Sodium forms a 1+ ion, while fluorine forms a 1-lon. Write the electron configuration for each ion. Why don't these two elements form 2+ and 2-ions, respectively?

The electron configuration for;

First, we must understand stand that atoms of elements ionize to become ions in such a manner as to become electronically stable.

In essence, the aim of ionization is to attain the closest state of electronic stability.

Both atoms consequently become isolectronic with Neon, Ne.

Additionally, the two elements, Sodium and Flourine don't form 2+ and 2- ions respectively because, they do not attain electronic stability in such manner.

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Explanation:

Given elements:

    Sodium

    Fluorine

The ion Na⁺ is made up of 10 electrons, its electronic configuration is:

            1s² 2s² 2p⁶

Ion F⁻ is made up of 10 electrons, its electronic configuration is:

           1s² 2s² 2p⁶

These ions do not form +2 because they cannot attain stability by losing or gaining two electrons.

Sodium atom is made up of one valence electron. If it loses one electron, it will be isoelectronic with Neon.

Fluorine has 7 valence electrons, to attain stability, it must gain one electron to form an octet. This way it will be isoelectronic with Neon.

Losing or gaining two electrons will not make the elements attain stability.

a chemical reaction happens

explanation:

there are no statements provided but here is why:

sulfur belongs to group 16 because it can be found in nature whether it is in a free or combined state.

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