VITEEE Chemistry Syllabus

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 in VITEEE, not a summary of it.

1. 1

   Atomic Structure and Periodicity

   3 topics

   • Atomic Structure
     • Bohr's model and limitations
     • Quantum numbers and shapes of orbitals
     • Aufbau, Pauli and Hund's rules; electronic configuration
   • Periodic Classification
     • Modern periodic law and long form table
     • Periodic trends: atomic radius, ionization enthalpy, electronegativity
   • Chemical Bonding and Molecular Structure
     • Ionic, covalent and coordinate bonds
     • VSEPR theory and molecular geometry
     • Hybridisation, VBT and MOT (diatomic molecules)
2. 2

   States of Matter and Physical Chemistry

   4 topics

   • Solid State
     • Crystal lattices, unit cells and packing efficiency
     • Point defects and electrical/magnetic properties
   • Solutions
     • Concentration terms and Raoult's law
     • Colligative properties and Van't Hoff factor
   • Thermodynamics and Thermochemistry
     • First law, enthalpy and Hess's law
     • Entropy, Gibbs free energy and spontaneity
   • Chemical and Ionic Equilibrium
     • Law of mass action and Le Chatelier's principle
     • Acids, bases, pH and buffer solutions
     • Solubility product and common ion effect
3. 3

   Electrochemistry and Kinetics

   3 topics

   • Electrochemistry
     • Conductance and Kohlrausch's law
     • Galvanic cells, electrode potential and Nernst equation
     • Electrolysis and Faraday's laws; batteries and corrosion
   • Chemical Kinetics
     • Rate of reaction and rate laws
     • Order and molecularity; integrated rate equations
     • Arrhenius equation and collision theory
   • Surface Chemistry
     • Adsorption and catalysis
     • Colloids and emulsions
4. 4

   Inorganic Chemistry

   4 topics

   • p-Block Elements
     • Group 13 to 18: trends and important compounds
     • Allotropes, oxoacids and interhalogen compounds
   • d- and f-Block Elements
     • Transition elements: variable oxidation states and colour
     • Lanthanoids and actinoids; lanthanoid contraction
   • Coordination Compounds
     • Nomenclature, isomerism and Werner's theory
     • Valence bond and crystal field theory
   • Metallurgy and Hydrogen
     • Principles and processes of extraction of metals
     • Hydrogen, hydrides and water chemistry
5. 5

   Organic Chemistry I

   3 topics

   • Basic Concepts and Isomerism
     • IUPAC nomenclature and electronic effects
     • Inductive, resonance and hyperconjugation effects
     • Structural and stereoisomerism; chirality
   • Hydrocarbons
     • Alkanes, alkenes and alkynes: preparation and reactions
     • Aromatic hydrocarbons and electrophilic substitution
   • Haloalkanes and Haloarenes
     • SN1 and SN2 mechanisms
     • Elimination reactions and reactivity
6. 6

   Organic Chemistry II and Applied Chemistry

   4 topics

   • Oxygen-Containing Compounds
     • Alcohols, phenols and ethers
     • Aldehydes, ketones and carboxylic acids
   • Nitrogen-Containing Compounds
     • Amines: classification, preparation and basicity
     • Diazonium salts and their reactions
   • Biomolecules and Polymers
     • Carbohydrates, proteins, vitamins and nucleic acids
     • Classification of polymers and polymerisation
   • Chemistry in Everyday Life
     • Drugs and their classification
     • Detergents, dyes and food chemistry

Chemistry flashcards for VITEEE

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

1. State the quantum numbers and the maximum number of electrons in the n=3 shell.

   n=3 has subshells 3s, 3p, 3d. Maximum electrons = 2n^2 = 2(3)^2 = 18 electrons.

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

   lambda = h/(mv) = h/p, where h is Planck's constant, m is mass, v is velocity, and p is momentum.

3. State Heisenberg's uncertainty principle (equation).

   It is impossible to determine simultaneously the exact position and momentum of an electron: delta x * delta p >= h/(4*pi).

4. What does the Aufbau principle, Pauli exclusion principle, and Hund's rule each govern?

   Aufbau: electrons fill lowest-energy orbitals first. Pauli: no two electrons have all four quantum numbers identical (max 2 per orbital, opposite spins). Hund: orbitals of a subshell are singly filled before pairing, with parallel spins.

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

   E_n = -13.6/n^2 eV (or -2.18 x 10^-18/n^2 J) per atom.

6. Define ionization enthalpy and state its trend across a period and down a group.

   Ionization enthalpy is the energy needed to remove the outermost electron from a gaseous atom. It increases across a period (left to right) and decreases down a group.

7. Define electronegativity and name the most electronegative element.

   Electronegativity is the tendency of an atom to attract a shared electron pair toward itself in a bond. Fluorine is the most electronegative element.

8. What is the lanthanoid contraction and one of its consequences?

   The steady decrease in atomic/ionic size across the lanthanoid series due to poor shielding by 4f electrons. Consequence: the second and third transition series elements have nearly identical sizes (e.g., Zr and Hf).

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

   Atomic radius decreases across a period (increasing nuclear charge) and increases down a group (addition of new shells).

10. State VSEPR-predicted shapes for molecules with 2, 3, 4, 5, and 6 bond pairs (no lone pairs).

    2: linear; 3: trigonal planar; 4: tetrahedral; 5: trigonal bipyramidal; 6: octahedral.

11. What hybridization and shape does sp3d2 give, and give an example?

    sp3d2 hybridization gives an octahedral shape; example: SF6.

12. Compare sigma and pi bonds.

    Sigma bonds form by head-on (axial) overlap, are stronger, and allow rotation. Pi bonds form by sidewise (lateral) overlap of p-orbitals, are weaker, and prevent rotation.

13. According to MO theory, give the bond order and magnetic nature of O2.

    O2 has bond order 2 and is paramagnetic (two unpaired electrons in pi* antibonding orbitals).

14. State the bond order formula in molecular orbital theory.

    Bond order = (number of bonding electrons - number of antibonding electrons) / 2.

15. What is the difference between a face-centered cubic (FCC) and body-centered cubic (BCC) unit cell in atoms per cell?

    FCC contains 4 atoms per unit cell; BCC contains 2 atoms per unit cell. (Simple cubic = 1.)

16. State packing efficiencies for simple cubic, BCC, and FCC/HCP lattices.

    Simple cubic: 52.4%; BCC: 68%; FCC and HCP: 74%.

17. Distinguish Schottky and Frenkel defects.

    Schottky: equal numbers of cations and anions missing, lowering density (e.g., NaCl). Frenkel: a cation shifts to an interstitial site, no density change (e.g., AgCl, ZnS).

18. State Raoult's law for a solution of a non-volatile solute.

    Relative lowering of vapour pressure equals the mole fraction of the solute: (p0 - p)/p0 = x_solute. For volatile components, partial pressure = mole fraction x pure vapour pressure.

19. Write the formula for osmotic pressure and define the van't Hoff factor.

    pi = CRT (or pi = i C R T for electrolytes). The van't Hoff factor i = observed colligative property / calculated value; it accounts for dissociation or association.

20. List the four colligative properties.

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

21. Write the formulas for elevation of boiling point and depression of freezing point.

    Delta Tb = Kb * m and Delta Tf = Kf * m, where m is molality, Kb is the ebullioscopic constant, and Kf is the cryoscopic constant.

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