How many antibonding electron pair(s) is/are present in the \(O_{2}^{2-}\) ion?

In $P{O}_4^{-3}$, formal charge on every oxygen atom and P-O bond order respectively are:
1.  -0.75 and 1.25
2.  -0.5 and 2
3.  1 and 1.5
4.  -0.75 and 2

Increasing order of bond length is:

1. $N{O}^{-}$ $<$ $NO$ $<$ $N{O}^{+}$ $<$ $O_2^{-}$

2. $O_2^{-}$ $<$ $NO$ $<$ $N{O}^{-}$ $<$ $N{O}^{+}$ $$

3. $O_2^{-}$ $<$ $N{O}^{-}$ $<$ $NO<$ $N{O}^{+}$ $$

4. $N{O}^{+}$ $<$ $NO$ $<$ $N{O}^{-}$ $<$ $O_2^{-}$

The dipole moment of compound AB is 10.92 D and that of compound CD is 12.45 D. If the bond length of AB is 2.72 A° and that of CD is 2.56 A°, then for these compounds the correct statement is:
1.  More ionic nature in AB
2.  More ionic nature in CD
3.  Equal in both
4.  Cannot be predicted

Among the following, the compound that is electron deficient is:

1. BaCl₂

2. BCl₃

3. CCl₄

4. PCl₅

d$\mathrm{\pi }$ - p$\mathrm{\pi }$ bond is present in:

1. $C{O}_3^{2-}$

2. $P{O}_4^{-3}$

3. $N{O}_3^{-}$

4. $N{O}_2^{-}$

The compound that forms linear polymer due to H-bond is:

The correct order of dissociation energy of N₂ and N₂⁺ is:

Among the options given below, identify the Isoelectronic species:

1. CO, CN^–, NO⁺, C₂^2–

2. CO^–, CN, NO, C₂^–

3. CO⁺, CN⁺, NO^–, C₂

4. CO, CN, NO, C₂

A species that does not exhibit paramagnetism is:

1. N₂⁺

2. O₂^–

3. CO

4. NO