Which of the following represents the correct order of Cl−O bond lengths inClO−,ClO−2,ClO−3,ClO−4? ClO−4=ClO−3=ClO−2=ClO−ClO−<ClO−2<ClO−3<ClO−4ClO−4<ClO−3<ClO−2<ClO−ClO−3<ClO−4<ClO−2<ClO−

The correct order of Cl−O bond lengths in ClO−, ClO−2, ClO−3, ClO−4 is ClO− < ClO−2 < ClO−3 < ClO−4.

Here's why:

1. ClO−: In this ion, there is a single bond between Cl and O. Single bonds are typically longer because they involve only one shared pair of electrons.

2. ClO−2: In this ion, there is a double bond between Cl and O. Double bonds are shorter than single bonds because they involve two shared pairs of electrons.

3. ClO−3: In this ion, there is a double bond and a single bond between Cl and O. The average bond length is shorter than a single bond but longer than a double bond.

4. ClO−4: In this ion, there are two double bonds and two single bonds between Cl and O. The average bond length is the shortest because it involves the most shared pairs of electrons.

Therefore, as the number of shared electron pairs increases (from ClO− to ClO−4), the bond length decreases.