Did I ionize Mn2(CO3)3 correctly?
Mn2(CO3)3 --> 2Mn^(3+) + 3CO3^(2-)
yes
Yes, you correctly ionized Mn2(CO3)3. The equation you provided correctly shows the ionization of Mn2(CO3)3 into 2Mn^(3+) ions and 3CO3^(2-) ions.
To determine if you ionized Mn2(CO3)3 correctly, we need to check if the charges on each ion are balanced.
For Mn2(CO3)3, we have:
Mn2+ (cation) and CO3^2- (anion)
To ionize Mn2(CO3)3, we will break it up into its individual ions:
2Mn^3+ (cation) and 3CO3^2- (anion)
To verify if you ionized it correctly, we need to ensure that the charges balance out. In this case, we have 2 Mn^3+ cations, with a charge of +3 each, giving us a total of +6. And we also have 3 CO3^2- anions, with a charge of -2 each, giving us a total of -6.
Since the overall charge on the cations and anions both add up to zero, it appears that you correctly ionized Mn2(CO3)3 into 2Mn^3+ and 3CO3^2-.