COMEDK UGET Chemistry - Physical Chemistry Syllabus

Chemistry - Physical 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 - Physical Chemistry in COMEDK UGET, not a summary of it.

1. 1

   Basic Concepts and Atomic Structure

   3 topics

   • Some Basic Concepts of Chemistry
     • Mole concept and molar mass
     • Stoichiometry and limiting reagent
     • Concentration terms and empirical formula
   • Structure of Atom
     • Bohr and quantum mechanical models
     • Quantum numbers and orbitals
     • Electronic configuration and Aufbau principle
   • States of Matter
     • Gas laws and ideal gas equation
     • Kinetic molecular theory
     • Real gases and van der Waals equation
2. 2

   Energetics and Equilibrium

   3 topics

   • Thermodynamics
     • First law and enthalpy
     • Hess's law and enthalpy changes
     • Entropy, Gibbs energy and spontaneity
   • Chemical Equilibrium
     • Law of mass action and Kc, Kp
     • Le Chatelier's principle
   • Ionic Equilibrium
     • Acids, bases and pH
     • Buffers and hydrolysis of salts
     • Solubility product
3. 3

   Solutions and Electrochemistry

   3 topics

   • Solutions
     • Concentration and Raoult's law
     • Colligative properties
     • Abnormal molar mass and van't Hoff factor
   • Electrochemistry
     • Galvanic cells and electrode potential
     • Nernst equation
     • Conductance and Kohlrausch's law
     • Electrolysis and Faraday's laws
   • Redox Reactions
     • Oxidation number and balancing
     • Types of redox reactions
4. 4

   Kinetics, Surface and Solid State

   3 topics

   • Chemical Kinetics
     • Rate laws and order of reaction
     • Integrated rate equations
     • Arrhenius equation and activation energy
   • Surface Chemistry
     • Adsorption and isotherms
     • Catalysis
     • Colloids and emulsions
   • Solid State
     • Crystal lattices and unit cells
     • Packing efficiency and density
     • Point defects

Chemistry - Physical Chemistry flashcards for COMEDK UGET

24 of 51 cards from the Chemistry - Physical Chemistry deck — real questions with worked answers.

1. What is the value of one mole (Avogadro's number)?

   6.022 × 10²³ particles (atoms, molecules, ions, etc.).

2. State the law of conservation of mass.

   In a chemical reaction, mass is neither created nor destroyed; total mass of reactants equals total mass of products.

3. What does the law of multiple proportions state?

   When two elements combine to form more than one compound, the masses of one element that combine with a fixed mass of the other are in a ratio of small whole numbers.

4. Define empirical formula and molecular formula.

   Empirical formula gives the simplest whole-number ratio of atoms; molecular formula gives the actual number of atoms of each element in a molecule (molecular = n × empirical).

5. How is molarity (M) defined?

   Molarity = moles of solute / volume of solution in litres (mol/L).

6. How is molality (m) defined?

   Molality = moles of solute / mass of solvent in kilograms (mol/kg).

7. What is the de Broglie equation relating wavelength to momentum?

   λ = h/(mv) = h/p, where h is Planck's constant.

8. State Heisenberg's uncertainty principle.

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

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

   Principal (n) – energy/shell size; Azimuthal (l) – subshell/shape; Magnetic (mₗ) – orbital orientation; Spin (mₛ) – electron spin (+½ or −½).

10. State the Aufbau principle.

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

11. State the Pauli exclusion principle.

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

12. State Hund's rule of maximum multiplicity.

    Electrons occupy degenerate orbitals singly with parallel spins before pairing begins.

13. Give the Rydberg formula for the wavenumber of hydrogen spectral lines.

    1/λ = R_H (1/n₁² − 1/n₂²), where R_H = 1.097 × 10⁷ m⁻¹ and n₂ > n₁.

14. What is the energy of an electron in the nth orbit of a hydrogen atom (Bohr model)?

    Eₙ = −13.6/n² eV (energy is negative and increases toward zero as n increases).

15. State the postulates of the kinetic theory of gases (key points).

    Gas molecules are point masses in constant random motion, have negligible volume, exert no intermolecular forces, undergo perfectly elastic collisions, and average kinetic energy is proportional to absolute temperature.

16. State the ideal gas equation and the value of R.

    PV = nRT; R = 8.314 J K⁻¹ mol⁻¹ = 0.0821 L atm K⁻¹ mol⁻¹.

17. State Boyle's, Charles's, and Gay-Lussac's gas laws.

    Boyle's: V ∝ 1/P at constant T,n. Charles's: V ∝ T at constant P,n. Gay-Lussac's: P ∝ T at constant V,n.

18. What is the van der Waals equation for real gases?

    (P + an²/V²)(V − nb) = nRT, where 'a' corrects for intermolecular attraction and 'b' for molecular volume.

19. Define compressibility factor Z and its value for an ideal gas.

    Z = PV/nRT; Z = 1 for an ideal gas. Z < 1 indicates attractive dominance, Z > 1 repulsive/volume dominance.

20. State the first law of thermodynamics.

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

21. Define enthalpy (H) and the relation between ΔH and ΔU.

    H = U + PV; ΔH = ΔU + Δ(PV), and for gases ΔH = ΔU + Δn_g RT at constant T.

22. 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 (ΔH is path-independent, a state function).

23. State the second law of thermodynamics in terms of entropy.

    The entropy of an isolated system always increases for a spontaneous process; ΔS_universe > 0.

24. Give the Gibbs free energy equation and the spontaneity criterion.

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

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