Military Nursing Service (MNS) 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 Military Nursing Service (MNS) Entrance, not a summary of it.

1. 1

   Physical Chemistry

   6 topics

   • Atomic Structure
     • Quantum numbers and orbitals
     • Electronic configuration and Aufbau principle
   • States of Matter
     • Gaseous state and gas laws
     • Liquid and solid states
   • Chemical Thermodynamics
     • Enthalpy, entropy and Gibbs energy
     • Hess's law
   • Equilibrium
     • Chemical equilibrium and Le Chatelier's principle
     • Ionic equilibrium, pH and buffers
   • Electrochemistry
     • Electrochemical cells and EMF
     • Nernst equation and conductance
   • Chemical Kinetics
     • Rate of reaction and order
     • Factors affecting reaction rate
2. 2

   Inorganic Chemistry

   5 topics

   • Periodic Table and Periodicity
     • Modern periodic law and trends
     • Ionization energy, electronegativity, atomic radii
   • Chemical Bonding
     • Ionic, covalent and coordinate bonds
     • VSEPR theory and hybridization
     • Molecular orbital theory
   • s-Block and p-Block Elements
     • Alkali and alkaline earth metals
     • Group properties and anomalous behaviour
   • d and f Block Elements
     • Transition elements and properties
     • Coordination compounds and isomerism
   • Metallurgy and Extraction
     • Principles of metallurgical operations
3. 3

   Organic Chemistry

   4 topics

   • Basic Concepts of Organic Chemistry
     • IUPAC nomenclature
     • Isomerism and reaction mechanisms
     • Electronic effects (inductive, resonance, hyperconjugation)
   • Hydrocarbons
     • Alkanes, alkenes and alkynes
     • Aromatic hydrocarbons and benzene
   • Functional Group Chemistry
     • Haloalkanes and haloarenes
     • Alcohols, phenols and ethers
     • Aldehydes, ketones and carboxylic acids
     • Amines and nitrogen compounds
   • Biomolecules and Polymers
     • Carbohydrates, proteins and vitamins
     • Natural and synthetic polymers
4. 4

   Environmental and Applied Chemistry

   3 topics

   • Environmental Chemistry
     • Air and water pollution
     • Green chemistry concepts
   • Chemistry in Everyday Life
     • Drugs and medicines
     • Soaps, detergents and food chemistry
   • Surface Chemistry
     • Adsorption and catalysis
     • Colloids and emulsions

Chemistry flashcards for Military Nursing Service (MNS) Entrance

21 of 50 cards from the Chemistry deck — real questions with worked answers.

1. What are the four quantum numbers and what does each describe?

   Principal (n) — energy/shell size; Azimuthal/angular (l) — subshell shape (s,p,d,f); Magnetic (m_l) — orbital orientation; Spin (m_s) — electron spin (+1/2 or -1/2).

2. State Heisenberg's uncertainty principle and its mathematical form.

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

3. What is the Aufbau principle?

   Electrons fill atomic orbitals in order of increasing energy (lowest energy first), following the (n+l) rule.

4. State Hund's rule of maximum multiplicity.

   Electrons fill degenerate orbitals singly with parallel spins before any orbital is doubly occupied, maximizing total spin.

5. What is the Pauli exclusion principle?

   No two electrons in an atom can have the same set of all four quantum numbers; an orbital holds at most two electrons with opposite spins.

6. Write the de Broglie wavelength equation.

   λ = h/mv = h/p, relating a particle's wavelength to its momentum.

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

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

8. State 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 + ...

9. What is the difference between real gases and ideal gases?

   Ideal gases obey PV=nRT at all conditions, have no intermolecular forces and negligible molecular volume. Real gases deviate, especially at high pressure/low temperature, and follow the van der Waals equation.

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. State the first law of thermodynamics with its equation.

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

12. Define enthalpy (H) and write ΔH in terms of internal energy.

    Enthalpy H = U + PV (heat content at constant pressure). ΔH = ΔU + PΔV (or ΔH = ΔU + Δn_gRT for gaseous reactions).

13. 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.

14. What does the second law of thermodynamics state about entropy?

    The entropy of an isolated system always increases for a spontaneous process; total entropy of the universe tends toward a maximum (ΔS_universe > 0 for spontaneous change).

15. Write the Gibbs free energy equation and the criterion for spontaneity.

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

16. 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 (partially oppose) that change.

17. Write the relationship between ΔG° and the equilibrium constant K.

    ΔG° = −RT ln K.

18. Define pH and pOH and give their relationship at 25°C.

    pH = −log[H⁺], pOH = −log[OH⁻]. At 25°C, pH + pOH = 14.

19. What is a buffer solution and name its two types?

    A solution that resists change in pH on adding small amounts of acid or base. Types: acidic buffer (weak acid + its salt, e.g. CH₃COOH/CH₃COONa) and basic buffer (weak base + its salt, e.g. NH₄OH/NH₄Cl).

20. State the Henderson–Hasselbalch equation for an acidic buffer.

    pH = pKa + log([salt]/[acid]).

21. Define oxidation and reduction in terms of electrons.

    Oxidation is loss of electrons (increase in oxidation state); reduction is gain of electrons (decrease in oxidation state). Remember OIL RIG.

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