The electronic configuration:
`1s^(2),2s^(2)2p^(6),3s^(2)3p^(6),3d^(10),4s^(2)4p^(6)4d^(10),5s^(2)` is for:

Options

A. f-block element
B. d-block element
C. p-block element
D. s-block element

Explanation

To determine the element corresponding to the given electronic configuration \(1s^{2}, 2s^{2}, 2p^{6}, 3s^{2}, 3p^{6}, 3d^{10}, 4s^{2}, 4p^{6}, 4d^{10}, 5s^{2}\), we will analyze the configuration step by step.

### Step 1: Count the total number of electrons
The given electronic configuration can be broken down as follows:
- \(1s^{2}\) contributes 2 electrons
- \(2s^{2}\) contributes 2 electrons
- \(2p^{6}\) contributes 6 electrons
- \(3s^{2}\) contributes 2 electrons
- \(3p^{6}\) contributes 6 electrons
- \(3d^{10}\) contributes 10 electrons
- \(4s^{2}\) contributes 2 electrons
- \(4p^{6}\) contributes 6 electrons
- \(4d^{10}\) contributes 10 electrons
- \(5s^{2}\) contributes 2 electrons

Adding these together:
\[ 2 + 2 + 6 + 2 + 6 + 10 + 2 + 6 + 10 + 2 = 58 \text{ electrons} \]

### Step 2: Identify the element
The total number of electrons corresponds to the atomic number of the element. An atomic number of 58 indicates that the element is Cerium (Ce), which is located in the f-block of the periodic table.

### Step 3: Determine the block of the element
The last electron in the given configuration enters the \(5s\) orbital. However, since the configuration includes \(4d^{10}\) and \(3d^{10}\), it suggests that the element is primarily a d-block element, as the last electron enters a d-orbital.

### Conclusion
The electronic configuration \(1s^{2}, 2s^{2}, 2p^{6}, 3s^{2}, 3p^{6}, 3d^{10}, 4s^{2}, 4p^{6}, 4d^{10}, 5s^{2}\) corresponds to the element Cerium (Ce), which is a d-block element.

### Final Answer
The electronic configuration is for Cerium (Ce).

---