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KCET Chemistry Syllabus
The Chemistry syllabus for KCET in full: 6 chapters, 25 topics and 62 sub-topics, every one listed below, plus 51 Chemistry flashcards with answers.
Chemistry syllabus: all 6 chapters
Expand any chapter to see its topics and sub-topics.
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Physical Chemistry - Foundations
4 topics- Some Basic Concepts of Chemistry
- Mole concept and Avogadro number
- Stoichiometry and limiting reagent
- Empirical and molecular formula
- Structure of Atom
- Bohr model and quantum numbers
- Aufbau, Pauli and Hund's rules
- Shapes of s, p, d orbitals
- Chemical Bonding and Molecular Structure
- Ionic and covalent bonding
- VSEPR theory and molecular geometry
- Hybridisation and molecular orbital theory
- States of Matter
- Gas laws and ideal gas equation
- Kinetic molecular theory
- Real gases and van der Waals equation
- Some Basic Concepts of Chemistry
-
Physical Chemistry - Energetics and Equilibrium
3 topics- Thermodynamics
- Enthalpy, internal energy and Hess's law
- Spontaneity, entropy and Gibbs energy
- Chemical and Ionic Equilibrium
- Law of mass action and Kp, Kc
- Le Chatelier's principle
- pH, buffer solutions and solubility product
- Acids and Bases
- Arrhenius, Bronsted-Lowry and Lewis concepts
- Ionisation of weak acids and bases
- Thermodynamics
-
Physical Chemistry - Solutions, Electrochemistry and Kinetics
4 topics- Solutions
- Concentration terms: molarity, molality, mole fraction
- Raoult's law and ideal/non-ideal solutions
- Colligative properties and van't Hoff factor
- Electrochemistry
- Galvanic cells and electrode potential
- Nernst equation and EMF
- Conductance and Kohlrausch law
- Chemical Kinetics
- Rate of reaction and order/molecularity
- Integrated rate equations and half-life
- Arrhenius equation and activation energy
- Redox Reactions
- Oxidation number and balancing
- Types of redox reactions
- Solutions
-
Inorganic Chemistry
5 topics- Classification of Elements and Periodicity
- Modern periodic law and periodic trends
- Ionisation enthalpy, electronegativity, atomic radius
- Hydrogen and s-Block Elements
- Properties of hydrogen and water
- Alkali and alkaline earth metals
- p-Block Elements
- Groups 13 to 18 trends
- Compounds of boron, carbon, nitrogen and oxygen families
- d- and f-Block Elements
- Transition elements and variable oxidation states
- Lanthanoids and actinoids
- Coordination Compounds
- Werner's theory and nomenclature
- Isomerism in coordination compounds
- Valence bond and crystal field theory
- Classification of Elements and Periodicity
-
Organic Chemistry - Fundamentals and Hydrocarbons
4 topics- Basic Principles of Organic Chemistry
- IUPAC nomenclature
- Inductive, resonance and hyperconjugation effects
- Reaction intermediates and types of reactions
- Hydrocarbons
- Alkanes, alkenes and alkynes
- Markovnikov and anti-Markovnikov addition
- Aromatic hydrocarbons and benzene
- Haloalkanes and Haloarenes
- SN1 and SN2 mechanisms
- Preparation and properties
- Environmental Chemistry
- Air, water and soil pollution
- Green chemistry
- Basic Principles of Organic Chemistry
-
Organic Chemistry - Functional Groups and Biomolecules
5 topics- Alcohols, Phenols and Ethers
- Preparation and reactions of alcohols
- Acidity of phenols
- Aldehydes, Ketones and Carboxylic Acids
- Nucleophilic addition reactions
- Aldol and Cannizzaro reactions
- Acidity of carboxylic acids
- Amines and Nitrogen Compounds
- Classification and basicity of amines
- Diazonium salts and reactions
- Biomolecules
- Carbohydrates and proteins
- Vitamins, enzymes and nucleic acids
- Polymers and Chemistry in Everyday Life
- Addition and condensation polymers
- Drugs, soaps and detergents
- Alcohols, Phenols and Ethers
KCET Chemistry flashcards — 51 questions with answers
State the mole concept: what is one mole and what is Avogadro's number?
One mole is the amount of substance containing as many entities as atoms in 12 g of carbon-12. Avogadro's number = 6.022 x 10^23 entities per mole.
What is the formula relating molarity (M) to moles of solute and volume of solution?
Molarity (M) = moles of solute / volume of solution in litres.
Define empirical formula and molecular formula, and how they relate.
Empirical formula gives the simplest whole-number ratio of atoms; molecular formula gives the actual number of atoms. Molecular formula = (empirical formula) x n, where n = molecular mass / empirical formula mass.
State the four quantum numbers and what each describes.
Principal (n) = energy/shell size; Azimuthal/angular (l) = subshell shape; Magnetic (m_l) = orbital orientation; Spin (m_s) = electron spin (+1/2 or -1/2).
State the Heisenberg uncertainty principle as a formula.
Δx · Δp ≥ h/4π — the position and momentum of an electron cannot both be determined exactly simultaneously.
State Aufbau principle, Pauli exclusion principle, and Hund's rule.
Aufbau: orbitals fill in increasing energy order. Pauli: no two electrons have all four quantum numbers identical (max 2 per orbital, opposite spins). Hund: orbitals of a subshell fill singly first with parallel spins before pairing.
What is the difference between sigma (σ) and pi (π) bonds?
Sigma bonds form by head-on (axial) overlap of orbitals and are stronger; pi bonds form by sideways (lateral) overlap of p-orbitals and are weaker. A single bond is one σ; a double bond is one σ + one π.
According to VSEPR theory, what are the shapes for 2, 3, 4, 5, and 6 electron pairs?
2 = linear, 3 = trigonal planar, 4 = tetrahedral, 5 = trigonal bipyramidal, 6 = octahedral.
What hybridization corresponds to linear, trigonal planar, and tetrahedral geometries?
Linear = sp, trigonal planar = sp2, tetrahedral = sp3.
State the ideal gas equation and name its variables.
PV = nRT, where P = pressure, V = volume, n = moles, R = gas constant (0.0821 L·atm·mol⁻¹·K⁻¹), T = absolute temperature.
State Boyle's law, Charles's law, and Gay-Lussac's law.
Boyle: at constant T, P ∝ 1/V. Charles: at constant P, V ∝ T. Gay-Lussac: at constant V, P ∝ T.
State the first law of thermodynamics as an equation.
ΔU = q + w, where ΔU = change in internal energy, q = heat added to system, w = work done on system.
Give the relationship between ΔH and ΔU for a reaction.
ΔH = ΔU + Δn_g RT, where Δn_g = moles of gaseous products minus moles of gaseous reactants.
State the Gibbs free energy equation and the condition for spontaneity.
ΔG = ΔH − TΔS. A process is spontaneous when ΔG < 0, at equilibrium when ΔG = 0, non-spontaneous when ΔG > 0.
What is 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; ΔH depends only on initial and final states, not the path.
Write the expression for the equilibrium constant Kc for aA + bB ⇌ cC + dD.
Kc = [C]^c[D]^d / [A]^a[B]^b, using equilibrium molar concentrations.
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.
What is the relationship between Kp and Kc?
Kp = Kc(RT)^Δn_g, where Δn_g = moles of gaseous products − moles of gaseous reactants.
Define an acid and base according to the Bronsted-Lowry concept.
A Bronsted-Lowry acid is a proton (H⁺) donor; a base is a proton acceptor.
Define a Lewis acid and a Lewis base.
A Lewis acid is an electron-pair acceptor; a Lewis base is an electron-pair donor.
Show the other 31 Chemistry flashcards
What is the ionic product of water (Kw) at 25°C, and the relationship between pH and pOH?
Kw = [H⁺][OH⁻] = 1.0 x 10⁻¹⁴ at 25°C; pH + pOH = 14.
What is a buffer solution, and give the Henderson-Hasselbalch equation for an acidic buffer.
A buffer resists pH change on adding small amounts of acid or base. pH = pKa + log([salt]/[acid]).
State Raoult's law for a solution of a non-volatile solute.
The relative lowering of vapour pressure equals the mole fraction of the solute: (P° − P)/P° = x_solute.
Name the four colligative properties of solutions.
Relative lowering of vapour pressure, elevation of boiling point, depression of freezing point, and osmotic pressure.
Write the formula for osmotic pressure and the van't Hoff factor's role.
π = iCRT (or π = i·n RT/V), where i = van't Hoff factor accounting for dissociation/association, C = molar concentration.
State Henry's law for gas solubility.
At constant temperature, the solubility (or partial pressure) of a gas in a liquid is proportional to its partial pressure above the liquid: p = K_H · x.
What is the difference between a galvanic (voltaic) cell and an electrolytic cell?
A galvanic cell converts chemical energy to electrical energy via a spontaneous redox reaction; an electrolytic cell uses electrical energy to drive a non-spontaneous reaction.
Write the Nernst equation for an electrode at 298 K.
E = E° − (0.0591/n) log Q, where n = number of electrons transferred and Q = reaction quotient.
State Faraday's first law of electrolysis.
The mass of a substance deposited or liberated at an electrode is directly proportional to the quantity of electric charge passed (m ∝ Q); 1 Faraday = 96500 C = 1 mole of electrons.
What is the relationship between standard cell potential and Gibbs energy?
ΔG° = −nFE°cell, where n = moles of electrons, F = Faraday constant (96500 C/mol).
Define the rate law and order of a reaction.
The rate law expresses rate as rate = k[A]^x[B]^y; the order is the sum (x + y) of the exponents of concentration terms.
Give the integrated rate equation 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).
State the Arrhenius equation and what it describes.
k = A·e^(−Ea/RT), relating the rate constant to activation energy (Ea) and temperature; A is the pre-exponential factor.
Define oxidation and reduction in terms of electrons and oxidation number.
Oxidation = loss of electrons / increase in oxidation number; Reduction = gain of electrons / decrease in oxidation number.
What is a disproportionation reaction? Give an example.
A reaction in which the same element is simultaneously oxidised and reduced. Example: 2H₂O₂ → 2H₂O + O₂ (oxygen goes from −1 to −2 and 0).
State the modern periodic law.
The physical and chemical properties of elements are periodic functions of their atomic numbers.
How do atomic radius and ionization enthalpy vary across a period and down a group?
Across a period: atomic radius decreases, ionization enthalpy increases. Down a group: atomic radius increases, ionization enthalpy decreases.
Why is hydrogen placed with both group 1 and group 17 in some periodic tables?
Like group 1 it has one valence electron and forms H⁺; like group 17 it needs one electron to complete its shell and forms H⁻ (hydride), so it shows resemblance to both.
What is the trend in reactivity and atomic size down group 1 (alkali metals)?
Down group 1, atomic size increases and reactivity increases because the outer electron is more easily lost (lower ionization enthalpy).
What is the inert pair effect in p-block elements?
The reluctance of the ns² electrons to participate in bonding for heavier p-block elements, making lower oxidation states more stable down the group (e.g., Pb²⁺ more stable than Pb⁴⁺).
What are interhalogen compounds? Give the general types.
Compounds formed between two different halogens, of types XX', XX'3, XX'5, XX'7 (e.g., ClF, BrF₃, IF₅, IF₇).
Why do transition (d-block) elements show variable oxidation states and form coloured compounds?
Variable oxidation states arise from similar energies of (n−1)d and ns electrons; colour arises from d-d electronic transitions when partially filled d-orbitals absorb visible light.
What are lanthanoid contraction and its consequence?
The steady decrease in atomic/ionic radii across the lanthanoids due to poor shielding by 4f electrons; it causes second and third row transition elements to have similar sizes (e.g., Zr and Hf).
State Werner's coordination theory: primary and secondary valencies.
Primary valency = oxidation state, satisfied by negative ions, ionizable. Secondary valency = coordination number, satisfied by ligands, non-ionizable and directional, giving the complex its geometry.
Define ligand, coordination number, and denticity.
A ligand is an ion/molecule that donates a lone pair to the central metal. Coordination number = number of donor atoms bonded to the metal. Denticity = number of donor sites a ligand uses (mono-, bi-, polydentate).
What does crystal field theory say causes colour and magnetism in complexes?
Ligands split the metal d-orbitals into different energy levels (Δo for octahedral). d-d transitions across this gap give colour; the number of unpaired electrons (high vs low spin) determines magnetic behaviour.
What are electrophiles and nucleophiles?
Electrophiles are electron-deficient species that accept electron pairs (e.g., NO₂⁺, H⁺); nucleophiles are electron-rich species that donate electron pairs (e.g., OH⁻, CN⁻, NH₃).
Distinguish inductive effect, resonance effect, and hyperconjugation.
Inductive: permanent polarization of σ bonds due to electronegativity difference. Resonance: delocalization of π/lone-pair electrons over the molecule. Hyperconjugation: delocalization of σ(C-H) electrons into an adjacent empty p or π orbital.
State Markovnikov's rule and the anti-Markovnikov (peroxide) effect.
Markovnikov: in addition of HX to an unsymmetrical alkene, H adds to the carbon with more hydrogens. Peroxide effect: with HBr and peroxides, addition is anti-Markovnikov (free-radical mechanism).
Distinguish SN1 and SN2 mechanisms in haloalkanes.
SN1: two-step, carbocation intermediate, first-order, favoured by tertiary halides and polar protic solvents, gives racemization. SN2: one-step, single transition state, second-order, favoured by primary halides, gives inversion of configuration (Walden inversion).
Name the functional-group test to distinguish aldehydes from ketones.
Tollens' reagent (ammoniacal AgNO₃) gives a silver mirror with aldehydes but not ketones; Fehling's solution gives a red-brown Cu₂O precipitate with aliphatic aldehydes only.
KCET Chemistry FAQ
What is in the KCET Chemistry syllabus?
KCET Chemistry is split into 6 chapters: Physical Chemistry - Foundations, Physical Chemistry - Energetics and Equilibrium, Physical Chemistry - Solutions, Electrochemistry and Kinetics, Inorganic Chemistry, Organic Chemistry - Fundamentals and Hydrocarbons and Organic Chemistry - Functional Groups and Biomolecules. Together they contain 25 topics and 62 sub-topics.
How many chapters are in KCET Chemistry?
6 chapters, containing 25 topics and 62 sub-topics. The largest chapter is Inorganic Chemistry, with 5 topics.
Are there flashcards for KCET 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.