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SnCl3? The anion SnCl3- exists and in it Sn has an oxidation number of +2
The oxidation number of Sn in SnCl2 is +2. This is because Cl is more electronegative than Sn, so each Cl atom has an oxidation number of -1, leaving Sn with an oxidation number of +2 to balance the charges.
-1 for each Cl, +2 for Sn
The oxidation number for Sn (tin) can vary depending on the compound it is in. In the most common compounds, like SnCl2, Sn is typically in the +2 oxidation state. In other compounds, such as SnCl4, Sn can have an oxidation state of +4.
0 in the elemental form. +2 and +4 in its compounds
To convert SnCl2·2H2O (tin(II) chloride dihydrate) to SnCl3 (tin(III) chloride), you first need to oxidize the tin from the +2 oxidation state to the +3 oxidation state. This can be achieved by reacting SnCl2 with an appropriate oxidizing agent, such as chlorine gas (Cl2) or hydrogen peroxide (H2O2). After the oxidation, the SnCl3 can be formed by ensuring the proper stoichiometry of chlorine to tin, while removing any water from the initial dihydrate form.
O.S. of Sn = +2 O.S. of O = -2 O.N. of cpd = 0
The oxidation number of Sn changes from +4 in SnCl4 to +2 in SnCl2, resulting in a decrease of 2.
The oxidation number for Sn in SnO4^2- is +4. Oxygen is typically assigned an oxidation number of -2, so the sum of the oxidation numbers in the compound equals the overall charge of -2 for the ion.
The oxidation number of tin can vary depending on the compound it is in. In its elemental form (Sn), tin has an oxidation number of 0. In some compounds, tin can exhibit oxidation numbers of +2 and +4.
+1 for H -2 for each O +5 for Sn
The oxidation number for sulfur (S) in tin(IV) sulfate (Sn(SO4)2) is +6. This is because the overall charge of the sulfate ion (SO4) is -2, and there are two sulfate ions present in the compound, leading to a total charge of -4. The oxidation number of tin (Sn) in this compound is +4.