The shape/structure of [XeF₅]^– and XeO₃F₂, respectively, are :

1. Pentagonal planar and trigonal bipyramidal

2. Trigonal bipyramidal and pentagonal planar

3. Octahedral and square pyramidal

4. Trigonal bipyramidal and trigonal bipyramidal

Of the species, NO , NO⁺, NO²⁺ and NO^– , the one with minimum bond strength is: 

1.  NO²⁺

2.  NO⁺

3.  NO 

4.  NO^–

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 isostructural pairs among the following are:

1. C and D only
2. A and B only
3. A and C only
4. B and C only

According to molecular orbital theory, which of the following molecules is not expected to be stable?

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

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