Question
Step by step Explanation of the hybridization of one atom of boron and three atom of fluorine
Answers
GPT-4o mini
Hybridization is a concept in chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals, which can then be used to form chemical bonds. Let's go through the step-by-step explanation of the hybridization of one boron atom and three fluorine atoms, specifically focusing on the molecule boron trifluoride (BF₃).
### Step 1: Determine the Valence Electrons
- **Boron (B)**: Boron is in group 13 of the periodic table and has 3 valence electrons.
- **Fluorine (F)**: Fluorine is in group 17 of the periodic table and has 7 valence electrons. Since there are three fluorine atoms, their total contributes 3 x 7 = 21 valence electrons.
### Step 2: Total Valence Electrons
Now, sum the valence electrons from boron and the three fluorine atoms:
\[
\text{Total Valence Electrons} = 3 \, (\text{from B}) + 3 \times 7 \, (\text{from 3 Fs}) = 3 + 21 = 24\, \text{electrons}
\]
### Step 3: Draw the Lewis Structure
To draw the Lewis structure of BF₃:
1. Start with boron in the center because it is less electronegative than fluorine.
2. Connect each fluorine atom to boron with a single bond. Each bond uses 2 electrons, and since there are 3 bonds, that's 6 electrons used.
3. Place the remaining electrons around the fluorine atoms. Each fluorine needs 6 more electrons to complete its octet (3 bond pairs for each F).
Here's the Lewis structure:
```
F
|
F - B - F
|
F
```
### Step 4: Determine the Steric Number
- The steric number is the number of atoms bonded to the central atom plus the number of lone pairs on the central atom.
- In BF₃, boron is bonded to 3 fluorine atoms and has no lone pairs.
\[
\text{Steric Number} = 3 + 0 = 3
\]
### Step 5: Hybridization
With a steric number of 3, we can predict the hybridization of boron:
- The hybridization corresponding to a steric number of 3 is **sp²**.
- This involves the mixing of one s orbital and two p orbitals from the boron atom, creating three sp² hybrid orbitals.
### Step 6: Geometry of the Molecule
The arrangement of the three sp² hybrid orbitals will yield a trigonal planar geometry. The angles between the bonds will be approximately 120°.
### Summary
In BF₃:
- Boron undergoes **sp² hybridization** to form three equivalent hybrid orbitals.
- These orbitals form sigma bonds with the three fluorine atoms.
- The overall molecular shape is **trigonal planar**, with bond angles of approximately 120°.
This completes the step-by-step explanation of the hybridization of boron in the presence of three fluorine atoms in boron trifluoride (BF₃).
### Step 1: Determine the Valence Electrons
- **Boron (B)**: Boron is in group 13 of the periodic table and has 3 valence electrons.
- **Fluorine (F)**: Fluorine is in group 17 of the periodic table and has 7 valence electrons. Since there are three fluorine atoms, their total contributes 3 x 7 = 21 valence electrons.
### Step 2: Total Valence Electrons
Now, sum the valence electrons from boron and the three fluorine atoms:
\[
\text{Total Valence Electrons} = 3 \, (\text{from B}) + 3 \times 7 \, (\text{from 3 Fs}) = 3 + 21 = 24\, \text{electrons}
\]
### Step 3: Draw the Lewis Structure
To draw the Lewis structure of BF₃:
1. Start with boron in the center because it is less electronegative than fluorine.
2. Connect each fluorine atom to boron with a single bond. Each bond uses 2 electrons, and since there are 3 bonds, that's 6 electrons used.
3. Place the remaining electrons around the fluorine atoms. Each fluorine needs 6 more electrons to complete its octet (3 bond pairs for each F).
Here's the Lewis structure:
```
F
|
F - B - F
|
F
```
### Step 4: Determine the Steric Number
- The steric number is the number of atoms bonded to the central atom plus the number of lone pairs on the central atom.
- In BF₃, boron is bonded to 3 fluorine atoms and has no lone pairs.
\[
\text{Steric Number} = 3 + 0 = 3
\]
### Step 5: Hybridization
With a steric number of 3, we can predict the hybridization of boron:
- The hybridization corresponding to a steric number of 3 is **sp²**.
- This involves the mixing of one s orbital and two p orbitals from the boron atom, creating three sp² hybrid orbitals.
### Step 6: Geometry of the Molecule
The arrangement of the three sp² hybrid orbitals will yield a trigonal planar geometry. The angles between the bonds will be approximately 120°.
### Summary
In BF₃:
- Boron undergoes **sp² hybridization** to form three equivalent hybrid orbitals.
- These orbitals form sigma bonds with the three fluorine atoms.
- The overall molecular shape is **trigonal planar**, with bond angles of approximately 120°.
This completes the step-by-step explanation of the hybridization of boron in the presence of three fluorine atoms in boron trifluoride (BF₃).