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RUHS / State Nursing Entrance Chemistry Syllabus

The Chemistry syllabus for RUHS / State Nursing Entrance in full: 3 chapters, 13 topics and 30 sub-topics, every one listed below, plus 53 Chemistry flashcards with answers.

3Chapters
13Topics
30Sub-topics
53Flashcards

Chemistry syllabus: all 3 chapters

Expand any chapter to see its topics and sub-topics.

  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. 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. 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

RUHS / State Nursing Entrance Chemistry flashcards — 53 questions with 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).

Show the other 33 Chemistry flashcards

  1. 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.

  2. Define pH and give the pH of a neutral aqueous solution at 25 C.

    pH = -log[H+]; a neutral solution at 25 C has pH = 7.

  3. What is the relation between cell potential and Gibbs free energy?

    Delta G = -nFE_cell, where n is moles of electrons, F is the Faraday constant, and E_cell is cell potential.

  4. Write the Nernst equation for a cell at 298 K (using log base 10).

    E_cell = E0_cell - (0.0591/n) log Q, where Q is the reaction quotient.

  5. What happens at the anode and cathode in an electrochemical (galvanic) cell?

    Oxidation occurs at the anode (negative terminal); reduction occurs at the cathode (positive terminal).

  6. State Faraday's first law of electrolysis.

    The mass of substance deposited or liberated at an electrode is directly proportional to the quantity of electricity passed (m proportional to Q = It).

  7. What is the order of a reaction and how does it differ from molecularity?

    Order = sum of powers of concentration terms in the experimental rate law (can be fractional/zero); molecularity = number of reacting species in an elementary step (always a whole number).

  8. Write the integrated rate law and half-life expression for a first-order reaction.

    k = (2.303/t) log([A0]/[A]); half-life t1/2 = 0.693/k (independent of initial concentration).

  9. State the Arrhenius equation relating rate constant to temperature.

    k = A e^(-Ea/RT), where A is the frequency factor and Ea is the activation energy.

  10. On what basis is the modern periodic table arranged, and state the modern periodic law.

    Arranged by increasing atomic number; the modern periodic law states that properties of elements are a periodic function of their atomic numbers.

  11. How do atomic radius and ionization energy vary across a period (left to right)?

    Atomic radius decreases and ionization energy generally increases across a period.

  12. Define electronegativity and name the most electronegative element.

    Electronegativity is the tendency of an atom to attract a shared electron pair in a bond; fluorine is the most electronegative element.

  13. How are elements classified into s, p, d, and f blocks?

    By the subshell receiving the last (differentiating) electron: s-block (s), p-block (p), d-block (d, transition metals), f-block (f, lanthanides/actinides).

  14. Why are alkali metals (Group 1) highly reactive and good reducing agents?

    They have a single loosely held valence electron and low ionization energy, so they readily lose it to form +1 ions.

  15. Why is the first ionization enthalpy of nitrogen higher than that of oxygen?

    Nitrogen has a stable half-filled 2p3 configuration, which requires extra energy to remove an electron compared with oxygen.

  16. What is diagonal relationship? Give one example pair.

    Similarity in properties between an element and the element diagonally placed in the next group/period; e.g., Li and Mg, or Be and Al.

  17. Name the inert (noble) gases and state why they are chemically unreactive.

    He, Ne, Ar, Kr, Xe, Rn; they have completely filled (stable octet/duplet) valence shells, so they have little tendency to gain, lose or share electrons.

  18. Why do transition (d-block) elements typically show variable oxidation states?

    Because the energies of the (n-1)d and ns orbitals are close, electrons from both can participate in bonding, giving multiple oxidation states.

  19. Why are many transition metal compounds coloured?

    Due to d-d electronic transitions, where electrons absorb visible light to move between split d-orbitals (crystal field splitting).

  20. Define coordination number and ligand in a coordination compound.

    Coordination number = number of donor atoms (ligand sites) directly bonded to the central metal ion; a ligand is an ion/molecule that donates an electron pair to the metal.

  21. What is the oxidation state of Fe and the coordination number in [Fe(CN)6]^4-?

    Iron is +2 and the coordination number is 6.

  22. What is metallurgy, and what is the difference between an ore and a mineral?

    Metallurgy is the science of extracting and refining metals from ores. A mineral is a naturally occurring substance containing a metal; an ore is a mineral from which a metal can be extracted profitably.

  23. Name the processes used to concentrate (i) sulphide ores and (ii) oxide ores.

    (i) Sulphide ores: froth flotation. (ii) Oxide ores: hydraulic washing / gravity separation (and magnetic separation if magnetic).

  24. What is the difference between calcination and roasting?

    Calcination = heating an ore (usually carbonate/hydroxide) in limited/absence of air to drive off volatile matter. Roasting = heating a sulphide ore strongly in excess air to convert it to oxide.

  25. Why is hydrogen sometimes placed with Group 1 and sometimes with Group 17?

    Like Group 1 it has one valence electron and forms H+; like Group 17 it needs one electron for a stable configuration and forms H- (hydride), so it shows dual behaviour.

  26. What is hybridization of carbon in alkanes, alkenes and alkynes?

    Alkanes: sp3; alkenes: sp2; alkynes: sp.

  27. Define homologous series and give two of its characteristics.

    A series of compounds with the same general formula and functional group, differing by CH2; members have similar chemical properties and a gradual gradation in physical properties.

  28. What is the difference between inductive effect and resonance effect?

    Inductive effect is the permanent shifting of sigma-bond electrons due to electronegativity differences (transmitted through bonds, weakening with distance); resonance is delocalization of pi/lone-pair electrons over the molecule giving extra stability.

  29. What is Markovnikov's rule for addition of HX to an unsymmetrical alkene?

    The hydrogen of HX adds to the doubly bonded carbon already bearing more hydrogens, and the halogen adds to the carbon with fewer hydrogens.

  30. What general type of reaction do alkanes, alkenes/alkynes, and aromatics characteristically undergo?

    Alkanes: free-radical substitution; alkenes/alkynes: electrophilic addition; aromatic (benzene): electrophilic substitution.

  31. Identify the functional groups: -OH, -CHO, -COOH, and -NH2.

    -OH = alcohol (hydroxyl); -CHO = aldehyde; -COOH = carboxylic acid; -NH2 = amine (amino).

  32. Name the four main classes of biomolecules and one example of each.

    Carbohydrates (glucose), proteins (albumin/enzymes), lipids (fats/oils), and nucleic acids (DNA/RNA).

  33. What is the difference between an addition polymer and a condensation polymer? Give an example of each.

    Addition polymers form by repeated addition of monomers with no by-product (e.g., polythene); condensation polymers form by joining monomers with loss of a small molecule like water (e.g., nylon, polyester).

RUHS / State Nursing Entrance Chemistry FAQ

What is in the RUHS / State Nursing Entrance Chemistry syllabus?

RUHS / State Nursing Entrance Chemistry is split into 3 chapters: Physical Chemistry, Inorganic Chemistry and Organic Chemistry. Together they contain 13 topics and 30 sub-topics.

How many chapters are in RUHS / State Nursing Entrance Chemistry?

3 chapters, containing 13 topics and 30 sub-topics. The largest chapter is Physical Chemistry, with 5 topics.

Are there flashcards for RUHS / State Nursing Entrance Chemistry?

Yes — a 53-card Chemistry deck, printed in full in the flashcards section of this page and available in the Examius app with spaced repetition. The free plan covers one exam of your choice, including its flashcards; Examius Pro, a one-time purchase, unlocks every other exam and deck.