To answer which metal shows the highest and maximum number of oxidation states, we need to consider the electronic configuration and the chemistry of transition metals.
Transition metals are known for exhibiting multiple oxidation states due to the involvement of their d-electrons in bonding. Let's analyze the given options:
Manganese (Mn):
The electron configuration of manganese is [\text{Ar}] \, 3d^5 \, 4s^2.
Manganese can exhibit oxidation states from -3 to +7. It is capable of forming compounds in oxidation states such as +2, +3, +4, +5, +6, and +7.
The +7 oxidation state is exemplified in potassium permanganate (KMnO_4).
Iron (Fe):
The electron configuration of iron is [\text{Ar}] \, 3d^6 \, 4s^2.
Iron typically shows oxidation states of +2 and +3, but it can also exhibit +1, +4, and +6 in rare cases.
Cobalt (Co):
The electron configuration of cobalt is [\text{Ar}] \, 3d^7 \, 4s^2.
Cobalt commonly exhibits oxidation states of +2 and +3, with +1, +4 also observed in some compounds.
Chromium (Cr):
The electron configuration of chromium is [\text{Ar}] \, 3d^5 \, 4s^1.
Chromium can show oxidation states ranging from +2 to +6, with +3 and +6 being the most stable.
Among the given options, manganese (Mn) shows the highest and maximum number of oxidation states. This property is attributed to its half-filled 3d sublevel, which allows it to lose varying numbers of electrons, ranging from none to all seven (in the d and s orbitals), thereby exhibiting a wide range of oxidation states.
Hence, the correct answer is Mn.
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