Lewis structure of SbF5

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The Lewis structure of SbF₅ contains five single bonds, with antimony in the center, and five fluorines on either side. There are three lone pairs on each fluorine atom, and the antimony atom does not have any lone pair.

Steps

By using the following steps, you can easily draw the Lewis structure of SbF₅.

#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… antimony is a group 15 element and fluorine is a group 17 element. Hence, antimony has five valence electrons and fluorine has seven valence electrons.

Now SbF₅ has one antimony atom and five fluorine atoms.

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

Therefore, the total number of valence electrons = 5 + 35 = 40

• 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 antimony and fluorine as follows:

Electronegativity value of antimony = 2.05
Electronegativity value of fluorine = 3.98

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

So now, put antimony in the center and fluorines on either side. And draw the rough skeleton structure for the Lewis structure of SbF₅ something like this:

Also read: How to draw Lewis structure of C₅H₁₂ (3 steps)

#2 Show chemical bond

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

Also read: How to draw Lewis structure of SbCl₅ (4 steps)

#3 Mark lone pairs

As calculated earlier, we have a total of 40 valence electrons. And in the above structure, we have already used ten valence electrons. Hence, thirty valence electrons are remaining.

Two valence electrons represent one lone pair. So thirty valence electrons = fifteen lone pairs.

Note that antimony 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 (antimony) will not get any lone pair, because all fifteen lone pairs are used.

So the Lewis structure of SbF₅ looks something like this:

In the above structure, you can see that the octet is completed on the central atom (antimony), 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 CH₃SH (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 antimony atom

Valence electrons = 5
Nonbonding electrons = 0
Bonding electrons = 10

Formal charge = 5 – 0 – ½ (10) = 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 SbF₅ looks something like this:

In the above structure, you can see that the formal charges of both (antimony and fluorine) are zero. Therefore, this is the stable Lewis structure of SbF₅.

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

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Related

• Lewis structure of C₅H₁₂
• Lewis structure of SbCl₅
• Lewis structure of CH₃SH
• Lewis structure of C₂H₂Br₂
• Lewis structure of N₂O₃

External links

• SbF5 Lewis Structure in 5 Steps (With Images) – Pediabay
• Use Lewis structures and VSEPR theory to predict the geometry and ideal bond angles of SbF5 – Homework.Study.com
• Antimony pentafluoride | SbF5 | CID 24557 – National Institutes of Health (.gov)
• What is the lewis structure is SbF5? – OneClass
• SbF5 (Antimony Pentafluoride) Oxidation Number – ChemicalAid