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 :

The correct bond angle for \(\mathrm{sp}^2\) hybridization is:
1. \(90^\circ\)
2. \(120^\circ\)
3. \(180^\circ\)
4. \(109^\circ\)

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

$\mathrm{A}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>1{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{p}}^6$
$\mathrm{B}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>1{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{p}}^6<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>3{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>3{\mathrm{p}}^3$
$\mathrm{C}<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>1{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{p}}^6<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>3{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>3{\mathrm{p}}^5$

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

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

$\mathrm{A}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>1{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{p}}^6$
$\mathrm{B}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>1{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{p}}^6<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>3{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>3{\mathrm{p}}^3$
$\mathrm{C}<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>1{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{p}}^6<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>3{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>3{\mathrm{p}}^5$

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. ${\mathrm{BC}}_5$

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

$\mathrm{A}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>1{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{p}}^6$
$\mathrm{B}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>1{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{p}}^6<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>3{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>3{\mathrm{p}}^3$
$\mathrm{C}<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>1{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2{\mathrm{p}}^6<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>3{\mathrm{s}}^2<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>3{\mathrm{p}}^5$

The bond between B and C will be : 

Among the following, the correct order of energies of molecular orbitals of N₂ is:

1. $\left(\mathrm{\pi }2{\mathrm{p}}_{\mathrm{y}}\right)<\left(\mathrm{\sigma }2{\mathrm{p}}_{\mathrm{z}}\right)<(\mathrm{\pi }*2{\mathrm{p}}_{\mathrm{x}})\approx (\mathrm{\pi }*2{\mathrm{p}}_{\mathrm{y}})$

2. $\left(\mathrm{\pi }2{\mathrm{p}}_{\mathrm{y}}\right)>\left(\mathrm{\sigma }2{\mathrm{p}}_{\mathrm{z}}\right)>(\mathrm{\pi }*2{\mathrm{p}}_{\mathrm{x}})\approx (\mathrm{\pi }*2{\mathrm{p}}_{\mathrm{y}})$

3. $\left(\mathrm{\pi }2{\mathrm{p}}_{\mathrm{y}}\right)<\left(\mathrm{\sigma }2{\mathrm{p}}_{\mathrm{z}}\right)\approx <mspace\; width="1em"></mspace>(\mathrm{\pi }*2{\mathrm{p}}_{\mathrm{x}})\approx (\mathrm{\pi }*2{\mathrm{p}}_{\mathrm{y}})$

4. $\left(\mathrm{\pi }2{\mathrm{p}}_{\mathrm{y}}\right)>\left(\mathrm{\sigma }2{\mathrm{p}}_{\mathrm{z}}\right)<(\mathrm{\pi }*2{\mathrm{p}}_{\mathrm{x}})\approx (\mathrm{\pi }*2{\mathrm{p}}_{\mathrm{y}})$

From the perspective of molecular orbital theory, which statement is false?

What is the correct sequence of bond order for the specified species?