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

Chemistry (NEET-UG Academic Component) syllabus — full chapter and topic list

Expand any chapter to see its topics and sub-topics. This is the whole examinable outline for Chemistry (NEET-UG Academic Component) in AFMC / NEET-linked AFMC Admission, not a summary of it.

1. 1

   Physical Chemistry

   6 topics

   • Some Basic Concepts of Chemistry
     • Mole concept and stoichiometry
     • Empirical and molecular formula
     • Concentration terms and limiting reagent
   • Atomic Structure
     • Bohr model and hydrogen spectrum
     • Quantum numbers and orbitals
     • Aufbau, Pauli, Hund's rules
   • States of Matter and Thermodynamics
     • Gas laws and ideal gas equation
     • First law, enthalpy and Hess's law
     • Entropy, Gibbs free energy and spontaneity
   • Equilibrium
     • Chemical equilibrium and Le Chatelier's principle
     • Ionic equilibrium, pH, buffers
     • Solubility product and common ion effect
   • Electrochemistry and Kinetics
     • Nernst equation and electrochemical cells
     • Conductance and electrolysis
     • Rate laws, order, molecularity and Arrhenius equation
   • Solutions and Surface Chemistry
     • Colligative properties and Raoult's law
     • Adsorption, catalysis and colloids
2. 2

   Inorganic Chemistry

   5 topics

   • Periodic Classification
     • Modern periodic law and trends
     • Ionization enthalpy, electronegativity, atomic radii
   • Chemical Bonding
     • Ionic and covalent bonding
     • VSEPR theory and hybridisation
     • Molecular orbital theory and hydrogen bonding
   • s-Block and p-Block Elements
     • Alkali and alkaline earth metals
     • Groups 13 to 18 and their compounds
   • d- and f-Block Elements
     • Transition elements and variable oxidation states
     • Lanthanoids and actinoids
   • Coordination Compounds
     • Werner's theory and nomenclature
     • Isomerism and crystal field theory
3. 3

   Organic Chemistry

   5 topics

   • Basic Principles and Hydrocarbons
     • IUPAC nomenclature and isomerism
     • Electronic effects: inductive, resonance, hyperconjugation
     • Alkanes, alkenes, alkynes and aromatic hydrocarbons
   • Reaction Mechanisms
     • Nucleophilic substitution (SN1, SN2)
     • Electrophilic addition and aromatic substitution
     • Elimination reactions
   • Oxygen-Containing Functional Groups
     • Alcohols, phenols and ethers
     • Aldehydes, ketones and carboxylic acids
   • Nitrogen-Containing Compounds and Polymers
     • Amines and diazonium salts
     • Polymers and classification
   • Biomolecules
     • Carbohydrates, proteins and amino acids
     • Nucleic acids, vitamins and hormones
4. 4

   Applied and Everyday Chemistry

   3 topics

   • Chemistry in Everyday Life
     • Drugs and their classification
     • Soaps, detergents and food additives
   • Environmental and Green Chemistry
     • Air and water pollution
     • Green chemistry principles
   • Purification and Analysis
     • Methods of purification and chromatography
     • Qualitative and quantitative analysis

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

21 of 55 cards from the Chemistry (NEET-UG Academic Component) deck — real questions with worked answers.

1. State the SI unit and definition of one mole, and the value of Avogadro's number.

   A mole is the amount of substance containing as many entities as there are atoms in 12 g of carbon-12. Avogadro's number = 6.022 x 10^23 entities per mole.

2. What is the difference between molarity and molality, including their units?

   Molarity (M) = moles of solute per litre of solution (mol/L); it varies with temperature. Molality (m) = moles of solute per kilogram of solvent (mol/kg); it is temperature-independent.

3. State the law of multiple proportions with an example.

   When two elements combine to form more than one compound, the masses of one element that combine with a fixed mass of the other are in a small whole-number ratio. Example: in CO and CO2, the masses of oxygen per fixed mass of carbon are in the ratio 1:2.

4. What are the four quantum numbers and what does each specify?

   Principal (n): shell/energy and size. Azimuthal/orbital angular momentum (l): subshell/shape. Magnetic (m_l): orbital orientation. Spin (m_s): electron spin (+1/2 or -1/2).

5. State Hund's rule of maximum multiplicity.

   Electrons fill degenerate orbitals singly with parallel spins before any orbital is doubly occupied, giving maximum total spin (maximum multiplicity).

6. Give the de Broglie equation relating wavelength to momentum.

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

7. State Heisenberg's uncertainty principle as a formula.

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

8. Write the ideal gas equation and name the variables.

   PV = nRT, where P is pressure, V is volume, n is number of moles, R is the universal gas constant (8.314 J/mol/K), and T is absolute temperature in kelvin.

9. State the first law of thermodynamics as an 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.

10. Define enthalpy and write the relation between delta(H) and delta(U).

    Enthalpy H = U + PV. For a reaction, delta(H) = delta(U) + delta(n_g)RT, where delta(n_g) is the change in moles of gas.

11. 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, because enthalpy is a state function.

12. Write the Gibbs free energy equation and the criterion for spontaneity.

    delta(G) = delta(H) - T*delta(S). A process is spontaneous when delta(G) < 0, at equilibrium when delta(G) = 0, and non-spontaneous when delta(G) > 0.

13. 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.

14. Write the relationship between Kp and Kc for a gaseous equilibrium.

    Kp = Kc(RT)^(delta(n_g)), where delta(n_g) = moles of gaseous products minus moles of gaseous reactants.

15. Define pH and pOH, and state their relationship at 25 degrees C.

    pH = -log[H+] and pOH = -log[OH-]. At 25 degrees C, pH + pOH = 14.

16. What is the Henderson-Hasselbalch equation for an acidic buffer?

    pH = pKa + log([salt]/[acid]), where pKa is the negative log of the acid dissociation constant.

17. Define the common ion effect.

    The suppression of the ionization of a weak electrolyte by the addition of a strong electrolyte that shares a common ion, shifting equilibrium per Le Chatelier's principle.

18. Write the Nernst equation for an electrode at 298 K (in log form).

    E = E0 - (0.0591/n) log Q, where E0 is the standard electrode potential, n is the number of electrons transferred, and Q is the reaction quotient.

19. 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 electricity passed: m proportional to Q (where Q = It).

20. Define molar conductivity and state how it changes with dilution.

    Molar conductivity (Lambda_m) is the conductance of all ions from one mole of electrolyte: Lambda_m = kappa x 1000 / C. It increases with dilution for both strong and weak electrolytes.

21. 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.

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