# 8.4: Anion Formation

How do you transform a deadly gas into something you can sprinkle on your eggs and eat for breakfast? Chlorine in its free form is very dangerous if you breathe the fumes or come in contact with the gas. However, after reaction with sodium, we have sodium chloride formed as the sodium atom gives up an electron to chlorine which accepts the electron to form the chloride anion.

## Anions

Anions are the negative ions formed from the gain of one or more electrons. When nonmetal atoms gain electrons, they often do so until their outermost principal energy level achieves an octet. This process is illustrated below for the elements fluorine, oxygen, and nitrogen.

$\begin{array}{lcl} \ce{F} + \ce{e^-} & \rightarrow & \ce{F^-} \\ 1s^2 \: 2s^2 \: 2p^5 & & 1s^2 \: 2s^2 \: 2p^6 \: \text{(octet)} \end{array}$

$\begin{array}{lcl} \ce{O} + 2 \ce{e^-} & \rightarrow & \ce{O^{2-}} \\ 1s^2 \: 2s^2 \: 2p^4 & & 1s^2 \: 2s^2 \: 2p^6 \: \text{(octet)} \end{array}$

$\begin{array}{lcl} \ce{N} + 3 \ce{e^-} & \rightarrow & \ce{N^{3-}} \\ 1s^2 \: 2s^2 \: 2p^3 & & 1s^2 \: 2s^2 \: 2p^6 \: \text{(octet)} \end{array}$

All of these anions are isoelectronic with each other and with neon. They are also isoelectronic with the three cations from the previous section. Under typical conditions, three electrons is the maximum that will be gained in the formation of anions.

Outer electron configurations are constant within a group, so this patter of ion formation repeats itself for Periods 3, 4, and following (see below).

It is important not to misinterpret the concept of being isoelectronic. A sodium ion is very different from a neon atom because the nuclei of the two contain different numbers of protons. One is an essential ion that is a part of table salt, while the other is an unreactive gas that is a very small part of the atmosphere. Likewise, sodium ions are very different than magnesium ions, fluoride ions, and all the other members of this isoelectronic series $$\left( \ce{N^{3-}}, \: \ce{O^{2-}}, \: \ce{F^-}, \: \ce{Ne}, \: \ce{Na^+}, \: \ce{Mg^{2+}}, \: \ce{Al^{3+}} \right)$$.