General

[quote=MarshMallows]Hmm..try +2 for the Na one and -2 for the fluorine one[/quote]

I had that from the start, it kept saying it was wrong.

I'll just ask her tomorrow, it doesn't really matter because I would get a 94 anyway

[quote=Omelet]I put in 1+ for sodium and 1- for fluorine and it is saying it's wrong.

it probably isn't she probably just made a mistake.[/quote]

Hmm..try +2 for the Na one and -2 for the fluorine one

[quote=MarshMallows]You're having trouble crossing charges..
Na is +1 ALWAYS
The ion Co3 is always -2

Lead (PB) has multiple oxidation states but the one in the picture is +2
Fluorine ALWAYS has a charge of -1[/quote]

I put in 1+ for sodium and 1- for fluorine and it is saying it's wrong.

it probably isn't she probably just made a mistake.

edit: doesn't matter, just got locked out of the question.

you guys are right, the answer key is probably just wrong.

[quote=Omelet]The thing is, I can't put that..
If it did exist somehow, what would it's oxidation number be?[/quote]

You're having trouble crossing charges..
Na is +1 ALWAYS
The ion Co3 is always -2

Lead (PB) has multiple oxidation states but the one in the picture is +2
Fluorine ALWAYS has a charge of -1

Edit: This may help.
[url]http://wiki.answers.com/Q/How_do_chemistry_formulas_work[/url]

[quote=iNerd]First link: Sodium does not exist diatomically.
Second link: Diatomic flourine is a neutral molecule.[/quote]

The thing is, I can't put that..
If it did exist somehow, what would it's oxidation number be?

[quote=iNerd]First link: Sodium does not exist diatomically.
Second link: Diatomic flourine is a neutral molecule.[/quote]

He's talking about the synthesis of Na and the ion Co3 -2 which would result in Na2Co3

Alright, I should have just given you this from the start
http://imageshack.us/photo/my-images/28/chemx.png/
http://imageshack.us/photo/my-images/202/chem1.png/

Also, my teacher completely blows, I doubt she even took 2 chemistry courses in college.
She didn't go over this at all.

[quote=Omelet]it's not that it doesn't exist, it gave me the cation/anion and I separated it into sodium (na_2) and carbonate (co_3)
it's asking for the formula for each one, with oxidation number

sorry if i'm being confusing[/quote]

You mean, Na2Co3 - Sodium carbonate?
It disassociates into Na +1 ions and Co3 -2 ions

[quote=iNerd]I'm pretty sure two sodiums together isn't possible, and flourine's oxidation # is 0, as fluorine exists as a diatomic molecule.

EDIT: Unless the fluorine is negatively charged, then its oxidation # is -1. Otherwise, it's 0.[/quote]

it's not that it doesn't exist, it gave me the cation/anion and I separated it into sodium (na_2) and carbonate (co_3)
it's asking for the formula for each one, with oxidation number

sorry if i'm being confusing

all elements in pure form have a state of 0?

[quote=Fronz]Fluorine ALWAYS has an oxidation number of -1.[/quote]

Even in fluorine gas state?

[quote=TenthPole]How about you get off basilmarket and ask real people?[/quote]

First off, it's nearly midnight and I'm just starting on this because I was zonked with homework.

OT: It's two sodiums and two fluorines.
Oxidation numbers

I think sodium is 2+ and fluorine is 2-, they are not together.