Which metal in the first series of transition metals exhibits +1 oxidation state most frequently and why?
Copper (Cu) exhibits +1 oxidation state most frequently in the first series of transition metals. From Table 4.3, Cu shows +1 as one of its common oxidation states, which is unique among the first row transition elements.
The reason is that Cu has the electronic configuration [Ar] 3d¹⁰ 4s¹. When it loses one electron from the 4s orbital to form Cu⁺, it achieves a stable d¹⁰ configuration. This completely filled d-subshell provides extra stability to the +1 oxidation state, making it the most frequently exhibited oxidation state for copper among the first transition series metals.
Explanation
The question specifically asks about +1 oxidation state in the first transition series. From Table 4.3 in the context, Cu is the only element that shows +1 as a common oxidation state. The stability of Cu⁺ comes from its d¹⁰ configuration - a completely filled d-subshell is energetically stable. The context mentions that at the end of the series (where Cu and Zn are located), elements have more d electrons and fewer orbitals available for sharing, which explains why Cu shows fewer oxidation states and why +1 is stable for it.
Solution Steps
Step 1: Identify from Table 4.3 that Cu shows +1 oxidation state, which is unique among first row transition elements.
Step 2: Explain that Cu achieves stable d¹⁰ configuration in +1 oxidation state, making it the most frequently exhibited state.