NEET Chemistry Sample Paper with Solutions PDF Download

IMPORTANT TOPICS OF NEET CHEMISTRY SAMPLE PAPER

PHYSICAL CHEMISTRY 

NAME OF THE CHAPTER

TOPICS

Some Basic Concepts in Chemistry 

Matter and its nature, Dalton’s atomic theory: Concept of atom, molecule, element, and compound; Law of chemical combination; Atomic and molecular masses, mole concept, molar mass, percentage composition, empirical and molecular formulae: Chemical equations and stoichiometry. 

Atomic Structure

Nature of electromagnetic radiation, photoelectric effect; Spectrum of the hydrogen atom. Bohr model of a hydrogen atom - its postulates, derivation of the relations for the energy of the electron and radii of the different orbits, limitations of Bohr’s model; Dual nature of matter, de Broglie’s relationship. Heisenberg uncertainty principle. Elementary ideas of quantum mechanics, the quantum mechanical model of the atom, and its important features. 

Quantum numbers and their significance; shapes of s, p, and d- orbitals, electron spin, and spin quantum number: Rules for filling electrons in orbitals - Aufbau principle. Pauli’s exclusion principle and Hund’s rule, electronic configuration of elements.

Chemical Bonding and Molecular Structure 

Kossel-Lewis approach to chemical bond formation, the concept of ionic and covalent bonds.
Ionic Bonding: formation of ionic bonds, factors affecting the formation of ionic bonds; calculation of lattice enthalpy. 

Covalent Bonding: concept of electronegativity, Fajan’s rule, dipole moment: Valance Shell Electron Pair Repulsion (VSEPR) theory and shapes of simple molecules. 

Quantum mechanical approach to covalent bonding: Valence bond theory - its important features, the concept of hybridization involving s, p, and d orbitals; Resonance. 

Molecular Orbital Theory - Its important features. LCAOs, types of molecular orbitals (bonding, antibonding), sigma and pi-bonds, molecular orbital electronic configurations of homonuclear diatomic molecules, the concept of bond order, bond length, and bond energy. 

Chemical Thermodynamics

Fundamentals of thermodynamics: System and surroundings, extensive and intensive properties, state functions, types of processes. 

The first law of thermodynamics - concept of work, heat internal energy and enthalpy, heat capacity, molar heat capacity; Hess’s law of constant heat summation; Enthalpies of bond dissociation, combustion, formation, atomization, sublimation, phase transition, hydration, ionization, and solution. 

The second law of thermodynamics - Spontaneity of processes, ∆S of the universe, and ∆G of the system as criteria for spontaneity.

Solutions 

Different methods for expressing the concentration of solution - molality, molarity, more fraction, percentage (by volume and mass both), the vapor pressure of solutions and Raoult’s Law - Ideal and non-ideal solutions, vapor pressure-composition; Colligative properties of dilute solutions - a relative lowering of vapor pressure, depression of freezing point, the elevation of boiling point and osmotic pressure; Determination of molecular mass using colligative properties; Abnormal value of molar mass, van’t Hoff factor and its significance. 

Equilibrium 

Meaning of equilibrium, the concept of dynamic equilibrium.

Equilibria involving physical processes: Solid-liquid, liquid-gas, and solid-gas equilibria, Henry’s Law. General characteristics of equilibrium involving physical processes. 

Equilibrium involving chemical processes: Law of chemical equilibrium, constants and their significance, factors affecting equilibrium concentration, pressure, temperature, the effect of catalyst; Le Chatelier’s principle. 

Ionic equilibrium: Weak and strong electrolytes, the ionization of electrolytes, various concepts of acids and bases (Arrhenius. Bronsted Lowry and Lewis), and their ionization, acid-base equilibria and ionization constants, ionization of water, pH factor, common ion effect, hydrolysis of salts and pH of their solutions, buffer solutions. 

Redox Reactions and Electrochemistry

Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning oxidation number, balancing of redox reactions. 

Electrolytic and metallic conduction, conductance in electrolytic solutions, molar conductivities and their variation with concentration: Kohlrausch’s law and its applications. 

Electrochemical cells - Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half-cell and cell reactions, emf of a Galvanic cell and its measurement: Nernst equation and its applications; Relationship between cell potential and Gibb’s energy change: Dry cell and lead accumulator; Fuel cells.

Chemical Kinetics

Rate of chemical reaction, factors affecting the rate of reactions: concentration, temperature, pressure, and catalyst; elementary and complex reactions, order and molecularity of reactions, rate law, rate constant and its units, differential and integral forms of zero and first-order reactions, their characteristics and half-lives, the effect of temperature on the rate of reactions, Arrhenius theory, activation energy and its calculation, collision theory of bimolecular gaseous reactions (no derivation).

INORGANIC CHEMISTRY 

Classification of Elements and Periodicity in Properties

Modern periodic law and present form of the periodic table, s, p, d, and f-block elements, periodic trends in properties of elements atomic and ionic radii, ionization enthalpy, electron gain enthalpy, valence, oxidation states, and chemical reactivity. 

P-Block Elements

Group 13 to Group 18 Elements

General Introduction: Electronic configuration and general trends in physical and chemical properties of elements across the periods and down the groups; unique behavior of the first element in each group. 

D and F-Block Elements

Transition Elements

General Introduction: electronic configuration, occurrence, and characteristics, general trends in properties of the first-row transition elements - physical properties, ionization enthalpy, oxidation states, atomic radii, color, catalytic behavior, magnetic properties, complex formation, interstitial compounds, alloy formation.

Inner Transition Elements

Lanthanoids - electronic configuration, oxidation states, and lanthanoid concentration. 

Actinoids - electronic configuration, and oxidation states. 

Co-ordination Compounds

Introduction to coordination compounds. Werner’s theory; ligands, coordination number, denticity. Chelation; IUPAC nomenclature of mononuclear coordination compounds, isomerism; Bonding-Valence bond approach basic ideas of Crystal field theory, color and magnetic properties; Importance of coordination compounds (in qualitative analysis, extraction of metals, and biological systems).

ORGANIC CHEMISTRY

Purification and Characterization of Organic Compounds

Purification - Crystallization, sublimation, distillation, differential extraction, and chromatography - principles and their applications. 

Qualitative analysis - Detection of nitrogen, sulfur, phosphorus, and halogens.

Quantitative analysis (basic principle only) - Estimation of carbon, hydrogen, nitrogen, halogens, sulfur, and phosphorus. 

Calculations of empirical formulae and molecular formulae: Numerical problems in organic quantitative analysis.

Some Basic Principles of Organic Chemistry

Tetravalency of carbon: Shapes of simple molecules - hybridization (s and p): Classification of organic compounds based on functional groups: and those containing halogens, oxygen, nitrogen, and sulfur’ Homologous series: Isomerism - structural and stereoisomerism. 

Nomenclature (Trivial and IUPAC)

Covalent bond fission - Homolytic and heterolytic: free radicals, carbocations, and carbanions; stability of carbocations and free radicals, electrophiles, and nucleophiles. 

Electronic displacement in a covalent bond

Inductive effect, electromeric effect, resonance, and hyperconjugation. 

Common types of organic reactions - Substitution, addition, elimination, and rearrangement.

Hydrocarbons 

Classification, isomerism, IUPAC nomenclature, general methods of preparation, properties, and reactions. 

Alkanes - Conformations: Sawhorse and Newman projections (of ethane): Mechanism of halogenation of alkanes.

Alkenes - Geometrical isomerism: Mechanism of electrophilic addition: addition of hydrogen, halogens, water, and hydrogen halides (Markownikoffs and peroxide effect): Ozonolysis and polymerization.

Alkynes - Acidic character: Addition of hydrogen, halogens, water, and hydrogen halides: Polymerization.

Aromatic hydrocarbons - Nomenclature, benzene - structure and aromaticity: Mechanism of electrophilic substitution: halogenation, nitration. 

Friedel - Craft’s alkylation and acylation, directive influence of the functional group in mono-substituted benzene. 

Organic Compounds Containing Halogens

General methods of preparation, properties, and reactions; Nature of C-X bond; Mechanisms of substitution reactions.

Uses; Environmental effects of chloroform, iodoform, freons, and DDT.

Organic Compounds Containing Oxygen

General methods of preparation, properties, reactions, and uses.

Alcohols: Identification of primary, secondary, and tertiary alcohols; mechanism of dehydration.

Phenols: Acidic nature, electrophilic substitution reaction: halogenation, nitration, and sulphonation. Reimer - Tiemann reaction. 

Ethers: Structure

Aldehyde and Ketones: Nature of carbonyl group; Nucleophilic addition to >C=O group, relative reactivities of aldehydes and ketones, Grignard reagent; oxidation: reduction (Wolff Kishner and Clemmensen); aldol condensation, Cannizzaro reaction. Haloform reaction, Chemical tests to distinguish between aldehydes and ketones.

Carboxylic Acids: Acidic strength and factors affecting it.

Organic Compounds Containing Nitrogen 

General methods of preparation, properties, reactions, and uses. 

Amines: Nomenclature, classification structure, basic character, and identification of primary, secondary, and tertiary amines and their basic character. 

Diazonium Salts: Importance in synthetic organic chemistry. 

Biomolecules 

General introduction and importance of biomolecules. 

Carbohydrates - Classification; aldoses and ketoses: monosaccharides (glucose and fructose) and constituent monosaccharides of oligosaccharides (sucrose, lactose, and maltose).

Proteins - Elementary idea of amino acids, peptide bonds, polypeptides. Proteins: primary, secondary, tertiary, and quaternary structure (qualitative idea only), denaturation of proteins, enzymes. 

Vitamins - Classification and functions.

Nucleic Acids - Chemical constitution of DNA and RNA, biological functions of nucleic acids. Hormones (general introduction).