Bond Parameters

The configuration of superoxide ion,

(I) In , electronegativity of -atom is greater than .



In , electronegativity of -atom is greater than . Therefore, direction of all dipole moment with lone pairs lies in same direction, hence net dipole moment increases.



In , electronegativity of is greater than . Therefore, direction of dipole moment are opposite from the lone pair, hence, net dipole decreases.



Correct order of dipole moment will be



(II) Covalent bond length



as electronegativity difference increases then bond length decreases but lone pair-lone pair repulsion increases the bond length.

(III ) Bond order = Number of bonding electron


$C _{2}=\sigma l s^{2}

We know that the bond order of a molecule is calculated as:

Bond order = 1/₂ (number of bonding electrons - number of antibonding electrons)

For the molecules:

• NO (15 electrons) has a bond order of 2.5.
• CO (14 electrons) has a bond order of 3.0.
• O₂ (16 electrons) has a bond order of 2.0.
• O₂ (17 electrons) has a bond order of 1.5.

Thus, the correct matching is a-iii, b-iv, c-ii, d-i.