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Jharkhand Board Class 11 Chemistry Syllabus (JAC)


BIOLOGY:         SET-1(Download) —SET-2(Download) —SET-3(Download)
PHYSICS:          SET-1(Download) —SET-2(Download) —SET-3(Download)
CHEMISTRY:    SET-1(Download) —SET-2(Download) —SET-3(Download)
MATH:               SET-1(Download) —SET-2(Download) —SET-3(Download)

Unit I: Some Basic Concepts of Chemistry
  • General Introduction: Importance and scope of chemistry. 
  • The historical approach to particulate nature of matter,  laws of chemical combination.
  • Dalton’s atomic theory: the concept of elements, atoms, and molecules. 
  • Atomic and molecular masses. 
  • Mole concept and molar mass; percentage composition and empirical and molecular formula; chemical reactions, stoichiometry and calculations based on stoichiometry.

Unit II: Structure of Atom

  • 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.
  • The 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, the Pauli exclusion principle, and Hund’s rule, electronic configuration of atoms, the stability of half-filled and completely filled orbitals.

Unit III: Classification of Elements and Periodicity in Properties

  • Significance of classification, a brief history of the 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, inert gas radii, ionization enthalpy, electron gain enthalpy, electronegativity, valence. 
  • Nomenclature of elements with atomic numbers greater than 100.

Unit IV: Chemical Bonding and Molecular Structure

  • Valence electrons, ionic bond, covalent bond, bond parameters, Lewis structure, the polar character of a covalent bond, the covalent character of an ionic bond, valence bond theory, resonance, the geometry of covalent molecules, VSEPR theory, the concept of hybridization involving s, p and d orbitals, and shapes of some simple molecules, molecular orbital theory of homonuclear diatomic molecules (qualitative idea only).
  •  Hydrogen bond.

Unit V: States of Matter: Gases and Liquids

  • Three states of matter, intermolecular interactions, types of bonding, melting and boiling points, the 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 behaviour, empirical derivation of gas equation, Avogadro number, ideal gas equation. 
  • Kinetic energy and molecular speeds (elementary idea), deviation from ideal behaviour, liquefaction of gases, critical temperature. 
  • Liquid State – Vapour pressure, viscosity and surface tension (qualitative idea only, no mathematical derivations).

Unit VI: Thermodynamics

  • 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, Second law of thermodynamics, Gibbs energy change for the spontaneous and non-spontaneous process, criteria for equilibrium. 
  • Third law of thermodynamics –Brief introduction

Unit VII: Equilibrium
  • Equilibrium in physical and chemical processes, dynamic nature of equilibrium, the law of mass action, the 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, the concept of pH., Hydrolysis of salts (elementary idea),, buffer solutions, Henderson equation, solubility product, common ion effect (with illustrative examples).

Unit VIII: Redox Reactions

  • 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.

Unit IX: Hydrogen

  • Position of hydrogen in the periodic table, occurrence, isotopes, preparation, properties and uses of hydrogen; hydrides – ionic, covalent and interstitial; physical and chemical properties of water, heavy water; hydrogen peroxide-preparation, reactions, use and structure; hydrogen as a fuel.

Unit X: s- Block Elements (Alkali and Alkaline earth metals)

  • Group 1 and Group 2 elements: General introduction, electronic configuration, occurrence, anomalous properties of the first element of each group, diagonal relationship, trends in the variation of properties (such as ionization enthalpy, atomic and ionic radii), trends in chemical reactivity with oxygen, water, hydrogen and halogens; uses. Preparation and Properties of Some Important Compounds: Sodium carbonate, sodium chloride, sodium hydroxide and sodium hydrogen carbonate, biological importance of sodium and potassium. CaO, CaCO3 , and industrial use of lime and limestone, biological importance of Mg and Ca

Unit XI: Some p-Block Elements

  • General Introduction to p-Block Elements Group 13 elements: General introduction, electronic configuration, occurrence, the variation of properties, oxidation states, trends in chemical reactivity, anomalous properties of the first element of the group; Boronphysical and chemical properties, some important compounds: borax, boric acids, boron hydrides. 
  • Aluminium: uses, reactions with acids and alkalies. 5 Group 14 elements: General introduction, electronic configuration, occurrence, the variation of properties, oxidation states, trends in chemical reactivity, anomalous behaviour of the first element. 
  • Carbon - catenation, allotropic forms, physical and chemical properties; uses of some important compounds: oxides. Important compounds of silicon and a few uses: silicon tetrachloride, silicones, silicates and zeolites, their uses.

Unit XII: Organic Chemistry – Some Basic Principles and Techniques

  • General introduction, methods of purification, qualitative and quantitative analysis, classification and IUPAC nomenclature of organic compounds. 
  • Electronic displacements in a covalent bond: inductive effect, electromeric effect, resonance and hyperconjugation. Homolytic and heterolytic fission of a covalent bond: free radicals, carbocations, carbanions; electrophiles and nucleophiles, types of organic reactions.

Unit XIII: Hydrocarbons

  • Classification of Hydrocarbons. Aliphatic Hydrocarbons: Alkanes – Nomenclature, isomerism, conformations (ethane only), physical properties, chemical reactions including free radical mechanism of halogenation, combustion and pyrolysis. 
  • Alkenes– Nomenclature, the structure of double bond (ethene), geometrical isomerism, physical properties, methods of preparation; chemical reactions: addition of hydrogen, halogen, water, hydrogen halides (Markovnikov’s addition and peroxide effect), ozonolysis, oxidation, mechanism of electrophilic addition. Alkynes – Nomenclature, the structure of triple bond (ethyne), physical properties, methods of preparation, chemical reactions: acidic character of alkynes, addition reaction of - hydrogen, halogens, hydrogen halides and water. 
  • Aromatic hydrocarbons – Introduction, IUPAC nomenclature; Benzene: resonance, aromaticity ; chemical properties: mechanism of electrophilic substitution – nitration sulphonation, halogenation, Friedel Craft’s alkylation and acylation; directive influence of the functional group in mono-substituted benzene; carcinogenicity and toxicity.

Unit XIV: Environmental Chemistry

  • Environmental pollution – Air, water and soil pollution,
  • Chemical reactions in the atmosphere, smog, major atmospheric pollutants.
  • Acid rain, ozone and its reactions, effects of depletion of the ozone layer, greenhouse effect and global warming – pollution due to industrial wastes.
  • Green chemistry as an alternative tool for reducing pollution, strategy for control of environmental pollution.


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