Syllabus Of Grade XI - Chemistry Theory (CH1105)

Instructions:

  • This Syllabus is divided into two parts first is theoretical and second is practical. All the parts are compulsory.
  • Separate marks are given with each unit.
Unit Area Covered Marks
Unit 1 Some Basic Concepts of Chemistry 05 read more
Unit 2 Structure of Atom 05 read more
Unit 3 Classification of Elements And Periodicity in Properties 05 read more
Unit 4 Chemical Bonding and Molecular Structure 05 read more
Unit 5 States of Matter: Gases and Liquids 05 read more
Unit 6 Thermodynamics 05 read more
Unit 7 Equilibrium 05 read more
Unit 8 Redox Reactions 05 read more
Unit 9 Hydrogen 05 read more
Unit 10 S-Block Elements 05 read more
Unit 11 Some P-Block Elements 05 read more
Unit 12 Organic Chemistry - Some Basic Principles 05 read more
Unit 13 Aliphatic Hydrocarbons 05 read more
Unit 14 Environmental Chemistry 05 read more
Total Marks 70 Time: 3 Hours

Syllabus Of Grade XI - Chemistry Practical (PCH1105)

Instructions:

  • All the units are compulsory.
  • Separate marks are given with each unit.
Unit Area Covered Marks
Unit 1 BASIC LABORATORY TECHNIQUES 05 read more
Unit 2 CHARACTERIZATION AND PURIFICATION OF CHEMICAL SUBSTANCE 05 read more
Unit 3 EXPERIMENTS RELATED TO pH CHANGE 05 read more
Unit 4 CHEMICAL EQUILIBRIUM 05 read more
Unit 5 QUANTITATIVE ESTIMATION 05 read more
Unit 6 QUALITATIVE ANALYSIS 05 read more
Total Marks 30 Time: 3 Hours

Unit 1

Some Basic Concepts of Chemistry (05 Marks)

  • General Introduction
  • Measurement of Properties of Matter The International System of units Uncertainty in measurement
  • Laws of Chemical Combination
    • Statement of laws of chemical combination
    • Importance of laws of chemical combination
    • Dalton's Atomic Theory
  • Empirical Formula and Molecular Formula
    • Atomic mass
    • Molar mass
    • Empirical formula
    • Molecular formula
  • Mole Concept and Stoichiometry
    • Mole concept
    • Stoichiometric calculations

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Unit 2

Structure of Atom (05 Marks)

  • Introduction to Structure of Atom
  • Atomic models
    • Thomson model
    • Rutherford model
    • Bohr model
    • Dual behaviour
  • Quantum Mechanical Model
    • Concept of orbitals
    • Heisenberg's uncertainty principle
    • Quantum numbers
  • Shapes of Atomic Orbitals
    • Shape of s, p and d orbitals
    • Node and nodal surface
    • Shielding effect
  • Rules for Filling Electrons in Orbitals
    • Aufbau principle
    • Pauli's exclusion principle
    • Hund's rule
    • Electronic configuration of atoms
  • Stability of Completely Filled and half-filled Orbitals

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Unit 3

Classification of Elements And Periodicity in Properties (05 Marks)

  • General Introduction
  • Historical Attempts towards Classification
    • Mendeleev Periodic table
  • Modern Periodic Table
    • Periodicity of properties
    • Groups and periods
    • Nomenclature of elements with atomic numbers greater than 100
  • Periodic Trends in Physical Properties
    • Atomic radii
    • Ionic radii
    • Lanthanide Contraction
    • Ionization enthalpy
    • Electron gain enthalpy
    • Electronegativity
  • Periodic Trends in Physical Properties
    • Valency and oxidation state
    • Anomalous properties of second period elements
    • Periodic trends and chemical reactivity

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Unit 4

Chemical Bonding and Molecular Structure (05 Marks)

  • General Introduction
  • Types of Chemical Bonds
    • Ionic bond
    • Covalent bond
    • Polar covalent bond
  • Valence Bond Theory
    • Hybridization
    • VSEPR theory
    • Resonance
  • Molecular Orbital Theory
    • Magnetic characteristics
    • Bond order
  • Hydrogen Bond
    • Intermolecular hydrogen bonding
    • Intramolecular hydrogen bonding

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Unit 5

States of Matter: Gases and Liquids (05 Marks)

  • General Introduction to three States of Matter
  • Intermolecular Forces
    • Types of intermolecular forces
    • Nature of intermolecular forces
  • Laws Governing Gaseous State
    • Boyle's law
    • Charles law
    • Gay-Lussac's law
    • Avogadro law
  • Ideal Behaviour
    • Ideal gas equation
    • Dalton's law of partial pressure
    • Kinetic theory of gases
  • Deviation from Ideal Behaviour
    • Compressibility factor
    • Boyle's temperature
  • Liquefaction of Gases
    • Critical temperature, critical pressure and critical volume
  • Liquid State
    • Vapour pressure
    • Viscosity
    • Surface tension

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Unit 6

Thermodynamics (05 Marks)

  • Introduction to Thermodynamics
  • Thermodynamic Terms Concepts of :
    • system, surrounding
    • types of system
    • state of a system
    • state function and path function
    • extensive and intensive properties
    • reversible and irreversible process
  • Thermodynamic Quantities
    • Work
    • Heat
  • First Law of Thermodynamics
    • Internal Energy
    • Enthalpy
    • Heat capacity
    • Measurement of ΔU and ΔH
  • Thermochemistry
    • Enthalpy change in a chemical reaction
    • Endothermic and Exothermic reactions
    • Standard enthalpy of reactions
    • Enthalpy changes during phase transformations
    • Standard enthalpy of formation
    • Thermochemical equations
    • Hess's Law of Constant Heat Summation
    • Enthalpies for different types of reactions
  • Spontaneity
    • Entropy
    • Second law of Thermodynamics
    • Gibb's energy change for spontaneous and non-spontaneous processes
    • Criteria for equilibrium
    • Third Law of Thermodynamics

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Unit 7

Equilibrium (05 Marks)

  • Introduction to The students will be able to:
    • Dynamic nature of dynamic nature.
  • Equilibrium in Physical Processes
    • Solid - liquid equilibrium
    • Liquid - vapour equilibrium
    • Solid – vapour equilibrium
    • Equilibrium involving dissolution of solid and gases in liquids
  • Equilibrium in Chemical Processes
    • Dynamic nature of chemical equilibrium
    • Law of Chemical Equilibrium
    • Equilibrium constant
  • Types of Chemical Equilibria
    • Homogenous Equilibria
    • Heterogeneous Equilibria
  • Applications of Equilibrium Constant
    • Predicting the extent of a reaction
    • Predicting the direction of the reaction
    • Calculating Equilibrium Concentrations
  • Factors Affecting Equilibria
    • Chatelier's principle
  • Ionic Equilibrium in Solution
    • Strong and weak electrolytes
    • Acids, bases and salts
  • Ionization of Acids and Bases
    • Ionic product of Water
    • pH scale
    • Ionization constant of weak acids and bases
    • Factors affecting acid strength
    • Common ion effect
  • Buffer Solutions
  • Solubility Equilibria of Sparingly Soluble Salts
    • Solubility product
    • Common ion effect of solubility of ionic salts

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Unit 8

Redox Reactions (05 Marks)

  • Introduction to Redox Reactions
  • Oxidation and Reduction Reactions
  • Redox Reactions in Terms of Electron Transfer Reactions
    • Competitive electron transfer reactions
  • Oxidation Number
    • Calculation of oxidation number
  • Types of Redox Reactions
  • Balancing of Redox Reactions
    • Oxidation number method
    • Half reaction method
  • Redox Titrations

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Unit 9

Hydrogen (05 Marks)

  • General Introduction
    • Position of hydrogen in the periodic table
  • Dihydrogen
    • Occurrence of dihydrogen
    • Isotopes of hydrogen
    • Methods of preparation of hydrogen
    • Properties of hydrogen
    • Uses of hydrogen
  • Hydrides
    • Classification
    • General methods of preparation
    • General properties
  • Water
    • General characteristics
    • Hard and soft water
    • Heavy water
  • Hydrogen peroxide
    • Preparation
    • Properties
    • Uses

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Unit 10

S-Block Elements (05 Marks)

  • General Introduction
  • Group 1 Elements
    • Electronic configuration
    • Physical Properties
    • Chemical properties
    • Diagonal relationship
    • Biological importance
    • Some Alkali metal compounds
  • Group 2 Elements
    • Electronic configuration
    • Physical Properties
    • Chemical properties
    • Diagonal relationship
    • Biological importance
    • Some Alkaline earth metal compounds

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Unit 11

Some P-Block Elements (05 Marks)

  • General Introduction
  • Group 13 Elements
    • Electronic configuration
    • Occurrence
    • Inert pair effect
    • Reactivity
    • Some compounds of Group 13 elements
  • Group 14 Elements
    • Electronic configuration
    • General properties
    • Catenation
    • Allotropic forms of carbon
    • Carbides
    • Some compounds of Group 14 elements

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Unit 12

Organic Chemistry - Some Basic Principles (05 Marks)

  • General Introduction
    • Origin of organic chemistry
    • Organic chemistry as a separate discipline
  • Types of Hybridization of Carbon
    • Types of hybridization in carbon compounds
    • Shapes of organic molecules
    • 2D and 3D structural representations of organic compounds
  • Classification of Organic Compounds
    • based on functional groups
    • based on structure
  • IUPAC Nomenclature of Organic Compounds
    • Priority order of functional groups
    • Prefixes and suffixes for functional groups
    • Derivation of structural formula from a given IUPAC name and vice-versa
  • Stereochemistry and Isomerism
    • Structural isomerism
    • Stereochemistry and stereoisomerism
    • Projection formulae
    • Interconversion of projection formulas
    • Conformations and their relative stabilities (ethane and butane)
    • Geometrical isomerism (cis and trans)
    • Optical isomerism
    • Absolute and relative nomenclature of optical isomers
  • Homolytic and Heterolytic Fission of a Covalent Bond
    • carbocation
    • carbanion
    • free radical
  • Basics of Organic Reaction
    • Electrophilic and nucleophilic
    • reagents Types of organic reactions
  • Electronic Displacements in a Covalent Bond
    • inductive effect
    • electromeric effect
    • resonance
    • hyperconjugation
  • Aromaticity
    • Huckel's rule
    • Stability of aromatic compounds
  • Acidity and Basicity (Bronsted and Lowry's Concept)
    • Relative acidity of carboxylic acids, phenols and alcohols
    • Relative basicity of amines

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Unit 13

Aliphatic Hydrocarbons (05 Marks)

  • General Introduction
    • Classification of hydrocarbons
  • Alkanes (Upto 5 Carbon Atoms)
    • Methods of preparation (Reduction, Wurtz reaction, Kolbe's electrolysis)
    • Physical properties Chemical reactions (Halogenation, Isomerisation, Oxidation, Aromatization, Combustion, Pyrolysis)
  • Alkenes (Upto 5 Carbon Atoms)
    • Methods of preparation (Partial reduction, dehydrohalogenati on, dehydration, dehalogenation)
    • Physical properties Chemical reactions (Addition of H2, X2, Markovnikov's and anti-Markovnikov's addition of HX, and H2O, ozonolysis, xidation and polymerisation)
  • Alkynes (Upto 5 Carbon Atoms)
    • Methods of preparation (Hydrolysis of calcium carbide, dehydrohalogenation)
    • Physical properties Chemical reactions (Addition of H2, X2, HX, and H2O and polymerisation)

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Unit 14

Environmental Chemistry (05 Marks)

  • General Introduction
  • Environmental Pollution
    • Environmental pollution
    • Conservation of natural resources
  • Air Pollution
    • Greenhouse effect
    • Depletion of stratospheric ozone
    • Sulphur oxides
    • Nitrogen oxides
  • Water Pollution
    • Types of water pollutants
    • Treatment of water pollution
    • BOD
  • Industrial Pollution
    • Industrial and agricultural chemicals that cause environmental
    • degradation Industrial waste management

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Chemistry Practical

Unit 1 : LABORATORY TECHNIQUES (05 Marks)

  • Cutting glass tube and glass rod
  • Bending a glass tube
  • Drawing out a glass jet
  • Boring a cork

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Unit 2 : LABORATORY TECHNIQUES (05 Marks)

  • Determination of melting point of an organic compound.
  • Determination of boiling point of an organic compound.
  • Crystallization involving impure sample of any one of the following:
    • Alum, Copper Sulphate, Benzoic Acid.

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Unit 3 : EXPERIMENTS RELATED TO pH CHANGE (05 Marks)

  • Any one of the following experiments:
    • Determination of pH of some solutions obtained from fruit juices, solutions of known and varied concentrations of acids, bases and salts using pH paper or universal indicator.
    • Comparing the pH of solutions of strong and weak acid of same concentration.
    • Study the pH change in the titration of a strong acid with a strong base using universal indicator.
  • Study of pH change by common-ion effect in case of weak acids and weak bases.

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Unit 4 : CHEMICAL EQUILIBRIUM (05 Marks)

One of the following experiments:

  • Study the shift in equilibrium between ferric ions and thiocynate ions by increasing /decreasing the concentration of either of the ions.
  • Study the shift in equilibrium between [Co (H2 O)6 ] 2+and chloride ions by changing the concentration of either of the ions.

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Unit 5 : QUANTITATIVE ESTIMATION (05 Marks)

One of the following experiments:

  • Using a chemical balance.
  • Preparation of standard solution of oxalic acid.
  • Determination of strength of a given solution of sodium hydroxide by titrating it against standard solution of oxalic acid.
  • Preparation of standard solution of sodium carbonate.
  • Determination of strength of a given solution of hydrochloric acid by titrating it against standard sodium carbonate solution.

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Unit 6 : QUANTITATIVE ESTIMATION (05 Marks)

  • Determination of one anion and one cation in a given salt.Cations: Pb2+,Cu2+,As3+,Al3+,Fe3+,Mn2+,Ni2+,Zn2+,Co2+,Ca2+,Sr2+,Ba2+,Mg2+,NH+4
    Anions: CO2−3,S2−,SO2−3,NO−2,NO−3,Cl−,I−,PO3−4,C2O2−4,CH3COO−
    (Note: Insoluble salts excluded)
  • Detection of nitrogen, sulphur, chlorine, in organic compounds.

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