Which doubly positive ion has the ground-state electron configuration 1s2 2s2 2p6?

Verified step by step guidance

1. Step 1: Identify the given electron configuration: 1s^2 2s^2 2p^6. This configuration represents a total of 10 electrons.
2. Step 2: Recognize that the configuration 1s^2 2s^2 2p^6 corresponds to the noble gas neon (Ne), which has 10 electrons in its neutral state.
3. Step 3: Since the problem asks for a doubly positive ion, consider that the ion has lost 2 electrons from its neutral state.
4. Step 4: Determine the neutral atom that, when it loses 2 electrons, results in the electron configuration of neon. This would be an atom with 12 electrons in its neutral state.
5. Step 5: Identify the element with 12 electrons in its neutral state, which is magnesium (Mg). Therefore, the doubly positive ion is Mg^{2+} with the electron configuration 1s^2 2s^2 2p^6.