Question

by molecular orbital theory explain magnetic nature and bond order of O2,O-²,O²-​

Answer 1

Solution:

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Let us calculate the bond order

Bond order (B.O) 1/2 × [Number of an electron in antibonding molecular orbitals] – [Number of electrons in bonding molecular orbitals]

The higher the order of the bond the greater the pull between the two atoms and the shorter the length of the bond.

(1) B.O for O2 = 1/2 × [10 – 6]

B.O for O2 = 2

(2) B.O for O2– = 1/2 × [10 – 7]

B.O for O2– = 1.5

(3) B.O for O2+ = 1/2 × [10 – 5]

B.O for O2+ = 2.5

(4) B.O for O22- = 1/2 × [10 – 8]

B.O for O22- = 1

∴ The increasing order of bond length for these species is

O2+ < O2 < O2– < O22-

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