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Posted: Wed Feb 20, 2019 10:18 am
Are there any trends to predict whether a compound is acting as a reduction or oxidation agent? Or can all act as either depending on the reaction?
Posted: Wed Feb 20, 2019 12:12 pm
There are several molecules that are fairly constant in their oxidation state, such as Oxygen with -2 or Hydrogen with +1. Most of the metals can go either way.
Posted: Wed Feb 20, 2019 12:19 pm
There are trends for oxidization states. I expect he will tell us them later but some are:
H is usually +1 unless attached to a less electronegative element then it becomes -1
oxidization of a free element is always 0
oxygen is usually -2 unless in peroxide O2 then its -1
Posted: Wed Feb 20, 2019 1:39 pm
I personally would just use the reaction as your way of finding out reducing/oxidizing agents. It can get confusing quite easily if you try to use rules of thumb, especially when the reactions involve d-block metals
Posted: Wed Feb 20, 2019 2:43 pm
You can use the periodic table to figure out regular states of molecules, however for transition metals, use the molecules you know to figure out the reaction value of the metal. For example, in SO4 2-. we know oxygen is 2-, multiply by 4 gives us -8. The overall charge is -2 so Sulfur must be +6.
Posted: Wed Feb 20, 2019 7:39 pm
How would we figure put the oxidation number for the transition metals or the ones in the d-block, such as Mn for example? Will it be given to us on the exam?