Question

During a chemical reacion, an iron atom beacme the ion Fe+2. what happened to the iron atom?

Answer 1

Answer:

That iron atom is oxidized. It loses two electrons.

Explanation:

Compare the formula of an iron atom and an iron(II) ion:

• Iron atom: $\mathrm{Fe}$;
• Iron(II) ion: $\mathrm{Fe^{2+}}$.

The superscript $+2$ in the iron(II) ion is the only difference between the two formulas. This superscript indicates a charge of $+2$ on each ion. Atoms and ions contain protons. In many cases, they also contain electrons. Each proton carries a positive charge of $+1$ and each electron carries a charge of $-1$. Atoms are neutral for they contain an equal number of protons and electrons.

Protons are located at the center of atoms inside the nuclei. They cannot be gained or lost in chemical reactions. However, electrons are outside the nuclei and can be gained or lost. When an atom loses one or more electrons, it will carry more positive charge than negative charge. It will becomes a positive ion. Conversely, when an atom gains one or more electrons, it becomes a negative ion.

An iron atom $\mathrm{Fe}$ will need to lose two electrons to become a positive iron(II) ion $\mathrm{Fe^{2+}}$ with a charge of $+2$ on each ion. That is:

$\rm Fe \to Fe^{2+} + 2\;e^{-}$.

• Oxidation is Losing one or more electrons;
• Reduction is Gaining one or more electrons.

This definition can be written as the acronym OILRIG. (Khan Academy.)

In this case, each iron atom loses two electrons. Therefore the iron atoms here are oxidized.