MHT CET Chemistry Syllabus: Check the Latest Syllabus

• Pure substances versus mixtures

1. Metals
2.  Non-metals
3. Metalloids

• States of matter

• Properties and Measurement of Matter
• SI Units and Base Quantities

• Introduction
• Experiment

• Atomic Mass
• Average Atomic Mass
• Molecular Mass
• Formula Mass

• Definition: Mole
• Definition: Avogadro's Number

• Definition: Atom
• Definition: Molecule
• Definition: Avogadro's Law

• Discovery of electron
• Discovery of proton
• Discovery of neutron

• Definition: Atomic Number
• Definition: Mass Number

• Definition: Isotopes
• Examples

• Wave particle duality of electromagnetic radiation
• Line emission spectrum of hydrogen
• Radii of the Orbits
• Energy of the Electrons
• Limitations of Bohr’s Model
• De Broglie’s Explanation

• Explanation of the line spectrum of hydrogen using Bohr theory
• Bohr's theory and atomic spectrum of hydrogen
• Ionization energy

• Schrodinger wave equation
• Physical significance of Ψ and Ψ²
• Radial probability distribution curves
• Difference between orbit and orbital
• Atomic orbitals and quantum numbers
• Shapes of atomic orbitals
• Energies of orbitals
• Aufbau principle
• Electronic configuration of atoms and its representation 
• Electronic configurations of Cu and Cr

1. Chromium
2. Copper
3. Isoelectronic species

• Definition: Chemical Bond

• Kossel and Lewis theory
• Lewis symbols
• Significance of Lewis symbols
• Lewis symbols and valence of elements

• Definition: Ion
• Definition: Cation
• Definition: Anion
• Definition: Electropositive Element
• Definition: Electronegative Element
• Definition: Electrovalent Bond
• Definition: Electrovalent (or Ionic) Compounds
• Definition: Electrovalency

• Definition: Covalent Compound
• Definition: Covalent Molecule
• Key Points: The Covalent Bond

• VSEPR theory
• Main postulates of VSEPR theory
• Geometry of some molecules
• Geometry of some molecules
• Steps to predict the molecular geometry using VSEPR theory

• Postulates of Valence Bond Theory
• Interacting forces during covalent bond formation
  i) Force of repulsion
  ii) Force of attraction
• Formation of hydrogen molecule on the basis of valence bond theory (VBT)
• Overlap of atomic orbitals
• Limitation of VBT

• Steps considered in Hybridization
  i. Formation of excited state
  ii. Mixing and Recasting of orbitals
• Types of Hybridization and Geometry of Molecules

1. sp³ Hybridization
2. sp² Hybridization
3. sp Hybridization

• Formation of molecular orbitals
• Conditions for the combination of Atomic Orbitals
• Types of molecular orbitals
• Energy levels and electronic configuration
• Key ideas of MO theory
• MO description of simple diatomic Molecules

• Bond angle
• Bond Enthalpy
• Bond length
• Bond Order
• Polarity of a Covalent Bond

• Classical ideas of redox reactions
• Redox reaction in terms of electron transfer

• Rules to assign oxidation number
• Stock notation
• Redox reaction in terms of oxidation number

• Oxidation number method
• Ion electron method (Half reaction method)

Standard electrode potential

• Occurrence
• Position of hydrogen in the periodic table
• Isotopes of Hydrogen
• Preparation of dihydrogen
• Properties of dihydrogen
• Uses of dihydrogen

• Electronic configuration of elements of group 1 and group 2
• Trends in atomic and physical properties of elements of group 1 and group 2
• Chemical properties of elements of group 1 and group 2
• Diagonal Relationship
• Uses of elements of group 1 and group 2
• Biological importance of elements of group 1 and group 2

• Sodium Carbonate (washing soda) Na₂CO₃.10H₂O
• Sodium hydroxide (caustic soda) NaOH
• Calcium Carbonate (CaCO₃)
• Hydrogen peroxide (H₂O₂)
• Lithium aluminium hydride (LiAlH₄)

• Types of Intermolecular Forces

1. Dipole-dipole interactions
2. Ion-dipole interactions
3. Dipole-Induced dipole interaction
4. London Dispersion Force
5. Hydrogen Bonding

• Intermolecular Forces and Thermal energy

• Definition: Gas Equation
• Definition: Absolute Scale or Klevin Scale
• Law: Boyle's Law
• Law: Charle's Law

• Kinetic molecular theory of gases
• Postulates of kinetic molecular theory
• Kinetic gas equation
• Calculation of kinetic energy (K.E.)
• Molecular speeds
• Types of speed
  a) Most probable speed (u_mp)
  b) Average speed (u_av)
  c) Root mean square speed (u_r.m.s.)
• Relation between molecular speeds, temperature, and molecular mass

1. Ideal Gas
2. Real Gas

1. Vapour Pressure
2. Surface Tension
3. Viscosity

• Unbalanced forces
• Why does adsorption occur?
• Desorption
• Sorption

• Types of adsorption

1. Physical adsorption (Physisorption or van der Waals' adsorption)
2. Chemical adsorption (Chemisorption or activated adsorption)

• Difference between physisorption and chemisorption

• Factors affecting adsorption of gases on solids

1. Nature of the gas (adsorbate)
2. Nature of adsorbent
3. Surface area of the adsorbent
4. Temperature of the surface
5. Pressure of gas

• Adsorption isotherm
• Freundlich adsorption isotherm
• Langmuir adsorption isotherm

• Catalyst
• Catalysis and Theories of Catalysis
• Homogeneous Catalysis
• Heterogeneous Catalysis
• Inhibitors

• Important features of solid catalysts

1. Catalytic activity
2. Catalytic selectivity
3. Shape selective catalysis by zeolites

• Examples of colloids
• Classification of colloids
• Preparation of Colloids
• Purification of colloidal solution
• Properties of colloidal dispersions
• Methods to effect coagulation
• Emulsions
• Applications of colloids
• Dispersed phase and dispersion medium
• True solutions, colloids, and suspensions
• Types of colloidal systems

• Definition: Organic Chemistry
• Definition: Inorganic Chemistry

• Condensed formula
• Bond line formula or zig-zag formula
• Drawing the molecules in three dimensions

1. Wedge formula
2. Fischer projection formula or cross formula
3. Newman projection formula
4. Sawhorse or andiron or perspective formula

• Classification based on carbon skeleton
• Classification based on functional group
• Homologous Series

• Definition: Nomenclature
• Key Points: Nomenclature of Carbon Compounds

• Definition: Isomers

• Types of cleavage of covalent bond

1. Homolytic cleavage
2. Heterolytic cleavage

•  Types of reagent

1. Electrophiles
2. Nucleophiles

• Electronic effects in organic reaction
• Inductive effect
• Resonance structures
• Resonance Effect
• Electromeric effect
• Hyperconjugation

• Definition: Alkanes

• Definition: Alkynes

• Definition: Alkenes

• Benzene
• Structure of benzene
• Aromatic character (Huckel Rule)
• Preparation of aromatic compounds
• Physical properties of benzene
• Chemical properties of benzene
• Directive influence of a functional group in monosubstituted benzene
• Carcinogenicity and Toxicity

• Reactions in solutions

1. Mass percentage
2. Mole fraction
3. Molarity
4. Molality
5. Volume percentage

• Definition: Molecular Formula

• Food quality chemistry
  (i) Browning of cut fruit/vegetables
  (ii) Rancidity of oils and fats
  (iii) Saturated, unsaturated and trans fats
  (iv) Omega-3
  (v) Antioxidants as food additives

• Analgesics and antipyretics
• Antimicrobials 
  a) Antiseptics and disinfectants
  b) Antibiotics
• Traditional knowledge in medicine

• Crystalline Forms
• Diamond
• Uses of Diamond

• Solubility equilibria
• Relationship between solubility and solubility product
• Condition of precipitation

• Metallic conduction
• Electrolytic or ionic conduction
• Information provided by measurement of conductivities of solutions

• Electrolysis of molten NaCl
• Electrolysis of aqueous NaCl
• Quantitative aspects of electrolysis 

• Definition: Electrochemical Series

• Crystalline Forms
• Diamond
• Uses of Diamond

• Chlorine
• Hydrogen Chloride

• Compounds of Xenon

1. Xenon fluorides
   a) Xenon difluoride (XeF₂)
   b) Xenon tetrafluoride (XeF₄)
   c) Xenon hexafluoride (XeF₆)
2. Xenon oxides
   a) Xenon trioxide (XeO₃)
   b) Xenon tetraoxide (XeO₄)
   c) XeOF₄ and XeO₂F₂

• Preparation of potassium permaganate
• Chemical properties of KMnO₄
• Uses of KMnO₄
• K₂Cr₂O₇ : Preparation of potassium dichromate
• Chemical properties of K₂Cr₂O₇

• Key Points: Extraction of Metals

• Definition: Metallurgy
• Key Points: Metallurgy

• Lanthanoids and Actinoids

• Classification of carboxylic acids

1. Aliphatic carboxylic acids
   a) Mono-carboxylic acids
   b) Dicarboxylic acids
   c) Tricarboxylic acids
   d) Polycarboxylic acids
2. Aromatic carboxylic acids
   a) Aromatic mono-carboxylic acids
   b) Aromatic dicarboxylic acids