What is the electronic configuration of ${{O}^{2-}}$ ion?

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Hint: Write the electronic configuration of oxygen atom in its neutral state. Then add two electrons to the outermost orbital of the configuration.

Complete answer:
For writing the electronic configuration of any element, we have to know its atomic number. The atomic number of an element is the number of protons present inside the nucleus of its atom or the number of electrons present inside a neutral atom of that element.
On the periodic table, the element oxygen occupies the position at the crossing of the second period and sixteenth group. The atomic number of oxygen is “$8$”. So, its electronic configuration is as below:
The orbital arrangement of electrons for the above configuration is shown below:

As you can see, there are two unpaired electrons in the valence subshell of the oxygen element. In${{O}^{2-}}$ion, there are two extra electrons which means, the unpaired electrons are paired now. So the electronic configuration becomes:
This is the electronic configuration of neon, which is a noble gas. The orbital arrangement for the above configuration is as shown below:

Additional Information:
- Oxygen is the second most electronegative element in the periodic table after fluorine.
- The oxygen element is relatively stable in its anionic state than other elements because of its higher electronegativity and small size.
- The small size of oxygen is due to its position in the periodic table. As you know, the size of an atom increases as we go down the group and across a period.

Note: Fluorine is more stable than oxygen in its anionic state because it is the most electronegative element in the whole periodic table.
Even if more electronegative elements are quite stable in their anionic forms, they cannot exist for much time if they are not supported by external agents. An example of such an external agent is water. The water molecules dissociate and surround these anions to stabilise the excess negative charge.