KrCl4 Lewis structure

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KrCl₄ has one krypton atom and four chlorine atoms.

In KrCl₄ Lewis structure, there are four single bonds around the krypton atom, with four chlorine atoms attached to it. Each chlorine atom has three lone pairs, and the krypton atom has two lone pairs.

Steps

Here’s how you can easily draw the KrCl₄ Lewis structure step by step:

#1 Draw a rough skeleton structure
#2 Mention lone pairs on the atoms
#3 If needed, mention formal charges on the atoms

Now, let’s take a closer look at each step mentioned above.

#1 Draw a rough skeleton structure

• First, determine the total number of valence electrons

In the periodic table, krypton lies in group 18, and chlorine lies in group 17.

Hence, krypton has eight valence electrons and chlorine has seven valence electrons.

Since KrCl₄ has one krypton atom and four chlorine atoms, so…

Valence electrons of one krypton atom = 8 × 1 = 8
Valence electrons of four chlorine atoms = 7 × 4 = 28

And the total valence electrons = 8 + 28 = 36

Learn how to find: Krypton valence electrons and Chlorine valence electrons

• Second, find the total electron pairs

We have a total of 36 valence electrons. And when we divide this value by two, we get the value of total electron pairs.

Total electron pairs = total valence electrons ÷ 2

So the total electron pairs = 36 ÷ 2 = 18

• Third, determine the central atom

We have to place the least electronegative atom at the center.

Since krypton is less electronegative than chlorine, assume that the central atom is krypton.

Therefore, place krypton in the center and chlorines on either side.

• And finally, draw the rough sketch

#2 Mention lone pairs on the atoms

Here, we have a total of 18 electron pairs. And four Kr — Cl bonds are already marked. So we have to only mark the remaining fourteen electron pairs as lone pairs on the sketch.

Also remember that krypton is a period 4 element, so it can keep more than 8 electrons in its last shell. And chlorine is a period 3 element, so it can keep more than 8 electrons in its last shell.

Always start to mark the lone pairs from outside atoms. Here, the outside atoms are chlorines.

So for each chlorine, there are three lone pairs, and for krypton, there are two lone pairs.

Mark the lone pairs on the sketch as follows:

#3 If needed, mention formal charges on the atoms

Use the following formula to calculate the formal charges on atoms:

Formal charge = valence electrons – nonbonding electrons – ½ bonding electrons

For krypton atom, formal charge = 8 – 4 – ½ (8) = 0

For each chlorine atom, formal charge = 7 – 6 – ½ (2) = 0

Here, both krypton and chlorine atoms do not have charges, so no need to mark the charges.

In the above structure, you can see that the central atom (krypton) forms an octet. And the outside atoms (chlorines) also form an octet. Hence, the octet rule is satisfied.

Therefore, this structure is the stable Lewis structure of KrCl₄.

Next: PS₃^– Lewis structure

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External links

• https://www.chegg.com/homework-help/questions-and-answers/draw-lewis-structure-krcl4-answer-following-questions-many-valence-electrons-present-compo-q8551701
• https://www.numerade.com/ask/question/draw-the-lewis-structure-for-krcl4-and-answer-the-following-questions-how-many-valence-electrons-are-present-in-this-compound-how-many-bonding-electrons-are-present-in-this-compound-how-many-69355/
• https://brainly.com/question/29593377
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