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. ${\mathrm{BC}}_5$

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

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?

1. ${\mathrm{Be}}_2$ is not a stable molecule.

2. ${\mathrm{He}}_2$ is not stable but ${\mathrm{He}}_2^{+}$ is expected to exist.

3. Bond strength of ${\mathrm{N}}_2$ is maximum amongst the homonuclear diatomic molecules belonging to the second period.

4. The order of energies of molecular orbitals in ${\mathrm{N}}_2$ molecule is: 

${\mathrm{\sigma }}_{2\mathrm{s}}<{\mathrm{\sigma }}_{2\mathrm{s}}^{*}<{\mathrm{\sigma }}_{2{\mathrm{p}}_{\mathrm{z}}}<({\mathrm{\pi }}_{2{\mathrm{p}}_{\mathrm{x}}}\approx {\mathrm{\pi }}_{2{\mathrm{p}}_{\mathrm{y}}})$
$<({\mathrm{\pi }}_{2{\mathrm{p}}_{\mathrm{x}}}^{*}\approx {\mathrm{\pi }}_{2{\mathrm{p}}_{\mathrm{y}}}^{*})<{\mathrm{\sigma }}_{2{\mathrm{p}}_{\mathrm{z}}}^{*}$

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

Match the species in Column I with the type of hybrid orbitals in Column II.

Codes