No clue how to explain this. Just don't understand it:

Which formation of the monatomic ion of oxygen is the most energetically favorable?
A) O2-
B) O2+
C) O4+
D) O-
E)O6+

the formation of which monatomic ion oxygen is the most energetically favorable

To determine which formation of the monatomic ion of oxygen is the most energetically favorable, we need to analyze the electron configuration and the stability of each ion.

Let's break down each option:

A) O2-
This ion has gained two electrons. To understand its stability, we must consider the electron configuration of oxygen, which has an atomic number of 8. The electron configuration of a neutral oxygen atom is 1s^2 2s^2 2p^4. By gaining two electrons, the oxygen forms a stable octet in its valence shell, resembling the nearest noble gas configuration, neon. This stability makes the O2- ion energetically favorable.

B) O2+
This ion has lost one electron. Losing an electron means the oxygen atom will have an unfilled valence shell, which is less energetically stable. Therefore, the O2+ ion is less favorable compared to O2-.

C) O4+
This ion suggests that oxygen has gained four electrons, which would make its electron configuration 1s^2 2s^2 2p^10 3s^2 3p^6. However, oxygen typically forms stable octets, so gaining four electrons would be energetically unfavorable. Thus, the O4+ ion is unlikely to occur.

D) O-
This ion has gained one electron, resulting in an electron configuration of 1s^2 2s^2 2p^6. This configuration forms a stable octet, similar to the O2- ion. However, the O- ion has one less electron and is therefore less stable than the O2- ion.

E) O6+
This ion suggests that oxygen has gained six electrons, which would make its electron configuration highly unfavorable. As mentioned earlier, oxygen typically forms octets, so gaining six electrons would result in a highly unstable configuration. Thus, the O6+ ion is unlikely to occur.

Based on the analysis above, the most energetically favorable formation of the monatomic ion of oxygen is A) O2-.

o2-

02-

O2-