The electronic configuration of given speices `(X)` is `1s^(2), 2s^(2)2p^(6), 3s^(2)3p^(6)3d^(5), 4s^(1)`. This can be its

Options

A. Cationic form `X^(o+)`
B. Anionic form `X^(ɵ)`
C. Excited state
D. Ground state

Explanation

To determine the species \( X \) based on the given electronic configuration, we will follow these steps:

### Step 1: Count the Total Number of Electrons
The electronic configuration provided is:
\[ 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^5, 4s^1 \]

Let's count the total number of electrons:
- \( 1s^2 \) contributes 2 electrons
- \( 2s^2 \) contributes 2 electrons
- \( 2p^6 \) contributes 6 electrons
- \( 3s^2 \) contributes 2 electrons
- \( 3p^6 \) contributes 6 electrons
- \( 3d^5 \) contributes 5 electrons
- \( 4s^1 \) contributes 1 electron

Adding these together:
\[ 2 + 2 + 6 + 2 + 6 + 5 + 1 = 24 \]

### Step 2: Identify the Atomic Number
The total number of electrons corresponds to the atomic number \( Z \) of the element. Since we have 24 electrons, the atomic number \( Z = 24 \).

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

### Step 4: Analyze the Electronic Configuration
The electronic configuration \( 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^5, 4s^1 \) is indeed the ground state configuration for Chromium. This configuration shows that it has 5 electrons in the 3d subshell and 1 electron in the 4s subshell, which is characteristic of Chromium.

### Step 5: Conclusion
Since the configuration matches that of Chromium and is in its ground state, we conclude that the species \( X \) is Chromium.

### Final Answer
The species \( X \) is Chromium (Cr).

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