In ${\mathrm{PO}}_4^{3-}$ ion, the formal charge on each oxygen atom and P-O bond order respectively are :

1. -0.75, 0.6

2. -0.75, 1.0

3. -0.75, 1.25

4. -3.1, 1.25

Which of the following pairs of compounds is isoelectronic and isostructural?
(1) BeCl_2, XeF₂
(2) Tel_2, XeF₂
(3) ${\mathrm{IBr}}_2^{-}$_, XeF₂
(4) IF₃, XeF₂

The hybridisations of atomic orbitals of nitrogen in ${\mathrm{NO}}_2^{+},<mspace\; width="1em"></mspace>{\mathrm{NO}}_3^{-}$ and ${\mathrm{NH}}_4^{+}$ are

(a) sp, sp³ and sp²               (b) sp², sp³ and sp

(c) sp, sp² and sp³               (d) sp², sp and sp³

What is the dominant intermolecular force on bond that must be overcome in converting

liquid CH₃OH to a gas?

1. Hydrogen bonding

2. Dipole-dipole interaction

3. Covalent bonds

4. London dispersion force

Correct order of strength of H-bond in the following compounds is : 

(1) $H_{2}O<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>H_2{O}_2<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>HF<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>H_{2}S$ 

(2) $HF<mspace\; width="1em"></mspace>\ge <mspace\; width="1em"></mspace>H_2{O}_2<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>H_{2}O<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>H_{2}S$

(3) $HF<mspace\; width="1em"></mspace>>\hspace{0.17em}{H}_{2}O<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>H_{2}S<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>H_2{O}_2$

(4) $HF<mspace\; width="1em"></mspace>>\hspace{0.17em}{H}_2{O}_2<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>H_{2}O<mspace\; width="1em"></mspace>><mspace\; width="1em"></mspace>H_{2}S$