In a chemical reaction, an iron atom became the ion Fe2+. What happened to the iron atom?

Question

1.) It lost electrons and was oxidized.
2.) It lost electrons and was reduced.
3.) It gained electrons and was oxidized.
4.) It gained electrons and was reduced

Answer 1

1. Metallic iron is Fe (0). For iron to become Fe2+ it must lose 2 electrons (2 negative charges). "Oxidized" means lost electrons, in redox chemistry.

http://en.wikipedia.org/wiki/Redox

(BTW there is a lot of misinformation below. I was a Chem major in college with all A's, and now have a PhD and work in science.)

Answer 2

If iron was neutral (as it is in its elemental state), then it had zero charge. If it's now positive, it must have lost negative charges, that is, electrons. How many? Well, now it's doubly positive charged (iron can also go to the +3 state), so it must have lost two electrons.

Oxidation is the loss of electrons. It can occur rapidly (in burning--and yes, you can burn finely divided iron in a pure oxygen atmosphere) or slowly, as in rusting.

When iron rusts, it forms ferrous and ferric oxides, in which the iron is in its plus two or plus three state.

Answer 3

the oxidation number of an iron atom is 0
the oxidation number of ion Fe2+ is +2
so it means,the iron atom gained electrons, and gaining electrons means it was oxidized.

Answer 4

(1) is correct. fe has lost 2 electrons and therefore 2 protons r extra in ion now leading to +2 chrge.
and oxidation is defined as loss of electrons so it has got oxidised.