Course Content
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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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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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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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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Class 11th Chemistry Online Class For 100% Result
About Lesson

Introduction

Equilibrium is actually a state, when forces from both the side become equal. According to chemistry: It is a point in a chemical reaction, when rate of forward reaction becomes equal to rate of backward reaction.  Or we can say, it is the state when concentration of reactants becomes equal to concentration of products.

Types of equilibrium

There are two types of equilibrium:

  • Chemical equilibrium
  • Ionic equilibrium

 Let us study both the types of equilibrium in detail:

Physical equilibrium: It is achieved in all physical processes, when all state variables like pressure, temperature etc becomes constant. These are basically of three types:

Let us take examples referring to above type of equilibrium:

  • Solid to  liquid  or liquid to solid

For example: Conversion of ice to water.

In this forward reaction is: Ice to water (Melting).

In this backward reaction is: Water to Ice (Freezing).

So, when equilibrium is achieved: Rate of melting = Rate of freezing.

The temperature at which both solid and liquid states co exist is called Melting point. To attain melting point, we need to have certain state variable constant that is pressure.

  • Liquid to  gas or gas to liquid

For example: Conversion of water to water vapour.

In this, forward reaction is: Evaporation

In this, backward reaction is: Condensation

At equilibrium: Rate of evaporation = Rate of condensation

Boiling point: Is that constant temperature, at which vapour pressure of liquid becomes equal to atmospheric pressure. The state variable that becomes constant is temperature.

  • Solid to gas or gas to liquid

For example: Sublimation of Naphthalene, Camphor etc.

In this forward reaction is: Evaporation.

In this backward reaction is: Solidification. 

At equilibrium: Rate of evaporation = Rate of solidification. The state variable that becomes constant is temperature.

Equilibrium involving dissolution of solids

When any solid dissolves in liquid it is called as dissolution.

For example: When we add salt to water it dissolves .In this, the forward reaction is dissolution. When the solvent can’t dissolve more solute the process of crystallization occur in backward reaction.

At equilibrium: Rate of dissolution = Rate of crystallization .The state variable that becomes constant is concentration.

General characteristics of physical equilibrium

  • The measurable properties become constant.
  • It can be established only in closed vessel.
  • At equilibrium, the opposing forces become equal.
  • The equilibrium is dynamic in nature .That is the reaction keeps on going only the rate becomes constant.
  • At equilibrium, the concentration becomes constant.
  • The magnitude of equilibrium value, gives indication about the extent of reaction.
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