WBJEE Physical Chemistry Syllabus

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 Physical Chemistry in WBJEE, not a summary of it.

1. 1

   Atomic Structure and States of Matter

   3 topics

   • Atomic Structure
     • Bohr model and hydrogen spectrum
     • Quantum numbers and orbitals
     • Electronic configuration and Aufbau principle
   • Gaseous and Liquid States
     • Gas laws and ideal gas equation
     • Kinetic theory and real gases
     • Liquefaction and critical phenomena
   • Solid State
     • Crystal lattices and unit cells
     • Packing efficiency and density
     • Defects in solids
2. 2

   Solutions and Thermodynamics

   3 topics

   • Solutions and Colligative Properties
     • Concentration terms and Raoult's law
     • Colligative properties and van't Hoff factor
     • Osmosis and osmotic pressure
   • Chemical Energetics and Thermodynamics
     • First law and enthalpy changes
     • Hess's law and bond enthalpy
     • Entropy, Gibbs energy and spontaneity
   • Some Basic Concepts and Stoichiometry
     • Mole concept and molar mass
     • Empirical and molecular formula
     • Stoichiometric calculations and limiting reagent
3. 3

   Equilibrium and Redox

   3 topics

   • Chemical Equilibrium
     • Law of mass action and Kc, Kp
     • Le Chatelier's principle
   • Ionic Equilibrium
     • Acids, bases and pH
     • Buffer solutions and solubility product
     • Hydrolysis of salts
   • Redox Reactions
     • Oxidation number and balancing equations
     • Redox titrations
4. 4

   Kinetics, Electrochemistry and Surface Chemistry

   3 topics

   • Chemical Kinetics
     • Rate of reaction and rate law
     • Order and molecularity
     • Arrhenius equation and activation energy
   • Electrochemistry
     • Conductance and Kohlrausch's law
     • Electrochemical cells and EMF
     • Nernst equation and electrolysis
   • Surface Chemistry
     • Adsorption and catalysis
     • Colloids and their properties

Physical Chemistry flashcards for WBJEE

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

1. State the de Broglie relation and define each term.

   $\lambda = \dfrac{h}{mv} = \dfrac{h}{p}$, where $\lambda$ is wavelength, $h$ is Planck's constant, $m$ is mass, $v$ is velocity, and $p$ is momentum. It links the wave and particle nature of matter.

2. What is the Heisenberg uncertainty principle and its mathematical form?

   It is impossible to simultaneously determine the exact position and momentum of a microscopic particle. $\Delta x \cdot \Delta p \geq \dfrac{h}{4\pi}$

3. Give the expression for the energy of an electron in the $n^{th}$ Bohr orbit of a hydrogen atom (in eV).

   $E_n = -\dfrac{13.6}{n^{2}}\ \text{eV}$ (per atom); negative sign indicates the electron is bound.

4. State the formula for the radius of the $n^{th}$ Bohr orbit of hydrogen.

   $r_n = 0.529 \times \dfrac{n^{2}}{Z}\ \text{\AA}$, where $Z$ is the nuclear charge. For hydrogen ($Z=1$), $r_1 = 0.529\ \text{\AA}$.

5. State Bohr's quantization condition for angular momentum.

   Angular momentum is quantized: $mvr = \dfrac{nh}{2\pi}$, where $n = 1, 2, 3, \dots$

6. Write the Rydberg formula for the wavenumber of hydrogen spectral lines.

   $\bar{\nu} = \dfrac{1}{\lambda} = R_H Z^{2}\left(\dfrac{1}{n_1^{2}} - \dfrac{1}{n_2^{2}}\right)$, with $R_H = 1.097 \times 10^{7}\ \text{m}^{-1}$ and $n_2 > n_1$.

7. Name the spectral series of hydrogen lying in the visible region and its lower energy level.

   The Balmer series, with $n_1 = 2$ (transitions from $n_2 = 3, 4, 5, \dots$ to $n=2$).

8. Match the hydrogen spectral series to their region: Lyman, Paschen, Brackett.

   Lyman ($n_1=1$): ultraviolet; Paschen ($n_1=3$): infrared; Brackett ($n_1=4$): infrared (far). Balmer ($n_1=2$) is visible.

9. What do the four quantum numbers $n$, $l$, $m_l$, and $m_s$ represent?

   $n$ = principal (energy/shell size); $l$ = azimuthal (subshell/shape); $m_l$ = magnetic (orbital orientation); $m_s$ = spin ($+\tfrac{1}{2}$ or $-\tfrac{1}{2}$).

10. What are the allowed values of the azimuthal quantum number $l$ and corresponding subshells?

    $l = 0, 1, 2, \dots, (n-1)$. $l=0 \to s$, $l=1 \to p$, $l=2 \to d$, $l=3 \to f$.

11. How many orbitals and electrons can a shell with principal quantum number $n$ hold?

    Number of orbitals $= n^{2}$; maximum electrons $= 2n^{2}$.

12. What is the range of values for the magnetic quantum number $m_l$?

    $m_l = -l, \dots, 0, \dots, +l$, giving $(2l+1)$ values (orbitals) for each $l$.

13. Give the formula for the number of radial nodes and angular nodes of an orbital.

    Radial nodes $= n - l - 1$; angular nodes $= l$; total nodes $= n - 1$.

14. State the Aufbau principle.

    Electrons fill atomic orbitals in order of increasing energy, lowest energy first. Order follows the $(n+l)$ rule; for equal $(n+l)$, the orbital with lower $n$ fills first.

15. State Hund's rule of maximum multiplicity.

    Electrons occupy degenerate (equal-energy) orbitals singly with parallel spins before any orbital is doubly occupied, maximizing total spin.

16. State the Pauli exclusion principle.

    No two electrons in an atom can have all four quantum numbers identical; equivalently, an orbital holds at most two electrons with opposite spins.

17. Write the ground-state electronic configuration of chromium ($Z=24$) and explain the anomaly.

    $\ce{[Ar]} 3d^{5} 4s^{1}$. The half-filled $3d^{5}$ and $4s^{1}$ configuration gives extra stability due to symmetry and exchange energy, rather than $3d^{4}4s^{2}$.

18. State Boyle's law and its mathematical form.

    At constant temperature and amount of gas, volume is inversely proportional to pressure: $PV = \text{constant}$, or $P_1V_1 = P_2V_2$.

19. State Charles's law and its mathematical form.

    At constant pressure, volume is directly proportional to absolute temperature: $\dfrac{V}{T} = \text{constant}$, or $\dfrac{V_1}{T_1} = \dfrac{V_2}{T_2}$.

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