Which is the following pairs of species have identical shapes ?

$1. {\mathrm{NO}}_2^{+} \mathrm{and} {\mathrm{NO}}_2^{-}$
$2. {\mathrm{PCI}}_5 \mathrm{and} {\mathrm{BrF}}_5$
$3. {\mathrm{XeF}}_4 \mathrm{and} {\mathrm{ICI}}_4^{-}$
$4. {\mathrm{TeCl}}_4 \mathrm{and} {\mathrm{XeO}}_4$

Which of the following leads to bonding orbital?

1.
2.
3.
4.

Which of the following overlap is incorrect (assuming Z-axis is internuclear axis) ?

(A) $2{\mathrm{p}}_{\mathrm{y}} + 2{\mathrm{p}}_{\mathrm{y}} \to \mathrm{\pi }$ - Bond formation

(B) $2{\mathrm{p}}_{\mathrm{x}} + 2{\mathrm{p}}_{\mathrm{x}} \to \mathrm{\sigma }$ - Bond formation

(C) $3{\mathrm{d}}_{\mathrm{xy}} + 3{\mathrm{dp}}_{\mathrm{xy}} \to \mathrm{\pi }$ - Bond formation

(D) $2\mathrm{s} + 2{\mathrm{p}}_{\mathrm{y} }\to \mathrm{\pi }$ - Bond formation

(E) $3{\mathrm{d}}_{\mathrm{xy}} + 3{\mathrm{d}}_{\mathrm{xy}} \to \mathrm{\delta }$ - Bond formation

(F) $2{\mathrm{p}}_{\mathrm{z}} + 2{\mathrm{p}}_{\mathrm{z}} \to \mathrm{\sigma }$ - Bond formation

1. A, B, C

2. C, F

3. B, E

4. B, C, D

Which of the following is not present in ${\mathrm{XeO}}_3$ molecule ?

$1. {\mathrm{sp}}^3 + {\mathrm{p}}_{\mathrm{x}}$
$2. {\mathrm{sp}}^3 + {\mathrm{p}}_{\mathrm{y}}$
$3. {\mathrm{d}}_{\mathrm{xz}} +\hspace{0.17em}{\mathrm{p}}_{\mathrm{x}}$
$4. {\mathrm{sp}}^3 +\hspace{0.17em}\mathrm{s}$

The incorrect order of lattice energy is :

$1. {\mathrm{AIF}}_3 > {\mathrm{MgF}}_2$
$2. {\mathrm{Li}}_3\mathrm{N} > {\mathrm{Li}}_2\mathrm{O}$
$3. \mathrm{NaCl} > \mathrm{LiF}$
$4. \mathrm{TiC} > \mathrm{ScN}$

The bond angles of  NH₃, NH₄⁺ and NH₂^-  are in the order :

1. NH₂^- > NH₃ > NH₄⁺

2. ${\mathrm{NH}}_4^{+}>{\mathrm{NH}}_3>{\mathrm{NH}}_2^{-}$

3. ${\mathrm{NH}}_3>{\mathrm{NH}}_2^{-}>{\mathrm{NH}}_4^{+}$

4. ${\mathrm{NH}}_3>{\mathrm{NH}}_4^{+}>{\mathrm{NH}}_2^{-}$

The "O-N-O" bond angle is maximum in 

1. ${\mathrm{N}}_2\mathrm{O}$

2. ${\mathrm{NO}}_2^{+}$

3. ${\mathrm{NO}}_2^{-}$

4. ${\mathrm{NO}}_3^{-}$

The correct statement regarding $S{O}_2$ molecule is-

1. Two $p\mathrm{\pi }-\mathrm{d\pi }$ bonds

2. Molecules has 2 lone pair, 2$\sigma$ bonds and 2$\pi$ bonds

3. Two $p\pi -p\pi$ bonds

4. One $p\pi -p\pi$ and one $p\mathrm{\pi }-\mathrm{d\pi }$ bond

Calculate the maximum ionic character possible in a bond between two atoms in the periodic table according to Hanny Smith equation. [Electronegativeity of Li=1.0, Na=0.9, K=0.8, Rb=0.8, Cs=0.7, Fr=0.7]

1.  $~90\%$

2.  $~97\%$

3.  $~80\%$

4.  $~75\%$

${\mathrm{AsF}}_5$ molecule is trigonal bipyramidal. The hybrid orbitals used by As-atoms for bonding are

1.  ${\mathrm{d}}_{{\mathrm{x}}^2-{\mathrm{y}}^2}, {\mathrm{d}}_{{\mathrm{z}}^2}, \mathrm{s}, {\mathrm{p}}_{\mathrm{x}}, {\mathrm{p}}_{\mathrm{y}}$

2.  ${\mathrm{d}}_{\mathrm{xy}}, \mathrm{s}, {\mathrm{p}}_{\mathrm{x}}, {\mathrm{p}}_{\mathrm{y}}, {\mathrm{p}}_{\mathrm{z}}$

3.  $\mathrm{s}, {\mathrm{p}}_{\mathrm{x}}, {\mathrm{p}}_{\mathrm{y}}, {\mathrm{p}}_{\mathrm{z}}, {\mathrm{d}}_{{\mathrm{z}}^2}$

4.  ${\mathrm{d}}_{{\mathrm{x}}^2-{\mathrm{y}}^2}, \mathrm{s}, {\mathrm{p}}_{\mathrm{x}}, {\mathrm{p}}_{\mathrm{y}}, {\mathrm{p}}_{\mathrm{z}}$