Final answer:
When Tin (II) chloride is mixed with Manganese metal, a redox reaction could potentially form Manganese(II) Chloride and tin metal. However, without specific reaction conditions, it's not certain which compounds will form, but SnCl2 and MnCl2 are possibilities.
Step-by-step explanation:
When Tin (II) chloride, which is an ionic solid, is mixed with Manganese metal, a redox reaction can occur if the conditions permit. Since Tin (II) chloride is SnCl2, it contains Sn2+ ions. Manganese (Mn) has a higher reduction potential than Tin (II), which means that in a suitable reaction, Manganese could potentially be oxidized to Mn2+, forming Manganese(II) Chloride, or MnCl2, and reducing Tin (II) to tin metal, Sn.
The corresponding chemical equation would be: Mn(s) + SnCl2(s) → MnCl2(s) + Sn(s). However, other reaction conditions must be met for this chemical reaction to occur. For instance, a solvent or specific temperature could be required to initiate the process. Without additional information on the reaction conditions, it is not possible to accurately predict all compounds that may form.
Given the provided information, possible compounds that could exist afterwards include Manganese(II) Chloride and tin metal, as well as unreacted Tin (II) Chloride. However, unless the reaction is complete, unreacted SnCl2 may still be present.