Tommorrow is the midterm and i'm doing practice problems to check my understanding. theres this one problem that i am totally confused about.
2e. Write the correct name for the formula: FeCO3.
I put Iron(III) carbonite cause i thought the 3 was the charge for the Iron element (Fe), and since that left nothing for CO, i ended with -ite.
but when i look at the solution manual to check, it says Iron(II) carbonate?
From what i read, if it were ending in -ate, wouldn't it be Fe(CO3)2, and if it was a matter of adding the charge (Fe+2, as the solution said), then wouldn't be either FeCO[2+ canceling 3-]
or FeCO5 [2+ added to 3+]
I hope i'm making sense here..........if not then here's a simpler question
why/how is FeCO3 become Iron (II) carbonate???
2e. Write the correct name for the formula: FeCO3.
I put Iron(III) carbonite cause i thought the 3 was the charge for the Iron element (Fe), and since that left nothing for CO, i ended with -ite.
but when i look at the solution manual to check, it says Iron(II) carbonate?
From what i read, if it were ending in -ate, wouldn't it be Fe(CO3)2, and if it was a matter of adding the charge (Fe+2, as the solution said), then wouldn't be either FeCO[2+ canceling 3-]
or FeCO5 [2+ added to 3+]
I hope i'm making sense here..........if not then here's a simpler question
why/how is FeCO3 become Iron (II) carbonate???
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We refer to CO3 as a radical. And it has an effective charge of -2. So the -2 for the carbonate ion cancels out the +2 from the ferrous ion (Fe 2+).
If it was ferric ion (Fe 3+) and CO3 2- it would have been Fe2(CO3)3
Hope this helps.
Goodluck!
If it was ferric ion (Fe 3+) and CO3 2- it would have been Fe2(CO3)3
Hope this helps.
Goodluck!
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Carbonate (CO3) has a charge of 2- (negative ions tend to end in -ATE)
So for a neutral molecule, Iron must have a charge of 2+!
So for a neutral molecule, Iron must have a charge of 2+!