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Title: How do you deduce the oxidation state of these few elements in a chemical equation? Post by: tlk_85 on Sep 18, 2012 2FeSO4 (aq) + Cl2 (g) + H2SO4 (aq) ---> Fe2(SO4)3 + 2HCl
How do you calculate the oxidation state of Fe,Cl,Fe and Cl? Each element from the sequence of ionic compounds.Thanks! Title: How do you deduce the oxidation state of these few elements in a chemical equation? Post by: tlaw92 on Sep 18, 2012 You work on the assumption that H is always +1 in a compound and oxygen is -2 in a compound. Metals will have an oxidation state equal to to the "ionic" charge it would have if it were in solution as an ion. The oxidation number of polyatomic ions are well known. (i.e. sulfate is -2) Lastly, the oxidation number of any element in the elemental state is zero.
The sum of the oxidation numbers of all of the elements in a comopund is zero. The sum of the oxidation numbers of all the elements in a polyatomic ion is equal to the charge on the ion. With all of that in mind we can easily assign oxidation numbers. +2 +6 -2 ...........0...........+1+6-2 ............. +3..+6-2 ....... +1-1 2FeSO4 (aq) + Cl2 (g) + H2SO4 (aq) ---> Fe2(SO4)3 + 2HCl Title: How do you deduce the oxidation state of these few elements in a chemical equation? Post by: tkwilke on Sep 18, 2012 2FeSO4 (aq) + Cl2 (g) + H2SO4 (aq) ---> Fe2(SO4)3 + 2HCl
Oxidation states Fe +2 SO4 -2 Cl 0 H+1 SO4 -2 Fe 3+ SO4 -2 H +1 Cl -1 Cl normally -1 in compounds , element 0 by definition Fe is +2 or +3 ... compare with sulphates [-2 overall] |