In $\stackrel{1}{\mathrm{C}}{\mathrm{H}}_2=\stackrel{2}{\mathrm{C}}=\stackrel{3}{\mathrm{C}}\mathrm{H}-\stackrel{4}{\mathrm{C}}{\mathrm{H}}_3$ molecule, the hybridization of carbon 1,2,3 and 4 respectively are :

1. ${\mathrm{sp}}^3,\mathrm{sp},{\mathrm{sp}}^3,{\mathrm{sp}}^3$

2. ${\mathrm{sp}}^2,{\mathrm{sp}}^2,{\mathrm{sp}}^2,{\mathrm{sp}}^3$

3. ${\mathrm{sp}}^2,\mathrm{sp},{\mathrm{sp}}^2,{\mathrm{sp}}^3$

4. ${\mathrm{sp}}^2,{\mathrm{sp}}^3,{\mathrm{sp}}^2,{\mathrm{sp}}^3$

The molecule in which hybrid MOs involve only one d-orbital of the central atom is:

The structure of PCl₅ in the solid state is: 

1. Square pyramidal.
2. Tetrahedral [PCl₄]⁺ and octahedral [PCl₆]^–
3. Square planar [PCl₄] and octahedral [PCl₆]^–
4. Trigonal bipyramidal.

The compound that has the largest H–M–H bond angle (M=N, O, S, C), is:

The ion that has sp³d² hybridization for the central atom is:

1. [ICl₄]^–

2. [ICl₂]^–

3. [BrF₂]^–

4. [IF₆]^–

How many lone pairs of electrons are present in \({I }_{3}^{-}\) ion?

In which of the following pairs the two species are not isostructural?

1. PCl₄⁺ and SiCl₄

2. PF₅  and BrF₅

3. AlF₆³⁻ and SF₆

4. CO₃²⁻ and NO₃⁻

Which of the following compounds has the smallest bond angle?

1. SO₂ 

2. H₂O 

3. H₂S 

4. NH₃