The hybridization of Sin `SF_(4)` is

Options

A. `sp^(3)d^(2)`
B. `sp^(3)d`
C. `sp^(3)d^(3)`
D. `sp^(3)`

Answer

To determine the hybridization of sulfur (S) in sulfur tetrafluoride (SF₄), we can follow these steps:

### Step 1: Determine the Valence Electrons
- Sulfur (S) has 6 valence electrons.
- Each fluorine (F) atom has 7 valence electrons, and there are 4 fluorine atoms.
- Total valence electrons = 6 (from S) + 4 × 7 (from F) = 6 + 28 = 34 valence electrons.

**Hint:** Remember to add the valence electrons from all atoms in the molecule.

### Step 2: Count the Electrons Used in Bonding
- In SF₄, sulfur forms 4 bonds with 4 fluorine atoms.
- Each bond uses 2 electrons, so 4 bonds use 4 × 2 = 8 electrons.

**Hint:** Each bond consists of a pair of electrons shared between the two atoms.

### Step 3: Calculate Remaining Electrons
- Remaining electrons = Total valence electrons - Electrons used in bonding = 34 - 8 = 26 electrons.

**Hint:** This step helps to understand how many electrons are left after forming bonds.

### Step 4: Distribute Remaining Electrons
- Place the remaining 26 electrons around the fluorine atoms first to complete their octets.
- Each fluorine needs 6 more electrons (since they already share 2 with sulfur), totaling 24 electrons for 4 fluorine atoms.
- After placing 24 electrons, 2 electrons remain, which will be placed as a lone pair on the central sulfur atom.

**Hint:** Always complete the octets of surrounding atoms before placing electrons on the central atom.

### Step 5: Analyze the Central Atom
- The sulfur atom now has 4 bond pairs (from the 4 S-F bonds) and 1 lone pair of electrons.
- This arrangement corresponds to a trigonal bipyramidal geometry.

**Hint:** The geometry can help you visualize how the hybridization occurs.

### Step 6: Determine the Hybridization
- Sulfur's electronic configuration is [Ne] 3s² 3p⁴.
- In the excited state, one of the 3s electrons can be promoted to the 3d orbital.
- This results in 1 electron in the 3d orbital, 3 electrons in the 3p orbital, and 2 electrons remain in the 3s orbital.
- The hybridization is thus sp³d, as there are 5 regions of electron density (4 bond pairs + 1 lone pair).

**Hint:** The hybridization type can be determined by counting the total number of bonding and lone pairs around the central atom.

### Conclusion
The hybridization of sulfur in SF₄ is **sp³d**.

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