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 with 1s having two arrows, 2s having two arrows, 2p having two arrows in one box and one arrow in another box
1s 2s 2p
b. orbital diagram with 1s having two arrows, 2s having one arrow, 2p having two arrows in one box and two single arrows in other boxes
1s 2s 2p
c. orbital diagram with 1s having two arrows, 2s having two arrows, 2p having three single arrows
1s 2s 2p
d. orbital diagram with 1s having two arrows, 2s having two arrows, 2p having two arrows in one box and two single arrows in other boxes
1s 2s 2p
see periodic table see hint see hint

Explanation:

Step1: Determine oxygen's electron - count

Oxygen has 8 electrons in its neutral state. An oxygen cation \(O^{+}\) has 7 electrons.

Step2: Recall electron - filling rules

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

Step3: Analyze each option

• Option A: Has a total of 8 electrons (\(2 + 2+4\)), so it is incorrect.
• Option B: Has 7 electrons (\(2 + 1+4\)) and follows the electron - filling rules. The \(1s\) is filled with 2 electrons, the \(2s\) has 1 electron, and the \(2p\) has 4 electrons with the correct spin and orbital - occupancy pattern.
• Option C: Has 7 electrons (\(2 + 2+3\)) but the \(2s\) orbital should have 2 electrons before filling the \(2p\) orbitals according to the Aufbau principle, so it is incorrect.
• Option D: Has 8 electrons (\(2 + 2+4\)), so it is incorrect.

Answer:

B.