Which ionic compound has the largest amount of lattice energy?

$\left(a\right)<mspace\; width="1em"></mspace>NaF<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>\left(b\right)Al{F}_3<mspace\; width="1em"></mspace>$
$<mspace\; width="1em"></mspace>\left(c\right)AIN<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>\left(d\right)Mg{F}_2$

The incorrect statement regarding $\mathrm{O}{\left({\mathrm{SiH}}_3\right)}_2$ and ${\mathrm{OCl}}_2$ molecule is/are:

(i) The strength of back bonding is more in $\mathrm{O}{\left({\mathrm{SiH}}_3\right)}_2$ molecule than ${\mathrm{OCl}}_2$ molecule

(ii) $\mathrm{Si}—\mathrm{O}—\mathrm{Si}$ bond angle in $\mathrm{O}{\left({\mathrm{SiH}}_3\right)}_2$ is greater than $\mathrm{Cl}—\mathrm{O}—\mathrm{Cl}$ bond angle in ${\mathrm{OCl}}_2$

(iii) The nature of back bond in both molecules is $2{\mathrm{p}}_{\sigma }‐3{\mathrm{d}}_{\mathrm{\pi }}$

(iv) Hybridization of the central $\mathrm{O}‐\mathrm{atom}$ in both molecules is the same
 
1. i and ii
2. ii, iii, and iv
3. ii and iii
4. iii and iv
 

Which of the following compound have the same no. of lone pair with their central atom?

(i)$<mspace\; width="1em"></mspace>{\mathrm{XeF}}_5^{-<mspace\; width="1em"></mspace>}$             

(ii) ${\mathrm{BrF}}_3$                 

(iii) ${\mathrm{XeF}}_2$                     

(iv) ${\mathrm{H}}_3{\mathrm{S}}^{+}$               

(v) Triple Methylene     

options are as follows :        

(1) (iv) and (v)                                     

(2) (i) and (iii) 

(3) (i) and (ii)                                     

(4) (ii) (iv), (v)

The incorrect order of the force of attraction among the given species is :

1. HI > HBr> ${\mathrm{Cl}}_2$

2. ${\mathrm{CCl}}_4>{\mathrm{CH}}_2{\mathrm{Cl}}_2>{\mathrm{CH}}_3\mathrm{Cl}>{\mathrm{CH}}_4$

3. n- Pentane > iso-Pentane > neo-Pentane

4. ${\mathrm{OH}}_2>\mathrm{O}{\left({\mathrm{CH}}_3\right)}_2>{\mathrm{OBr}}_2$

The "O$-$N$-$O" bond angle is maximum in:

$\left(a\right)<mspace\; width="1em"></mspace>N_{2}O<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>\left(b\right)N{O_2}^{+}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$
$<mspace\; width="1em"></mspace>\left(C\right)N{O_2}^{-}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>\left(d\right)<mspace\; width="1em"></mspace>N{O_3}^{-}$

Among following molecule $\mathrm{N}—\mathrm{Si}$ bond length is shortest:

(1) $\mathrm{N}({\mathrm{SiH}}_3{)}_3$                           

(2) $\mathrm{N}({\mathrm{SiH}}_3{)}_2$

(3) ${\mathrm{NH}}_2\left({\mathrm{SiH}}_3\right)$                         

(4) All have equal $\mathrm{N}—\mathrm{Si}$ bond length

The geometry with respect to the central atom of the following molecules are:

$\mathrm{N}({\mathrm{SiH}}_3{)}_3;<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>{\mathrm{Me}}_3\mathrm{N};<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>({\mathrm{SiH}}_3{)}_3<mspace\; width="1em"></mspace>\mathrm{P}$

(1) planar, pyramidal, planar

(2) planar, pyramidal, pyramidal 

(3) pyramidal, pyramidal, pyramidal

(4) pyramidal, planer, pyramidal

Incorrect statement regarding ${\mathrm{BF}}_2{\mathrm{NH}}_2$ molecule is :

(1) FBF bond angle $<120\%$                     

(2) HNH bond angle $>109°28\text{'}$

(3) Exhibits intermolecular H-bond             

(4) Hybridization of N-atom is ${\mathrm{sp}}^3$

Molecule that has $\mu$ (observed) greater than $\mu$ (theoretical) is : 

1.	CHCl3	2.
3.		4.

The bond having minimum bond energy is :

(1) $\mathrm{C}—\mathrm{C}$                             

(2) $\mathrm{O}—\mathrm{O}$

(3) $\mathrm{S}—\mathrm{S}$                               

(4) $\mathrm{P}—\mathrm{P}$