Chemistry Handwritten notes CHEMICAL BONDING

Chemical bonding and Molecular Structure - CLASS 11 Chemistry

TOPICS AND BRIEF INTRODUCTION ABOUT THE CONTENTS IN THIS CHAPTER

Chemical bonding is the most important and high weightage chapter in chemistry according to NEET

Every year 3-4 questions are being asked from this CHAPTER. 

DIFFICULTY LEVEL of MCQs asked from this chapter is "EASY-AVERAGE"

How to learn this chapter starting from now :

1. Watch our YouTube explanatory video to know the most important topics, Previous year questions, must do NCERT BOOK BACK QUESTIONS, examples, inext and crash course

2. Download notes from this blog

3. Practice it

4. Solve about told questions

5. Solve previous years jee and Neet MCQS

6. Revise through our CRASH COURSE series in YouTube

7. Take mini and micro mock test periodically

Octet Rule-

Every atom tries to attain the octet configuration (presence of eight electrons) in its valence shell by losing, gaining or sharing of electrons. This is known as the octet rule

Lewis Symbols- 

Lewis introduced the concept representing valence electrons with dots, which are called Lewis symbols.

Electrovalent Bond- 

The bond formed as a result of the electrostatic attraction between positive and negative ions is termed the electrovalent bond. The electrovalence is thus equal to the number of unit charge on the ion.

Covalent Bond- 

When two same or different atoms share their valence electron to attain the noble gas configuration, it is known as a COVALENT BOND.

Formal Charge- 

 The difference between the number of valence electrons of that atom in an isolated or free state and the number of electrons assigned to that atom in the Lewis structure.

Hybridisation: 

Mixing of two atomic orbitals with the same energy level to give a degenerated new type of orbitals Bond Length- Bond length is the equilibrium distance between the nuclei of two bonded atoms in a molecule.

Bond Angle- 

The angle between the orbitals containing bonding electron pairs around the central atom in a molecule/complex ion.

Bond Enthalpy- Bond enthalpy is the amount of energy required to break one mole of bonds of a particular type between two atoms in a gaseous state.

BOND ORDER-

According to Lewis, bond order is given by the number of bonds between two atoms in a molecule.

VALENCE BOND THEORY-

  ELECTRONS in a covalent bond reside in a region which is at the overlap of individual atomic orbitals.

Sigma (σ) bond- 

The covalent bond formed because of overlapping of atomic orbitals along the internuclear axis is called the σ-bond.

Pi (π) bond- 

The covalent bond formed by sidewise overlapping of atomic orbitals is called π-bond.

VSEPR Theory-

 The Lewis concept is unable to explain the shapes of molecules. Sidgwick and Powell provided a useful idea for predicting shapes and geometries of molecules. The theory was based on the repulsions between electron pairs, known as valence shell electron pair repulsion (VSEPR) theory

Link for the PDF for the notes:

Chemical Bonding

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