AsF6- Lewis structure

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AsF₆^– has one arsenic atom and six fluorine atoms.

In AsF₆^– Lewis structure, there are six single bonds around the arsenic atom, with six fluorine atoms attached to it, and on each fluorine atom, there are three lone pairs.

Also, there is a negative (-1) charge on the arsenic atom.

Steps

Use these steps to correctly draw the AsF₆^– Lewis structure:

#1 First draw a rough sketch
#2 Mark lone pairs on the atoms
#3 Calculate and mark formal charges on the atoms, if required

Let’s discuss each step in more detail.

#1 First draw a rough sketch

• First, determine the total number of valence electrons

In the periodic table, arsenic lies in group 15, and fluorine lies in group 17.

Hence, arsenic has five valence electrons and fluorine has seven valence electrons.

Since AsF₆^– has one arsenic atom and six fluorine atoms, so…

Valence electrons of one arsenic atom = 5 × 1 = 5
Valence electrons of six fluorine atoms = 7 × 6 = 42

Now the AsF₆^– has a negative (-1) charge, so we have to add one more electron.

So the total valence electrons = 5 + 42 + 1 = 48

Learn how to find: Arsenic valence electrons and Fluorine valence electrons

• Second, find the total electron pairs

We have a total of 48 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 = 48 ÷ 2 = 24

• Third, determine the central atom

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

Since arsenic is less electronegative than fluorine, assume that the central atom is arsenic.

Therefore, place arsenic in the center and fluorines on either side.

• And finally, draw the rough sketch

#2 Mark lone pairs on the atoms

Here, we have a total of 24 electron pairs. And six As — F bonds are already marked. So we have to only mark the remaining eighteen electron pairs as lone pairs on the sketch.

Also remember that arsenic 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.

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

So for each fluorine, there are three lone pairs, and for arsenic, there is zero lone pair because all eighteen electron pairs are over.

Mark the lone pairs on the sketch as follows:

#3 Calculate and mark formal charges on the atoms, if required

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

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

For arsenic atom, formal charge = 5 – 0 – ½ (12) = -1

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

Here, the arsenic atom has a charge, so mark it on the sketch as follows:

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

Therefore, this structure is the most stable Lewis structure of AsF₆^–.

And since the AsF₆^– has a negative (-1) charge, mention that charge on the Lewis structure by drawing brackets as follows:

Next: CH₃O^– Lewis structure

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External video

• AsF6- Lewis Structure: How to Draw the Lewis Structure for Arsenic Hexafluoride ion – YouTube • Wayne Breslyn

External links

• https://www.thegeoexchange.org/chemistry/bonding/Lewis-Structures/AsF6-Lewis-structure.html
• https://lambdageeks.com/asf6-lewis-structure/
• https://homework.study.com/explanation/draw-lewis-structure-for-a-co-b-asf6.html
• https://www.chegg.com/homework-help/questions-and-answers/lewis-structure-asf6-q1611779