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VITEEE Chemistry Syllabus

The Chemistry syllabus for VITEEE in full: 6 chapters, 21 topics and 48 sub-topics, every one listed below, plus 51 Chemistry flashcards with answers.

6Chapters

21Topics

48Sub-topics

51Flashcards

Chemistry syllabus: all 6 chapters

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

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)
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
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
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
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
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

VITEEE Chemistry flashcards — 51 questions with answers

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.
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.
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).
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.
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.
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.
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.
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).
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).
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.
What hybridization and shape does sp3d2 give, and give an example?
sp3d2 hybridization gives an octahedral shape; example: SF6.
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.
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).
State the bond order formula in molecular orbital theory.
Bond order = (number of bonding electrons - number of antibonding electrons) / 2.
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.)
State packing efficiencies for simple cubic, BCC, and FCC/HCP lattices.
Simple cubic: 52.4%; BCC: 68%; FCC and HCP: 74%.
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).
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.
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.
List the four colligative properties.
Relative lowering of vapour pressure, elevation of boiling point, depression of freezing point, and osmotic pressure.

Show the other 31 Chemistry flashcards

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.
State the first law of thermodynamics (equation).
Delta U = q + w, where Delta U is change in internal energy, q is heat absorbed by the system, and w is work done on the system.
Relate enthalpy change Delta H to internal energy change Delta U for a gaseous reaction.
Delta H = Delta U + Delta(ng)RT, where Delta(ng) is the change in moles of gas.
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; enthalpy is a state function.
Give the Gibbs free energy equation and the condition for spontaneity.
Delta G = Delta H - T*Delta S. A reaction is spontaneous when Delta G < 0; at equilibrium Delta G = 0.
How is standard Gibbs free energy related to the equilibrium constant?
Delta G0 = -RT ln K (where K is the equilibrium constant, R the gas constant, T the temperature in K).
State Le Chatelier's principle.
If a system at equilibrium is disturbed by a change in concentration, pressure, or temperature, the equilibrium shifts in the direction that counteracts the disturbance.
Write the expression for Kp in terms of Kc.
Kp = Kc(RT)^(Delta ng), where Delta ng is the change in number of moles of gas (products - reactants).
Define pH and give the relation between Ka and Kb of a conjugate acid-base pair.
pH = -log[H+]. For a conjugate pair: Ka * Kb = Kw = 1.0 x 10^-14 at 25 C.
What is the common ion effect?
The suppression of the dissociation of a weak electrolyte upon adding a strong electrolyte that shares a common ion (e.g., adding NaCl reduces ionization of HCl-bearing systems / decreasing solubility).
Write the Henderson-Hasselbalch equation for an acidic buffer.
pH = pKa + log([salt]/[acid]).
Define solubility product (Ksp) for a salt AB.
For AB <-> A+ + B-, Ksp = [A+][B-]. A precipitate forms when the ionic product exceeds Ksp.
Write the Nernst equation for an electrode at 298 K.
E = E0 - (0.0591/n) log Q (Q = reaction quotient, n = number of electrons transferred).
State the relation between standard cell potential and Gibbs free energy.
Delta G0 = -nFE0_cell, where n is moles of electrons, F is the Faraday constant (96500 C/mol).
State Faraday's first law of electrolysis.
The mass of substance deposited at an electrode is directly proportional to the quantity of electricity passed: m = (M/nF) * Q, where Q = I * t.
Define molar conductivity and how it varies with dilution for a strong electrolyte.
Molar conductivity = kappa/c (conductivity divided by concentration). For a strong electrolyte it increases slightly with dilution and follows the Debye-Huckel-Onsager equation; limiting value is at infinite dilution.
Write the integrated rate law and half-life of a first-order reaction.
k = (2.303/t) log([A0]/[A]); half-life t(1/2) = 0.693/k, independent of initial concentration.
State the Arrhenius equation and what each term means.
k = A e^(-Ea/RT), where A is the frequency/pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is temperature in K.
Define order and molecularity of a reaction.
Order: the sum of the powers of concentration terms in the experimental rate law (can be zero or fractional). Molecularity: the number of reacting species in an elementary step (always a whole number, >=1).
Distinguish physisorption from chemisorption.
Physisorption: weak van der Waals forces, low heat of adsorption, reversible, multilayer, decreases with temperature. Chemisorption: chemical bonds, high heat of adsorption, irreversible, monolayer, highly specific.
What is the Tyndall effect and what does it indicate?
The scattering of a light beam by colloidal particles, making the path visible. It distinguishes a colloidal sol from a true solution.
Why does Group 15 nitrogen not form pentahalides while phosphorus does?
Nitrogen lacks d-orbitals in its valence shell, so it cannot expand its octet; phosphorus has accessible 3d orbitals and forms compounds like PCl5.
Write the equations for the contact process step that forms SO3 and the catalyst used.
2 SO2 + O2 -> 2 SO3 in the presence of V2O5 catalyst (vanadium pentoxide); SO3 is then absorbed to make oleum and sulphuric acid.
Why do transition (d-block) metals show variable oxidation states?
Because the energies of (n-1)d and ns orbitals are very close, electrons from both can participate in bonding, allowing multiple oxidation states.
Why are many transition metal compounds coloured?
Due to d-d electronic transitions: electrons absorb visible light to jump between split d-orbitals, and the complementary colour is transmitted/observed.
State Werner's primary and secondary valences in coordination compounds.
Primary valence = oxidation state of the metal (ionizable, satisfied by anions). Secondary valence = coordination number (non-ionizable, satisfied by ligands, fixed and directional).
What is a chelate ligand? Give an example.
A chelate is a polydentate ligand that binds a central metal through two or more donor atoms forming a ring. Example: ethylenediamine (en) or EDTA.
Name the principal ore and the reduction step for extracting iron in a blast furnace.
Iron is extracted from haematite (Fe2O3). In the blast furnace it is reduced by carbon monoxide: Fe2O3 + 3CO -> 2Fe + 3CO2.
Distinguish chain, position, and functional isomerism.
Chain isomerism: different carbon-skeleton arrangements. Position isomerism: same skeleton but different position of a functional group/substituent. Functional isomerism: same molecular formula but different functional groups.
State Markovnikov's rule for addition of HX to an unsymmetrical alkene.
When HX adds to an unsymmetrical alkene, the hydrogen atom adds to the carbon that already has more hydrogens (so the halogen goes to the more substituted carbon, via the more stable carbocation).
What are SN1 and SN2 mechanisms and how does substrate structure affect them?
SN1: two-step, via a carbocation, first-order, favored by tertiary substrates and polar protic solvents, gives racemization. SN2: one-step backside attack, second-order, favored by primary substrates and polar aprotic solvents, gives inversion of configuration.

VITEEE Chemistry FAQ

What is in the VITEEE Chemistry syllabus?

VITEEE Chemistry is split into 6 chapters: Atomic Structure and Periodicity, States of Matter and Physical Chemistry, Electrochemistry and Kinetics, Inorganic Chemistry, Organic Chemistry I and Organic Chemistry II and Applied Chemistry. Together they contain 21 topics and 48 sub-topics.

How many chapters are in VITEEE Chemistry?

6 chapters, containing 21 topics and 48 sub-topics. The largest chapter is States of Matter and Physical Chemistry, with 4 topics.

Are there flashcards for VITEEE Chemistry?

Yes — a 51-card 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.