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It would probably be best to read on and come back to these links if you feel you need to.We are going to look at some examples from vanadium chemistry.
The zinc has gone from the zero oxidation state in the element to 2. Example 2 This is the equation for the reaction between manganate(VII) ions and iron(II) ions under acidic conditions. Looking at it quickly, it is obvious that the iron(II) ions have been oxidised to iron(III) ions.
They have each lost an electron, and their oxidation state has increased from 2 to 3.
Remember that each time an oxidation state changes by one unit, one electron has been transferred.
If one substance's oxidation state in a reaction falls by 2, that means that it has gained 2 electrons.
If you don't know anything about vanadium, it doesn't matter in the slightest.
Vanadium forms a number of different ions - for example, V. Notice that the oxidation state isn't simply counting the charge on the ion (that was true for the first two cases but not for this one).
Using oxidation states In naming compounds You will have come across names like iron(II) sulphate and iron(III) chloride.
The (II) and (III) are the oxidation states of the iron in the two compounds: 2 and 3 respectively.
That tells you that they contain Fe In each of the following examples, we have to decide whether the reaction involves redox, and if so what has been oxidised and what reduced.
Example 1: This is the reaction between magnesium and hydrochloric acid or hydrogen chloride gas: Have the oxidation states of anything changed?