The orbitals of iron involved in the hybridization in `Fe(CO)_(5)` are

Options

A. `s,p_(x),p_(y),P_(z) and d_(x^(2)-y^(2))`
B. `s,p_(x),p_(y),P_(z^(2)) and d_(x^(2)-y^(2))`
C. `s,px,py,pz and d_(z^(2))`
D. `s,p_(x),p_(z),P_(xy) and d_(x^(2)-y^(2))`

Answer

To determine the orbitals of iron involved in the hybridization in the complex `Fe(CO)_(5)`, we can follow these steps:

### Step 1: Determine the Oxidation State of Iron
- The oxidation state of iron (Fe) in `Fe(CO)_(5)` can be calculated. Since carbonyl (CO) is a neutral ligand, the oxidation state of iron is 0.

### Step 2: Write the Electronic Configuration of Iron
- The outer electronic configuration of iron (atomic number 26) is `3d^6 4s^2`. This means there are 6 electrons in the 3d subshell and 2 electrons in the 4s subshell.

### Step 3: Consider the Nature of the Ligand
- Carbon monoxide (CO) is a strong field ligand. Strong field ligands cause pairing of electrons in the d-orbitals, leading to the formation of low-spin complexes.

### Step 4: Pair the Electrons
- In the presence of CO, the electrons in the 4s and 3d orbitals will pair up. The 4s electrons will be used to fill the vacant d-orbitals. The pairing will result in the following configuration:
- 3d: ↑↓ ↑↓ ↑↓ ↑ ↑ (3d has 6 electrons, all paired)
- 4s: ↑↓ (4s has 2 electrons, both paired)
- 4p: ↑ ↑ ↑ (4p has 3 unoccupied orbitals)

### Step 5: Identify the Orbitals Involved in Hybridization
- After pairing, we have:
- 1 vacant d orbital (from 3d)
- 1 vacant s orbital (from 4s)
- 3 p orbitals (from 4p)

- Thus, the orbitals involved in hybridization are:
- 1 d orbital (3d)
- 1 s orbital (4s)
- 3 p orbitals (4p)

### Step 6: Determine the Hybridization Type
- The hybridization formed from these orbitals is `dsp^3`, as we have 1 d orbital, 1 s orbital, and 3 p orbitals.

### Conclusion
- The orbitals of iron involved in the hybridization in `Fe(CO)_(5)` are 1 d orbital, 1 s orbital, and 3 p orbitals, leading to a hybridization of `dsp^3`.