Atoms like to make double or triple bonds because it helps them become more stable. They do this to fill up their outer layer of electrons. This idea comes from something called the octet rule. It says that atoms feel safest when they have eight electrons in their outer layer.

Key Points:

1. Covalent Bonding:

   • Single Bonds: These involve one pair of shared electrons.
     (For example, $H_2$ and $Cl_2$)

   • Double Bonds: These involve two pairs of shared electrons.
     (For example, $O_2$ and $C_2H_4$)

   • Triple Bonds: These involve three pairs of shared electrons.
     (For example, $N_2$ and $C_2H_2$)

2. Bond Strength:

   • Single Bonds: These are the weakest. They have an average bond energy around 200-400 kJ/mol.

   • Double Bonds: These are stronger, with an average bond energy of about 600-800 kJ/mol.

   • Triple Bonds: These are the strongest, with an energy of about 800-1000 kJ/mol.

3. Molecular Formation:

   • Double and triple bonds allow atoms to share more electrons. This makes the molecules more stable and can change how they look and how they react with other substances.