Course Content
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
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
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
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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The  dihydrogen combines with number of elements to form Hydrides . The general formula for hydrides are given below where E is any element.

Class 11th Chemistry Hydrogen Notes and NCERT Solution
 Class 11th Chemistry Hydrogen Notes and NCERT Solution
Class 11th Chemistry Hydrogen Notes and NCERT Solution

Covalent or molecular hydrides

They are mainly formed by p block elements and some s block elements ,which have less electronegativity difference than hydrogen.


  1. They are binary compounds .
  2. They have covalent bond : Example – CH4(methane) , NH3(ammonia) , H2O(water) and  HF(hydrogen fluoride).
  3. They are of three types :
  • Electron deficient : They have less electrons than its octet .

Example :  BH3 (Boron hydride-only 6electrons present ).Therefore, exist as B2 H6 (dimer).They act as Lewis acids .

  • Electron precise :They have have sufficient electrons .

Example : CH4(Methane) , SiH(Silicon hydride -have 8 electrons )

  • Electron rich : They have extra electrons that is more than the octet.

Example : Hydrides of group 15,16,17 act as Lewis bases .

Metallic  hydrides –

In this Hydrogen combines with  with d & f elements .Out of all group 6,7,8,9 does not form hydrides, but  group 3,4,5,10,11,12   can form hydrides.

This is called Hydride  gap (the inability of these groups  to form hydrides is called Hydride gap ).

  Characterstics :

  1. They are deficient in Hydrogen
  2. These are also called non-stochiometric hydrides.
  3. Hydrogen occupy interstitial spaces between these atoms.

Ni , Pt , Pd , Ce , Ac , have these structure.

  1. The catalytic reduction & Hydrogenation involves trapping of H2 between these atoms and this factor is  responsible for catalytic action.
  2. They are good conductor of electricity.
  3. They are harder than parent metal.
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