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

• Concept of Mole
• Quantities Related on Mole Concept and Their Formula
• Experiment

• Order of magnitude
• Significant figures
• Addition and subtraction of significant figures
• Multiplication and division of significant figures
• Rules for limiting the result to the required number of significant figures
• Rules for arithmetic operations with significant figures
• Rounding-off in the measurement

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

• 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

• Chemical bond
• Causes of chemical combination
  i) Tendency to acquire stability
  ii) Tendency to acquire noble gas configuration

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

• Ionic bond or Electrovalent bond
• Mechanism of formation of ionic bond
• Lattice enthalpy
• Factors affecting the formation of an ionic bond
  i) Low ionization enthalpy
  ii) High negative electron gain enthalpy
  iii) Large lattice enthalpy
• Characteristics of ionic or electrovalent compounds
• Difference between ionic bond and covalent bond
• Covalent character in ionic bond
• Fajan's rules

• Introduction of Covalent Bond
• Formation of Covalent Bonds
• Properties of Covalent Compounds

• 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

• The Gas Laws
• Standard variables for gas laws

1. The volume (V)
2. The pressure (P)
3. The temperature (T)

• Ideal behaviour of gases
• Gases law: Boyle's law, Charles' law, Gay Lussac's law, Avogadro's law
• Universal gas constant
• Ideal gas equation
• Ideal gas
• Nature of universal gas constant 'R'
• Values of universal gas constant 'R' in different units
• Combined gas equation
• Relation between density (d), molar mass (M), and pressure (P) of a gas
• Expression for Molar mass

• 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

• 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

• Common Naming System
• IUPAC Nomenclature

• Structural isomerism

1. Chain isomerism
2. Position isomerism
3. Functional group isomerism
4. Metamerism
5. Tautomerism

• Stereoisomerism
• Geometrical isomerism/Cis-trans isomerism
• Optical isomerism: enantiomers, dextrorotatory, laevorotatory, diastereomers, racemic mixture/ racemate, resolution.

• 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

• Isomerism in alkanes
• Conformations in alkanes
• Industrial preparation of alkanes
• Physical properties of alkanes
• Chemical properties of alkanes
• Uses of alkanes

• Isomerism in alkynes
• Preparation of alkynes
• Physical properties of alkynes
• Chemical properties of alkynes
• Uses of acetylene

• Isomerism in alkenes
• Preparation of alkenes
• Physical properties of alkenes
• Chemical properties of alkenes
• Uses of 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

• Percent composition and empirical 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

• Allotropy
• Allotropes of Carbon

• Crystalline solids
• Amorphous solids
• Isomorphism and polymorphism 

• Classification of crystalline solids

1. Molecular solids:
   a) Polar molecular solids
   b) Non-polar molecular solids
   c) Hydrogen-bonded molecular solids
2. Ionic Solids
3. Metallic solids
4. Covalent or Network Solids

• Structure and properties of diamond, graphite, and fullerene

• Crystal, lattice and basis
• Unit Cell
• Types of unit cell
• Crystal systems

• Number of particles in cubic unit cells
• Relationship between molar mass, density of the substance and unit cell edge length, is deduced in the following steps

• Close packed structures
• Coordination number in close packed structure
• Number of voids per atom in hcp and ccp

• Band theory
• Metals
• Insulators
• Semiconductors
• Extrinsic semiconductors and doping

• Diamagnetic solids
• Paramagnetic solids
• Ferromagnetism

1. Gaseous Solutions
2. Liquid Solutions
3. Solid Solutions

• Factors affecting solubility

1. Nature of solute and solvent
2. Effect of temperature on solubility
3. Effect of pressure on solubility

• Raoult’s law
• Ideal and nonideal solutions

• Raoult’s law for solutions of nonvolatile solutes
• Relative lowering of vapour pressure
• Molar mass of solute from vapour pressure lowering

• Boiling point elevation as a consequence of vapour pressure lowering
• Boiling point elevation and concentration of solute
• Molar mass of solute from boiling point elevation

• Freezing point depression as a consequence of vapour pressure lowering
• Freezing point depression and concentration of solute
• The molar mass of solute from freezing point depression

• Osmosis
• Osmotic pressure
• Isotonic, hypertonic and hypotonic solutions
• Osmotic pressure and concentration of solution
• Molar mass of solute from osmotic pressure
• Reverse osmosis

•  van’t Hoff factor(i)
• Modification of expressions of colligative properties
• van’t Hoff factor and degree of dissociation

• Strong electrolyte
• Weak electrolyte
• Degree of dissociation (∝)

• Arrhenius theory of acids and bases
• Bronsted - Lowry theory 
• Lewis theory

• Dissociation constant of weak acids and weak bases
• Ostwald's dilution law

• pH of a solution
• pH scale
• Relationship between pH and pOH
• Approximate pH values of some substances
• Acidity, basicity, and neutrality of aqueous solutions
• pK value
• Measurement of pH of a solution
• Indicators
• Titration curves

• Salts of strong acids and strong bases
• Salts of strong acids and weak bases
• Salts of weak acids and strong bases
• Salts of weak acids and weak bases

• Types of buffer solutions
• Buffer action
• Buffer capacity and buffer index
• Henderson - Hasselbalch equation
• Properties of buffer solution
• Applications of buffer solution

1. In biochemical system
2. Agriculture
3. Industry
4. Medicine
5. Analytical chemistry

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

Common ion effect and solubility

• System and surrounding
• Types of system
• Properties of system
• State functions
• Path Functions
• Thermodynamic equilibrium
• Process and its types

• Nature of work (W)
• Nature of heat (Q)
• Sign conventions of W and Q

• Free expansion
• Units of energy and work

Expression for the maximum work

• First law of thermodynamics
• Formulation of first law of thermodynamics
• First law of thermodynamics for various processes

1. Isothermal process
2. Adiabatic process
3. Isochoric process
4. Isobaric process

• Justification
• Mathematical expression
• Some useful conclusions are drawn from the law
• Limitations
• Expressions for the work done by an ideal gas under different conditions

• Enthalpy
• Relationship between ∆H and ∆U for chemical reactions
• Work done in chemical reaction

• Enthalpy of phase transition
• Enthalpy for the atomic / molecular change

• Enthalpy of chemical reaction (∆_rH)
• Exothermic and endothermic reactions
•  Standard enthalpy of reaction(∆_rH⁰)
• Thermochemical equation 
• Standard enthalpy of formation (∆_fH⁰)
• Standard enthalpy of reaction from standard enthalpies of formation
• Standard enthalpy of combustion (∆_cH⁰)
• Bond enthalpy
• Hess’s law of constant heat summation

• Energy and spontaneity
• Entropy
• Entropy and spontaneity (Second law of Thermodynamics)
•  Second law of thermodynamics
• Gibbs energy
• Gibbs energy and spontaneity
• Sponaneity and ∆H or ∆S
• Temperature of equilibrium
• Gibbs function and equilibrium constant

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

•  Conductivity (k)
• Molar conductivity (∧)
• Relation between k and ∧
• Variation of conductivity with concentration
•  Variation of molar conductivity with concentration
• Variation of molar conductivity with concentration
• Kohlrausch law of independent migration of ions
• Molar conductivity and degree of dissociation of weak electrolytes
• Measurement of conductivity

• Electrochemical reactions
• Electrodes
• Types of electrochemical cells

1. Galvanic cell
2. Electrolytic cells

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

• Salt bridge
• Formulation or short notation of galvanic cells
• Writing of cell reaction

• Electrode potential
• Cell potential or e.m.f.
• Difference between e.m.f. and potential difference
• Standard electrode potential
• Dependence of cell potential on concentration (Nernst equation)

• Gibbs energy of cell reactions and cell potential
•  Standard cell potential and equilibrium constant

•  Standard hydrogen electrode (SHE)

• Dry cell (Leclanche' cell)
• Lead storage battery (Lead accumulator)
• Nickel-Cadmium or NICAD storage cell
• Mercury battery

• Fuel cells
• Hydrogen-oxygen fuel cell
• Advantage and disadvantage of fuel cell

• Electrochemical series
• Convention used in the construction of electrochemical series
• Applications of electrochemical series

• Average rate of chemical reaction
• Instantaneous rate

• Rate law
• Writing the rate law
• Order of the reaction

• Elementary reaction
• Complex reactions
• Molecularity of reaction
• Order and molecularity of elementary reactions
• Rate determining step
• Reaction intermediate
• Differences between order and molecularity

• Collision between reactant molecules
• Activation
• Orientation of reactant molecules
• Potential energy barrier

• Arrhenius equation
• Graphical determination of activation energy
• Determination of activation energy
• Graphical description of effect of temperature

• Atomic properties of Group 16, 17 and 18 elements
• Physical properties of group 16, 17 and 18 elements

• Oxidation state
• Chemical Reactivity towards hydrogen
• Reactivity towards oxygen
• Reactivity towards halogens
• Reactivity towards metals

• Allotropy
• Allotropes of Carbon

• Oxoacids of sulfur
• Oxoacids of halogens

• Dioxygen
• Simple Oxides
• Ozone

• 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

• Atomic and ionic radii 
• Ionisation Enthalpy
• Metallic character
• Magnetic Properties
• Colour
• Catalytic Properties
• Formation of interstitial compounds
• Formation of Alloys

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

• Metallurgy
• Extraction of Iron from Haematite ore using Blast furnace

• Introduction
• Metallurgical Process

• Lanthanoids and Actinoids

• Occurrence and characteristics of transition metals

• Electronic configuration
• Oxidation state
• Colour and Spectra
• Atomic and ionic radii (Lanthanoid Contraction)

• Monodentate ligands
• Polydentate ligands
• Ambidentate ligand

• Coordination sphere
• Charge number of complex ion and oxidation state of metal ion
• Coordination number (C.N.) of central metal ion
• Double salt and coordination complex
• Werner theory of coordination complexes

• Classification on the basis of types of ligands
• Classification on the basis of charge on the complex

• Stereoisomers
• Structural isomers (Constitutional isomers)
• Optical Isomerism

• Stability of coordination compounds
• Factors which govern stability of the complex

1. Charge to size ratio of the metal ion
2. Nature of the ligand
3. Stability of chelates

• Valence bond theory (VBT)
• Octahedral, complexes
• Tetrahedral complex
• Square planar complex
•  Limitations of VBT
• Crystal Field theory (CFT)
• Factors affecting Crystal Field Splitting parameter (∆₀)
• Colour of the octahedral complexes
• Tetrahedral complexes

• Classification of monohalogen compounds

•  From alcohol
• From hydrocarbon
• Halogen exchange
• Electrophilic substitution
• Sandmeyer's reaction

• Nature of intermolecular forces
• Boiling point
• Solubility

• Chiral atom and molecular chirality
• Plane polarized light
• Optical activity
• Enantiomers
• Representation of configuration of molecules

• Laboratory test of haloalkanes
• Nucleophilic substitution reactions of haloalkanes
• Mechanism of S_N reaction
• Factors influencing S_N1 and S_N2 mechanism
• Elimination reaction : Dehydrohalogenation

• Dichloromethane/methylene chloride (CH₂Cl₂)
• Chloroform/trichloromethane (CHCl₃)
• Carbon tetrachloride/tetrachloromethane (CCl₄)
• Idoform or triiodomethane (CHI₃)
• Freons
• Dichlorodiphenyltrichloroethane (DDT)

• Reaction of haloarenes

• Alcohols - Mono, di, tri and polyhydric compounds
• Phenols - Mono, Di and trihydric phenols
• Ethers - simple or symmetrical, mixed or unsymmetrical

• Nomenclature of aldehydes and carboxylic acid
• Trivial and IUPAC names of ketones

1. By oxidation of alcohols
2. By dehydrogenation of alcohols
3. From hydrocarbons
   (i) By ozonolysis of alkenes
   (ii) By hydration of alkynes

• From nitriles and amides
• From acyl chloride and anhydrides
• From esters
• From alkyl benzene
• From alkenes
• From Grignard reagent

• Reactivity of aldehydes and ketones

• Laboratory tests for aldehydes and ketones
• Chemical reactions of aldehydes and ketones with nucleophile
• Oxidation and reduction reactions of aldehydes and ketones
• Electrophilic substitution reactions

• Acidic character of carboxylic acids
• Laboratory tests for carboxyl (-COOH) group
• Formation of acyl chloride
• Reaction with ammonia
• Formation of acid anhydride
• Decarboxylation of carboxylic acids
• Reduction of carboxylic acids

• 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

• Classification of amines

1. Aliphatic amines
2. Aromatic amines

• Common names
• IUPAC names

• Basic strength of aliphatic amines
• Basicity of arylamines

• Reactions involving displacement of diazo group
• Reactions involving retention of diazo group: (Coupling reactions)

• Classification of polymers on the basis of source or origin
• Classification of polymers on the basis of structure
• Classification of polymers on the basis of mode of polymerization
• Classification of polymers on the basis of intermolecular forces
• Classification of polymers on the basis of type of different monomers
• Classification of polymers on the basis of biodegradability

• Poly β-hydroxybutyrate – co-β-hydroxy valerate (PHBV)
• Nylon 2– nylon 6
• Biodegradable and non-biodegradable polymers

• Case Study - Indira Gandhi Canal (Nahar) Command Area
• Measures for Promotion of Sustainable
  Development

• Prevention of waste or by products
• Atom economy
• Less hazardous chemical synthesis
• Desigining Safer Chemicals
• Use Safer solvent and auxilaries
• Design for energy efficiency
• Use of renewable feedstocks
• Reduce derivatives : [Minimization of steps]
• Use of catalysis
• Design for degradation
• Real-time Analysis Pollution Prevention
• Safer chemistry for Accident prevention

• Colour
• Surface area
• Catalytic activity
• Mechanical properties
• Electrical conductivity

• Wet chemical synthesis of Nanomaterials
• Analysis or characterization of nanomaterials
• Photographs of instruments