The Lewis structure of BF3 contains three single bonds, with boron in the center, and three fluorines on either side. There are three lone pairs on each fluorine atom, and the boron atom does not have any lone pair.
Steps
By using the following steps, you can easily draw the Lewis structure of BF3:
#1 Draw skeleton
#2 Show chemical bond
#3 Mark lone pairs
#4 Calculate formal charge and check stability (if octet is already completed on central atom)
Let’s one by one discuss each step in detail.
#1 Draw skeleton
In this step, first calculate the total number of valence electrons. And then, decide the central atom.
- Let’s calculate the total number of valence electrons
We know that… boron is a group 13 element and fluorine is a group 17 element. Hence, boron has three valence electrons and fluorine has seven valence electrons.
Now BF3 has one boron atom and three fluorine atoms.
So the total number of valence electrons = valence electrons of boron atom + (valence electrons of fluorine atom × 3)
Therefore, the total number of valence electrons = 3 + 21 = 24
- Now decide the central atom
The atom with the least electronegative value is placed at the center. By looking at the periodic table, we get the electronegativity values for boron and fluorine as follows:
Electronegativity value of boron = 2.04
Electronegativity value of fluorine = 3.98
Obviously, boron is less electronegative than fluorine. Hence, assume that boron is the central atom.
So now, put boron in the center and fluorines on either side. And draw the rough skeleton structure for the Lewis structure of BF3 something like this:
Also read: How to draw Lewis structure of SO3 (6 steps)
#2 Show chemical bond
Place two electrons between the atoms to show a chemical bond. Since boron is surrounded by three fluorines, use six electrons to show three chemical bonds as follows:
Also read: How to draw Lewis structure of O3 (5 steps)
#3 Mark lone pairs
As calculated earlier, we have a total of 24 valence electrons. And in the above structure, we have already used six valence electrons. Hence, eighteen valence electrons are remaining.
Two valence electrons represent one lone pair. So eighteen valence electrons = nine lone pairs.
Note that both (boron and fluorine) are the period 2 elements, so they can not keep more than 8 electrons in their last shell.
Also, make sure that you start marking these lone pairs on outside atoms first. And then, on the central atom.
The outside atoms are fluorines, so each fluorine will get three lone pairs. And the central atom (boron) will not get any lone pair, because all nine lone pairs are used.
So the Lewis structure of BF3 looks something like this:
In the above structure, you can see that the octet is completed on outside atoms. But, the central atom (boron) doesn’t form an octet.
Now boron has an exception in BF3, that it does not require eight electrons to complete its octet.
So one last thing we need to do is, calculate the formal charge and check the stability of the above structure.
Also read: How to draw Lewis structure of H2S (4 steps)
#4 Calculate formal charge and check stability
The following formula is used to calculate the formal charges on atoms:
Formal charge = valence electrons – nonbonding electrons – ½ bonding electrons
Collect the data from the above structure and then, write it down below as follows:
- For boron atom
Valence electrons = 3
Nonbonding electrons = 0
Bonding electrons = 6
Formal charge = 3 – 0 – ½ (6) = 0
- For each fluorine atom
Valence electrons = 7
Nonbonding electrons = 6
Bonding electrons = 2
Formal charge = 7 – 6 – ½ (2) = 0
Mention the formal charges of atoms on the structure. So the Lewis structure of BF3 looks something like this:
In the above structure, you can see that the formal charges of both (boron and fluorine) are zero. Therefore, this is the stable Lewis structure of BF3.
And each horizontal line drawn in the above structure represents a pair of bonding valence electrons.
Related
- Lewis structure of SO3
- Lewis structure of O3
- Lewis structure of H2S
- Lewis structure of C2H2
- Lewis structure of SF4
External video
- BF3 Lewis Structure: How to Draw the Lewis Structure for BF3 – Wayne Breslyn
External links
- Drawing the Lewis Structure for BF3 – The University of Maryland
- BF3 Lewis Structure in 5 Steps (With Images) – Pediabay
- BF3 Lewis Structure, Molecular Geometry, Hybridization, and Polarity – Geometry of Molecules
- BF3 Lewis structure| Molecular geometry, Hybridization, and Polarity – What’s Insight
- Lewis Structure of Boron Trifluoride (BF3) – Chemistry School
- Boron Trifluoride Overview & Lewis Structure | What is BF3 in Chemistry? – Study.com
- BF3 Lewis Structure, Molecular Geometry, and Hybridization – Techiescientist
- Molecular Geometry of Boron Trifluoride (BF3) – Chemistry Learner
- BF3 lewis structure, molecular geometry, bond angle, hybridization – Topblogtenz
- VSEPR calculation for boron trifluoride, BF3 – University of Sheffield
- How to draw BF3 Lewis Structure? – Science Education and Tutorials
- Using Lewis symbols and Lewis structures, diagram the formation of BF3 from B and F atoms, showing valence-shell electrons – Pearson
- BF3 Lewis Structure, hybridization – UO Chemists
- Chemical Bonding: BF3 Lewis Structure – The Geoexchange
- Draw Lewis structures for Boron Trifluoride, BF3 – Bartleby
- The molecular structure of boron trifluoride, BF3 – The Royal Society Publishing
- Lewis Structure for BF3 – Laurence Lavelle
- Why is Boron Trifluoride written in two ways in the lewis dot diagram structure? – Socratic
- Determine the correct Lewis structure for BF3 – Numerade
- BF3 lewis structure – Chemical Forums
- BF3 Lewis Structure (Boron Trifluoride) – Pinterest
- Molecular Geometry of BF3 [with video and free study guide] – AceOrganicChem
- Draw the Lewis structure for the BF3 compound – Quizlet
- BF3 Geometry and Hybridization – Chemistry Steps
- Choose a Lewis structure for BF3 – OneClass
- Boron Trifluoride BF3 Molecular Geometry & Polarity – Tutor-Homework.com
Deep
Rootmemory.com was founded by Deep Rana, who is a mechanical engineer by profession and a blogger by passion. He has a good conceptual knowledge on different educational topics and he provides the same on this website. He loves to learn something new everyday and believes that the best utilization of free time is developing a new skill.