Mar 12, 2018 · Well, as usual, the oxidation number of H is +I as is typical.... And the sum of the individual oxidation numbers is equal to the charge on the ion... And so N_"oxidation number"+4xxI^+=+1 N_"oxidation number"=-III For a few more examples .... see this older answer. ii. In a compound MX , find out the oxidation number of M and X. 3 iii. Why the oxidation number of oxygen in OF is +2 2 iv. In HS, SO and HSO the sulphur atom has different oxidation number. 2 2 2 4 Find out the oxidation number of sulphur in each compound. v. An element X has oxidation state 0. What will be its oxidation state when it gains ...
Firstly, the overall (addition of all) oxidation state of a neutral compound must be zero. In [Pt(NH3)3Cl]Cl, the central metal atom is the Platinum(Pt). Elements like H, F, Cl, O, N have its usual oxidation state as +1,-1,-1,-2,-3 respectively. If we plug these oxidation states into the compound, [x+3*(-3+3)-1]+(-1) will be the case. Oxygen has an oxidation number of -2 in most compounds and ions. Peroxides (O2-1) are the exception and if oxygen is bonded to fluorine, the oxygen’s charge is a +2. 4. The sum of the oxidation numbers of all the atoms in a particle must equal the charge of that ion.
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