MHT CET Chemistry Syllabus

Chemistry syllabus — full chapter and topic list

Expand any chapter to see its topics and sub-topics. This is the whole examinable outline for Chemistry in MHT CET, not a summary of it.

1. 1

   Physical Chemistry I

   3 topics

   • Solid State
     • Unit cells and crystal lattices
     • Packing efficiency and density of unit cell
     • Point defects and properties of solids
   • Solutions
     • Concentration terms and Raoult's law
     • Colligative properties and abnormal molar mass
     • Van't Hoff factor
   • States of Matter: Gases and Liquids
     • Gas laws and ideal gas equation
     • Kinetic molecular theory and real gases
2. 2

   Physical Chemistry II

   4 topics

   • Chemical Thermodynamics
     • First law, enthalpy and Hess's law
     • Entropy, Gibbs free energy and spontaneity
   • Ionic Equilibria
     • Acids, bases and Ostwald's dilution law
     • pH, buffer solutions and solubility product
   • Chemical Kinetics
     • Rate of reaction and order, molecularity
     • Integrated rate laws and half-life
     • Arrhenius equation and collision theory
   • Electrochemistry
     • Conductance and Kohlrausch's law
     • Electrochemical cells and Nernst equation
     • Batteries, fuel cells and corrosion
3. 3

   Inorganic Chemistry

   4 topics

   • Elements of Groups 16, 17 and 18
     • Trends in p-block elements
     • Oxoacids and interhalogen compounds
     • Noble gas compounds
   • Transition and Inner Transition Elements
     • Electronic configuration and oxidation states
     • Lanthanoid contraction and properties
   • Coordination Compounds
     • Werner's theory and nomenclature
     • Isomerism in coordination compounds
     • Valence bond and crystal field theory
   • Chemistry of Metals and Extraction
     • Occurrence and concentration of ores
     • Thermodynamics of extraction, Ellingham diagram
4. 4

   Organic Chemistry Fundamentals

   3 topics

   • Basic Principles and Hydrocarbons
     • IUPAC nomenclature and isomerism
     • Electronic effects: inductive, resonance, hyperconjugation
     • Reaction intermediates and mechanisms
   • Halogen Derivatives
     • Haloalkanes and haloarenes
     • SN1 and SN2 mechanisms
   • Alcohols, Phenols and Ethers
     • Preparation and properties of alcohols
     • Acidic nature and reactions of phenols
5. 5

   Organic Chemistry: Functional Groups and Biomolecules

   4 topics

   • Aldehydes, Ketones and Carboxylic Acids
     • Nucleophilic addition reactions
     • Aldol and cannizzaro reactions
     • Acidity of carboxylic acids
   • Amines and Nitrogen Compounds
     • Classification, basicity and preparation
     • Diazonium salts and their reactions
   • Biomolecules
     • Carbohydrates and proteins
     • Nucleic acids, enzymes and vitamins
   • Polymers and Green Chemistry
     • Classification and methods of polymerisation
     • Addition and condensation polymers

Chemistry flashcards for MHT CET

21 of 60 cards from the Chemistry deck — real questions with worked answers.

1. In a face-centered cubic (fcc) unit cell, how many atoms are present per unit cell?

   4 atoms (8 corners x 1/8 + 6 faces x 1/2 = 1 + 3 = 4).

2. What is the packing efficiency of fcc/ccp and hcp structures versus bcc?

   fcc/ccp and hcp = 74%; bcc = 68%; simple cubic = 52.4%.

3. Define a Schottky defect and state its effect on density.

   A point defect where equal numbers of cations and anions are missing from the lattice; it decreases the density of the crystal. Common in ionic solids with high coordination number (e.g., NaCl).

4. Define a Frenkel defect and its effect on density.

   A defect where an ion (usually the smaller cation) is displaced from its lattice site to an interstitial site; density remains unchanged. Seen in ZnS, AgCl, AgBr.

5. State Raoult's law for a solution of two volatile liquids.

   The partial vapour pressure of each component is proportional to its mole fraction: p_A = p_A° x_A and p_B = p_B° x_B; total pressure p = p_A° x_A + p_B° x_B.

6. Write the formula for elevation in boiling point and depression in freezing point.

   ΔT_b = i·K_b·m and ΔT_f = i·K_f·m, where i = van't Hoff factor, K = molal constant, m = molality.

7. Write the equation for osmotic pressure and define the colligative property it represents.

   π = i·C·R·T (or πV = nRT). Osmotic pressure is a colligative property depending on the number of solute particles, not their identity.

8. What is the van't Hoff factor (i) and its value for NaCl, BaCl2, and a non-electrolyte (assuming complete dissociation)?

   i = observed number of particles / formula units dissolved. NaCl: i = 2; BaCl2: i = 3; non-electrolyte (e.g., glucose): i = 1.

9. State the four assumptions / consequence: write the ideal gas equation and the value of R in SI units.

   PV = nRT; R = 8.314 J K⁻¹ mol⁻¹ (or 0.0821 L atm K⁻¹ mol⁻¹).

10. Write the van der Waals equation for n moles of a real gas.

    (P + an²/V²)(V − nb) = nRT, where 'a' corrects for intermolecular attraction and 'b' for molecular volume.

11. Define critical temperature (T_c) of a gas.

    The temperature above which a gas cannot be liquefied no matter how much pressure is applied. The corresponding pressure is the critical pressure.

12. State the first law of thermodynamics with its mathematical expression.

    Energy can neither be created nor destroyed: ΔU = q + w, where ΔU = change in internal energy, q = heat absorbed, w = work done on the system.

13. Define enthalpy (H) and relate ΔH to ΔU.

    H = U + PV. At constant pressure ΔH = ΔU + ΔngRT, where Δng = moles of gaseous products − reactants.

14. State Hess's law of constant heat summation.

    The total enthalpy change of a reaction is the same whether it occurs in one step or several steps, depending only on initial and final states.

15. Write the Gibbs free energy equation and the criterion for a spontaneous process.

    ΔG = ΔH − TΔS. A process is spontaneous when ΔG < 0, at equilibrium ΔG = 0, non-spontaneous when ΔG > 0.

16. Define entropy and give the sign of ΔS for melting of ice.

    Entropy (S) is a measure of randomness/disorder of a system. For melting of ice, ΔS > 0 (disorder increases).

17. What is the ionic product of water (Kw) at 25°C, and how are pH and pOH related?

    Kw = [H⁺][OH⁻] = 1.0 x 10⁻¹⁴ at 25°C; pH + pOH = 14.

18. State Ostwald's dilution law for a weak electrolyte.

    For a weak electrolyte, Ka = Cα²/(1−α); for small α, α ≈ √(Ka/C). Degree of dissociation increases on dilution.

19. Define a buffer solution and write the Henderson-Hasselbalch equation for an acidic buffer.

    A buffer resists change in pH on adding small amounts of acid or base. pH = pKa + log([salt]/[acid]).

20. What is the common ion effect?

    The suppression of dissociation (or solubility) of a weak electrolyte (or sparingly soluble salt) by adding a strong electrolyte having a common ion.

21. Define solubility product (Ksp) for AB2 type salt and the condition for precipitation.

    For AB2 → A²⁺ + 2B⁻, Ksp = [A²⁺][B⁻]². Precipitation occurs when ionic product (Qsp) > Ksp.

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