas. They do not believe in mugging up the reactions and formulas. At Matrix, chemistry is taught in a way to understand the underlying logic behind every formula. This approach has helped Matrix aspirants score 99%ile and above in JEE Main. Here are some effective tips to master chemistry formulas shared by Matrix toppers and faculty:

• Matrix topper Rishabh Meel (AIR 70, JEE Advanced) focused on creating a list of frequently occurring formulas in past papers. Rishabh suggests creating a chapter-wise formula sheet from the Matrix modules, which one can refer to while solving numercials as well as revising.
• Gaurav Pareek (99.988 %ile, JEE Main 2025) applied a different strategy where he focused heavily on revising high-scoring formulas. He did not rely on memorising all chemistry formulas at once.
• Matrix chemistry faculty advised to keep a separate notebook for organic reactions and mechanisms to refer to and revise constantly.
• TKD Sir, (Inorganic expert mentor) from Matrix, recommends to learn p-block and coordination formulas thoroughly. Get a good grasp of NCERT – focus more on periodic tables, oxoacids, and periodic trends as most MCQs come from these topics.
• According to Gaurav Jaiswal, sir, formulas from these chapters appear every year: d-block electronic configuration, oxidation state patterns, and stability formulas.
• Narendra Kok, sir (IIT Kharagpur Alumni), advises practising mixed-chapter numerical problems to help with faster formula application.

Best Books and Resources to Revise Chemistry Formulas

Instead of collecting various books for chemistry formulas, toppers advise sticking to the right resources. Matrix JEE Academy has formula booklets and Matrix JEE chemistry modules to master the subject. Buy the Matrix chemistry module book set, which includes topic-wise formula sheets, past year questions and more.

Conclusion

Every JEE topper has one habit of mastering the most important chemistry formulas to top this section. Matrix toppers believe smart study with smart revision is the key to acing the chemistry section in JEE Main. However, aspirants should focus on understanding the formulas and mechanisms as well as revising them regularly. Chemistry is the only section in JEE Main where similar formula-based and reaction-based questions repeat year after year. To crack this pattern, matrix chemistry teachers advise keeping the important formula list handy and revising it once every 10 days.

FAQs