The shape of $\mathrm{Xe}{{\mathrm{F}}_3}^{+}$ is:

1.	Trigonal planar	2.	Pyramidal
3.	Bent T-shape	4.	See-saw

The molecular geometry that is least likely to result from a trigonal bipyramidal electron geometry is:

On the left are given decreasing orders of elements for a certain property and on right side is given the property. The incorrect order for the given properties is:

1. ${\mathrm{AlF}}_3>\mathrm{MgO}>{\mathrm{MgF}}_2$    : Lattice energy

2. $\mathrm{Li}>\mathrm{Na}>\mathrm{Al}>\mathrm{Mg}$       : Electron affinity

3. ${\mathrm{PF}}_5>$ ${\mathrm{SF}}_6$ $>$ ${\mathrm{SiF}}_4$    : Lewis acidic character

4. ${\mathrm{SiCl}}_4>{\mathrm{SiBr}}_4$ $>{\mathrm{SiI}}_4$   : Decreasing ionic character

O$—$O bond length ($\mathrm{in} \stackrel{°}{\mathrm{A}}$ ) in  $H_2{O}_2$ and $O_2{F}_2$ is respectively:

The correct order of 'S$—$O' bond length is:

A compound having a metal-to-metal bond is:

1. Cupric chloride           

2. Stannous chloride

3. Mercurous chloride     

4. Mercuric chloride

Which of the following pair of elements can form an ionic compound?

The type of molecular forces of attraction present in the following compound is:

The correct statement among the following for a compound having a higher dipole moment is-

$PC{l}_5$ exists but $NC{l}_5$ does not because:

1. Nitrogen has no vacant d-subshells .

2. $NC{l}_5$ is unstable .

3. Nitrogen atom is much smaller than p .

4. Nitrogen is highly inert .