Define a transition metal and write the electronic configurations for Mn2+ and Fe2+ ions, explaining why Fe2+ is readily oxidized to Fe3+ but Mn2+ is not readily oxidized to Mn3+.

• Fe$^{2+}$ has an electronic configuration of $[Ar] 3d^6$.
• Fe$^{3+}$ has an electronic configuration of $[Ar] 3d^5$.
• Mn$^{2+}$ has an electronic configuration of $[Ar] 3d^5$.
• Mn$^{3+}$ has an electronic configuration of $[Ar] 3d^4$.

• The $3d^5$ configuration represents a half-filled d subshell, which is particularly stable due to exchange energy and symmetry.

• Fe$^{2+}$ ($3d^6$) readily loses an electron to form Fe$^{3+}$ ($3d^5$). This conversion is favorable because it results in the highly stable half-filled $3d^5$ configuration.

• Mn$^{2+}$ already possesses the highly stable half-filled $3d^5$ configuration. Oxidizing Mn$^{2+}$ to Mn$^{3+}$ would mean losing an electron from this stable $3d^5$ configuration to form a less stable $3d^4$ configuration. This process requires a significant amount of energy and is therefore not readily favorable.

3 (c) Give the transition metal or transition metal compound used as catalyst in the following conversions.
The conversions are not visible in the provided image. Please provide the conversions for this part.