-1 for each Cl, +2 for Sn
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The oxidation number of Sn in SnF2 is +2. This is because fluorine has an oxidation number of -1, and there are two fluorine atoms in SnF2, making the overall charge -2. In order to balance the charge, the oxidation number of Sn must be +2.
In this compound there is a tin ion attached to four chloride ions. Chloride ions have -1 charge. Therefore the oxidation number of tin is +4.
SnF2 is called stannous fluoride because it is the fluoride salt of stannous ion (Sn^2+). In this compound, the metal tin is in its +2 oxidation state, represented by the prefix "stannous."
The balanced chemical equation shows a 1:1 ratio between Sn and SnF2. Since Sn is limiting in this reaction, the maximum amount of SnF2 that can be produced will be equal to the amount of Sn used, which is 0.480 moles. Therefore, 0.480 moles of SnF2 can be produced.
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.
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.
The oxidation number of Sn can vary, but it is typically +2 or +4 in compounds.