JEE Main 2019 Chemistry Syllabus- Get Physical & Organic Chemistry Syllabus Here

JEE Main 2019 Chemistry Syllabus is available for the students who are appearing for the JEE Main Examination 2019. This examination is conducted by the National Testing Agency (NTA) Twice a year for taking admissions into various Engineering and Technology courses across the country.

The JEE Main Chemistry syllabus is based on the Class (Standard) XI and XII. Here we have provided the JEE Main 2019 Syllabus (Chemistry )which is divided into Unite wise section which is suitable for the students to get the clear Idea of Physical and Chemical Chemistry.

JEE Main Chemistry Syllabus is divided into three sections, i.e., Section A, SectionB and Section C, where Section A Contains Physical Chemistry which has 10 Units, and Section B Contains Organic Chemistry which has 8 Units, and Section C has 10 Units.

JEE Main Chemistry Syllabus 2019- PDF Available

NewJEE Main 2019 Chemistry Syllabus has been declared. Click Here to Download PDF.

Section A

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Physical Chemistry is the part of Section A, and It contains 10 Units.

Unit 1- Some Basic Concepts in ChemistryMatter and its nature, Dalton’s 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.
Unit 2– States of MatterClassification of matter into solid, liquid and gaseous states.

Gaseous State:

Measurable properties of gases; Gas laws – Boyle’s law, Charle’s law, Graham’s law of diffusion, Avogadro’s law, Dalton’s 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 behavior, compressibility factor and van der Waals equation.

Liquid State:

Properties of liquids – vapor pressure, viscosity and surface tension, and effect of temperature on them (qualitative treatment only).

Solid State:

Classification of solids: molecular, ionic, covalent and metallic solids, amorphous and crystalline solids (elementary idea); Bragg’s Law and its applications; Unit cell and lattices, packing in solids (fee, bec and hep lattices), voids, calculations involving unit cell parameters, imperfection in solids; Electrical and magnetic properties.

 

Unit 3– Atomic StructureThomson 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’s model; Dual nature of matter, de-Broglie’s relationship, Heisenberg uncertainty principle. Elementary ideas of quantum mechanics, a quantum mechanical model of the atom, its important features.

The concept of atomic orbitals as one electron wave functions.

Variation of t|/ and \|/2 with r for Is 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

Aufbau principle, Pauli’s exclusion principle, and Hund’s rule, electronic configuration of elements, the extra stability of half-filled and filled orbitals.

Unit 4-Chemical Bonding and Molecular StructureKossel – 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; Valence Shell Electron Pair Repulsion (VSEPR) theory and shapes of simple molecules.

Quantum mechanical approach to covalent bonding:

Valence bond theory – Its essential 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.

Elementary idea of metallic bonding. Hydrogen bonding and its applications.

 

Unit 5– Chemical ThermodynamicsFundamentals of thermodynamics: System and surroundings, extensive and intensive properties, state functions, types of processes.

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; AS of the universe and AG of the system as criteria for spontaneity, AG” (Standard Gibbs energy change) and equilibrium constant.

Unit 6– SolutionsDifferent methods for expressing concentration of solution – molality, molarity, mole fraction, percentage (by volume and mass both), vapour pressure of solutions and Raoult’s Law – 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’t Hoff factor and its significance.

Unit 7– EquilibriumMeaning of equilibrium, 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.

Equilibria involving chemical processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance, significance of AG and AG” in chemical equilibria, factors affecting equilibrium concentration, pressure, temperature, effect of catalyst; Le Chatelier’s principle.

 

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.

Unit 8–  Redox Reactions and ElectrochemistryElectronic 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 Gibbs’ energy change; Dry cell and lead accumulator; Fuel cells.

 

Unit 9– Chemical KineticsRate 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 .

Arrhenius theory, activation energy, and its calculation, collision theory of bimolecular gaseous reactions (no derivation).

Unit 10– Surface Chemistry

 

Adsorption- Physisorption and chemisorption and their characteristics, factors affecting the adsorption of gases on solids – Freundlich and Langmuir adsorption isotherms, adsorption from solutions.

Catalysis – Homogeneous and heterogeneous, activity and selectivity of solid catalysts, enzyme catalysis, and its mechanism.

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.

 

 

Section B

Organic Chemistry is the part of Section B, and It contains 8 Units.

 

Unit 11- Classification of Elements and Periodicity in PropertiesModem 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.

 

Unit 12– General Principles and Processes of Isolation of MetalsModes 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 removal of Al, Cu, Zn, and Fe; Thermodynamic and electrochemical principles involved in the extraction of metals.
Unit 13- HydrogenPosition of hydrogen in periodic table, isotopes, preparation, properties and uses of hydrogen; Physical and chemical properties of water and heavy water; Structure, development, reactions, and uses of hydrogen peroxide; Classification of hydrides – ionic, covalent and interstitial; Hydrogen as a fuel.
Unit 14- S-Block Elements (Alkali and Alkaline Earth Metals)

 

Group -1 and 2 Elements

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.

Preparation and properties of some important compounds – sodium carbonate and sodium hydroxide and sodium hydrogen carbonate; Industrial uses of lime, limestone, Plaster of Paris and cement; Biological significance of Na, K, Mg and Ca.

 

Unit 15- 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.

Groupwise study of the p – block elements Group -13

Preparation, properties, and uses of boron and aluminum; Structure, properties and uses of borax, boric acid, diborane, boron trifluoride, aluminum chloride and alums.

 

Group -14

The tendency for catenation; Structure, properties, and uses of Allotropes and oxides of carbon, silicon tetrachloride, silicates, zeolites and silicones.

 

Group -15

Properties and uses of nitrogen and phosphorus; Allotrophic forms of phosphorus; Preparation, properties, structure and methods of ammonia, nitric acid, phosphine and phosphorus halides, (PC13, PCI,); Structures of oxides and oxoacids of nitrogen and phosphorus.

 

Group -16

Preparation, properties, structures and uses of ozone; Allotropic forms of sulfur; Preparation, properties, structures, and uses of sulphuric acid (including its industrial preparation); Structures of oxoacids of sulfur.

 

Group -17

Preparation, properties, and uses of hydrochloric acid; Trends in the acidic nature of hydrogen halides; Structures of Interhalogen compounds and oxides and oxoacids of halogens.

 

Group-18

Occurrence and uses of noble gases; Structures of fluorides and oxides of xenon.

 

Unit 16- d and F Block ElementsTransition 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, colour, catalytic behaviour, magnetic properties, complex formation, interstitial compounds, alloy formation; Preparation, properties and uses of K2 Cr, 07 and Kmn04.

 

Inner Transition Elements

Lanthanoids – Electronic configuration, oxidation states and lanthanoid contraction.

Actinoids – Electronic configuration and oxidation states.

 

Unit 17– Co-Ordination CompoundsIntroduction to co-ordination compounds, Werner’s theory; ligands, coordination number, denticity, chelation; IUPAC nomenclature of mononuclear coordination compounds, isomerism; Bonding-Valence bond approach and basic ideas of Crystal field theory, colour and magnetic properties; Importance of co­ordination compounds (in qualitative analysis, extraction of metals and in biological systems).

 

Unit 18- Environmental ChemistryEnvironmental pollution – Atmospheric, water, and soil.

Atmospheric pollution – Tropospheric and Stratospheric

Tropospheric pollutants – Gaseous pollutants: Oxides of carbon, nitrogen, and sulfur, hydrocarbons; their sources, harmful effects and prevention; Green house effect and Global warming; Acid rain;

Particulate pollutants: Smoke, dust, smog, fumes, mist; their sources, harmful effects, and prevention.

Stratospheric pollution– Formation and breakdown of ozone, depletion of ozone layer – its mechanism and effects.

Water Pollution – Major pollutants such as pathogens, organic wastes, and chemical pollutants; their harmful effects and prevention.

Soil pollution – Major pollutants such as Pesticides (insecticides, herbicides and fungicides), their harmful effects and prevention.

Strategies to control environmental pollution.

Section C

Physical Chemistry is the part of Section and It contains 10 Units.

Unit 19– Purification and Characterization of Organic CompoundsPurification – Crystallization, sublimation, distillation, differential extraction and chromatography – principles and their applications.

Qualitative analysis – Detection of nitrogen, sulphur, phosphorus and halogens.

Quantitative analysis (basic principles only) – Estimation of carbon, hydrogen, nitrogen, halogens, sulphur, phosphorus.

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

 

Unit 20– 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 sulphur; 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.

 

Unit 21-HydrocarbonsClassification, 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 clcctrophilic addition: addition of hydrogen, halogens, water, hydrogen halides (Markownikoff s 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 functional group in mono-substituted benzene.

 

Unit 22– Organic Compounds Containing HalogensGeneral methods of preparation, properties and reactions; Nature of C-X bond; Mechanisms of substitution reactions.

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

 

Unit 23– Organic Compounds Containing OxygenGeneral methods of preparation, properties, reactions and uses.

 

ALCOHOLS, PHENOLS AND ETHERS

 

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

Phenols: Acidic nature, electrophilic substitution reactions: halogenation, nitration and sulphonation, Reitner – Tiemann reaction.

Ethers: Structure.

Aldehyde and Ketones: Nature of carbonyl group;Nucleophilic addition to >C=0 group, relative reactivities of aldehydes and ketones; Important reactions such as – Nucleophilic addition reactions (addition of HCN, NH, and its derivatives), Griguard reagent; oxidation; reduction (Wolff Kishner and Clemmensen); acidity of a-hydrogen, aldol condensation, Cannizzaro reaction, Hatoform reaction;

Chemical tests to distinguish between aldehydes and Ketones.

Carboxylic Acids

Acidic strength and factors affecting it.

Unit 24– Organic Compounds containing NitrogenGeneral 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.

 

Unit 25  PolymersGeneral introduction and importance of biomolecules.

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

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

Vitamins – Classification and functions.

Nucleic Acids – Chemical constitution of DN A and RNA.

Biological functions of nucleic acids.

Unit 26- BiomoleculesGeneral introduction and importance of biomolecules.

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

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

Vitamins – Classification and functions.

Nucleic Acids – Chemical constitution of DN A and RNA.

Biological functions of nucleic acids.

 

Unit 27–  Chemistry in Everyday LifeChemicals in medicines – Analgesics, tranquilizers, antiseptics, disinfectants, antimicrobials, antifertility drugs, antibiotics, antacids, antihistamins – their meaning and common examples.

Chemicals in food – Preservatives, artificial sweetening agents – common examples.

Cleansing agents – Soaps and detergents, cleansing action.

 

Unit 28– Principles Related to Practical ChemistryDetection of extra elements (N,S, halogens) in organic compounds; Detection of the following functional groups: hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketone), carboxyl and amino groups in organic compounds.

Chemistry involved in the preparation of the following:

Inorganic compounds: Mohr’s salt, potash alum. Organic compounds: Aeetanilide, pnitroacetanilide, aniline yellow, iodoform.

Chemistry involved in the titrimetric excercises -Acids bases and the use of indicators, oxalic-acid vs KMnO,, Mohr’s salt vs KMnO,.

Chemical principles involved in the qualitative salt analysis:

Cations – Pb2+, Cu!+, Af,+, Fe1+, Zn2+, Ni2+, Ca2+, Ba2+,

Mg2+, nh;.

Anions- CO,”, S2~, SO4″, NO”, NO~2, Cf, Br”, I” . (Insoluble salts excluded).

  • Chemical principles involved in the following experiments:

1. Enthalpy of solution of CuS04

2. Enthalpy of neutralization of strong acid and strong base.

3. Preparation of lyophilic and lyophobic sols.

4. Kinetic study of reaction of iodide ion with hydrogen peroxide at room temperature.

 

 

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