1. Why do transition elements show variable oxidation states? 2. Name the element showing the maximum number of oxidation states among the first series of transition metals from Sc (Z = 21) to Zn (Z = 30). 3. Name the element which shows only +3 oxidation state.

The first transition series element having the most oxidation states

• Manganese, i.e. Mn (Z = 25), has an electronic configuration [Ar]3d⁵4s².
• In the d-subshell, it has the most unpaired electrons.
• A total of 5 + 2 = 7 electrons are available for bond creation because both the d and s orbitals are employed to create bonds.
• Therefore, among the first series of transition metals, Mn has the greatest oxidation state of +7.

Element that only exhibits the +3 oxidation state

• In these series, scandium (Sc) has a +3 oxidation state.
• The electronic configuration of Scandium (Sc) is [Ar]3d¹4s².
• There are a total of 1 + 2 = 3 electrons available for bond creation because the d and s orbitals are both employed to create bonds.
• As a result, (Sc) displays a +3 oxidation state.

Summary:-

1. Because their valence electrons are in two separate sets of orbitals, namely in (n – 1)d and ns orbitals, the transition elements exhibit various oxidation states.
2. When compared to the other elements in the first series of transition metals, which range from Sc (Z = 21) to Zn (Z = 30), manganese exhibits the most oxidation states.
3. Scandium is an element that only exhibits +3 oxidation.

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