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

Choose the incorrect statement among the following.

1.  $\mathrm{HF}$ is the most volatile acid among $\mathrm{HX}$.

2.  ${\mathrm{Na}}_2{\mathrm{O}}_2$ is having ionic and covalent type of bonds.

3.  ${\mathrm{CH}}_3{\mathrm{CO}}_2\mathrm{Na}$ is having identical $\mathrm{C}-\mathrm{O}$ bond lengths while it is not true for ${\mathrm{CH}}_3{\mathrm{CO}}_2\mathrm{H}$.

4.  p-p overlap is more stronger compared to s-s overlap in axial type of bond formation.

Mark the molecular species, among the following, that is not electron-deficient:

1.  ${\mathrm{AlCl}}_3$

2.  ${\mathrm{BeH}}_2$

3.  ${{\mathrm{BH}}_4}^{-}$

4.  ${\mathrm{BF}}_3$

In which of the following molecule the intramolecular hydrogen bonding is not existing.

1.  Chloral hydrate

2.  O-chlorophenol

3.  Choral

4.  Salicylic acid

For the molecule ${\mathrm{MA}}_2{\mathrm{L}}_{\mathrm{n}}$ (where A is number of single bonded surrounding atoms, L indicates lone pair and 'n' is the number of lone pair and M is the central atom of 's' or 'p' block element) the possible range of 'n' is

1.  '1' to '4'

2.  zero to '4'

3.  '1' to '3'

4.  '0' to '3'

Carbon suboxide $\left({\mathrm{C}}_3{\mathrm{O}}_2\right)$ has

1.  Linear structure

2.  Bent structure

3.  Trigonal structure

4.  Distorted tetrahedral structure

${\mathrm{PCl}}_5$ is highly unstable and in solid state it exists as into ${\left[{\mathrm{PCl}}_4\right]}^{+} \mathrm{and} {\left[{\mathrm{PCl}}_6\right]}^{-}$ ions.
The geometry of ${\left[{\mathrm{PCl}}_6\right]}^{-}$ is

1.  Octahedral

2.  Tetrahedral

3.  Square pyramidal

4.  Square planar

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

The correct order of increasing bond angles in the following species is

1.  ${\mathrm{Cl}}_2\mathrm{O} < {\mathrm{ClO}}_2 < {\mathrm{ClO}}_2^{-}$

2.  ${\mathrm{ClO}}_2 < {\mathrm{Cl}}_2\mathrm{O} < {\mathrm{ClO}}_2^{-}$

3.  ${\mathrm{Cl}}_2\mathrm{O} < {\mathrm{ClO}}_2^{-} < {\mathrm{ClO}}_2$

4.  ClO₂^- < Cl₂O < ClO₂