Among the given species  the isostructural pair is : 

1. $\left[{\mathrm{NF}}_3 \mathrm{and} {\mathrm{BF}}_3\right]$

2. $\left[{\mathrm{BF}}_4^{-} \mathrm{and} {\mathrm{NH}}_4^{+}\right]$

3. $\left[{\mathrm{BCl}}_3 \mathrm{and} {\mathrm{BrCl}}_3\right]$

4. $\left[{\mathrm{NH}}_3 \mathrm{and} {\mathrm{NO}}_3^{-}\right]$

The molecule among the following having the highest dipole moment is:

1. CO₂
2. HI
3. H₂O
4. SO₂

The hybridization of nitrogen in ${\mathrm{NO}}_2^{+},$ ${\mathrm{NO}}_3^{-}$ and ${\mathrm{NH}}_4^{+}$ respectively is : 

1. sp, sp^3, and sp²

2. sp, sp^2, and sp³

3. sp², sp, and sp³

4. sp², sp^3, and sp

The correct order of the boiling points of ${\mathrm{H}}_2\mathrm{O} , \mathrm{HF} , {\mathrm{NH}}_3$ is: 

1. HF > H₂O > NH₃

2. H₂O > HF > NH₃

3. NH₃ > HF > H₂O

4. NH₃ > H₂O > HF

In ${\mathrm{PO}}_4^{3-}$ ion, the formal charge on the oxygen atom of the P-O bond is : 

In ${\mathrm{NO}}_3^{-}$ ion, the number of bond pairs and lone pairs of electrons on the nitrogen atom is

1. 2, 2

2. 3, 1

3. 1, 3

4. 4, 0

Which species lacks tetrahedral geometry?

1. ${\mathrm{BH}}_4^{-}$

2. ${\mathrm{NH}}_2^{-}$

3. ${\mathrm{CO}}_3^{2-}$

4. ${\mathrm{H}}_3{\mathrm{O}}^{+}$

The number of $\mathrm{\pi }$ bonds and $\mathrm{\sigma }$ bonds in the following structure is :

The species doesn't have unpaired electrons is:

In which of the following molecule/ion all the bonds are not equal?

1.  ${\mathrm{XeF}}_4$

2. ${\mathrm{BF}}_4^{-}$

3. ${\mathrm{C}}_2{\mathrm{H}}_4$

4. ${\mathrm{SiF}}_4$