## Oxidation states

Gwynneth Orlino 1B
Posts: 26
Joined: Wed Nov 21, 2018 12:18 am

### Oxidation states

How do you find the oxidation state of an element?

Yilun Ding
Posts: 31
Joined: Tue Jun 25, 2019 12:15 am

### Re: Oxidation states

By reference to the periodic table, the Group 1 metals are more likely to lose an electron to become octet, then it has +1 oxidation state. However, because of relatively high ionization energy, the Group 7 non-metals will not lose electrons, instead, they usually gain an electron to become octet. Therefore, they usually have -1 oxidation state. These trends, however, will not be applied to transition metals since they usually have more than one oxidation states.

205458163
Posts: 33
Joined: Wed Jun 26, 2019 12:15 am

### Re: Oxidation states

You can calculate the oxidation state of a certain atom by using the sum of all positive and negative equal to 0.

Karina Vasquez 1D
Posts: 35
Joined: Fri Mar 01, 2019 12:15 am

### Re: Oxidation states

205458163 wrote:You can calculate the oxidation state of a certain atom by using the sum of all positive and negative equal to 0.

What do you mean by using the "sum of all positive and negative equal to 0"?

Chris Charton 1B
Posts: 69
Joined: Mon Jun 17, 2019 7:23 am

### Re: Oxidation states

I think they might be referring to finding the oxidation state of a metal in a coordination compound.

hannabarlow1A
Posts: 37
Joined: Mon Jun 17, 2019 7:23 am

### Re: Oxidation states

For coordination compounds, based on the charge of the overall compound, you can figure out the oxidation state of the central ion based on the known charges of the ligands and ions. For example, [Pt (NH3)5 Cl] Br3 has no net charge, so you know that the sum of all the charges must be 0. NH3 has no charge, Cl has a -1 charge, and Bromine has a -3 charge (-1 charge for each bromine atom). Therefore, the oxidation state of Platinum must be 4 because: 4 -1-3=0