Question

part 2 (1 point) which of the orbital diagrams represent(s) an excited - state nitrogen atom? choose one or more: a. orbital diagram for 1s, 2s, 2p b. orbital diagram for 1s, 2s, 2p c. orbital diagram for 1s, 2s, 2p d. orbital diagram for 1s, 2s, 2p

Explanation:

Step1: Recall nitrogen's electron - configuration

Nitrogen has an atomic number of 7. Its ground - state electron configuration is $1s^{2}2s^{2}2p^{3}$. In the orbital diagram of the ground state, the 1s and 2s orbitals are filled with 2 electrons each (spin - paired), and the 2p orbitals have 3 unpaired electrons (following Hund's rule).

Step2: Analyze each option

• Option A: In this diagram, the 2p orbitals do not follow Hund's rule for the ground state. But it has the correct number of electrons and is an excited - state configuration as the electrons are not arranged in the lowest - energy way.
• Option B: The 2s orbital is not fully filled while there are electrons in the 2p orbitals. This is an excited - state configuration since the ground state has the 2s orbital filled before populating the 2p orbitals.
• Option C: This is the ground - state orbital diagram of nitrogen as it follows the Aufbau principle, Pauli exclusion principle, and Hund's rule.
• Option D: This is also an excited - state configuration as the electron distribution in the 2p orbitals is not in the lowest - energy (ground - state) arrangement.

Answer:

A. Option A, B. Option B, D. Option D