When $O_2$ is adsorbed on a metallic surface, electron transfer occurs from the ,metal to $O_2$. The wrong statements(s) regarding this adsorption is (are): 

(1) $O_2$ is physisorbed 

(2) Heat is released

(3) Occupancy of $\pi *2p$ of $O_2$ is increased 

(4) Bond length of $O_2$ is increased

Born Haber cycle is used to determine:

(1) lattice energy 

(2) electron affinity 

(3) ionization energy 

(4) either of them 

The molecule having the smallest bond angle is-

Select the most ionic and most covalent compounds respectively from the following.

$Cr{O}_5,M{n}_2{O}_7,PbO,<mspace\; width="1em"></mspace>P_4{O}_{10},<mspace\; width="1em"></mspace>Sn{O}_2$

(A) $Cr{O}_5,<mspace\; width="1em"></mspace>M{n}_2{O}_7$                                (B)  $PbO,<mspace\; width="1em"></mspace>M{n}_2{O}_7$

(C) $Cr{O}_5,<mspace\; width="1em"></mspace>P_4{O}_{10}$                                 (D) $Sn{O}_2,<mspace\; width="1em"></mspace>Cr{O}_5$

In which of the following sets the central atom of each member involves $s{p}^3$ hybridisation?

(A) $I{O_4}^{‐}IC{l_4}^{‐}and<mspace\; width="1em"></mspace>I{F_4}^{+}$                                      (B) $Xe{O}_3,<mspace\; width="1em"></mspace>Xe{O}_4,<mspace\; width="1em"></mspace>Xe{F}_4$

(C) $S{O}_3,\hspace{0.17em}S{O_3}^{2‐},<mspace\; width="1em"></mspace>S{O_4}^{2‐}$                                    (D) $PC{l_4}^{+},<mspace\; width="1em"></mspace>B{F_4}^{‐},<mspace\; width="1em"></mspace>Cl{O_4}^{‐}$

In which of the following groups all the members have linear shape?

(1) $N{O}_2,<mspace\; width="1em"></mspace>{N_3}^{‐},<mspace\; width="1em"></mspace>IC{l_2}^{+}$                          

(2) ${N_3}^{‐},<mspace\; width="1em"></mspace>{I_3}^{‐},<mspace\; width="1em"></mspace>N{O_2}^{+}$

(3) $Xe{F}_2,<mspace\; width="1em"></mspace>C_2{H}_2,<mspace\; width="1em"></mspace>S{O}_2$                        

(4) $C{O}_2,<mspace\; width="1em"></mspace>BeC{l}_2,<mspace\; width="1em"></mspace>SnC{l}_2$

Which reaction involves a change in the HYBRIDIZATION for the under lined geometry?

(A) $\underline{B}{F}_3+<mspace\; width="1em"></mspace>F\to <mspace\; width="1em"></mspace>B{F_4}^{-}$                           (B) $\underline{N}{H}_3<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>H^{+}\to <mspace\; width="1em"></mspace>\underline{N}{H_4}^{+}$

(C) $2\underline{S}{O}^2+O_2\to 2\underline{S}{O}_3$                        (D) $H_2\underline{O}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>H^{+}\to <mspace\; width="1em"></mspace>H_3{\underline{O}}^{+}$

The ${\mathrm{BF}}_3$ is a planar molecule whereas ${\mathrm{NF}}_3$ is pyramidal because:

1. $\mathrm{B}-\mathrm{F}$ bond is more polar than $\mathrm{N}-\mathrm{F}$ bond.

2. Boron atom is bigger than nitrogen atom.

3. Nitrogen is more electronegative than boron.

4. ${\mathrm{BF}}_3$ has no lone pair but ${\mathrm{NF}}_3$ has a lone pair of electrons.

Which of the following statement is true for $I{O}_2{F_2}^{-}$according to VSEPR theory?

(A) The lone pair and two I-O double bonds occupy the equatorial positions of trigonal
bipyramid.

(B) It has $s{p}^3$ hybridization and is T-shaped.

(C)  Its structure is analogous to $S{F}_4$.

(D) (A) and (C) both

The compound with a maximum number of lone pairs of electrons on
the central atom among the following is:

1. $XeO{F}_4$                       

2. $I{F_4}^{+}$

3. $Xe{F}_2$                         

4. $Br{F}_3$