All right so I've got this question asking how to correct certain formulas. They gave me Fe2O. Since Iron has a full valence, and oxygen needs 2 more electrons for a full one, would that formula be correct? Or is that even an ionic bond? Obviously since it's between a metal and a nonmetal (oxygen) then it ought to be ionic. But what should I do for the full valence? Sorry, it might be a stupid question but someone ought to know.
2006-11-08 08:16:04 · 2 answers · asked by E 2 in Science & Mathematics ➔ Chemistry
I dont understand what you mean by "correcting certain formulas", but it appears Fe bears +1 oxidation state, if oxygen is -2. However, Fe does not bear such oxidation state, normally; it can bear 0, +2, +3, +4 and +6. With oxygen, what you will get, most likely, are FeO and Fe2O3. So, I would expect the the compound was a mixture of iron metal and one/several of these oxides. It appears that your compound could be 1:1 mixture of iron and iron(II) oxide.
If the question states that the compound was pure, check your calculation again; if you have done nothing wrong, the compound could be iron(II) peroxide [iron bears +2, oxygen bears -1]; it's not stable [I'm not sure whether it exists or not], or the strange iron(I) oxide [again, never seen this compound before, not sure it actually exists or not].
2006-11-08 09:52:06 · answer #1 · answered by nickyTheKnight 3 · 0⤊ 0⤋
mm..im not so sure whether Fe has full valence or not, but as a transition metal, it is known to have varying oxidation states of +2 and even +3. That's how you have your Iron (III) Chloride and Iron (III) Oxide, as well as Iron (II) Sulphate.
In the case of Fe2O, the oxidation state of Fe is +1, which could be a special case. Chemistry is full of exceptions. So do not worry too much about it.
**I don't understand what you mean by correcting tt formula, but Fe2O3 will be correct. It shld be quite common in labs.
Hope this helps=)
apl
2006-11-08 16:24:15 · answer #2 · answered by luv_phy 3 · 0⤊ 0⤋