Lewis structure of SF5-

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The Lewis structure of SF₅^– contains five single bonds, with sulfur in the center, and five fluorines on either side. There are three lone pairs on each fluorine atom, and one lone pair on the sulfur atom.

Plus, there is a negative (-1) charge on the sulfur atom.

Steps

By using the following steps, you can easily draw the Lewis structure of SF₅^–.

#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… sulfur is a group 16 element and fluorine is a group 17 element. Hence, sulfur has six valence electrons and fluorine has seven valence electrons.

Now SF₅^– has one sulfur atom and five fluorine atoms.

So the total number of valence electrons = valence electrons of sulfur atom + (valence electrons of fluorine atom × 5)

And SF₅^– has a negative (-1) charge, so we have to add one more electron.

Therefore, the total number of valence electrons = 6 + 35 + 1 = 42

• 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 sulfur and fluorine as follows:

Electronegativity value of sulfur = 2.58
Electronegativity value of fluorine = 3.98

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

So now, put sulfur in the center and fluorines on either side. And draw the rough skeleton structure for the Lewis structure of SF₅^– something like this:

Also read: How to draw Lewis structure of SeF₂ (4 steps)

#2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since sulfur is surrounded by five fluorines, use ten electrons to show five chemical bonds as follows:

Also read: How to draw Lewis structure of NO₄^3- (5 steps)

#3 Mark lone pairs

As calculated earlier, we have a total of 42 valence electrons. And in the above structure, we have already used ten valence electrons. Hence, thirty-two valence electrons are remaining.

Two valence electrons represent one lone pair. So thirty-two valence electrons = sixteen lone pairs.

Note that sulfur is a period 3 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 (sulfur) will get one lone pair.

So the Lewis structure of SF₅^– looks something like this:

In the above structure, you can see that the octet is completed on the central atom (sulfur), 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 SF₃⁺ Lewis structure (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 sulfur atom

Valence electrons = 6
Nonbonding electrons = 2
Bonding electrons = 10

Formal charge = 6 – 2 – ½ (10) = -1

• 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 SF₅^– looks something like this:

In the above structure, you can see that the formal charges of atoms are closer to zero. Therefore, this is the most stable Lewis structure of SF₅^–.

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

Now SF₅^– is an ion having a negative (-1) charge, so draw brackets around the above Lewis structure and mention that charge on the top right corner. And then, the Lewis structure of SF₅^– looks something like this:

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Related

• Lewis structure of SeF₂
• Lewis structure of NO₄^3-
• SF₃⁺ Lewis structure
• Lewis structure of C₂Cl₂
• Lewis structure of CH₃CH₂NH₂

External video

• How to Draw the Lewis Dot Structure for SF5 – – Wayne Breslyn

External links

• SF5- Lewis Structure in 5 Steps (With Images) – Pediabay
• Draw an appropriate Lewis structure for SF5- – Chegg
• Draw the Lewis structure for the SF5- ion – Homework.Study.com
• Draw an appropriate lewis structure for the anion sf5- – Brainly
• What is the Lewis structure for the ion SF5-? – OneClass