Question

C2- bond order

Answer 1

[AI-generated answer — Bot GPT 3.5]

Bond order is a measure of the number of chemical bonds between a pair of atoms in a molecule. It can be calculated by the difference in the number of bonding and antibonding electrons divided by 2.

In general, a higher bond order indicates a stronger and shorter bond between two atoms, while a lower bond order indicates a weaker and longer bond.

For example, if we consider the diatomic molecule O2, each oxygen atom contributes six electrons (2 from 2s orbital and 4 from 2p orbitals). In the molecule, there are a total of 12 electrons in the bonding molecular orbitals (2 electrons in the σ1s, 2 electrons in the σ*1s, 2 electrons in the σ2s, 2 electrons in the σ*2s, 2 electrons in the π2p, and 2 electrons in the π*2p) and no electrons in the antibonding molecular orbitals. Therefore, the bond order of O2 is calculated as:

Bond order = (Number of bonding electrons - Number of antibonding electrons)/2
= (12 - 0)/2
= 6/2
= 3.

Therefore, the bond order of O2 is 3, indicating a strong and short bond between the two oxygen atoms.