I am trying to determine if it is reduction or oxidation.
In the initial molecule I calculate the overall oxidation numbers as:
ox(Cl)*6 + ox(H)*6 + ox(C)*6 = 0 -6 + 6 +ox(c)*6 = 0 hence, ox(c) = 0
In the subsequent molecule, I calculated the oxidation numbers as:
ox(Cl)*4 + ox(H)*6 + ox(C)*6 = 0 -4 + 6 +ox(c)*6 = 0 hence, ox(c) = 6/2 = 1/3
However, my textbook says the oxidation number of ALL carbon in the second molecule is 2. I am very confused by this, since if all the carbons have an oxidation number of 2 then the molecule would be charged overall? Then I am unsure if my oxidation numbers can be fractional. Is my textbook wrong, and I wrong or are we both wrong?
Overall, what I am really trying to get at is if the molecule is being oxidized or reduced, and how many electrons are being transferred. Is there a better way of doing this?
Thank you kindly