SHF Lewis structure

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SHF has one sulfur atom, one hydrogen atom, and one fluorine atom.

In SHF Lewis structure, there are two single bonds around the sulfur atom, with one hydrogen atom and one fluorine atom attached to it. The fluorine atom has three lone pairs, and the sulfur atom has two lone pairs.

Steps

Here’s how you can easily draw the SHF 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, sulfur lies in group 16, hydrogen lies in group 1, and fluorine lies in group 17.

Hence, sulfur has six valence electrons, hydrogen has one valence electron, and fluorine has seven valence electrons.

Since SHF has one sulfur atom, one hydrogen atom, and one fluorine atom, so…

Valence electrons of one sulfur atom = 6 × 1 = 6
Valence electrons of one hydrogen atom = 1 × 1 = 1
Valence electrons of one fluorine atom = 7 × 1 = 7

And the total valence electrons = 6 + 1 + 7 = 14

Learn how to find: Sulfur valence electrons, Hydrogen valence electrons, and Fluorine valence electrons

• Second, find the total electron pairs

We have a total of 14 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 = 14 ÷ 2 = 7

• Third, determine the central atom

Here hydrogen can not be the central atom. Because the central atom is bonded with at least two other atoms, and hydrogen has only one electron in its last shell, so it can not make more than one bond.

Now we have to choose the central atom from sulfur and fluorine. Place the least electronegative atom at the center.

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

Therefore, place sulfur in the center and hydrogen and fluorine on either side.

• And finally, draw the rough sketch

#2 Mention lone pairs on the atoms

Here, we have a total of 7 electron pairs. And two bonds are already marked. So we have to only mark the remaining five electron pairs as lone pairs on the sketch.

Also remember that sulfur is a period 3 element, so it can keep more than 8 electrons in its last shell. Hydrogen is a period 1 element, so it can not keep more than 2 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 hydrogen and fluorine. But no need to mark on hydrogen, because hydrogen already has two electrons.

So for fluorine, there are three lone pairs, and for sulfur, 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 sulfur atom, formal charge = 6 – 4 – ½ (4) = 0

For hydrogen atom, formal charge = 1 – 0 – ½ (2) = 0

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

Here, the atoms do not have charges, so no need to mark the charges.

In the above structure, you can see that the central atom (sulfur) forms an octet. The outside atom (fluorine) also forms an octet, and hydrogen forms a duet. Hence, the octet rule and duet rule are satisfied.

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

Next: SeS₃ Lewis structure

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External links

• https://www.numerade.com/ask/question/draw-the-lewis-structure-for-shf-and-give-the-shape-name-and-if-its-polar-or-nonpolar-covalent-bond-91941/
• https://www.answers.com/Q/What_is_the_Lewis_structure_FOR_SHF
• https://www.chegg.com/homework-help/questions-and-answers/draw-lewis-structure-shf-give-shape-name-polar-nonpolar-covalent-bond-q58669681