Statement I: `Cu^(+)` is repelled by magnetic field.
Statement II: All electrons are paired up in `Cu^(+)` ion. 

Options

A. If both Statement I and Statement II are true and Statement II is the correct explanation of Statement I.
B. If both Statement I and Statement II are true but Statement II is not the correct explanation for Statement I.
C. If Statement I is true but Statement II is false.
D. If Statement I is false but Statement II is true.

Answer

To analyze the statements regarding the `Cu^(+)` ion, we can break down the problem into clear steps:

### Step 1: Determine the Electron Configuration of `Cu^(+)`
Copper (Cu) has an atomic number of 29. The electron configuration of neutral copper is:
- 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s¹

When copper loses one electron to form the `Cu^(+)` ion, it loses the 4s electron. Therefore, the electron configuration for `Cu^(+)` is:
- 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰

### Step 2: Analyze the Electron Pairing in `Cu^(+)`
In the `Cu^(+)` ion, the 3d subshell contains 10 electrons. Since each orbital can hold a maximum of 2 electrons and all 10 electrons in the 3d subshell are paired (2 electrons in each of the 5 d orbitals), we conclude that all electrons in `Cu^(+)` are indeed paired.

### Step 3: Determine the Magnetic Properties of `Cu^(+)`
Diamagnetic substances are characterized by having all their electrons paired. Since `Cu^(+)` has all its electrons paired, it is classified as diamagnetic. Diamagnetic materials are repelled by a magnetic field.

### Step 4: Evaluate the Statements
- **Statement I**: `Cu^(+)` is repelled by a magnetic field. (True, because it is diamagnetic)
- **Statement II**: All electrons are paired up in `Cu^(+)`. (True, as established from the electron configuration)

### Conclusion
Both statements are true, and thus the correct answer is that both statements are correct.

### Final Answer
Both Statement I and Statement II are true.

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