AFMC / NEET-linked AFMC Admission Chemistry (NEET-UG Academic Component) Syllabus

Give the integrated rate law and half-life expression for a first-order reaction.

k = (2.303/t) log([A0]/[A]); half-life t(1/2) = 0.693/k, which is independent of initial concentration.

State the Arrhenius equation relating rate constant to temperature.

k = A*e^(-Ea/RT), where A is the pre-exponential (frequency) factor, Ea is activation energy, R is the gas constant, and T is absolute temperature.

State Raoult's law for a solution of two volatile liquids.

The partial vapour pressure of each component is proportional to its mole fraction: p_total = p_A0*x_A + p_B0*x_B.

List the four colligative properties of dilute solutions.

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

Define the van't Hoff factor (i).

i is the ratio of the observed colligative property to the calculated value assuming no association/dissociation; it equals the actual number of particles in solution per formula unit (i > 1 for dissociation, i < 1 for association).

Differentiate between physisorption and chemisorption.

Physisorption involves weak van der Waals forces, is reversible, has low enthalpy, and decreases with temperature. Chemisorption involves chemical bonds, is irreversible, has high enthalpy, and is specific.

State the periodic trends in atomic radius across a period and down a group.

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

How do ionization enthalpy and electronegativity vary across a period?

Both ionization enthalpy and electronegativity generally increase across a period from left to right, due to increasing effective nuclear charge and decreasing atomic size.

State VSEPR theory and predict the shape of a molecule with 4 bonding pairs and no lone pairs.

VSEPR theory states that electron pairs around a central atom arrange to minimize repulsion. Four bonding pairs with no lone pairs give a tetrahedral shape (109.5 degrees), e.g., CH4.

Define hybridization and give the geometry for sp, sp2, and sp3.

Hybridization is the mixing of atomic orbitals to form equivalent hybrid orbitals. sp = linear (180 degrees), sp2 = trigonal planar (120 degrees), sp3 = tetrahedral (109.5 degrees).

What is the bond order formula in molecular orbital theory?

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

Distinguish between sigma and pi bonds.

A sigma bond forms by head-on (axial) overlap of orbitals and is stronger; a pi bond forms by sidewise (lateral) overlap of p-orbitals and is weaker. Single bonds are sigma; double/triple bonds contain pi bonds.

Why does the s-block contain alkali and alkaline earth metals, and what is their general reactivity?

The s-block has groups 1 (alkali metals, ns1) and 2 (alkaline earth metals, ns2). They are highly reactive, electropositive metals; reactivity increases down each group.

What is the diagonal relationship, with an example from the s-block?

Certain elements in period 2 resemble the element diagonally placed in period 3, group adjacent. Example: lithium resembles magnesium, and beryllium resembles aluminium.

Why is the +1 oxidation state increasingly stable down group 13 and 14 (inert pair effect)?

The inert pair effect: the ns2 electrons become reluctant to participate in bonding down the group due to poor shielding by d and f electrons, stabilizing a lower oxidation state (e.g., Tl+1, Pb+2).

Define transition elements and explain why they show variable oxidation states.

Transition (d-block) elements have partially filled d-orbitals in atoms or common ions. They show variable oxidation states because the energies of (n-1)d and ns electrons are similar, so both can be lost.

Why are most transition metal compounds coloured?

Because of d-d electronic transitions: when d-orbitals split in a ligand field, electrons absorb visible light to jump between d levels, and the complementary colour is transmitted.

What are lanthanoid contraction and its consequence?

Lanthanoid contraction is the steady decrease in atomic/ionic size across the lanthanoid series due to poor shielding by 4f electrons. It causes second- and third-row transition elements (e.g., Zr and Hf) to have similar sizes.

State Werner's coordination theory in brief.

Metals show two valencies: primary (ionizable, satisfied by anions) and secondary (non-ionizable, satisfied by ligands, equal to coordination number). Secondary valencies are directional and fix the geometry.

State the rule for naming the coordination sphere and give the formula meaning of [Co(NH3)6]Cl3.

Ligands are named alphabetically before the metal, with the metal's oxidation state in Roman numerals. [Co(NH3)6]Cl3 is hexaamminecobalt(III) chloride: Co3+ with six ammine ligands, coordination number 6.

What is crystal field splitting in an octahedral complex?

In an octahedral field the five degenerate d-orbitals split into a lower t2g set (dxy, dyz, dxz) and a higher eg set (dx2-y2, dz2), separated by the crystal field splitting energy (delta_o).

State Markovnikov's rule for addition of HX to an unsymmetrical alkene.

The negative part (X) of the reagent adds to the carbon bearing fewer hydrogen atoms, while H adds to the carbon with more hydrogens, giving the more stable carbocation intermediate.

Define and order the stability of carbocations.

A carbocation is a positively charged carbon species. Stability order: tertiary > secondary > primary > methyl, due to increasing hyperconjugation and the +I (inductive) effect of alkyl groups.

Distinguish between SN1 and SN2 reaction mechanisms.

SN1 is two-step via a carbocation, first-order kinetics, favoured by tertiary substrates, and gives racemization. SN2 is one-step concerted, second-order kinetics, favoured by primary substrates, and proceeds with inversion of configuration.

What is Markovnikov's anti rule (peroxide/Kharasch effect)?

In the presence of peroxides, HBr adds to an unsymmetrical alkene against Markovnikov's rule (anti-Markovnikov) via a free-radical mechanism, placing Br on the carbon with more hydrogens.

Name the reactions for: (a) aldehyde/ketone + HCN, and (b) two molecules of aldehyde under dilute base.

(a) Nucleophilic addition forming a cyanohydrin. (b) Aldol condensation, giving a beta-hydroxy aldehyde/ketone that can dehydrate to an alpha,beta-unsaturated carbonyl.

What is the difference between an aldehyde and a ketone in terms of structure and oxidation?

An aldehyde has the carbonyl carbon bonded to at least one H (R-CHO) and is easily oxidized to a carboxylic acid. A ketone has the carbonyl carbon bonded to two carbons (R-CO-R') and resists mild oxidation.

Describe the Hofmann bromamide degradation reaction.

A primary amide is treated with Br2 and aqueous (or alcoholic) KOH/NaOH to give a primary amine with one fewer carbon atom: R-CONH2 to R-NH2.

Differentiate addition polymers from condensation polymers with one example each.

Addition polymers form by repeated addition of monomers with no by-product (e.g., polythene from ethene). Condensation polymers form by combination of monomers with loss of a small molecule like water (e.g., nylon-6,6).

Name the four major classes of biomolecules and their building blocks.

Carbohydrates (monosaccharides), proteins (amino acids), nucleic acids (nucleotides), and lipids (fatty acids and glycerol).

What are essential and non-essential amino acids?

Essential amino acids cannot be synthesized by the body and must be obtained from the diet; non-essential amino acids can be synthesized within the body.

Distinguish between BOD and COD as water-quality indicators.

BOD (Biochemical Oxygen Demand) is the oxygen used by microorganisms to decompose organic matter biologically. COD (Chemical Oxygen Demand) is the oxygen required to chemically oxidize all organic/inorganic matter; COD is usually higher than BOD.

Define green chemistry and one of its core goals.

Green chemistry is the design of chemical products and processes that reduce or eliminate the use and generation of hazardous substances; a core goal is preventing waste rather than treating it after formation.

How does Lassaigne's test detect nitrogen in an organic compound?

The compound is fused with sodium to convert nitrogen to sodium cyanide (NaCN); adding ferrous sulphate and ferric ions produces Prussian blue (ferric ferrocyanide), confirming nitrogen.

On what principle does chromatography separate components of a mixture?

Differential distribution (adsorption or partition) of components between a stationary phase and a moving mobile phase, so components travel at different rates and separate.