Class 11 Chemistry Chapter 4 Chemical Bonding and Molecular Structure
Ionic bonding is possible due to large difference in the electronegativity of two atoms combining with each other. What will happen if both the atom combining chemically have similar electronegativity? This results in the formation of covalent bond. Lewis suggested that atoms having similar electronegativity, can be combine together by sharing of valence electrons. Such a bond formed by sharing of electrons is called covalent bond
Characteristics of Covalent Bond
- Covalent bonds are formed by sharing equal number of unpaired electrons in an atom.
- Shared electron in a covalent bond belongs to both atoms which are combined chemically.
- By sharing electrons each atom try to achieve nearest noble gas configuration. For example, if an atom has two electron this suggest that atom has attained electronic configuration of noble gas Helium.
- Bond formed by sharing of electron is represented by ‘-’ between the symbols of atom. For example, Cl-Cl.
- Covalent bond can be classified into single covalent bond, double covalent bond and triple covalent bond.
Types of covalent bond
Types of Covalent Bond
- Single covalent bond:
The covalent bond formed due to sharing of one each or one pair of electrons between two atoms is called as single covalent bond. It is denoted by ‘-’. For example, molecules like H2, Cl2, H2O, CH4, CCl4 shows single covalent bond or simply single bond.
- Double covalent bond:
The covalent bond formed due to sharing of two electrons each or two pairs of electron is called as double covalent bond. It is denoted by ‘=’. For example, molecules like O2, CO2, C2H4 shows double covalent bond or simply double bond.
- Triple covalent bond:
The covalent bond formed by sharing of three electrons each or three pairs of electrons is called triple covalent bond. It is denoted by ‘≡’. For example, molecules like N2, C2H2 are formed by triple covalent bond or simply triple bond.
Keywords: Ionic bond, Single bond, Double bond, Triple bond, Electronegativity
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