Question

Electronic configuration of C in its exited state is

• A. \(1s^2\ 2s^2\ 2p_x^0\ 2p_y^2\ 2p_z^0 \)
• B. \(1s^2\ 2s^2\ 2p_x^2\ 2p_y^0\ 2p_z^0 \)
• C. \(1s^2\ 2s^2\ 2p_x^1\ 2p_y^1\ 2p_z^0 \)
• D. \(1s^2\ 2s^1\ 2p_x^1\ 2p_y^1\ 2p_z^1 \)

Answer 1

The Correct Option is D

The ground state electronic configuration of carbon (atomic number 6) is: 1s² 2s² 2p² In the ground state, the 2p electrons occupy different orbitals according to Hund's rule: 1s² 2s² 2pₓ¹ 2pᵧ¹ 2p𝓏⁰
In the excited state, one of the electrons from the 2s orbital is promoted to the 2p orbital to allow bonding (especially in covalent molecules like CH₄), resulting in: 1s² 2s¹ 2pₓ¹ 2pᵧ¹ 2p𝓏¹
This configuration reflects the hybridization readiness of carbon (sp³) seen in many organic compounds.

The correct option is (D): \(1s^2\ 2s^1\ 2p_x^1\ 2p_y^1\ 2p_z^1 \)