`SF_(4)` has _____shape.

Options

A. T-shape
B. Bent
C. Octahedral
D. see saw

Answer

To determine the shape of SF₄ (sulfur tetrafluoride), 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 fluorine (F) atom has 7 valence electrons, and since there are 4 fluorine atoms, they contribute a total of 28 valence electrons (4 × 7 = 28).

**Total valence electrons = 6 (from S) + 28 (from 4 F) = 34 valence electrons.**

### Step 2: Draw the Lewis Structure
In the Lewis structure of SF₄, sulfur will form single bonds with each of the four fluorine atoms. Each bond uses 2 electrons. Therefore, 4 bonds will use 8 electrons (4 × 2 = 8).

**Remaining electrons = 34 - 8 = 26 electrons.**

After forming the bonds, the remaining electrons will be placed on the sulfur atom as lone pairs. Since sulfur can expand its octet, it can accommodate more than 8 electrons.

### Step 3: Account for Lone Pairs
After forming 4 bonds with fluorine, sulfur will have 2 lone pairs of electrons left.

### Step 4: Determine the Electron Geometry
The electron geometry around sulfur can be determined by counting the total number of regions of electron density (bonding pairs + lone pairs). In SF₄, there are:
- 4 bonding pairs (from the 4 S-F bonds)
- 1 lone pair

This gives a total of 5 regions of electron density.

### Step 5: Identify the Molecular Shape
The electron geometry for 5 regions of electron density is trigonal bipyramidal. However, the presence of the lone pair affects the molecular shape. The lone pair occupies one of the equatorial positions, leading to a distortion of the shape.

The resulting molecular shape is **seesaw**.

### Conclusion
Thus, the shape of SF₄ is **seesaw**.

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