Oxidation States

[Lusin_Yengibaryan_3B]

How do we find the oxidation state of the metal species in a given complex?

[Emma Healy 2J]

For finding oxidation states, I would look at the charges that you know and use algebra to find the oxidation state of the metal.

[Emma Healy 2J]

For example, if you had [Fe(CN)6]^4-, you know that the overall charge is -4. CN has an oxidation state of -1 and -1x6=-6. Using algebra, x+(-6)=-4, x=2. So Fe would have to have an oxidation state of +2.

[Arnav Saud 2C]

Generally, try to find all the negative charged molecules/atoms. Then find all the positive charged molecules/atoms. Add up all the negative and positive charges together. The leftover negative charge should then be turned positive and that should be the charge.
A simple example is Titanium(4) Dioxide. It has 2 oxygens which give an overall -4 charge. In order to make the charge 0, Titanium has to be +4.

[Francesca_Borchardt_2D]

I have trouble with this as well. All of the tips really helped. Thank you guys!

[Neha Jonnalagadda 2D]

The oxidation state of a metal can be found by looking at the molecular formula and the charges on the non metal. Using those charges that you know, you can find what the metal's positive charge is.

[Nicole Ton 3C]

To find the oxidation state of a transition metal, I would first look at the overall charge of the coordination compound since the charges/oxidation states of all the compound's components need to add up to this number. Then, I would start looking at the charges I know for sure, such as that CN is -1 charge and NH3 is neutral, and use these to then see what oxidation state the transition metal has to be for the sum of the charges to equal the overall charge of the coordination compound.