Complete question:
Which of the following electron configurations represents an excited state of the indicated atom?A) Ne: 1s2 2s2 2p6B) Na: 1s2 2s2 2p6 3s2 3p2 4s1C) P: 1s2 2s2 2p6 3s2 3p2 4s1D) N: 1s2 2s2 2p3
Answer:
C) P: 1s² 2s² 2p⁶ 3s² 3p² 4s¹ → excited state
Explanation:
An excited state configuration is a higher energy arrangement of electrons.
A) Ne: (Neon has 10 electrons)
Ground state configuration: 1s² 2s² 2p⁶
Given configuration: 1s² 2s² 2p⁶ → ground state
B) Na: (sodium has 11 electrons)
Ground state configuration: 1s² 2s² 2p⁶ 3s¹
Given configuration: 1s² 2s² 2p⁶ 3s² 3p² 4s¹ → excess electrons
C) P: (Phosphorus has 15 electrons)
Ground state configuration: 1s² 2s² 2p⁶ 3s² 3p³
Given configuration: 1s² 2s² 2p⁶ 3s² 3p² 4s¹ → excited state
D) N: (Nitrogen has 7 electrons)
Ground state configuration: 1s² 2s² 2p³
Given configuration: 1s² 2s² 2p³ → ground state
