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electrons = 7. To achieve a stable electron configuration (according to the octet

rule) one electron is needed, so the Lewis structure for the formation of HCl
To achieve stability, the H and Cl atoms need one additional electron. The H

atom donates 1 electron to be used together so that it fulfils the duplet rule while
Cl donates 1 electron to be used together so that it reaches the octet rule.

2. Double Covalent Bond
Double bonds are formed by non-metal atoms that donate two unpaired

electrons to bond so that they fulfil the octet rule. Example: formation of O2
Formation of O2

2
2
6
4
2
16O electron configuration: 1s 2s 2p 3s 3p so that the valence electrons = 6,
to achieve a stable electron configuration (according to the octet rule) 2
electrons are needed, so the Lewis structure for the formation of O2

If two O atoms bond with each other, each O atom will donate two electrons to

be shared so that the O atoms obey the octet rule. There are two pairs of bonding
electrons in this bond.

3. Triple Covalent Bond
Triple covalent bonds are formed by non-metallic atoms that donate three

unpaired electrons to bond so that they fulfil the octet rule. Triple covalent bonds
are covalent bonds that have 3 pairs of PEI. An example of a compound

containing a triple covalent bond is the N2 molecule.

Formation of N2
3
7N electron configuration: 1s 2s 2p so that the valence electrons = 5, to
2
2
achieve a stable electron configuration (according to the octet rule) 3 electrons
are needed, so the Lewis structure for the formation of N2

Covalent Compound| 6