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

Chemical equilibrium

It is of two types:

  • Homogeneous
  • Heterogeneous

Homogenous: Is that when the reactants and products are in same phase.

Heterogeneous: When reactants and products are in different phase .

Characteristics of K

  1. At equilibrium, K is applicable only when concentration of reactants is equal to concentration of products.
  2. The value of K is independent of initial concentration of reactants.
  3. Equilibrium constant has a definite value for each reaction. This value remains same till the time temperature remains constant.
  4. For reversible reaction, K also reverses.
  5. Value of K is independent of catalyst.
Equilibrium notes class 11 and ncert solution for excel in the exam
equilibrium notes class 11

Application of Equilibrium constant

  1. Predicting the extent of reaction: The equilibrium constant is directly proportional to extent of reaction.
  • If value of k is large, the reaction goes in forward reaction.
  • If value of k is less, the reaction goes in backward reaction.
  • If k>103, the extent in this case is large and a reaction proceed almost to completion.
  • If value of k is less than 10-3, then the reaction proceeds to smaller extent.
  • If value of k is between 10-3 to 103, then there is a appreciable concentration of reactants and products.
  1. Predicting the direction of reaction: It tells us whether the reaction is going towards product or reactant. Reaction quotient = Q.
  • If Q<k, then reactants predominate.
  • If Q=k, then the reaction is at equilibrium.
  • If Q>k, then the products predominate.
  1. Calculation of equilibrium constant and concentrations.

K= [Products]/ [Reactants]

Equilibrium notes class 11 and ncert solution for excel in the exam
equilibrium notes class 11

Factors affecting state of equilibrium “Le Chartlier’s principle

Le chartlier’s principle: We know that at equilibrium, the state variables become constant. If we disturb any state variable, the reaction gets disturbed and the reaction diverts itself in a direction where disturbance is reduced.

So, according to this “ if any kind of reaction is subjected to any kind of stress, then the reaction proceeds in a direction where the stress gets reduced “.

  • Effect of change in concentration : For this consider a reaction:
Equilibrium notes class 11 and ncert solution for excel in the exam
equilibrium notes class 11

Substances: electrolytes and non electrolytes

In this part we will study equilibrium between ions .So, before we start let’s learn about types of substances (depending upon whether they conduct electricity or not).

We classify substances in to two types:

  • Electrolytes
  • Non electrolytes

Electrolytes: The substances which dissociate into ions in solution on passing current.

For example: ABàA+ + B

Non electrolytes: The substances that do not dissociate into ions, when current is passed through them.

That is AB à on passing current , nothing happens .

Further we can classify electrolytes as:

  • Strong electrolyte
  • Weak electrolyte

Strong electrolyte: The substances which completely dissociate into ions, when current is passed through them. It means if take an example of AB then on passing current it dissociate completely without leaving AB anywhere in solution .

Example: HCl,H2SO4 etc

Weak electrolyte: The substances which do not completely dissociate into ions, when current is passed through them. It means, if take an example of AB then on passing current it dissociate partially and we will find AB also in solution.

Example: Acetic acid CH3COOH etc

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