{"id":21784,"date":"2019-09-03T12:20:41","date_gmt":"2019-09-03T06:50:41","guid":{"rendered":"https:\/\/www.entrancezone.com\/engineering\/?p=21784"},"modified":"2020-01-07T18:02:12","modified_gmt":"2020-01-07T12:32:12","slug":"jee-main-2020-chemistry-syllabus","status":"publish","type":"post","link":"https:\/\/www.entrancezone.com\/engineering\/jee-main-2020-chemistry-syllabus\/","title":{"rendered":"JEE Main 2020 Chemistry Syllabus: Important Topics"},"content":{"rendered":"

JEE Main 2020 Chemistry Syllabus<\/strong> is released by NTA along with Information booklet. Chemistry section consists of three parts i.e. Physical Chemistry, Inorganic chemistry and organic chemistry. So, the knowledge of complete JEE Main 2020 syllabus is essential to perform well in the examination. The aspiring candidates must read the below article for complete and detailed information related to JEE Main 2020 Chemistry Syllabus<\/strong>.<\/p>\n

Latest Update: National Testing Agency has released the JEE Mains<\/a> Application Form on 03 September 2019.<\/strong><\/p>\n

JEE Main 2020 Chemistry Syllabus: Section – A<\/h2>\n

The JEE MAIN 2020 Chemistry Syllabus is published by NTA along with Information Brochure every year. There is no change till last year and expected that there will be no change this year also. if there will be any change this year in JEE MAIN Brochure we will update it here.<\/p>\n

Physical Chemistry<\/h3>\n

Unit 1 – Some Basic Concepts in Chemistry<\/strong><\/p>\n

Matter and its nature, Dalton\u2019s atomic theory; Concept of atom, molecule, element, and compound; Physical quantities and their measurements in Chemistry, precision, and accuracy, significant figures, S.I. Units, dimensional analysis; Laws of chemical combination; Atomic and molecular masses, mole concept, molar mass, percentage composition, empirical and molecular formulae; Chemical equations and stoichiometry.<\/p>\n

Unit 2 – States of Matter<\/strong><\/p>\n

Classification of matter into solid, liquid and gaseous states.<\/p>\n

Gaseous State: Measurable properties of gases; Gas laws – Boyle\u2019s law, Charle\u2019s law, Graham\u2019s law of diffusion, Avogadro\u2019s law, Dalton\u2019s law of partial pressure; Concept of Absolute scale of temperature; Ideal gas equation; Kinetic theory of gases (only postulates); Concept of average, root mean square and most probable velocities; Real gases, deviation from Ideal behaviour, compressibility factor and van der Waals equation.<\/p>\n

Liquid State: Properties of liquids – vapour pressure, viscosity and surface tension and effect of temperature on them (qualitative treatment only).<\/p>\n

Solid State: Classification of solids: molecular, ionic, covalent and metallic solids, amorphous and crystalline solids (elementary idea); Bragg\u2019s Law and its applications; Unit cell and lattices, packing in solids (fcc, bcc and hcp lattices), voids, calculations involving unit cell parameters, imperfection in solids; Electrical, magnetic and dielectric properties.<\/p>\n

Unit 3 – Atomic Structure<\/strong><\/p>\n

Thomson and Rutherford atomic models and their limitations; Nature of electromagnetic radiation, photoelectric effect; Spectrum of hydrogen atom, Bohr model of hydrogen atom – its postulates, derivation of the relations for energy of the electron and radii of the different orbits, limitations of Bohr\u2019s model; Dual nature of matter, de Broglie’s relationship, Heisenberg uncertainty principle. Elementary ideas of quantum mechanics, the quantum mechanical model of the atom, its important features. Concept of atomic orbitals as one-electron wave functions; Variation of \u03a8 and \u03a82<\/sup> with r for 1s and 2s orbitals; various quantum numbers (principal, angular momentum and magnetic quantum numbers) and their significance; shapes of s, p and d – orbitals, electron spin and spin quantum number; Rules for filling electrons in orbitals \u2013 Aufbau principle, Pauli\u2019s exclusion principle and Hund\u2019s rule, electronic configuration of elements, extra stability of half-filled and completely filled orbitals.<\/p>\n

Unit 4 – Chemical Bonding and Molecular Structure<\/strong><\/p>\n

Kossel – Lewis approach to chemical bond formation, the concept of ionic and covalent bonds.<\/p>\n

Ionic Bonding: Formation of ionic bonds, factors affecting the formation of ionic bonds; calculation of lattice enthalpy.<\/p>\n

Covalent Bonding: Concept of electronegativity, Fajan\u2019s rule, dipole moment; Valence Shell Electron Pair Repulsion (VSEPR) theory and shapes of simple molecules.\u00a0Quantum mechanical approach to covalent bonding: Valence bond theory – Its important features, the concept of hybridization involving s, p, and d orbitals; Resonance.<\/p>\n

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.<\/p>\n

Elementary idea of metallic bonding. Hydrogen bonding and its applications.<\/p>\n

Unit 5 – Chemical Thermodynamics<\/strong><\/p>\n

Fundamentals of thermodynamics: System and surroundings, extensive and intensive properties, state functions, types of processes.<\/p>\n

The first law of thermodynamics – Concept of work, heat internal energy and enthalpy, heat capacity, molar heat capacity; Hess\u2019s law of constant heat summation; Enthalpies of bond dissociation, combustion, formation, atomization, sublimation, phase transition, hydration, ionization, and solution.<\/p>\n

The second law of thermodynamics; Spontaneity of processes; \u0394S of the universe and \u0394G of the system as criteria for spontaneity, \u0394G\u00b0 (Standard Gibbs energy change) and equilibrium constant.<\/p>\n

Unit 6 – Solutions<\/strong><\/p>\n

Different methods for expressing concentration of solution – molality, molarity, mole fraction, percentage (by volume and mass both), vapour pressure of solutions and Raoult\u2019s Law \u2013 Ideal and non-ideal solutions, vapour pressure – composition, plots for ideal and non-ideal solutions; Colligative properties of dilute solutions – relative lowering of vapour pressure, depression of freezing point, elevation of boiling point and osmotic pressure; Determination of molecular mass using colligative properties; Abnormal value of molar mass, van\u2019t Hoff factor and its significance.<\/p>\n

Unit 7 – Equilibrium<\/strong><\/p>\n

Meaning of equilibrium, the concept of dynamic equilibrium.<\/p>\n

Equilibria involving physical processes: Solid-liquid, liquid – gas and solid \u2013 gas equilibria, Henry\u2019s law, general characteristics of equilibrium involving physical processes.<\/p>\n

Equilibria involving chemical processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance, the significance of \u0394G and \u0394G\u00b0 in chemical equilibria, factors affecting equilibrium concentration, pressure, temperature, effect of catalyst; Le Chatelier\u2019s principle.<\/p>\n

Ionic equilibrium: Weak and strong electrolytes, ionization of electrolytes, various concepts of acids and bases (Arrhenius, Bronsted – Lowry and Lewis) and their ionization, acid-base equilibria (including multistage ionization) and ionization constants, ionization of water, pH scale, common ion effect, hydrolysis of salts and pH of their solutions, solubility of sparingly soluble salts and solubility products, buffer solutions.<\/p>\n

Unit 8 – Redox Reactions and Electrochemistry<\/strong><\/p>\n

Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning oxidation number, balancing of redox reactions.<\/p>\n

Electrolytic and metallic conduction, conductance in electrolytic solutions, specific and molar conductivities and their variation with concentration: Kohlrausch\u2019s law and its applications.<\/p>\n

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 Gibbs\u2019 energy change; Dry cell and lead accumulator; Fuel cells.<\/p>\n

Unit 9 – Chemical Kinetics<\/strong><\/p>\n

Rate of a 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, effect of temperature on rate of reactions \u2013 Arrhenius theory, activation energy and its calculation, collision theory of bimolecular gaseous reactions (no derivation).<\/p>\n

Unit 10 – Surface Chemistry<\/strong><\/p>\n

Adsorption- Physisorption and chemisorption and their characteristics, factors affecting the adsorption of gases on solids – Freundlich and Langmuir adsorption isotherms, adsorption from solutions.<\/p>\n

Colloidal state – distinction among true solutions, colloids, and suspensions, classification of colloids – lyophilic, lyophobic; multi molecular, macromolecular and associated colloids (micelles), preparation and properties of colloids – Tyndall effect, Brownian movement, electrophoresis, dialysis, coagulation, and flocculation; Emulsions and their characteristics.<\/p>\n

JEE Main 2020 Chemistry Syllabus: Section – B<\/h3>\n

Inorganic Chemistry<\/h3>\n

Unit 11 – Classification of Elements and Periodicity in Properties<\/strong><\/p>\n

Modem 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>\n

Unit 12 – General Principles and Processes of Isolation of Elements<\/strong><\/p>\n

Modes of occurrence of elements in nature, minerals, ores; Steps involved in the extraction of metals – concentration, reduction (chemical and electrolytic methods) and refining with special reference to the extraction of Al, Cu, Zn and Fe; Thermodynamic and electrochemical principles involved in the extraction of metals.<\/p>\n

Unit 13 – Hydrogen<\/strong><\/p>\n

Position of hydrogen in periodic table, isotopes, preparation, properties and uses of hydrogen; Physical and chemical properties of water and heavy water; Structure, preparation, reactions, and uses of hydrogen peroxide; Hydrogen as a fuel.<\/p>\n

Unit 14 – S – Block Elements (Alkali and Alkaline Earth Metals)<\/strong><\/p>\n

Group – 1 and 2 Elements<\/p>\n

General introduction, electronic configuration and general trends in physical and chemical properties of elements, anomalous properties of the first element of each group, diagonal relationships.<\/p>\n

Preparation and properties of some important compounds – sodium carbonate and sodium hydroxide; Industrial uses of lime, limestone, Plaster of Paris and cement; Biological significance of Na, K, Mg and Ca.<\/p>\n

Unit 15 – P – Block Elements<\/strong><\/p>\n

Group – 13 to Group 18 Elements<\/p>\n

General Introduction: Electronic configuration and general trends in physical and chemical properties of elements across the periods and down the groups; unique behaviour of the first element in each group.<\/p>\n

Groupwise study of the p \u2013 block elements<\/p>\n