The ground state electron configuration of the nitrogen atom is A. 1s22s22px1 B. 1s22s22px1py1 C. 1s22s22px1py1pz1 D. 1s22s 2单项选择题
A
A
B
B
C
C
D
D

Question

The ground state electron configuration of the nitrogen atom is A. 1s22s22px1 B. 1s22s22px1py1 C. 1s22s22px1py1pz1 D. 1s22s 2

BlackTom AI · Accepted Answer

Nitrogen has atomic number 7, so it contains seven electrons to place into atomic orbitals following the Aufbau principle, the Pauli exclusion principle, and Hund’s rule.

Relevant concepts:
- Aufbau principle: fill lower-energy orbitals before higher-energy ones (1s → 2s → 2p).
- Pauli exclusion: each orbital holds at most two electrons with opposite spins.
- Hund’s rule: for degenerate orbitals (the three 2p orbitals) place one electron in each orbital with parallel spins before pairing.

Step-by-step reasoning and intermediate counting:
1. Total electrons = 7 (from atomic number).
2. Fill 1s: 1s can hold 2 electrons → 7 − 2 = 5 remaining. So 1s^2.
3. Fill 2s: 2s can hold 2 electrons → 5 − 2 = 3 remaining. So 2s^2.
4. Fill 2p: there are three degenerate 2p orbitals (2p_x, 2p_y, 2p_z). We must place the remaining 3 electrons into these orbitals.
   - By Hund’s rule, place one electron in each 2p orbital rather than pairing any. That yields 2p_x^1 2p_y^1 2p_z^1.

Thus the ground-state electron configuration is 1s^2 2s^2 2p_x^1 2p_y^1 2p_z^1.

Why answer C is correct:
Option C explicitly lists one electron in each of the three 2p orbitals, which matches the distribution required by Hund’s rule for three 2p electrons.

Why the other options are incorrect:
- A (1s^2 2s^2 2p_x^1) accounts for only one 2p electron instead of three.
- B (1s^2 2s^2 2p_x^1 2p_y^1) accounts for only two 2p electrons, not three.
- D (1s^2 2s^2) accounts for only four total electrons, missing the three 2p electrons.

Confirming final answer: therefore the correct ground-state configuration is option C: 1s^2 2s^2 2p_x^1 2p_y^1 2p_z^1.

The ground state electron configuration of the nitrogen atom is A. 1s22s22px1 B. 1s22s22px1py1 C. 1s22s22px1py1pz1 D. 1s22s 2单项选择题

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