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How to determine the charge on the transition elements

Submitted by harley08 on Sat, 10/11/2008 - 20:23

I am having a time understanding how to determine the charge on the transitional elements. I think I have the representative elements down pat, but not the trans. 

Many of the transition elements have more than one common charge or oxidation state.

It comes with time but here are a few of the more common ones you should memorize.

Cu and Hg 1+ and 2+
Cr, Fe, Co 2+ and 3+
Sn and Pb 2+ and 4+

Ag always 1+
Zn, Cd always 2+


Okay, I think I am understanding. Do you mind to see if I got the following correct.
The question was  toename the following Binary ionic compounds, using aroman numeral to indicate the charge on the metal.

Formula's        My answers
FeBr2 =    I got Iron II Bromide
FeBr3 =            Iron III Bromide
AuCl3 =          Gold III Chloride
AuCl  =          Gold I Chloride
FeS  =            Iron II Sulfide
FeS2 =            Iron III Sulfide
CrF2 =          Chromium II Fluoride?
CrF3 =            Chromium III Fluroide?
NiP  =              Nickel II Phosphide
NiP2 =            Nickel III Phosphide

Am I close to being on the right track?
Thank you.

FeS2 =            Iron III Sulfide
NiP  =              Nickel II Phosphide
NiP2 =            Nickel III Phosphide

Double check these (group 15 anions are 3- and group 16 anions are 2-).


Okay I've tried this again, so if you don't mind to check me again. If I've gotten anny wrong do you mind to give me a little direction as to where I am going wrong?
Ni3P2 would be Nckel (III) Phosphide
NiP2 Nickel (II) Phosphide
FeS2 Iron (I) Sulfide :-\

Oxidation state of sulfur is 2-, since you have 2 the total negative charge is 4-
Therefore iron must be 4+ so the compound has a net charge of zero. Iron (IV) sulfide

Phosphide is a group 15 so has an oxidation state of 3-, therefore nickle must have a 3+ so the compound has a net charge of zero. Ni(III) phosphide

So? What is the name of NiP2 ...