CFTRI M.Sc. (Food Technology) 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 CFTRI M.Sc. (Food Technology), not a summary of it.

1. 1

   The Gas Laws

   1 topic

   • Properties of Gases
2. 2

   Colligative Properties

   overview

   Examined as a single unit within Chemistry — no further topic split in the official outline.

3. 3

   Thermochemistry

   overview

   Examined as a single unit within Chemistry — no further topic split in the official outline.

4. 4

   Chemical Bonds

   5 topics

   • Chemical Equilibria
   • Chemical Kinetics
   • Concept of pH and Buffer
   • Molecular Orbital Theory
   • Chemical Bonds and Forces
5. 5

   Periodic Table

   overview

   Examined as a single unit within Chemistry — no further topic split in the official outline.

6. 6

   Aliphatic and Aromatic Hydrocarbons

   overview

   Examined as a single unit within Chemistry — no further topic split in the official outline.

7. 7

   Organic Substitution Reactions

   2 topics

   • Electrophilic Reactions
   • Nucleophilic Reactions
8. 8

   Isomerism

   2 topics

   • Structural Isomers
   • Optical Isomers
9. 9

   Food Chemistry

   3 topics

   • Composition of Foods
   • Minerals in Foods
   • Water Activity in Foods
10. 10

    Carbohydrates

    7 topics

    • Mono and Disaccharides
    • Reducing and Non-Reducing Sugars
    • Mutarotation
    • Starch
    • Cellulose
    • Pectins
    • Plant Acids
11. 11

    Proteins

    6 topics

    • Primary Structure of Proteins
    • Secondary Structure of Proteins
    • Tertiary Structure of Proteins
    • Protein Denaturation
    • Peptide Bond
    • Amino Acids

Chemistry flashcards for CFTRI M.Sc. (Food Technology)

21 of 51 cards from the Chemistry deck — real questions with worked answers.

1. State the ideal gas equation and define each term.

   PV = nRT, where P = pressure, V = volume, n = number of moles, R = universal gas constant (8.314 J/mol·K), and T = absolute temperature (K).

2. What do Boyle's Law and Charles's Law state for an ideal gas?

   Boyle's Law: at constant temperature, V ∝ 1/P (PV = constant). Charles's Law: at constant pressure, V ∝ T (V/T = constant).

3. Under what conditions do real gases deviate most from ideal behaviour?

   At high pressure and low temperature, because molecular volume and intermolecular attractions become significant (described by the van der Waals equation).

4. State Le Chatelier's principle.

   If a system at equilibrium is disturbed by a change in concentration, pressure, or temperature, the equilibrium shifts in the direction that counteracts the disturbance.

5. Write the equilibrium constant expression Kc for the reaction aA + bB ⇌ cC + dD.

   Kc = ([C]^c [D]^d) / ([A]^a [B]^b), using equilibrium molar concentrations.

6. How is Kp related to Kc for a gaseous equilibrium?

   Kp = Kc(RT)^Δn, where Δn = (moles of gaseous products) − (moles of gaseous reactants).

7. Define the rate law and order of a reaction.

   The rate law expresses reaction rate as rate = k[A]^m[B]^n; the overall order is the sum of the exponents (m + n), determined experimentally.

8. Give the integrated rate equation and half-life expression for a first-order reaction.

   ln[A] = ln[A]₀ − kt (or k = (2.303/t)log([A]₀/[A])); half-life t₁/₂ = 0.693/k, independent of initial concentration.

9. State the Arrhenius equation and the meaning of activation energy.

   k = A·e^(−Ea/RT), where A = pre-exponential factor, Ea = activation energy (minimum energy needed for reaction), R = gas constant, T = temperature.

10. Define pH and pOH and give the relation between them at 25°C.

    pH = −log[H⁺] and pOH = −log[OH⁻]; at 25°C, pH + pOH = 14 (since Kw = [H⁺][OH⁻] = 1×10⁻¹⁴).

11. What is a buffer solution and what are its two types?

    A buffer resists pH change on adding small amounts of acid or base. Types: acidic buffer (weak acid + its salt, e.g. acetic acid/sodium acetate) and basic buffer (weak base + its salt, e.g. NH₄OH/NH₄Cl).

12. Write the Henderson–Hasselbalch equation for an acidic buffer.

    pH = pKa + log([salt]/[acid]) (i.e. pH = pKa + log([conjugate base]/[acid])).

13. What are the key postulates of Molecular Orbital Theory?

    Atomic orbitals combine to form an equal number of molecular orbitals (bonding and antibonding); electrons fill MOs following Aufbau, Pauli, and Hund's rules; bonding MOs are lower in energy than the parent atomic orbitals.

14. Define bond order in MO theory and what it predicts.

    Bond order = ½(number of bonding electrons − number of antibonding electrons). It predicts bond strength/stability; a bond order of zero means the molecule does not exist.

15. Why is the O₂ molecule paramagnetic according to MO theory?

    Its molecular orbital configuration places two unpaired electrons in the degenerate π* (antibonding) orbitals, giving O₂ paramagnetism.

16. Compare ionic, covalent, and metallic bonds.

    Ionic: electrostatic attraction between transferred-electron cations and anions. Covalent: sharing of electron pairs between atoms. Metallic: attraction between metal cations and a delocalized 'sea' of electrons.

17. What are the main types of intermolecular (van der Waals) forces, weakest to strongest?

    London dispersion forces (weakest) < dipole–dipole forces < hydrogen bonding (strongest among van der Waals interactions).

18. Define an electrophile and give two examples.

    An electrophile is an electron-deficient species that accepts an electron pair. Examples: NO₂⁺, H⁺, AlCl₃, carbocations, Br⁺.

19. Outline the general mechanism of electrophilic aromatic substitution.

    The electrophile attacks the aromatic ring forming a resonance-stabilized arenium ion (sigma complex/carbocation), then loss of a proton restores aromaticity. Example: nitration, halogenation.

20. Define a nucleophile and give two examples.

    A nucleophile is an electron-rich species that donates an electron pair to form a bond. Examples: OH⁻, CN⁻, NH₃, H₂O, alkoxides.

21. Compare SN1 and SN2 nucleophilic substitution mechanisms.

    SN1: two-step, first-order (rate = k[substrate]), carbocation intermediate, favoured by tertiary substrates, gives racemization. SN2: one-step, second-order (rate = k[substrate][nucleophile]), backside attack, favoured by primary substrates, gives inversion of configuration.

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