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NEET UG Physical Chemistry Syllabus
The Physical Chemistry syllabus for NEET UG in full: 8 chapters, 97 topics and 19 sub-topics, every one listed below, plus 52 Physical Chemistry flashcards with answers.
Physical Chemistry syllabus: all 8 chapters
Expand any chapter to see its topics and sub-topics.
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UNIT 1: Some Basic Concepts of Chemistry
10 topics- Matter and its nature
- Dalton’s atomic theory
- Laws of chemical combination
- Concept of elements, atoms, and molecules
- Atomic and molecular masses
- Mole concept and molar mass
- Percentage composition
- Empirical and molecular formulae
- Chemical reactions
- Stoichiometry
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UNIT 2: Structure of Atom
15 topics- Discovery of electron, proton, and neutron
- Atomic number, isotopes and isobars
- Thompson’s model and its limitations
- Rutherford’s model and its limitations
- Bohr’s model and its limitations
- Concept of shells and subshells
- Dual nature of matter and light
- de Broglie’s relationship
- Heisenberg uncertainty principle
- Concept of orbitals
- Quantum numbers
- Shapes of s, p and d orbitals
- Rules for filling electrons in orbitals – Aufbau principle, Pauli exclusion principle, Hund’s rule
- Electronic configuration of atoms
- Stability of half-filled and filled orbitals
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UNIT 3: Classification of Elements and Periodicity in Properties
4 topics- Significance of classification
- Development of the periodic table
- Modern periodic law and the present form of the periodic table
- Periodic trends in properties of elements
- Atomic radii
- Ionic radii
- Ionization enthalpy
- Electron gain enthalpy
- Electronegativity
- Valence
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UNIT 4: Chemical Bonding and Molecular Structure
14 topics- Valence electrons
- Ionic bond
- Covalent bond
- Bond parameters
- Lewis structure
- Polar character of covalent bond
- Covalent character of ionic bond
- Valence bond theory
- Resonance
- Geometry of covalent molecules
- VSEPR theory
- Concept of hybridization involving s, p, and d orbitals
- Molecular orbital theory of homonuclear diatomic molecules (qualitative idea only)
- Hydrogen bond
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UNIT 5: States of Matter: Gases and Liquids
8 topics- Three states of matter
- Intermolecular interactions
- Types of bonding
- Melting and boiling points
- Role of gas laws in elucidating the concept of the molecule
- Boyle’s law
- Charle’s law
- Gay Lussac’s law
- Avogadro’s law
- Ideal behavior
- Empirical derivation of gas equation
- Avogadro number
- Ideal gas equation
- Kinetic energy and molecular speeds (elementary idea)
- Deviation from ideal behavior
- Liquefaction of gases
- Critical temperature
- Liquid State
- Vapour pressure
- Viscosity
- Surface tension (qualitative idea only, no mathematical derivations)
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UNIT 6: Thermodynamics
25 topics- Concepts of system
- Types of systems
- Surroundings
- Work
- Heat
- Energy
- Extensive and intensive properties
- State functions
- The first law of thermodynamics – internal energy and enthalpy
- Heat capacity and specific heat
- Measurement of ΔU and ΔH
- Hess’s law of constant heat summation
- Enthalpy of bond dissociation
- Combustion
- Formation
- Atomization
- Sublimation
- Phase transition
- Ionization
- Solution and dilution
- Introduction of entropy as a state function
- The second law of thermodynamics
- Gibbs energy change for spontaneous and non-spontaneous process
- Criteria for equilibrium
- The third law of thermodynamics – a brief introduction
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UNIT 7: Equilibrium
16 topics- Equilibrium in physical and chemical processes
- Dynamic nature of equilibrium
- Law of mass action
- Equilibrium constant
- Factors affecting equilibrium – Le Chatelier’s principle
- Ionic equilibrium – ionization of acids and bases
- Strong and weak electrolytes
- Degree of ionization
- Ionization of polybasic acids
- Acid strength
- Concept of pH
- Hydrolysis of salts (elementary idea)
- Buffer solutions
- Henderson equation
- Solubility product
- Common ion effect (with illustrative examples)
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UNIT 8: Redox Reactions
5 topics- Concept of oxidation and reduction
- Redox reactions
- Oxidation number
- Balancing redox reactions in terms of loss and gain of electron and change in oxidation numbers
- Applications of redox reactions
NEET UG Physical Chemistry flashcards — 52 questions with answers
State the law of conservation of mass.
In a chemical reaction, matter is neither created nor destroyed; the total mass of reactants equals the total mass of products.
Define a mole and give 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 particles per mole.
What is the difference between molarity (M) and molality (m)?
Molarity = moles of solute per litre of solution (temperature-dependent). Molality = moles of solute per kilogram of solvent (temperature-independent).
State the law of multiple proportions.
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 ratio of small whole numbers.
How do you calculate percentage yield of a reaction?
Percentage yield = (actual yield / theoretical yield) x 100.
Write 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.
State Heisenberg's uncertainty principle with its formula.
It is impossible to determine simultaneously the exact position and momentum of an electron: delta x . delta p >= h / (4*pi).
What are the four quantum numbers and what does each describe?
Principal (n) = energy/shell size; Azimuthal (l) = subshell/shape; Magnetic (m_l) = orbital orientation; Spin (m_s) = electron spin (+1/2 or -1/2).
State the Aufbau principle.
Electrons fill atomic orbitals in order of increasing energy, lowest-energy orbitals first.
State Hund's rule of maximum multiplicity.
Electrons occupy degenerate orbitals singly with parallel spins before pairing occurs.
State Pauli's exclusion principle.
No two electrons in an atom can have the same set of all four quantum numbers; an orbital holds at most two electrons with opposite spins.
Give the Rydberg formula for the hydrogen atom spectral lines.
1/lambda = R_H (1/n1^2 - 1/n2^2), where R_H = 109677 cm^-1 and n2 > n1.
What is the basis of the modern periodic law?
The physical and chemical properties of elements are periodic functions of their atomic numbers.
How does atomic radius vary across a period and down a group?
It decreases across a period (increasing nuclear charge) and increases down a group (added shells).
How does ionization enthalpy vary across a period and down a group?
It increases across a period 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. Fluorine is the most electronegative element.
Why is the second ionization enthalpy always greater than the first?
Removing an electron from a positively charged cation requires more energy because the remaining electrons are held more tightly by the same nuclear charge.
State Boyle's law.
At constant temperature and amount of gas, the volume is inversely proportional to pressure: PV = constant.
State Charles's law.
At constant pressure, the volume of a fixed amount of gas is directly proportional to its absolute temperature: V/T = constant.
Write the ideal gas equation and identify R's value in SI units.
PV = nRT, where R = 8.314 J K^-1 mol^-1.
Show the other 32 Physical Chemistry flashcards
State Dalton's law of partial pressures.
The total pressure of a mixture of non-reacting gases equals the sum of the partial pressures of the individual gases.
State Graham's law of diffusion.
At constant temperature and pressure, the rate of diffusion of a gas is inversely proportional to the square root of its density (or molar mass).
Write the van der Waals equation for real gases.
(P + an^2/V^2)(V - nb) = nRT, where 'a' corrects for intermolecular attraction and 'b' for molecular volume.
State the first law of thermodynamics with its equation.
Energy can neither be created nor destroyed. delta U = q + w, where q is heat added and w is work done on the system.
Define enthalpy (H) in terms of internal energy.
H = U + PV; enthalpy is the heat content of a system at constant pressure.
What is an extensive vs an intensive property? Give one example each.
Extensive properties depend on amount of matter (e.g. mass, volume, enthalpy); intensive properties do not (e.g. temperature, density, pressure).
State the second law of thermodynamics in terms of entropy.
The entropy of an isolated system always increases for a spontaneous process; total entropy of the universe tends to a maximum.
Write the Gibbs free energy equation and the spontaneity condition.
delta G = delta H - T*delta S. A process is spontaneous when delta G < 0.
State the third law of thermodynamics.
The entropy of a perfect crystalline substance is zero at absolute zero (0 K).
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.
Define enthalpy of combustion.
The enthalpy change when one mole of a substance is completely burnt in excess oxygen; it is always negative (exothermic).
Define enthalpy of formation.
The enthalpy change when one mole of a compound is formed from its elements in their standard states.
Write the relation 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.
State Le Chatelier's principle.
If a system at equilibrium is disturbed by a change in concentration, pressure or temperature, the equilibrium shifts to counteract the change.
Define pH and give the formula.
pH = -log[H+]; it measures the acidity of a solution. Neutral pH = 7 at 25 C.
What is the ionic product of water (Kw) at 25 C?
Kw = [H+][OH-] = 1.0 x 10^-14 at 25 C.
State the common ion effect.
The suppression of ionization of a weak electrolyte by adding a strong electrolyte that shares a common ion.
Write the Henderson-Hasselbalch equation for an acidic buffer.
pH = pKa + log([salt]/[acid]).
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_A x_A + P_B x_B.
Name the four colligative properties.
Relative lowering of vapour pressure, elevation of boiling point, depression of freezing point, and osmotic pressure.
Write the formula for osmotic pressure.
pi = CRT = (n/V)RT, where C is molar concentration of solute.
State Henry's law for gas solubility.
The solubility (mole fraction) of a gas in a liquid is directly proportional to its partial pressure: p = K_H x.
What is the van't Hoff factor (i) and what does i > 1 indicate?
i = observed colligative property / calculated value; i > 1 indicates dissociation of the solute.
What is the difference between physisorption and chemisorption?
Physisorption involves weak van der Waals forces, is reversible and low-enthalpy; chemisorption involves chemical bonds, is irreversible and high-enthalpy.
What is the Tyndall effect?
The scattering of light by colloidal particles, making the path of a light beam visible through a colloid.
Define an emulsion and give an example.
A colloidal dispersion of one liquid in another immiscible liquid; e.g. milk (oil/fat in water).
Write the Nernst equation for an electrode at 298 K.
E = E° - (0.059/n) log Q, where n is the number of electrons transferred and Q is the reaction quotient.
State Faraday's first law of electrolysis.
The mass of substance deposited at an electrode is directly proportional to the quantity of electricity (charge) passed through the electrolyte.
How is the EMF of a cell calculated from electrode potentials?
E°cell = E°cathode - E°anode (both as reduction potentials).
What is the integrated rate equation for a first-order reaction?
k = (2.303/t) log([A0]/[A]); the half-life t(1/2) = 0.693/k 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 factor and Ea is the activation energy.
What is the n-factor and oxidation number change for an oxidizing agent in a redox reaction?
An oxidizing agent gains electrons and is reduced; its oxidation number decreases. The n-factor equals the number of electrons gained per molecule.
NEET UG Physical Chemistry FAQ
What is in the NEET UG Physical Chemistry syllabus?
NEET UG Physical Chemistry is split into 8 chapters: UNIT 1: Some Basic Concepts of Chemistry, UNIT 2: Structure of Atom, UNIT 3: Classification of Elements and Periodicity in Properties, UNIT 4: Chemical Bonding and Molecular Structure, UNIT 5: States of Matter: Gases and Liquids, UNIT 6: Thermodynamics, UNIT 7: Equilibrium and UNIT 8: Redox Reactions. Together they contain 97 topics and 19 sub-topics.
How many chapters are in NEET UG Physical Chemistry?
8 chapters, containing 97 topics and 19 sub-topics. The largest chapter is UNIT 6: Thermodynamics, with 25 topics.
Are there flashcards for NEET UG Physical Chemistry?
Yes — a 52-card Physical 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.