Course Content
CHAPTER 1: SOME BASIC CONCEPTS OF CHEMISTRY
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Introduction of Chemistry
14:32
Matter || Pure Substance || Properties of Matter
Quantitative property || The International System of Units (SI) || Prefixes used in SI System || Scientific Notation
Precision & Accuracy || Significant figures || Dimensional Analysis
Law of Chemical Combination
Dalton’s Atomic Theory || Atomic Mass || Average Atomic Mass || Molecular Mass
Mole Concept and Molar Masses || Percentage Composition || Empirical Formula for Molecular formula
Stoichiometry || Limiting Reagent
Reactions in Solution – Mass per cent or weight percent || Mole fraction || Molarity || Molality
NCERT Solutions for Class 11 Chemistry Chapter 1 Some basic Concepts of Chemistry
CBSE Class 11 Chemistry Chapter-1 Important Questions
Chemistry Question Bank || NEET || JEE || AIIMS
Class 11th Chemistry Chapter 1 Quiz Test For Students
01:30:00
CHAPTER 2: STRUCTURE OF ATOM
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INTRODUCTION || DISCOVERY OF ELECTRON
30:35
DISCOVERY OF PROTON || DISCOVERY OF NEUTRON || ATOMIC MODELS OF ATOM
ISOTOPES || ISOBARS || ISOTONES || ISOELECTRONIC
DUAL NATURE OF LIGHT: DEVELOPMENT LEADING TO BOHR’S MODEL || Black body radiation and Photoelectric effect
Planck’s quantum theory || BOHR’S THEORY
EXPLANATION OF HYDROGEN SPECTRA || LIMITATIONS OF BOHR MODEL OF AN ATOM || DUAL NATURE OF PARTICLE || QUANTUM MECHANICS || Pauli’s exclusion Principle
NCERT Solutions for Class 11 Chemistry Chapter 2 Structure of Atom
CHAPTER 3: CLASSIFICATION OF ELEMENTS
Section Name Topic Name 3 Classification of Elements and Periodicity in Properties 3.1 Why do we Need to Classify Elements ? 3.2 Genesis of Periodic Classification 3.3 Modern Periodic Law and the present form of the Periodic Table 3.4 Nomenclature of Elements with Atomic Numbers > 100 3.5 Electronic Configurations of Elements and the Periodic Table 3.6 Electronic Configurations and Types of Elements: s-, p-, d-, f – Blocks 3.7 Periodic Trends in Properties of Elements
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Introduction || Doberneiner’s Triads
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Newland’s Law of Octave || Limitations of Newlands’ law of octaves
Mendeléev’s periodic table || Achievements of Mendeléev’s periodic table || Limitation of Mendeleev’s classification
The Modern Periodic Table || Position of Element in Modern Periodic Table || Trends in the modern periodic table
NCERT Solutions for Class 11 Chemistry Chapter 3 Classification of Elements and Periodicity in Properties
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CHAPTER 4: CHEMICAL BONDING AND MOLECULAR STRUCTURE
4 Chemical Bonding and Molecular Structure 4.1 Kössel-Lewis Approach to Chemical Bonding 4.2 Ionic or Electrovalent Bond 4.3 Bond Parameters 4.4 The Valence Shell Election Pair Repulsion (VSEPR) Theory 4.5 Valence Bond Theory 4.6 Hybridisation 4.7 Molecular Orbital Theory 4.8 Bonding in Some Homonuclear Diatomic Molecules 4.9 Hydrogen Bonding
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Introduction || Kossel and Lewis Approach
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Types of chemical bond || Factors affecting the formation of ionic bond || General properties of ionic compounds
COVALENT BOND || COORDINATE BOND
Bond parameters : Bond Length , Bond Angle, Bond Enthalpy, Bond Order || Resonance
Polarity & Dipole moment || Ionic Percentage || Polarization
VSEPR THEORY || Hybridization || Valence bond theory || Overlapping: sigma and pi bond || Molecular orbital theory
Hydrogen bonding || Hydrogen bonding in ice and water
NCERT Solutions for Class 11 Chemistry Chapter 4 Chemical Bonding and Molecular Structure
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Chemical Bonding & Molecular Structure Question For NEET || JEE || AIIMS
CHAPTER 5: STATE OF MATTER
Section Name Topic Name 5 States of Matter 5.1 Intermolecular Forces 5.2 Thermal Energy 5.3 Intermolecular Forces vs Thermal Interactions 5.4 The Gaseous State 5.5 The Gas Laws 5.6 Ideal Gas Equation 5.7 Kinetic Energy and Molecular Speeds 5.8 Kinetic Molecular Theory of Gases 5.9 Behaviour of Real Gases: Deviation from Ideal Gas Behaviour 5.10 Liquefaction of Gases 5.11 Liquid State
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Introduction || State of Matter
27:52
Intermolecular Forces || Dispersion Forces or London Forces
Dipole – Dipole Forces || Dipole – Induced Dipole Force || Hydrogen Bond || Thermal Energy
Intermolecular Forces Vs Thermal Interations || Boyle’s Law || Charles’ Law || Gay Lussac’s Law
Avogadro Law || Ideal Gas Equation || Density and Molar Mass of a Gaseous Substance
Dalton’s Law of Partial Pressure || Partial pressure in terms of mole fraction || Kinetic molecular theory of gases || Behaviour of real gases: deviation from ideal gas behaviour || Surface Tension
Viscosity
NCERT Solutions for Class 11 Chemistry Chapter 5 States of Matter
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State of Matter Question For NEET || JEE || AIIMS
CHAPTER 6: THERMODYNAMICS
Section Name Topic Name 6 Thermodynamics 6.1 Thermodynamic Terms 6.2 Applications 6.3 Measurement of ∆U and ∆H: Calorimetry 6.4 Enthalpy Change, ∆rH of a Reaction – Reaction Enthalpy 6.5 Enthalpies for Different Types of Reactions 6.6 Spontaneity 6.7 Gibbs Energy Change and Equilibrium
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Thermodynamics of Thermodynamics || Universe || System || Surrounding || types of systems || Internal Energy
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1st Law of Thermodynamics || Enthalpy || Heat capacity || Types of molar heat capacities || Relation between Cp &Cv || Calorimeter
Enthalpies of Reaction || Enthalpy of Combustion || Calorific value || Hess’s law of heat summation || Other type of enthalpies || Born- Haber cycle || Enthalpies of phase transition || Bond enthalpy || Limitation of 1st law of thermodynamics
Entropy || How s & q related? || How S&T related? || Second law of thermodynamics || Standard molar entropy || Gibbs free energy || Third law of thermodynamics
NCERT Solutions for Class 11 Chemistry Chapter 6 Thermodynamics
NCERT Solutions for Class 11 Chemistry Chapter 6 Very Short Answer Type Questions
NCERT Solutions for Class 11 Chemistry Chapter 6 Short Answer Type Questions
NCERT Solutions for Class 11 Chemistry Chapter 6 Long Answer Type Questions
CHAPTER 7: EQUILIBRIUM
Section Name Topic Name 7 Equilibrium 7.1 Equilibrium in Physical Processes 7.2 Equilibrium in Chemical Processes – Dynamic Equilibrium 7.3 Law of Chemical Equilibrium and Equilibrium Constant 7.4 Homogeneous Equilibria 7.5 Heterogeneous Equilibria 7.6 Applications of Equilibrium Constants 7.7 Relationship between Equilibrium Constant K, Reaction Quotient Q and Gibbs Energy G 7.8 Factors Affecting Equilibria 7.9 Ionic Equilibrium in Solution 7.10 Acids, Bases and Salts 7.11 Ionization of Acids and Bases 7.12 Buffer Solutions 7.13 Solubility Equilibria of Sparingly Soluble Salts
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Introduction || Types of equilibrium || Boiling point || Equilibrium involving dissolution of solids || General characteristics of physical equilibrium || Equilibrium Involving in Chemical Process
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Law of mass action || Characteristics of Equilibrium constant (k) || Characteristics of chemical equilibrium || Effect of temperature on K
Chemical equilibrium || Characteristics of K || Application of Equilibrium constant || Factors affecting state of equilibrium “Le Chartlier’s principle || Substances: electrolytes and non electrolytes
Acids, bases and salts || 2nd Concept: Bronsted Lowry concept || Conjugate acid –base concept || 3rd concept: Lewis concept || Expressing Hydrogen ion concentration: pH scale || Calculation of PH Value
Protic and non- Protic acids || Hydrolysis of salt || Different kind of salts || Buffer solution || Solubility product ||
NCERT Solutions for Class 11 Chemistry Chapter 7 Equilibrium
NCERT Solutions for Class 11 Chemistry Chapter 7 Very Short Answer Type Questions
CHAPTER 8: REDOX REACTIONS
Section Name Topic Name 8 Redox Reactions 8.1 Classical Idea of Redox Reactions-Oxidation and Reduction Reactions 8.2 Redox Reactions in Terms of Electron Transfer Reactions 8.3 Oxidation Number 8.4 Redox Reactions and Electrode Processes
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Introduction || Oxidation and Reduction || oxidation number || Redox reaction in terms of oxidation number
Balancing of Redox reactions || Types of Redox reactions
Redox couple || Electrochemical cell || Functions of salt bridge || Representation of the cell || Electrode potential || Electromotive force || Electromotive force || Electrochemical series || Redox reaction as the basis for Titrations
NCERT Solutions for Class 11 Chemistry Chapter 8 Redox Reactions
NCERT Solutions for Class 11 Chemistry Chapter 8 Very Short Answer Type Questions
NCERT Solutions for Class 11 Chemistry Chapter 8 Short Answer Type Questions
CHAPTER 9: HYDROGEN
Section Name Topic Name 9 Hydrogen 9.1 Position of Hydrogen in the Periodic Table 9.2 Dihydrogen, H2 9.3 Preparation of Dihydrogen, H2 9.4 Properties of Dihydrogen 9.5 Hydrides 9.6 Water 9.7 Hydrogen Peroxide (H2 O2) 9.8 Heavy Water,D2O 9.9 Dihydrogen as a Fuel
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Introduction || Characteristics of Hydrogen || Difference with alkali metals || Similarities with Halogens || Differences with Halogen || Dihydrogen
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Physical properties of H2 || Chemical Properties || Uses of H2
Hydrides || Covalent or molecular hydrides || Metallic  hydrides
Water || Physical properties || Chemical properties || Hardness of water  || Methods to remove hardness
Hydrogen peroxide || Physical Properties || Chemical Properties || Uses of Hydrogen peroxide
Heavy water || Physical properties || Chemical Properties
NCERT Solutions for Class 11 Chemistry Chapter 9 Hydrogen
NCERT Solutions for Class 11 Chemistry Chapter 9 Very Short , Short and Long Answer Type Questions
CHAPTER 10: S-BLOCK ELEMENTS
Section Name Topic Name 10 The s-Block Elements 10.1 Group 1 Elements: Alkali Metals 10.2 General Characteristics of the Compounds of the Alkali Metals 10.3 Anomalous Properties of Lithium 10.4 Some Important Compounds of Sodium 10.5 Biological Importance of Sodium and Potassium 10.6 Group 2 Elements : Alkaline Earth Metals 10.7 General Characteristics of Compounds of the Alkaline Earth Metals 10.8 Anomalous Behaviour of Beryllium 10.9 Some Important Compounds of Calcium 10.10 Biological Importance of Magnesium and Calcium
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Introduction || Diagonal Relationship || Atomic and Ionic Radii of alkali metals
25:32
Ionization Enthalpy and Hydration Enthalpy of alkali metals || Physical properties of alkali metals || Chemical Properties of alkali metals || Anomalous properties of lithium || Washing Soda
Preparation of washing soda by solvay’s process || Sodium Chloride || Caustic Soda || Baking Soda || Electronic Configuration of alkaline earth metal || Atomic and Ionic Radii of alkaline earth metal
Ionization Enthalpy of alkaline earth metal || Hydration Enthalpy of alkaline earth metal || Physical Properties of alkaline earth metal || Chemical Properties of alkaline earth metal
Quick Lime || Slaked Lime || Calcium Carbonate (CaCO3) || Plaster of Paris || Cement || Uses of s-block elements
NCERT Solutions for Class 11 Chemistry Chapter 10 The s-Block Elements
NCERT Solutions for Class 11 Chemistry Chapter 10 Very Short, Short & Long Answer Type Questions
CHAPTER 11: P-BLOCK ELEMENTS
Section Name Topic Name 11 The p-Block Elements 11.1 Group 13 Elements: The Boron Family 11.2 Important Trends and Anomalous Properties of Boron 11.3 Some Important Compounds of Boron 11.4 Uses of Boron and Aluminium and their Compounds 11.5 Group 14 Elements: The Carbon Family 11.6 Important Trends and Anomalous Behaviour of Carbon 11.7 Allotropes of Carbon 11.8 Some Important Compounds of Carbon and Silicon
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Introduction of p- block || Inert pair effect || Group 13 Elements
Chemical properties of group 13 || Important trends || Uses of Boron || Uses of Aluminum || Borax || PROPERTIES OF BORAX || Uses of Borax
Introduction of Group – 14 || Physical Properties of group 14 || Chemical properties of group 14 || Structure of CCl4 || Allotropes of carbon || Properties and Uses of diamond and graphite || Types of Charcoal || Uses of Carbon, Germanium, Lead, & Tin.
Carbon monoxide (CO) || Carbon dioxide (CO2) || Silicon dioxide (SiO2) || Crystalline form of silica || Structure of Silicon dioxide || Silicones || Silicates || Zeolites
NCERT Solutions for Class 11 Chemistry Chapter 11 The p-Block Elements
NCERT Solutions for Class 11 Chemistry Chapter 11 Very Short, Short & Long Answer Type Questions
CHAPTER 12: CHARACTERIZATION OF ORGANIC COMPOUND
Section Name Topic Name 12 Organic Chemistry – Some Basic Principles and Techniques 12.1 General Introduction 12.2 Tetravalence of Carbon: Shapes of Organic Compounds 12.3 Structural Representations of Organic Compounds 12.4 Classification of Organic Compounds 12.5 Nomenclature of Organic Compounds 12.6 Isomerism 12.7 Fundamental Concepts in Organic Reaction Mechanism 12.8 Methods of Purification of Organic Compounds 12.9 Qualitative Analysis of Organic Compounds 12.10 Quantitative Analysis
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Introduction || COMPOUNDS || Friedrich Wohler || IMPORTANT FEATURE OF π BONDS  || Branches of Organic Compounds || Functional Group
19:51
Homologous series || IUPAC system || Different Type of Organic Compounds ||  Alkyl halides
IUPAC and Common names of compounds || RULES FOR IUPAC || In case of double & triple bond
RULES FOR NAMING ORGANIC COMPOUND WITH FUNCTIONAL GROUP || PREFIX USED FOR SECONDARY FUNCTIONAL GROUP || NOMANCLATURE OF AROMATIC COMPOUNDS
ISOMERISM || The structural isomerism type || The different types of stereoisomerism || CONFORMATIONAL ISOMERISM
ELECTRON DISPLACEMENT IN COVALENT BONDS || HYPER CONJUGATION || Fundamental concepts of organic reactions || REACTION INTERMEDIATES
Types of Carbocations || Carboanion || Types of Carboanions ||  Attacking agents
Types of organic reactions || Addition Reaction || Elimination reaction
Methods of purification of organic compounds || Crystallisation || Distillation || Fractional distillation || Distillation under reduced pressure || Steam distillation
Differential extraction || Chromatography || Adsorption chromatography || Column chromatography || Thin layer chromatography || Position chromatography
Detection of carbon and hydrogen || Detection of other elements || Test for Nitrogen || Test for Sulphur || Test for halogens ||  Test for phosphorous || Quantitative analysis || Dumas method || Kjeldahl’s method
NCERT Solutions for Class 11th Chemistry Chapter 12 Organic Chemistry Some Basic Principles and Techniques
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CHAPTER 13: HYDROCARBON
Section Name Topic Name 13 Hydrocarbons 13.1 Classification 13.2 Alkanes 13.3 Alkenes 13.4 Alkynes 13.5 Aromatic Hydrocarbon 13.6 Carcinogenicity and Toxicity
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Introduction || Classification of hydrocarbons || Aromatic || Alkanes || Introduction of alkanes || Isomerism is alkanes
20:34
Classification of Alkanes || Preparation of alkanes
Physical Properties of alkanes || Chemical properties of alkanes
Conformational Isomerism || Torsional strain
Alkenes || ISOMERISM || Stereoisomerism || Stability of Alkenes || Preparation  of Alkenes ||  Physical Properties Of alkenes
Chemical properties of alkenes
Alkynes ||  Structure of ethyne || Isomerism || Preparation of Alkynes || Physical properties of alkynes || Chemical properties of alkynes
Aromatic Compounds || Nomenclature || Isomerism || Stability and structure of benzene || Huckle rule of Aromatic compounds || Preparation of Benzene || Physical properties of benzene || Chemical properties of benzene
NCERT Solutions for Class 11 Chemistry Chapter 13 Hydrocarbons
NCERT Solutions for Class 11 Chemistry Chapter 13 Very Short , Short and Long Answer Type Questions
CHAPTER 14: ENVIRONMENTAL CHEMISTRY
Section Name Topic Name 14 Environmental Chemistry 14.1 Environmental Pollution 14.2 Atmospheric Pollution 14.3 Water Pollution 14.4 Soil Pollution 14.5 Industrial Waste 14.6 Strategies to control Environmental Pollution 14.7 Green Chemistry
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Introduction || Atmosphere || Environmental chemistry || Environmental pollution || Atmospheric pollution || causes of pollution
Types of pollutants || Primary pollutant || Secondary pollutant || Biodegradable || Non-biodegradable
Types of pollution || Air pollution || Water pollution || Soil pollution
Green House Effect || Global warming || Acid rain || Hydrocarbons || Chlorofluorocarbons
Ozone || Ozone hole || Montreal protocol || Particulate pollutants
Smog and Photochemical smog
Water pollution
Soil pollution || Management of industrial waste
Green chemistry
NCERT Solutions for Class 11 Chemistry Chapter 14 Environmental Chemistry
NCERT Solutions for Class 11 Chemistry Chapter 14 Very Short, Short & Long Answer Type Questions
Class 11th Chemistry Online Class: Elevate Your CBSE Board Success
About Lesson

MORE QUESTIONS SOLVED

I. Very Short Answer Type Questions
Question 1. How is bond order related to the stability of a molecule?
Answer: Higher the bond order, greater is the stability.

Question 2. Write the type of hybridisation involved in CH4,C2H4 and C2H2.
Answer: CH4= sp3
C2H4 = sp2
C2H2 = sp

Question 3. Out of sigma and Π  bonds, which one is stronger and why?
Answer: sigma-bond is stronger. This is because sigma-bond is formed by head-on overlapping of atomic orbitals and Π bond is formed by side wise overlapping.

Question 4. Write the Lewis dot symbols of the following elements and predict their valencies. (i) Cl (ii) P
Answer:

Question 8. What is meant by bond pairs of electrons?
Answer: The electron pairs involved in the bond formation are known as bond pairs or shared pairs.

Question 9. Which of the following has larger bond angle in each pair?
(i) CO2, BF3 (ii) NH3, CH4
Answer: (i) CO2 (ii) CH4

Question 10.  Arrange the following, according to increasing covalent nature.
NaCl, MgCl2, AlCl3
Answer: NaCl < MgCl2 < AlCl3

Question 11. Define covalent bond according to orbital concept?
Answer: Covalent bond can be formed by the overlap of the orbitals belonging to the two atoms having opposite spins of electrons.

Question 15. State the types of hybrid orbitals associated with (i) P in PCl5 and (ii) S in SF6
Answer: (i) sp3d of P in PCl5 (ii) sp3d2 of S in SF6

Question 16. Why N2 is more stable than  O2? Explain on the basis of molecular orbital theory.
Answer: Bond order of N2 (= 3) is greater than that of O2 (= 2).

Question 17. How is bond order related to bond length of a molecule?
Answer:  Bond length is inversely proportional to bond order.

Question 18. Out of bonding and antibonding molecular orbitals, which one has lower energy and which one has higher stability?
Answer: Bonding molecular orbital has lower energy and higher stability.

Question 19. Define antibonding molecular orbital.
Answer: The molecular orbital formed by the subtractive effect of the electron waves of the combining atomic orbitals, is called antibonding molecular orbital.

Question 20. Name the two conditions which must be satisfied for hydrogen bonding to take place in a molecule.
Answer: (i) The molecule should contain highly electronegative atom like hydrogen atom. (ii) The size of electronegative atom should be small.

II. Short Answer Type Questions
Question 1.What is an electrovalent (or ionic) bond? Explain its formation with two examples.
Answer: When a chemical bond is formed by the complete transfer of electrons from one atom to another, so as to complete their outermost shell and therefore, aquire the stable noble gas configuration, the bond formed is called ionic bond or electrovalent bond. ‘
For Example,

Question 8. What are the main postulates of Valence Shell Electron Pair Repulsion (VSEPR) theory?
Answer: 

  •  The shape of a molecule depends upon the no. of electron pairs around the central atom.
  • There is a repulsive force between the electron pairs, which tend to repel one another.
  • The electron pairs in space tend to occupy such positions that they are at maximum distance so, that the repulsive force will be minimum.
  • A multiple bond is treated as if it is single bond and the remaining electron pairs which constitute the bond may be regarded as single super pair.

Question 9. Define bond order. How is it related to the stability of a molecule?
Answer: Bond order is defined as half of the difference between the number of electrons present in bonding and antibonding molecular orbitals.
Bond order (B.O.) = 1/2[Nb – Na ] z
If the bond order is positive (Nb > Na), the molecule or ion will be stable. If it is negative (Nb < Na)the molecule or ion will be unstable.

Question 10. Explain the diamagnetic behaviour of P2 molecule on the basis of molecular orbital theory.
Answer:

Question 2. (a) Define dipole moment. What are the units of dipole moment?
(b) Dipole moment values help in predicting the shapes of covalent molecules. Explain.
Answer: (a)Dipole moment: In a polar molecule, one end bears a positive charge and the other has a negative charge. Thus, the molecule has two poles with equal magnitude of the charges. The molecule is known as dipolar molecule and possesses dipole moment.
It is defined as the product of the magnitude of the positive or negative charge and the distance between the charges. µ (dipole moment) = q x d
SI unit of dipole moment is coulomb metre (m) or Debye.
(b)The dipole moment values are quite helpful in determining the general shapes of molecules.
For molecules with zero dipole moment, shapes will be either linear or symmetrical. For Example. BeF2 CO2etc. Molecules that possess dipole moments, their shape will not be symmetrical.

Question 3. Discuss the orbital structures of the following molecules on the basis of hybridisation, (i) BH3 (ii) C2H2
Answer:

Class 11th Chemical Bonding and Molecular Structure
Class 11th Chemical Bonding and Molecular Structure
Class 11th Chemical Bonding and Molecular Structure
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