Lewis structure of SF4

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The Lewis structure of SF₄ contains four single bonds, with sulfur in the center, and four fluorines on either side. There are three lone pairs on each fluorine atom, and one lone pair on the sulfur atom.

Steps

By using the following steps, you can easily draw the Lewis structure of SF₄:

#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 SF₄ has one sulfur atom and four fluorine atoms.

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

Therefore, the total number of valence electrons = 6 + 28 = 34

• 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 SF₄ something like this:

Also read: How to draw Lewis structure of CCl₄ (4 steps)

#2 Show chemical bond

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

Also read: How to draw Lewis structure of OF₂ (4 steps)

#3 Mark lone pairs

As calculated earlier, we have a total of 34 valence electrons. And in the above structure, we have already used eight valence electrons. Hence, twenty-six valence electrons are remaining.

Two valence electrons represent one lone pair. So twenty-six valence electrons = thirteen 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 SF₄ 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 Lewis structure of CS₂ (5 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 = 8

Formal charge = 6 – 2 – 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 SF₄ looks something like this:

In the above structure, you can see that the formal charges of both (sulfur and fluorine) are zero. Therefore, this is the stable Lewis structure of SF₄.

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

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Related

• Lewis structure of CCl₄
• Lewis structure of OF₂
• Lewis structure of CS₂
• Lewis structure of NO
• Lewis structure of NF₃

External video

• SF4 Lewis Structure: How to Draw the Lewis Structure for SF4 – YouTube • Wayne Breslyn

External links

• Drawing the Lewis Structure for SF4 – The University of Maryland
• SF4 (Sulfur tetrafluoride) Lewis Structure – Chemistry School
• SF4 Lewis structure, Molecular geometry, Bond angle, Hybridization – Topblogtenz
• SF4 Molecular Geometry, Lewis Structure, and Polarity – Geometry of Molecules
• SF4 Lewis Structure, Geometry – Kemicalinfo
• SF4 Lewis Structure, Molecular Geometry, Hybridization, and MO Diagram – Techiescientist
• SF4 Lewis Structure & Molecular Geometry – What’s Insight
• Molecular Geometry of Sulfur Tetrafluoride (SF4) – Chemistry Learner
• SF4 Lewis Structure in 5 Steps (With Images) – Pediabay
• What is the molecular geometry of SF4? – Quora
• Lewis Dot of Sulfur Tetrafluoride SF4 – Kent’s Chemistry
• How to draw SF4 Lewis Structure? – Science Education and Tutorials
• Draw the Lewis dot structure for SF4 – Homework.Study.com
• Sulfur Tetrafluoride, SF4 Molecular Geometry & Polarity – Tutor-Homework.com
• Chemical Bonding: SF4 Lewis Structure – The Geoexchange
• Draw the Lewis structure for sulfur tetrafluoride, SF4, and then draw the electron pair geometry. What’s the name of the molecular shape of sulfur tetrafluoride? – Course Hero
• Draw a Lewis structure for SF4 that has minimized formal charges. Include all nonbonding electrons and any nonzero formal charges – Brainly
• SF4 Geometry and Hybridization – Chemistry Steps
• What is the shape of SF4 (including bond angles)? – Socratic