Which species lacks tetrahedral geometry?

1. ${\mathrm{BH}}_4^{-}$

2. ${\mathrm{NH}}_2^{-}$

3. ${\mathrm{CO}}_3^{2-}$

4. ${\mathrm{H}}_3{\mathrm{O}}^{+}$

The number of $\mathrm{\pi }$ bonds and $\mathrm{\sigma }$ bonds in the following structure is :

The species doesn't have unpaired electrons is:

In which of the following molecule/ion all the bonds are not equal?

1.  ${\mathrm{XeF}}_4$

2. ${\mathrm{BF}}_4^{-}$

3. ${\mathrm{C}}_2{\mathrm{H}}_4$

4. ${\mathrm{SiF}}_4$

Hydrogen bond will be strongest in : 

1. HCl

2. H₂O

3. HI

4. H₂S

If the electronic configuration of an element is $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^{2}4{\mathrm{s}}^2$, the four electrons that participate in the chemical bond formation will be from :

1. $3{\mathrm{p}}^6$

2. $3{\mathrm{p}}^6, 4{\mathrm{s}}^2$

3. $3{\mathrm{p}}^6, 3{\mathrm{d}}^2$

4. $3{\mathrm{d}}^2, 4{\mathrm{s}}^2$

The correct bond angle for \(\mathrm{sp}^2\) hybridization is:

The electronic configurations of the elements A, B, and C are given below.

$\mathrm{A} = 1{\mathrm{s}}^2 2{\mathrm{s}}^2 2{\mathrm{p}}^6$
$\mathrm{B} = 1{\mathrm{s}}^2 2{\mathrm{s}}^2 2{\mathrm{p}}^6 3{\mathrm{s}}^2 3{\mathrm{p}}^3$
$\mathrm{C} = 1{\mathrm{s}}^2 2{\mathrm{s}}^2 2{\mathrm{p}}^6 3{\mathrm{s}}^2 3{\mathrm{p}}^5$

The stable form of A may be represented by the formula:

The electronic configurations of the elements A, B, and C are given below.

$\mathrm{A} = 1{\mathrm{s}}^2 2{\mathrm{s}}^2 2{\mathrm{p}}^6$
$\mathrm{B} = 1{\mathrm{s}}^2 2{\mathrm{s}}^2 2{\mathrm{p}}^6 3{\mathrm{s}}^2 3{\mathrm{p}}^3$
$\mathrm{C} = 1{\mathrm{s}}^2 2{\mathrm{s}}^2 2{\mathrm{p}}^6 3{\mathrm{s}}^2 3{\mathrm{p}}^5$

The stable form of C may be represented by the formula : 

The electronic configurations of three elements, A, B, and C are given below.  

A 1s² 2s² 2p⁶
B 1s² 2s² 2p⁶ 3s² 3p³
C 1s² 2s² 2p⁶ 3s² 3p⁵

The molecular formula of the compound formed from B and C will be 

1. $\mathrm{BC}$

2. ${\mathrm{B}}_2\mathrm{C}$

3. ${\mathrm{BC}}_2$

4. ${\mathrm{BC}}_5$