The atomic numbers of `Ni` and `Cu` are `28` and `29` respectively. The electronic configuration `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)3d^(10)` represent

Options

A. `Cu^(+)`
B. `Cu^(2+)`
C. `Ni^(2+)`
D. Ni

Explanation

To solve the question regarding the electronic configuration `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)3d^(10)`, we need to identify which element or ion it represents. We know that the atomic numbers for Nickel (Ni) and Copper (Cu) are 28 and 29, respectively.

### Step-by-Step Solution:

1. **Identify the Atomic Number**:
- The electronic configuration given is `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)3d^(10)`.
- Count the total number of electrons in the configuration:
- `1s^2` = 2
- `2s^2` = 2
- `2p^6` = 6
- `3s^2` = 2
- `3p^6` = 6
- `3d^10` = 10
- Total = 2 + 2 + 6 + 2 + 6 + 10 = 28 electrons.

2. **Determine the Element**:
- Since the atomic number is 28, this corresponds to Nickel (Ni).

3. **Consider the Ion**:
- The question asks for the representation of the electronic configuration. The configuration `3d^(10)` suggests that it could be for a neutral atom or an ion.
- Copper (Cu) has an atomic number of 29 and its neutral configuration is `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)3d^(10)4s^(1)`.
- The ion `Cu^+` would lose one electron from the `4s` orbital, resulting in the configuration `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)3d^(10)`, which matches the given configuration.

4. **Conclusion**:
- The electronic configuration `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)3d^(10)` represents the ion `Cu^+` (Copper ion).

### Final Answer:
The electronic configuration `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)3d^(10)` represents the ion **Cu^+** (Copper ion).