Final answer:
The question involves determining the oxidation states of transition metals in various compounds by applying set rules for calculating oxidation numbers, ensuring that the sum of oxidation states in a neutral compound is zero.
Step-by-step explanation:
The question asks to determine the oxidation states of transition metals in given compounds. The key concepts involved here include understanding the rules for calculating oxidation numbers and applying them to complex compounds.
Example Calculations
For Cu in CuCl, we see that chlorine typically has an oxidation state of -1. Since the compound is neutral overall, copper must have an oxidation state of +1 to balance out the two chloride anions, resulting in CuCl2.
Similarly, for Fe in FeSO4, sulfate (SO4) has a fixed oxidation state of -2. In order to achieve neutrality, iron must have an oxidation state of +2, aligning with Fe2+ in FeSO4.
Application of these principles can help understand other redox reactions and the changes in oxidation states of elements during such reactions.