Lewis Structure of SF2 and Hybridization of SF2 (Sulfur Difluoride)

Sulfur difluoride (SF2) is one sulfur atom connected to two fluorine atoms. They are both non-metals, so they share electrons to form covalent bonds.

Sulfur brings 6 valence electrons with it, and so needs two extra for have a full octet.

Fluorine brings 7 valence electrons with it, and so needs one extra to complete its octet.

This means that sulfur can share ONE electron with EACH of two fluorine atoms, completing all of their octets simultaneously.

Lewis Structure of SF2 (sulfur difluoride). Sulfur is single-bonded to each of two fluorine atoms, and has two lone pairs as well.

In the end, sulfur is single-bonded to each of two fluorine atoms (this is two bonding pairs) and has two lone pairs on it as well. This gives it a VSEPR notation of AX2E2, which is angular / bent / non-linear geometry.

What is the Hybridization of S in SF2?

The sulfur atom has no double bonds, which means that no pi-bonds are needed. This means its hybridization is sp3.

What is the Hybridization of F in SF2?

The hybridization of the fluorine atoms is sp3 as well, since they also do not have any double or triple bonds.

What is the Bond Angle in SF2?

Sulfur has two single bonds and two lone pairs around it, and this is four things, so the electron pair geometry is tetrahedral. Due to the lone pairs, most teachers want to hear that the bond angle is “less than 109.5 degrees”, since the lone pairs repel the bonding pairs and push the single bonds together more than they do in a tetrahedral molecule like CH4. In the case of SF2, the actual bond angle is just 98 degrees.

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