If the orbital angular momentum of iron chloride is `5sqrt6h` then the correct options for this given fact are:

Options

A. `FeCl_(3)`
B. `FeCl_(2)`
C. `Fe_(2)Cl_(6)`
D. None of these

Explanation

To solve the problem regarding the orbital angular momentum of iron chloride (FeCl3) and determine the correct options based on the given information, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Atomic Number of Iron:**
- The atomic number (Z) of iron (Fe) is 26.

2. **Write the Electronic Configuration of Iron:**
- The electronic configuration of iron can be written as:
\[ \text{Fe: } 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^2, 3d^6 \]

3. **Determine the Value of L for the d-Orbital:**
- For d-orbitals, the angular momentum quantum number (L) is equal to 2.

4. **Calculate the Orbital Angular Momentum:**
- The formula for calculating the orbital angular momentum (L) is:
\[ L = \sqrt{L(L + 1)} \cdot \frac{h}{2\pi} \]
- Substituting L = 2 into the formula:
\[ L = \sqrt{2(2 + 1)} \cdot \frac{h}{2\pi} = \sqrt{6} \cdot \frac{h}{2\pi} \]

5. **Relate the Given Orbital Angular Momentum to the Calculated Value:**
- The problem states that the orbital angular momentum of iron chloride is \(5\sqrt{6}h\).
- This can be expressed in terms of the calculated angular momentum:
\[ n \cdot \sqrt{6}h = 5\sqrt{6}h \]
- From this, we can deduce that \(n = 5\).

6. **Determine the Number of Unpaired Electrons:**
- The value of \(n\) corresponds to the number of unpaired electrons in the d-orbitals.
- For Fe in the +3 oxidation state (Fe³⁺), the electronic configuration is:
\[ \text{Fe}^{3+}: [Ar] 4s^2 3d^5 \]
- In this configuration, there are 5 unpaired electrons in the 3d subshell.

7. **Conclusion:**
- Therefore, the correct option based on the information provided is that FeCl3 contains Fe³⁺, which has 5 unpaired electrons.