The shape of `SCl_4` is best described as a

Options

A. is best described as a
B. Tetrahedron
C. Square pyramid
D. See–saw

Explanation

To determine the shape of \( \text{SCl}_4 \), we can follow these steps:

### Step 1: Determine the Valence Electrons
Sulfur (S) is in group 16 of the periodic table and has 6 valence electrons. Each chlorine (Cl) atom has 7 valence electrons. Since there are 4 chlorine atoms, the total number of valence electrons contributed by chlorine is \( 4 \times 7 = 28 \) electrons.

Total valence electrons = \( 6 + 28 = 34 \) electrons.

### Step 2: Draw the Lewis Structure
In the Lewis structure of \( \text{SCl}_4 \), sulfur will form 4 single bonds with the 4 chlorine atoms. This uses up 8 electrons (4 bonds × 2 electrons per bond).

Remaining electrons = \( 34 - 8 = 26 \) electrons.

Since sulfur has 6 valence electrons and has used 4 for bonding, it has 2 electrons left, which will be placed as a lone pair on sulfur.

### Step 3: Calculate the Steric Number
The steric number is calculated by adding the number of sigma bonds and the number of lone pairs around the central atom (sulfur in this case).

- Number of sigma bonds = 4 (one for each S-Cl bond)
- Number of lone pairs = 1 (the lone pair on sulfur)

Steric number = \( 4 + 1 = 5 \).

### Step 4: Determine the Hybridization
The hybridization can be determined from the steric number. A steric number of 5 corresponds to \( \text{sp}^3\text{d} \) hybridization.

### Step 5: Determine the Geometry and Shape
With \( \text{sp}^3\text{d} \) hybridization, the geometry is trigonal bipyramidal. However, the presence of one lone pair will affect the shape.

In a trigonal bipyramidal arrangement, the lone pair will occupy one of the equatorial positions to minimize repulsion. This leads to a shape that resembles a "see-saw".

### Conclusion
Thus, the shape of \( \text{SCl}_4 \) is best described as a **see-saw** shape.

---