Which of the following electronic configurations are associated with the formation of a molecule with expanded octet?

[H e] 2 s^{2} 2 p^{1}

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[H e] 2 s^{2} 2 p^{2}

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[N e] 3 s^{2} 3 p^{3}

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[N e] 3 s^{2} 3 p^{4}

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Solution

The correct options are
C $[N e] 3 s^{2} 3 p^{3}$
D $[N e] 3 s^{2} 3 p^{4}$
The electronic configurations $[N e] 3 s^{2} 3 p^{3}$ and $[N e] 3 s^{2} 3 p^{4}$ are associated with the formation of molecule with expanded octet. In these electronic configurations electrons can be excited from $3 p$ subshell to $3 d$ subshell. Elements belonging to second period of the periodic table do not form such stable molecules as they do not have d orbitals.

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= [N e] 3 s^{2} 3 p^{3}

= [A r] 3 d^{10} 4 s^{2} 4 p^{3}

= [H e] 2 s^{2} 2 p^{5}

= [N e] 3 s^{1}

[H e] 2 s^{1}

[H e] 3 s^{2}

[H e] 2 s^{2} 2 p^{2}

[N e] 3 s^{2} 3 p^{1}

X \to [N e] 3 s^{2} 3 p^{3}

(i) Write the electronic configurations of the following ions: (a) H^–(b) Na⁺ (c) O^2–(d) F^–

(ii) What are the atomic numbers of elements whose outermost electrons are represented by (a) 3s¹(b) 2p³ and (c) 3p⁵?

(iii) Which atoms are indicated by the following configurations?

(a) [He] 2s¹ (b) [Ne] 3s² 3p³ (c) [Ar] 4s² 3d¹.

[H e] 2 s^{1}

[H e] 3 s^{2}

[H e] 2 s^{2} 2 p^{2}

[N e] 3 s^{2} 3 p^{1}

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