The electronic configuration of Cu(II) is `3d^9 `whereas that of Cu(I) is `3d^(10)` Which of the following is correct?

Options

A. Cu(II) is more stable
B. Cu(II) is less stable
C. Cu(I) and Cu(II) are equally stable
D. Stability of Cu(I) and Cu(II) depends on nature of copper salts

Explanation

To determine the correct statement regarding the stability of Cu(I) and Cu(II) based on their electronic configurations, let's analyze the information step by step.

### Step 1: Identify the Electronic Configurations
- The electronic configuration of Cu(I) is \(3d^{10}\).
- The electronic configuration of Cu(II) is \(3d^{9}\).

### Step 2: Understand Stability of Electronic Configurations
- Generally, fully filled (\(3d^{10}\)) and half-filled (\(3d^{5}\)) orbitals are more stable compared to partially filled orbitals.
- Therefore, \(3d^{10}\) (Cu(I)) is a fully filled configuration, while \(3d^{9}\) (Cu(II)) is a partially filled configuration.

### Step 3: Compare the Stability of Cu(I) and Cu(II)
- Since Cu(I) has a fully filled \(3d^{10}\) configuration, it is expected to be more stable than Cu(II) which has a \(3d^{9}\) configuration.
- However, Cu(II) has a +2 oxidation state, which can lead to increased stability due to factors such as effective nuclear charge and smaller ionic radius.

### Step 4: Consider Hydration Energy
- Cu(II) can form stronger bonds due to higher hydration energy when it is in solution, which can contribute to its stability in certain contexts.
- The effective nuclear charge is greater in Cu(II), which can lead to stronger interactions with surrounding ligands.

### Step 5: Conclusion
- Although Cu(I) is more stable due to its fully filled configuration, Cu(II) can be more stable in certain conditions due to its ability to form stronger bonds and higher hydration energy.
- Therefore, the correct statement is that the stability of Cu(I) and Cu(II) depends on the nature of the copper salts and the environment in which they are present.

### Final Answer
The correct option is: **Option 4: The stability of Cu(I) and Cu(II) depends on the nature of copper salts.**