RUHS / State 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 RUHS / State Nursing Entrance, not a summary of it.

1. 1

   Physical Chemistry

   5 topics

   • Atomic Structure
     • Bohr model and quantum numbers
     • Electronic configuration and orbitals
   • States of Matter
     • Gas laws and ideal gas behaviour
     • Liquids and intermolecular forces
   • Chemical Bonding
     • Ionic and covalent bonds
     • VSEPR theory and molecular geometry
     • Hybridization and bond polarity
   • Thermodynamics and Equilibrium
     • Enthalpy, entropy and Gibbs energy
     • Chemical equilibrium and Le Chatelier principle
     • Ionic equilibrium, pH and buffers
   • Electrochemistry and Kinetics
     • Electrolysis and electrochemical cells
     • Rate of reaction and order
2. 2

   Inorganic Chemistry

   4 topics

   • Periodic Classification
     • Modern periodic law and trends
     • Atomic radius, ionization energy, electronegativity
   • s-Block and p-Block Elements
     • Alkali and alkaline earth metals
     • Group 13 to 18 elements and properties
   • d-Block and Coordination Compounds
     • Transition elements and properties
     • Coordination compounds and nomenclature
   • Metallurgy and Hydrogen
     • Extraction of metals
     • Hydrogen and water chemistry
3. 3

   Organic Chemistry

   4 topics

   • Basics of Organic Chemistry
     • IUPAC nomenclature
     • Isomerism and electronic effects
     • Reaction intermediates and mechanisms
   • Hydrocarbons
     • Alkanes, alkenes and alkynes
     • Aromatic hydrocarbons and benzene
   • Functional Group Chemistry
     • Alcohols, phenols and ethers
     • Aldehydes, ketones and carboxylic acids
     • Amines and nitrogen compounds
   • Biomolecules and Polymers
     • Carbohydrates, proteins and lipids
     • Polymers and chemistry in everyday life

Chemistry flashcards for RUHS / State Nursing Entrance

21 of 53 cards from the Chemistry deck — real questions with worked answers.

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

   2n^2 electrons.

2. State the Aufbau principle for filling atomic orbitals.

   Electrons fill orbitals in order of increasing energy (lowest energy first), following the (n+l) rule; for equal (n+l), the lower n fills first.

3. What does Hund's rule of maximum multiplicity state?

   Electrons occupy degenerate orbitals singly with parallel spins before any orbital is doubly occupied, minimizing electron repulsion.

4. Write the de Broglie equation relating wavelength to momentum.

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

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

   Principal (n) = energy/shell; Azimuthal (l) = subshell/shape; Magnetic (m_l) = orbital orientation; Spin (m_s) = electron spin (+1/2 or -1/2).

6. State Heisenberg's uncertainty principle as a formula.

   Delta x . Delta p >= h/4pi; position and momentum cannot both be measured exactly at the same time.

7. Write the combined gas law and the ideal gas equation.

   Combined: P1V1/T1 = P2V2/T2. Ideal gas: PV = nRT.

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

   Boyle's law: at constant T, P is inversely proportional to V (PV = constant). Charles's law: at constant P, V is directly proportional to T (V/T = constant).

9. What are the postulates conditions under which real gases behave most ideally?

   Real gases behave most ideally at high temperature and low pressure (when intermolecular forces and molecular volume are negligible).

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

    (P + an^2/V^2)(V - nb) = nRT, where 'a' corrects for intermolecular attraction and 'b' for molecular volume.

11. What is an ionic bond and give one example?

    An electrostatic attraction formed by transfer of electrons from a metal to a non-metal, producing cations and anions; e.g., NaCl.

12. What is a covalent bond and how does a coordinate (dative) bond differ?

    A covalent bond shares an electron pair contributed by both atoms; in a coordinate bond both shared electrons come from a single atom (e.g., NH4+).

13. According to VSEPR theory, what shape and bond angle does a molecule with 4 bonding pairs and no lone pairs have?

    Tetrahedral shape with bond angles of 109.5 degrees (e.g., CH4).

14. State the hybridization, shape and bond angle of BF3.

    sp2 hybridization, trigonal planar shape, 120 degree bond angles.

15. What is hydrogen bonding and name a substance where it strongly affects properties?

    An electrostatic attraction between H bonded to a highly electronegative atom (F, O, N) and a lone pair on another such atom; e.g., water (high boiling point).

16. State the first law of thermodynamics as an equation.

    Delta U = q + w, where Delta U is change in internal energy, q is heat added, and w is work done on the system.

17. Define enthalpy and write the relation between enthalpy change and internal energy change.

    Enthalpy H = U + PV; at constant pressure Delta H = Delta U + P.Delta V (= Delta U + Delta n_g RT for gases).

18. 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, because enthalpy is a state function.

19. Write the Gibbs free energy equation and the condition for spontaneity.

    Delta G = Delta H - T.Delta S; a process is spontaneous when Delta G < 0.

20. Write the expression for the equilibrium constant Kc for the reaction aA + bB <=> cC + dD.

    Kc = [C]^c [D]^d / ([A]^a [B]^b).

21. 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 the change.

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