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AP EAMCET / TS EAMCET Chemistry - Physical Chemistry Syllabus

The Chemistry - Physical Chemistry syllabus for AP EAMCET / TS EAMCET in full: 4 chapters, 13 topics and 27 sub-topics, every one listed below, plus 51 Chemistry - Physical Chemistry flashcards with answers.

4Chapters
13Topics
27Sub-topics
51Flashcards

Chemistry - Physical Chemistry syllabus: all 4 chapters

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

  1. Atomic Structure and Classification

     3 topics
    • Atomic Structure
      • Bohr's model and spectral series
      • Quantum numbers and orbitals
      • Electronic configuration and Aufbau principle
    • Periodic Classification
      • Modern periodic law
      • Periodic trends in properties
    • Stoichiometry
      • Mole concept and empirical formula
      • Redox reactions and equivalent concept

  2. States of Matter and Thermodynamics

     3 topics
    • States of Matter: Gases and Liquids
      • Gas laws and ideal gas equation
      • Kinetic molecular theory and real gases
    • Thermodynamics
      • First law, enthalpy and Hess's law
      • Entropy, Gibbs energy and spontaneity
    • Solid State
      • Crystal lattices and unit cells
      • Packing efficiency and defects

  3. Equilibrium

     3 topics
    • Chemical Equilibrium
      • Law of mass action and equilibrium constant
      • Le Chatelier's principle
    • Ionic Equilibrium
      • Acids, bases and pH
      • Buffers and salt hydrolysis
    • Solubility Equilibrium
      • Solubility product and common ion effect

  4. Solutions and Electrochemistry

     4 topics
    • Solutions
      • Concentration terms and Raoult's law
      • Colligative properties and van't Hoff factor
    • Electrochemistry
      • Conductance and Kohlrausch's law
      • Electrochemical cells and Nernst equation
      • Electrolysis and Faraday's laws
    • Chemical Kinetics
      • Rate, order and molecularity
      • Integrated rate laws and Arrhenius equation
    • Surface Chemistry
      • Adsorption and catalysis
      • Colloids and emulsions

AP EAMCET / TS EAMCET Chemistry - Physical Chemistry flashcards — 51 questions with answers

  1. State the Heisenberg Uncertainty Principle and give its mathematical form.

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

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

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

  3. State the Aufbau principle.

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

  4. State Hund's rule of maximum multiplicity.

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

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

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

  6. 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 2 electrons with opposite spins.

  7. Give the expression for the energy of an electron in the nth orbit of a hydrogen atom (Bohr model).

    E_n = -13.6/n² eV (or -2.18×10⁻¹⁸/n² J).

  8. What is the Rydberg formula for the spectral lines of hydrogen?

    1/λ = R_H (1/n₁² - 1/n₂²), where R_H = 109677 cm⁻¹ and n₂ > n₁.

  9. Define modern periodic law.

    The physical and chemical properties of elements are periodic functions of their atomic numbers.

  10. Define ionization enthalpy and state how it varies across a period and down a group.

    Energy required to remove an electron from a gaseous atom. It increases across a period and decreases down a group.

  11. Define electronegativity and name the most electronegative element.

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

  12. How does atomic radius vary across a period and down a group?

    It decreases across a period (increasing nuclear charge) and increases down a group (added shells).

  13. What are the blocks of the periodic table based on the last electron entering?

    s-block, p-block, d-block (transition), and f-block (inner transition/lanthanides & actinides).

  14. Define a mole and give Avogadro's number.

    A mole is the amount of substance containing as many entities as atoms in 12 g of carbon-12. Avogadro's number = 6.022×10²³.

  15. What is the difference between empirical and molecular formula?

    Empirical formula gives the simplest whole-number ratio of atoms; molecular formula gives the actual number of atoms in a molecule. Molecular = n × Empirical.

  16. Define limiting reagent.

    The reactant that is completely consumed first in a reaction, thereby limiting the amount of product formed.

  17. What is molarity (M) and what is its formula?

    Number of moles of solute per litre of solution. M = moles of solute / volume of solution (in L).

  18. 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·K⁻¹·mol⁻¹), T=absolute temperature.

  19. State Boyle's law.

    At constant temperature, the volume of a fixed mass of gas is inversely proportional to its pressure: PV = constant.

  20. State Charles's law.

    At constant pressure, the volume of a fixed mass of gas is directly proportional to its absolute temperature: V/T = constant.

Show the other 31 Chemistry - Physical Chemistry flashcards

  1. 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.

  2. 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.

  3. What is the expression for root mean square (rms) velocity of gas molecules?

    u_rms = √(3RT/M), where M is molar mass.

  4. State the first law of thermodynamics.

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

  5. Define enthalpy (H) and write ΔH in terms of ΔU.

    Enthalpy H = U + PV. ΔH = ΔU + ΔngRT (for gaseous reactions at constant T).

  6. 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.

  7. What does the sign of ΔG indicate about spontaneity?

    ΔG < 0: spontaneous; ΔG = 0: equilibrium; ΔG > 0: non-spontaneous. ΔG = ΔH - TΔS.

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

    The entropy of the universe increases for any spontaneous (irreversible) process: ΔS_universe > 0.

  9. What is the relationship between ΔG° and the equilibrium constant K?

    ΔG° = -RT ln K.

  10. What are the seven crystal systems in solid state chemistry?

    Cubic, Tetragonal, Orthorhombic, Monoclinic, Triclinic, Hexagonal, and Rhombohedral (Trigonal).

  11. Give the number of atoms per unit cell for simple cubic, BCC, and FCC.

    Simple cubic = 1, Body-centred cubic (BCC) = 2, Face-centred cubic (FCC) = 4 atoms per unit cell.

  12. What are the packing efficiencies of SC, BCC, and FCC?

    Simple cubic = 52.4%, BCC = 68%, FCC/CCP = 74%.

  13. Distinguish between Schottky and Frenkel defects.

    Schottky: equal numbers of cations and anions missing (decreases density). Frenkel: ion displaced to an interstitial site (density unchanged).

  14. State the law of chemical equilibrium / law of mass action.

    At equilibrium, the rate of a reaction is proportional to the product of the active masses (concentrations) of reactants, each raised to its stoichiometric coefficient.

  15. What is the relationship between Kp and Kc?

    Kp = Kc(RT)^Δn, where Δn = (moles of gaseous products) - (moles of gaseous reactants).

  16. State Le Chatelier's principle.

    When a system at equilibrium is disturbed by a change in concentration, temperature, or pressure, it shifts to counteract the change and re-establish equilibrium.

  17. Define pH and write its formula.

    pH is the negative logarithm of hydrogen ion concentration. pH = -log[H⁺]. For neutral water at 25°C, pH = 7.

  18. What is the ionic product of water (Kw) at 25°C?

    Kw = [H⁺][OH⁻] = 1.0×10⁻¹⁴ mol²/L². Also pH + pOH = 14.

  19. State the Henderson-Hasselbalch equation for an acidic buffer.

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

  20. Define a buffer solution.

    A solution that resists change in pH on addition of small amounts of acid or base; made of a weak acid and its salt (or weak base and its salt).

  21. Define the common ion effect.

    The suppression of ionization of a weak electrolyte by adding a strong electrolyte that has an ion in common with it.

  22. Define solubility product (Ksp) for a salt AB.

    Ksp = [A⁺][B⁻], the product of ionic concentrations in a saturated solution at equilibrium. Precipitation occurs when ionic product exceeds Ksp.

  23. State Raoult's law for a solution of two volatile liquids.

    The partial vapour pressure of each component is proportional to its mole fraction: P_total = P°_A x_A + P°_B x_B.

  24. Name the four colligative properties of solutions.

    Relative lowering of vapour pressure, elevation of boiling point, depression of freezing point, and osmotic pressure.

  25. Define the van't Hoff factor (i).

    The ratio of observed colligative property to the calculated (normal) value; i = (observed moles of particles)/(moles before dissociation/association). i>1 for dissociation, i<1 for association.

  26. State Henry's law for solubility of gases.

    At constant temperature, the solubility (mole fraction) of a gas in a liquid is proportional to the partial pressure of the gas: p = K_H · x.

  27. Write the Nernst equation for an electrode at 298 K.

    E = E° - (0.0591/n) log Q, where n is the number of electrons transferred and Q is the reaction quotient.

  28. State Faraday's first law of electrolysis.

    The mass of substance deposited at an electrode is directly proportional to the quantity of electricity (charge) passed: m = ZIt. One Faraday = 96500 C.

  29. What is the integrated rate law and half-life for a first-order reaction?

    k = (2.303/t) log([A]₀/[A]); half-life t₁/₂ = 0.693/k (independent of initial concentration).

  30. State the Arrhenius equation relating rate constant and temperature.

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

  31. Distinguish between physisorption and chemisorption.

    Physisorption: weak van der Waals forces, reversible, low enthalpy, decreases with temperature. Chemisorption: chemical bonds, irreversible, high enthalpy, specific.

AP EAMCET / TS EAMCET Chemistry - Physical Chemistry FAQ

What is in the AP EAMCET / TS EAMCET Chemistry - Physical Chemistry syllabus?

AP EAMCET / TS EAMCET Chemistry - Physical Chemistry is split into 4 chapters: Atomic Structure and Classification, States of Matter and Thermodynamics, Equilibrium and Solutions and Electrochemistry. Together they contain 13 topics and 27 sub-topics.

How many chapters are in AP EAMCET / TS EAMCET Chemistry - Physical Chemistry?

4 chapters, containing 13 topics and 27 sub-topics. The largest chapter is Solutions and Electrochemistry, with 4 topics.

Are there flashcards for AP EAMCET / TS EAMCET Chemistry - Physical Chemistry?

Yes — a 51-card Chemistry - Physical 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.