Which of the following configurations represents the `s-block` element?

Options

A. `[Ar]3d^(10)4s^(1)`
B. `[Ne]3s^(2)3p^(1)`
C. `[He]2s^(2)2p^(6)3s^(1)`
D. None of these

Explanation

To determine which of the given electronic configurations represents an s-block element, we need to understand the characteristics of s-block elements in the periodic table. S-block elements are those whose outermost electrons are in the s subshell. The last electron added to the atom will be in the s subshell.

### Step-by-Step Solution:

1. **Identify the Electronic Configurations**:
We need to look at the electronic configurations provided in the options. For this solution, let's assume the options are:
- A) Argon 3d10 4s1
- B) Neon 3s2 3p1
- C) Helium 2s2
- D) Argon 3d10 4p1

2. **Analyze Each Configuration**:
- **Option A: Argon 3d10 4s1**
- The last electron is in the 4s subshell, but since there are filled d orbitals (3d10), this configuration corresponds to a d-block element (Copper).

- **Option B: Neon 3s2 3p1**
- The last electron is in the 3p subshell. This configuration corresponds to a p-block element (Aluminum).

- **Option C: Helium 2s2**
- The last electron is in the 2s subshell. This configuration corresponds to an s-block element (Beryllium).

- **Option D: Argon 3d10 4p1**
- The last electron is in the 4p subshell. This configuration corresponds to a p-block element (Gallium).

3. **Conclusion**:
From the analysis, we find that the only configuration that represents an s-block element is **Option C: Helium 2s2**.

### Final Answer:
**Option C represents the s-block element.**