Question

Q6 - Find bond order of 02.02.07 and 0% and arrange these species in decreasing order of bond
lengths.​

Answer 1

Answer:

Answer:

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

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]

(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-