UP Board Class 11 Chemistry 2022-23 Reduced Syllabus

Chemistry is one of a few subjects that students really find interesting. Concepts of class 11 are directly asked in competitive examinations like JEE & NEET. It prepares you for a career in various domains like Pharmaceutical research, or environmental causes, etc. 

UP Board Class 11 Chemistry syllabus is a detailed set of content that covers all the topics taught in previous classes in a deeper way, which also makes it more extensive and tougher to cover for some students. The first step for any student to prepare for UP Board exams is to have a clear understanding of the syllabus.

In this page, we have provided direct and free access to the Reduced Class 11 Chemistry Syllabus PDF for the 2022-23 session.

Reduced Syllabus for 2022-23 Academic Session

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In the table given below, we have also provided the Reduced Syllabus for the 2022-23 session.

Chemistry 2022-23 Reduced Syllabus
Units Unit Names Marks
1 Some Basic Concepts of Chemistry 05
2 Structure of Atom 06
3 Classification of Elements and Periodicity in Properties 05
4 Chemical Bonding and Molecular Structure 05
5 States of Matter: Gases and Liquids 05
6 Chemical Thermodynamics 04
7 Equilibrium 06
8 Redox Reactions 05
9 Hydrogen 03
10 The s-block Elements 05
11 The p-block Elements 06
12 Organic Chemistry: Some basic Principles and Techniques 07
13 Hydrocarbons 08
PRACTICAL WORK* 30
TOTAL 100

No items found.

*Practical Work

  • Content based experimentation (04)
  • Volumetric analysis (08)
  • Salt Analysis (06)
  • Element analysis in organic compound (02)
  • Classroom records and project work (05)
  • Oral test (05)

CHEMISTRY CHAPTERS

Unit 1: Some Basic Concepts of Chemistry

  • General Introduction: Importance and scope of Chemistry. 
  • Atomic and molecular masses, mole concept and molar mass, percentage composition, empirical and molecular formula, chemical reactions, stoichiometry, and calculations based on stoichiometry.
  • <red> Nature of matter, laws of chemical combination, Dalton’s atomic theory: the concept of elements, atoms and molecules. <red> 

Unit 2: Structure of Atom

  • 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, the concept of orbitals, quantum numbers, shapes of s, p and d orbitals, rules for filling electrons in orbitals – Aufbau principle, Pauli’s exclusion principle and Hund’s rule, electronic configuration of atoms, the stability of half-filled and completely filled orbitals.
  • <red> Discovery of Electron, Proton, and Neutron, atomic number, isotopes, and isobars. Thomson’s model and its limitations. Rutherford’s model and its limitations. <red>

Unit 3: Classification of Elements and Periodicity in Properties

  • Modern periodic law and the present form of the periodic table, periodic trends in properties of elements -atomic radii, ionic radii, inert gas radii, Ionisation enthalpy, electron gain enthalpy, electronegativity, valency. Nomenclature of elements with atomic numbers greater than 100.
  • <red> Significance of classification, a brief history of the development of the periodic table. <red>

Unit 4: Chemical Bonding and Molecular Structure

  • 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 and shapes of some simple molecules, molecular orbital theory of homonuclear diatomic molecules (qualitative idea only), Hydrogen bond.

Unit 5: 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, Charles law, Gay Lussac’s law, Avogadro’s law, ideal behavior, empirical derivation of gas equation, Avogadro’s number, ideal gas equation and deviation from ideal behavior
  • <red> Liquefaction of gases, critical temperature, kinetic energy and molecular speeds (elementary idea), Liquid State- vapour pressure, viscosity, and surface tension (qualitative idea only, no mathematical derivations). <red>

Unit 6: Chemical Thermodynamics

  • Concepts of System and types of systems, surroundings, work, heat, energy, extensive and intensive properties, state functions. 
  • The first law of thermodynamics -internal energy and enthalpy, measurement of U and H, Hess’s law of constant heat summation, enthalpy of bond dissociation, combustion, formation, atomization, sublimation, phase transition, ionisation, solution, and dilution. The second law of Thermodynamics (brief introduction) 
  • Introduction of entropy as a state function, Gibb’s energy change for spontaneous and nonspontaneous processes.
  • Third law of thermodynamics (brief introduction).
  • <red> Heat capacity and specific heat, criteria for equilibrium. <red>

Unit 7: Equilibrium

  • Equilibrium in physical and chemical processes, dynamic nature of equilibrium, the law of mass action, equilibrium constant, factors affecting equilibrium – Le Chatelier’s principle, ionic equilibrium- ionisation of acids and bases, strong and weak electrolytes, degree of ionisation, ionisation of polybasic acids, acid strength, the concept of pH, buffer solution, solubility product, common ion effect (with illustrative examples).
  • <red> Hydrolysis of salts (elementary idea), Henderson Equation. <red>

Unit 8: Redox Reactions

  • Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox reactions, in terms of loss and gain of electrons and change in oxidation number.
  • <red> Applications of redox reactions. <red>

Unit 9: Hydrogen

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

Unit 10: 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 ionisation enthalpy, atomic and ionic radii), trends in chemical reactivity with oxygen, water, hydrogen, and halogens, uses. 
  • <red> Preparation and Properties of Some Important Compounds: Sodium Carbonate, Sodium Chloride, Sodium Hydroxide and Sodium Hydrogen carbonate, Biological importance of Sodium and Potassium. Calcium Oxide and Calcium Carbonate and their industrial uses, biological importance of Magnesium and Calcium. <red>

Unit 11: Some p-Block Elements

  • General Introduction to p -Block Elements 
  • Group 13 Elements: General introduction, electronic configuration, occurrence, a variation of properties, oxidation states, trends in chemical reactivity, anomalous properties of the first element of the group, Boron – physical and chemical properties.
  • Group 14 Elements: General introduction, electronic configuration, occurrence, a variation of properties, oxidation states, trends in chemical reactivity, anomalous behaviour of first elements. Carbon-catenation, allotropic forms, physical and chemical properties.
  • <red> Elements of group 13 – Some important compounds: Borax, Boric acid, Boron Hydrides, Aluminium: Reactions with acids and alkalis, uses. <red>  
  • <red> Elements of group 14 – Carbon: uses of some important compounds: oxides, Important compounds of Silicon and a few uses: Silicon Tetrachloride, Silicones, Silicates and Zeolites, their uses. <red>

Unit 12: Organic Chemistry -Some Basic Principles and Techniques

  • General introduction, 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. 
  • <red> Methods of purification, qualitative and quantitative analysis. <red>

Unit 13: Hydrocarbons

  • Classification of Hydrocarbons 
  • Aliphatic Hydrocarbons: 
  1. Alkanes – Nomenclature, isomerism, conformation (ethane only), physical properties, chemical reactions 
  2. 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.
  3. 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 Crafts alkylation and acylation, directive influence of the functional group in monosubstituted benzene. Carcinogenicity and toxicity.
  • <red> Free radical mechanism of halogenation, combustion, and pyrolysis. <red>

<red> Unit 14: Environmental Chemistry <red>

  • <red> Environmental pollution - air, water and soil pollution, chemical reactions in atmosphere, smog, major atmospheric pollutants, acid rain, ozone and its reactions, effects of depletion of ozone layer, greenhouse effect and global warming- pollution due to industrial wastes, green chemistry as an alternative tool for reducing pollution, strategies for control of environmental pollution. <red>

Unit XIV. Environmental Chemistry

  • Deleted Topics: 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, strategies for control of environmental pollution.