The shape of `BF_3` species is

Options

A. Tetrahedral
B. Square planar
C. Trigonal planar
D. Linear

Answer

To determine the shape of the BF₃ (Boron Trifluoride) molecule, we can follow these steps:

### Step 1: Identify the Central Atom
The central atom in BF₃ is Boron (B).

### Step 2: Count the Valence Electrons
Boron has 3 valence electrons, and each Fluorine (F) atom has 7 valence electrons. Since there are three Fluorine atoms, we calculate the total number of valence electrons:
- Boron: 3 electrons
- Fluorine: 3 × 7 = 21 electrons
- Total = 3 + 21 = 24 valence electrons

### Step 3: Draw the Lewis Structure
In the Lewis structure of BF₃, Boron is the central atom and is bonded to three Fluorine atoms. Each bond consists of a pair of electrons. The structure can be represented as:
```
F
|
F - B - F
```
Boron shares one electron with each Fluorine atom, forming three single bonds.

### Step 4: Determine the Steric Number
The steric number is calculated as the sum of the number of bond pairs and lone pairs around the central atom. In BF₃:
- Bond pairs = 3 (one for each B-F bond)
- Lone pairs = 0 (Boron has no lone pairs)

Thus, the steric number = 3 + 0 = 3.

### Step 5: Determine the Hybridization
The hybridization can be determined from the steric number:
- Steric number of 3 corresponds to sp² hybridization.

### Step 6: Determine the Molecular Shape
For a molecule with sp² hybridization and a steric number of 3, the molecular geometry is trigonal planar.

### Conclusion
The shape of the BF₃ species is **trigonal planar**.

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