Question

4th attempt 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: see periodic table see hint

Explanation:

Oxygen has an atomic number of 8. The $O^+$ cation has 7 electrons. The electron - filling order follows the Aufbau principle, Pauli exclusion principle, and Hund's rule. The ground - state electron configuration of $O^+$ is $1s^22s^22p^3$. In orbital diagrams, the 1s and 2s orbitals are filled with 2 electrons each (spin - paired), and the 2p orbitals have 3 unpaired electrons (one in each of the three 2p orbitals). We need to analyze each option based on these rules.

Answer:

We need to see the specific orbital diagrams in options A, B, C, D to determine the correct answer. Since the diagrams are not clearly described in text, we cannot give a definite letter answer. But the correct orbital diagram should have 2 electrons in 1s (spin - paired), 2 electrons in 2s (spin - paired), and 3 unpaired electrons in the three 2p orbitals.