The electronic configuration of an element is `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)3d^(5)4s^(1)` .This represents its

Options

A. Excited state
B. Ground state
C. Cationic form
D. None

Explanation

To determine the element represented by the electronic configuration `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)3d^(5)4s^(1)`, we can follow these steps:

### Step 1: Count the Total Number of Electrons
The electronic configuration can be broken down as follows:
- 1s²: 2 electrons
- 2s²: 2 electrons
- 2p⁶: 6 electrons
- 3s²: 2 electrons
- 3p⁶: 6 electrons
- 3d⁵: 5 electrons
- 4s¹: 1 electron

Now, we add these up:
\[ 2 + 2 + 6 + 2 + 6 + 5 + 1 = 24 \text{ electrons} \]

### Step 2: Identify the Element
The total number of electrons corresponds to the atomic number of the element. Since we have 24 electrons, the atomic number is 24.

### Step 3: Determine the Element Name
The element with atomic number 24 is Chromium (Cr).

### Step 4: Confirm the Electronic Configuration
Chromium has an expected electronic configuration of `1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁴ 4s²`. However, due to stability reasons, it actually adopts the configuration `3d⁵ 4s¹` to achieve a half-filled d-subshell, which is more stable.

### Conclusion
Thus, the electronic configuration `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)3d^(5)4s^(1)` represents the element Chromium (Cr).

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