Lewis structure of KrF4

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The Lewis structure of KrF₄ contains four single bonds, with krypton in the center, and four fluorines on either side. There are three lone pairs on each fluorine atom, and two lone pairs on the krypton atom.

Steps

By using the following steps, you can easily draw the Lewis structure of KrF₄.

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

Now KrF₄ has one krypton atom and four fluorine atoms.

So the total number of valence electrons = valence electrons of krypton atom + (valence electrons of fluorine atom × 4)

Therefore, the total number of valence electrons = 8 + 28 = 36

• 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 krypton and fluorine as follows:

Electronegativity value of krypton = 3.00
Electronegativity value of fluorine = 3.98

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

So now, put krypton in the center and fluorines on either side. And draw the rough skeleton structure for the Lewis structure of KrF₄ something like this:

Also read: How to draw Lewis structure of HClO₄ (5 steps)

#2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since krypton is surrounded by four fluorines, use eight electrons to show four chemical bonds as follows:

Also read: How to draw Lewis structure of MnO₄^– (5 steps)

#3 Mark lone pairs

As calculated earlier, we have a total of 36 valence electrons. And in the above structure, we have already used eight valence electrons. Hence, twenty-eight valence electrons are remaining.

Two valence electrons represent one lone pair. So twenty-eight valence electrons = fourteen lone pairs.

Note that krypton is a period 4 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 (krypton) will get two lone pairs.

So the Lewis structure of KrF₄ looks something like this:

In the above structure, you can see that the octet is completed on the central atom (krypton), 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 XeCl₂ (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 krypton atom

Valence electrons = 8
Nonbonding electrons = 4
Bonding electrons = 8

Formal charge = 8 – 4 – ½ (8) = 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 KrF₄ looks something like this:

In the above structure, you can see that the formal charges of both (krypton and fluorine) are zero. Therefore, this is the stable Lewis structure of KrF₄.

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

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Related

• Lewis structure of HClO₄
• Lewis structure of MnO₄^–
• Lewis structure of XeCl₂
• Lewis structure of SeCl₄
• Lewis structure of SeS₂

External links

• KrF4 Lewis Structure in 5 Steps (With Images) – Pediabay
• Predict the molecular structure of KrF4, whose Lewis structure is shown below – Homework.Study.com
• Consider the species KrF4 where the first atom is the central atom – Studocu
• Draw the Lewis structure of KrF4 – Chegg
• Draw the Lewis structure of KrF4 – Brainly
• The Lewis structure for KrF4 is shown – Bartleby
• What is the Lewis structure of KrF4? – Quizlet
• Draw the Lewis structure of KrF4 – Numerade
• What is the Lewis structure for KrF4? – OneClass