INC CET / BSc Nursing Entrance 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 INC CET / BSc Nursing Entrance, not a summary of it.

1. 1

   Physical Chemistry

   6 topics

   • Atomic Structure
     • Bohr model and quantum numbers
     • Electronic configuration and orbitals
     • Aufbau principle, Hund's rule, Pauli exclusion
   • States of Matter
     • Gas laws and ideal gas equation
     • Liquid and solid states
   • Chemical Bonding and Molecular Structure
     • Ionic, covalent and coordinate bonds
     • VSEPR theory and molecular geometry
     • Hybridisation and hydrogen bonding
   • Thermodynamics and Equilibrium
     • Enthalpy, entropy and Gibbs free energy
     • Chemical equilibrium and Le Chatelier's principle
     • Ionic equilibrium, pH and buffers
   • Solutions and Electrochemistry
     • Concentration terms and colligative properties
     • Redox reactions and electrochemical cells
     • Electrolysis and conductance
   • Chemical Kinetics
     • Rate of reaction and order
     • Factors affecting reaction rate
2. 2

   Inorganic Chemistry

   4 topics

   • Periodic Classification
     • Modern periodic law and table
     • Periodic trends: atomic radius, ionisation energy, electronegativity
   • Hydrogen and s-Block Elements
     • Properties of hydrogen and water
     • Alkali and alkaline earth metals
   • p-Block Elements
     • Group 13 to 18 trends
     • Important compounds and uses
   • Metallurgy and d-Block Elements
     • Principles of metal extraction
     • Transition elements and their properties
3. 3

   Organic Chemistry

   5 topics

   • Basic Concepts of Organic Chemistry
     • Classification and IUPAC nomenclature
     • Isomerism: structural and stereo
     • Inductive, resonance and hyperconjugation effects
   • Hydrocarbons
     • Alkanes, alkenes and alkynes
     • Aromatic hydrocarbons and benzene
   • Oxygen-Containing Functional Groups
     • Alcohols, phenols and ethers
     • Aldehydes, ketones and carboxylic acids
   • Nitrogen Compounds and Biomolecules
     • Amines and their reactions
     • Carbohydrates, proteins and vitamins
   • Chemistry in Everyday Life
     • Drugs, medicines and antibiotics
     • Soaps, detergents and food chemicals

Chemistry flashcards for INC CET / BSc Nursing Entrance

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

1. What is the maximum number of electrons that can occupy a shell with principal quantum number n?

   2n^2 electrons.

2. State the Heisenberg uncertainty principle and its mathematical form.

   It is impossible to determine simultaneously the exact position and momentum of an electron. Mathematically: Δx · Δp ≥ h/4π.

3. What do the four quantum numbers (n, l, m, s) describe about an electron?

   n = principal (shell/energy & size); l = azimuthal (subshell/shape); m = magnetic (orbital orientation); s = spin (+1/2 or −1/2).

4. State Hund's rule of maximum multiplicity.

   Electrons fill degenerate (equal-energy) orbitals singly with parallel spins before any orbital is doubly occupied.

5. What is the de Broglie wavelength equation for a moving particle?

   λ = h/mv (or λ = h/p), where h is Planck's constant, m mass, v velocity.

6. State Aufbau principle and the n+l rule for orbital filling order.

   Orbitals fill in order of increasing energy. Lower n+l fills first; for equal n+l, the orbital with lower n fills first (e.g., 4s before 3d).

7. Define absolute zero in Kelvin and degrees Celsius.

   0 K = −273.15 °C, the temperature at which molecular motion theoretically ceases.

8. State the ideal gas equation and identify each term.

   PV = nRT, where P = pressure, V = volume, n = moles, R = gas constant (0.0821 L·atm·mol⁻¹·K⁻¹), T = absolute temperature.

9. State Boyle's law and Charles's law.

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

10. What is Dalton's law of partial pressures?

    The total pressure of a mixture of non-reacting gases equals the sum of the partial pressures of the individual gases: P_total = P₁ + P₂ + P₃ + ...

11. State the VSEPR-predicted shapes and bond angles for 2, 3, and 4 bonding electron pairs.

    2 pairs: linear, 180°; 3 pairs: trigonal planar, 120°; 4 pairs: tetrahedral, 109.5°.

12. Define a sigma (σ) bond and a pi (π) bond.

    A σ bond forms by head-on (axial) overlap of orbitals; a π bond forms by sideways (lateral) overlap of p orbitals. Single bonds are σ; double/triple bonds have one σ plus π bonds.

13. What hybridization corresponds to linear, trigonal planar, and tetrahedral geometries?

    sp = linear (180°); sp² = trigonal planar (120°); sp³ = tetrahedral (109.5°).

14. Define electronegativity and name the most electronegative element.

    Electronegativity is the tendency of an atom to attract a shared pair of electrons in a bond. Fluorine is the most electronegative element.

15. State the octet rule.

    Atoms tend to gain, lose, or share electrons to achieve a stable outer shell of eight electrons (a noble-gas configuration).

16. State the first law of thermodynamics.

    Energy can neither be created nor destroyed. ΔU = q + w (change in internal energy = heat added + work done on the system).

17. Define enthalpy (H) and give the expression for enthalpy change.

    Enthalpy H = U + PV. At constant pressure, ΔH = q_p (heat exchanged); ΔH < 0 is exothermic, ΔH > 0 is endothermic.

18. State the relationship linking Gibbs free energy, enthalpy, and entropy, and the condition for spontaneity.

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

19. State Le Chatelier's principle.

    If a system at equilibrium is disturbed by a change in concentration, pressure, or temperature, the equilibrium shifts to counteract (oppose) that change.

20. 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.

21. Define molarity (M) and give its formula.

    Molarity is moles of solute per litre of solution: M = moles of solute / volume of solution (in L).

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