Lewis structure of XeF6

The information on this page is ✔ fact-checked.

The Lewis structure of XeF₆ contains six single bonds, with xenon in the center, and six fluorines on either side. There are three lone pairs on each fluorine atom, and one lone pair on the xenon atom.

Steps

By using the following steps, you can easily draw the Lewis structure of XeF₆.

#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… xenon is a group 18 element and fluorine is a group 17 element. Hence, xenon has eight valence electrons and fluorine has seven valence electrons.

Now XeF₆ has one xenon atom and six fluorine atoms.

So the total number of valence electrons = valence electrons of xenon atom + (valence electrons of fluorine atom × 6)

Therefore, the total number of valence electrons = 8 + 42 = 50

• 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 xenon and fluorine as follows:

Electronegativity value of xenon = 2.6
Electronegativity value of fluorine = 3.98

Obviously, xenon is less electronegative than fluorine. Hence, assume that xenon is the central atom.

So now, put xenon in the center and fluorines on either side. And draw the rough skeleton structure for the Lewis structure of XeF₆ something like this:

Also read: How to draw Cl^– Lewis structure (3 steps)

#2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since xenon is surrounded by six fluorines, use twelve electrons to show six chemical bonds as follows:

Also read: How to draw Lewis structure of IBr (4 steps)

#3 Mark lone pairs

As calculated earlier, we have a total of 50 valence electrons. And in the above structure, we have already used twelve valence electrons. Hence, thirty-eight valence electrons are remaining.

Two valence electrons represent one lone pair. So thirty-eight valence electrons = nineteen lone pairs.

Note that xenon is a period 5 element, so it can keep more than 8 electrons in its last shell. And fluorine is a period 2 element, so it can not keep more than 8 electrons in its 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 (xenon) will get one lone pair.

So the Lewis structure of XeF₆ looks something like this:

In the above structure, you can see that the octet is completed on the central atom (xenon), and also on the outside atoms. Therefore, the octet rule is satisfied.

After completing the octet, 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 SbF₅ (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 xenon atom

Valence electrons = 8
Nonbonding electrons = 2
Bonding electrons = 12

Formal charge = 8 – 2 – ½ (12) = 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 XeF₆ looks something like this:

In the above structure, you can see that the formal charges of both (xenon and fluorine) are zero. Therefore, this is the stable Lewis structure of XeF₆.

And each horizontal line drawn in the above structure represents a pair of bonding valence electrons.

📝 Your feedback matters. Visit our contact page.

Related

• Cl^– Lewis structure
• Lewis structure of IBr
• Lewis structure of SbF₅
• Lewis structure of C₅H₁₂
• Lewis structure of SbCl₅

External links

• Drawing the Lewis Structure for XeF6 – The Geoexchange
• XeF6 Lewis Structure in 5 Steps (With Images) – Pediabay
• XeF6 lewis structure, molecular geometry, bond angle, hybridization – Topblogtenz
• How to determine and draw the Lewis structure of XeF6 – Quora
• How many lone pairs of electrons are on the Xe atom in XeF6? – Socratic
• Draw and explain the molecular structure of XeF6 – Homework.Study.com
• Xenon hexafluoride – Wikipedia
• Something was strange about XeF6. Draw the Lewis Structure and comment on the shape of the molecule according to VSEPR – Chegg
• XeF6 (Xenon Hexafluoride) Oxidation Number – ChemicalAid
• The Lewis structure of XeF6 – Bartleby