MO Diagram, Molecular Geometry, Hybridization, Polarity, and SF2 Lewis Structure

Sulfur Fluoride is an inorganic chemical that is extremely unstable. This chemical is made up of one Sulfur atom and two Fluoride atoms and has a molar mass of 70.062 g/mol.

When sulphur dichloride interacts with either potassium fluoride or mercury (||) fluoride at low pressure, this chemical is generated.

SCl2   +   2KF   —–>    SF2     +    2 KCl
SCl2   +   HgF2    ——->    SF2    +    HgCl2

Sulfur DiFluoride can also be formed when oxygen difluoride interacts with hydrogen sulphide.

OF2    +    H2S    ——>    SF2   +   H2O

The substance is non-hazardous and does not necessitate special handling or storage.

The chemical, however, might cause respiratory irritation in severe cases.

Let’s look at the geometry and other fascinating characteristics of the compound now that we’ve seen how it’s made.

SF2 Lewis Structure

An arrangement of valence electrons between distinct atoms is known as the Lewis Structure. It’s critical to understand the Lewis Structure of SF2 before moving on to other features of the compound.

First, we’ll need to figure out how many valence electrons are in this molecule. Sulfur has six electrons in its valence shell. Fluorine has a total of seven valence electrons.

This chemical contains two fluorine atoms in total. Thus, the total number of valence electrons = Sulfur valence electrons + 2 Fluorine valence electrons

6 + 2*7 =

= 20 electrons of valence

As a result, Sulfur Difluoride has a total of 20 valence electrons.

These valence electrons are now forming a ring around the centre atom. Sulfur is the key atom here. This is due to the fact that it has a lower electronegative value than the other atom in the molecule, Fluorine.

To become stable, each atom must fill its outer shell.

Fluorine just need one electron to complete its octet in this case. As a result, each of the two Fluorine atoms shares one electron with two Sulfur atoms.

Because Sulfur and two atoms of Fluorine share one pair of electrons, only a single link is created between them.

When you know how many electrons are shared and how many electrons are left as lone pairs of electrons, you can understand and create Lewis’ structure.

So, after the formation of two bonds, only 16 valence electrons remain out of a total of 20. Four of the 16 valence electrons belong to the sulphur atom and six to each fluorine element.

As a result, Sulfur has two lone pairs of electrons that did not participate in bond formation.

Each Fluorine atom has three lone pairs of electrons, for a total of six pairs of lone electrons in the SF2 complex.

This clarifies SF2’s Lewis structure, how the bonds are formed, and how many lone pairs of electrons there are.

Let us now look at what SF2 hybridization entails.

SF2 hybridization is a process in which two SF2 molecules combine to form a new hybrid

Hybridization is the notion of determining and recognising the number of electrons present in various energy orbitals.

There are four different energy levels, each of which may hold a different amount of electrons. To learn more about each energy level’s capacity, look at the chart below.

You can see how the electrons are arranged in different energy orbitals in the example of SF2 by looking at the diagram below.

In SF2, the bond formation is a single bond, which is referred to as a sigma bond. The mixing of orbitals with various energies is referred to as hybridization.

Sulfur has the electrical structure 1s2 2s2 2p6 3s2 3p4. The electrons are first filled with 1s, then 2s, and so on.

Similarly, Fluorine’s electrical arrangement is 1s2 2s2 2p5. These configurations are determined by the quantity of electrons present in these elements.

When it comes to the electronic configuration of SF2, 3s2 3Px2 3Py1 3Pz1 comes to mind. As a result, we may derive the compound’s hybridization, which is sp3.

Calculating the steric number of SF2, which we can calculate using the equation below, is another means of determining the hybridization of SF2.

The steric number is equal to the sum of the number of bonds on the central atom and the number of lone pairs on the centre atom.

Sulfur is the key atom here.

On the sulphur atom, there are two bonds and two lone pairs of electrons, as we’ve seen. As a result, the Steric number is 2+2 = 4.

Each number corresponds to a single energy orbital. As a result, 4 deduces that four energy levels will be used.

As a result, SF2 hybridization is sp3.

Now that we know about the compound’s hybridization, we can investigate its molecular geometry.

SF2 Molecular Geometry

Any compound’s molecular geometry must be understood in order to understand its structure and how it appears in a plane.

In most cases, the VSEPR theory is used to calculate this.

Each atom in a compound is structured in such a way that the molecule becomes stable in nature, according to VSEPR theory. The repulsion between the atoms and their associated electrons should be as low as possible, and in order to do so, a compound must take on a distinct structure.

This shape is determined by various factors such as lone pairs of electrons, bonding electrons, and so on. Here’s a diagram that shows the various combinations of compounds that can be formed.

We can determine the molecular geometry of a compound based on the lone pair of electrons and bonds that are produced.

The core atom of SF2 has two bonds and two lone pairs of electrons.

As a result, the molecular geometry is of the type AX2E2, indicating that the compound is non-linear or bent.

As a result, the molecular geometry of SF2 is bent.

The presence of lone pairs and bonds on the core atom results in the bent structure. As a result, repulsions exist, and these repulsive forces cause bent geometry.

SF2’s Bond Angle

As we can see, the compound has a tiny bend in its shape, implying that there will undoubtedly be some bond angle.

In SF2, the angle that forms is around 98 degrees.

The lone pairs of Sulfur force both Fluorine atoms downward, resulting in a bond angle ranging from 180 to 98 degrees.

SF2 molecular orbital diagram

MO diagrams are a useful tool for representing a compound’s various features. Shape, bond energy, bond angle, and other qualities are among them.

We may see how much energy each energy orbital obtains and has with the help of this diagram.

The energy are spread in a MO diagram of another bent chemical, the bent shaped (SO2 molecule).

SF2’s polarity

We can now discuss the polarity of this chemical after we’ve looked at every facet of it, from Lewis’ structure to molecular geometry.

Why is it important to understand a compound’s polarity?

It is critical to understand the polarity of any compound since this allows us to determine whether the compound has a negative or positive charge. We learn how atoms bond to one another, what the attraction force is, and more.

When determining the polarity of a compound, we look at the lone pairs on the atom, the shape, and other factors.

In the case of SF2, the lone pair of electrons acts as a repulsive force on the Sulfur-Fluorine bonds.

The Fluorine atoms are pushed down as a result, giving the complex a bent form.

As a result, the charge on the compound is not evenly distributed, indicating that the dipole moment will not be zero.

We can safely assume that the chemical is Polar in nature because the form is not linear and there is repulsion.

You can also read about the polarity of SF2 in this article.


Let us now review what we’ve learnt and comprehended about the chemical SF2.

Sulfur is the core atom of SF2, which is surrounded by two Fluorine atoms. Because the dipole moments of Sulfur and Fluorine do not cancel each other, the compound is polar in nature. This compound’s hybridization is sp3, and its molecular geometry is bent or non-linear.

We hope you found the article to be informative and that you gained a thorough understanding of the subject. If you get stuck at any time, please contact us and we will gladly assist you.

You can contact our team if you have any questions or complaints about the article.

Thank you for taking the time to read this.

Read more: Diagram, Steps To Draw The Potassium Bohr Model

Misha Khatri
Misha Khatri is an emeritus professor in the University of Notre Dame's Department of Chemistry and Biochemistry. He graduated from Northern Illinois University with a BSc in Chemistry and Mathematics and a PhD in Physical Analytical Chemistry from the University of Utah.


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