AP EAMCET / TS EAMCET 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 AP EAMCET / TS EAMCET, not a summary of it.

1. 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. 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. 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. 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

Chemistry - Physical Chemistry flashcards for AP EAMCET / TS EAMCET

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

21. 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.

22. 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.

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

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

24. 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).

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