Question

part 1 (1 point)
which of the orbital diagrams represent(s) the ground - state electron configuration of an oxygen cation, o⁺?
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
part 2 (1 point)
which of the orbital diagrams represent(s) an excited - state nitrogen atom?
choose one or more:

Explanation:

Step1: Determine electron - count of O⁺

Oxygen has 8 electrons in its neutral state. O⁺ has 7 electrons (lost one electron).

Step2: Recall electron - filling rules

Electrons fill orbitals according to the Aufbau principle (low - energy orbitals first), Pauli exclusion principle (each orbital can hold at most 2 electrons with opposite spins), and Hund's rule (electrons occupy degenerate orbitals singly with parallel spins first). The order of filling is 1s, 2s, 2p. 1s can hold 2 electrons, 2s can hold 2 electrons, and the remaining 3 electrons go into 2p orbitals.

Step3: Analyze options for O⁺

For O⁺ with 7 electrons, the ground - state electron configuration is 1s²2s²2p³. Option A has 1s²2s²2p³ configuration which is correct for O⁺ ground state.

Step4: Determine electron - count of N

Nitrogen has 7 electrons in its neutral state. In the ground state, its electron configuration is 1s²2s²2p³ with 3 unpaired electrons in 2p orbitals according to Hund's rule.

Step5: Analyze options for excited - state N

An excited - state nitrogen atom has electrons promoted to higher - energy orbitals. Option B has an electron promoted from 2s to 2p (1s²2s¹2p⁴), which represents an excited state.

Answer:

Part 1: A.
Part 2: B.