SeO2 Lewis structure, molecular geometry, bond angle, hybridization (2024)

SeO₂ is the chemical formula for representing selenium dioxide, a colorless, lustrous crystalline solid. It is used as an oxidizing agent and a colorant in the chemical manufacturing, glass-making, and printing industry.

The IUPAC name for SeO₂ is selenium (IV) oxide, as Se has a +4 oxidation state in this compound. If you are curious to know the chemistry behind SeO₂, then this article is for you.

In this article, you will learn how to draw the Lewis dot structure of SeO₂, what is its molecular geometry or shape, electron geometry, bond angles, hybridization, formal charges, and/or whether SeO₂ is a polar or a non-polar molecule.

The Lewis structure of SeO₂ consists of a selenium (Se) atom at the center. It is double-covalently bonded to two oxygen (O) atoms at the sides. There are a total of 3 electron density regions around the central Se-atom in this Lewis structure comprising 2 Se=O bond pairs and 1 lone pair of electrons on the central atom.

If you want to learn how to draw the SeO₂ Lewis dot structure in the best and simplest way, then follow the steps given below.

Steps for drawing the Lewis dot structure of SeO₂

1. Count the total valence electrons in SeO₂

The very first step while drawing the Lewis structure of SeO₂is to calculate the total valence electronspresent in its concerned elemental atoms.

There are two different elemental atoms present in SeO₂, i.e., a selenium (Se) atom and two oxygen (O) atoms. When you look through the Periodic Table of elements, you will find that both selenium and oxygen are located in Group VI A (or 16). This denotes that both Se and O consist of a total of 6 valence electrons in each atom.

• Total number ofvalence electrons in selenium = 6
• Total number ofvalence electrons in oxygen= 6

∴ The SeO₂ molecule consists of 1 Se-atom and 2 O-atoms. Hence, the total valence electrons in the Lewis dot structure of SeO₂= 1(6) + 2(6) =18 valence electrons.

2. Choose the central atom

In this second step, usually the least electronegative atom out of all the concerned atoms is chosen as the central atom.

This is because the least electronegative atom is the one that is most likely to share its electrons with the atoms spread around it.

As selenium (Se) is less electronegative than oxygen (O) so, the Se-atom is placed at the center of the SeO₂Lewis structure while the two O-atoms are spread around it, as shown below.

3. Connect outer atoms with the central atom

At this step of drawing the Lewis structure of a molecule, we need to connect the outer atoms with the central atom using single straight lines.

As the two O-atoms are the outer atoms in the Lewis structure of selenium dioxide (SeO₂), both the oxygen atoms are joined to the central Se-atom using single straight lines, as shown below.

Each straight line represents a single covalent bond containing 2 electrons.

Now, if we count the total valence electrons used till this step out of the 18 available initially, there are a total of 2 single bonds in the structure drawn above. Thus, 2(2) = 4 valence electrons are used tillstep 3.

• Total valence electrons available – electrons used tillstep 3 = 18 – 4 = 14 valence electrons.
• This means we still have 14 valence electrons to be accommodated in the Lewis dot structure of SeO₂.

4. Complete the octet of the outer atoms

There are two O-atoms present as outer atoms in the Lewis structure of SeO₂. Each O-atom needs a total of 8 valence electrons in order to achieve a stable octet electronic configuration.

A Se-O single bond already represents 2 electrons, which means both the O-atoms require 6 more electrons each to complete their octets. Thus, these 6 valence electrons are placed as 3 lone pairs around each O-atom, as shown below.

5. Complete the octet of the central atom and convert a lone pair into a covalent bond if necessary

• Total valence electrons used tillstep 4= 2 single bonds + 2 (electrons placed around O-atom, shown as dots) =2(2) +2(6) = 16 valence electrons.
• Total valence electrons available – electrons used till step 4 =18-16 = 2 valence electrons.

So the remaining 2 valence electrons are placed as a lone pair on the central Se-atom.

However, a problem here is that the central Se-atom still has an incomplete octet. It consists of 2 single bonds and 1 lone pair that denotes a total of 6 valence electrons, consequently a deficiency of 2 more electrons in order to achieve a stable octet electronic configuration.

So, to solve this issue, a lone pair present on any one of the two outer O-atoms is converted into an additional covalent chemical bond between the central Se-atom and the respective O-atom, as shown below.

Now, you may notice that the central Se-atom has a complete octet with 1 single bond + 1 double bond + 1 lone pair = 8 valence electrons. The octet of both terminal O-atoms is also complete.

But is this Lewis structure stable? Let’s check that using the formal charge concept in the next step.

6. Check the stability of the SeO₂ Lewis structure using the formal charge concept

The fewer formal charges present on the atoms of a molecule, the better the stability of its Lewis structure.

The formal charges can be calculated using the formula given below.

• Formal charge = [ valence electrons – nonbonding electrons- ½ (bonding electrons)]

Now let us use this formula and the Lewis structure obtained instep 5to determine the formal charges on SeO₂ atoms.

For selenium atom

• Valence electrons of selenium = 6
• Bonding electrons =1 double bond + 1 single bond = 4 + 2 = 6 electrons
• Non-bonding electrons = 1 lone pair = 2 electrons
• Formal charge = 6-2-6/2 =6-2-3 = 6-5 = +1

For single-bonded oxygen atom

• Valence electrons of oxygen = 6
• Bonding electrons = 1 single bond = 2 electrons
• Non-bonding electrons = 3 lone pairs = 3(2) = 6 electrons
• Formal charge = 6-6-2/2 = 6-6-1 = 6-7 = -1

For double-bonded oxygen atom

• Valence electrons of oxygen = 6
• Bonding electrons = 1 double bond = 4 electrons
• Non-bonding electrons = 2 lone pairs = 2(2) = 4 electrons
• Formal charge = 6-4-4/2 = 6-4-2 = 6-6 = 0

The above calculation shows that as per the SeO₂ Lewis structure obtained so far, the central Se-atom carries a +1 formal charge while the single-bonded O-atom carries a -1 formal charge.

But wait a minute; we learned that the fewer the formal charges, the more stable the Lewis representation of a molecule. So can we reduce Se and O formal charges?

The good news is that we can do so by converting another lone pair into a covalent chemical bond.

7. Minimize formal charges by converting another lone pair into a covalent chemical bond and again check the stability of Lewis’s structure

At this step, a lone pair on the single-bonded O-atom is converted into an extra bond between the central Se-atom and the respective O-atom, as shown below.

In this way, the central Se-atom is uniformly bonded to two O-atoms via double covalent bonds.

According to the above Lewis structure, the central Se-atom now has a total of 10 valence electrons surrounding it.

This situation falls under the expanded octet rule. Atoms such as sulfur, phosphorus and selenium can accommodate more than 8 valence electrons owing to the presence of a d-subshell in their outermost shell.

After completely filling the 4p-subshell in Se, the extra incoming electrons start occupying 4d orbitals.

Both the terminal O-atoms have a complete octet with 1 double bond +2 lone pairs each in the above structure.

Finally, we again need to check the stability of the Lewis structure obtained in step 7 by applying the formal charge formula to ensure that overall formal charges are minimized, as expected.

For selenium atom

• Valence electrons of selenium = 6
• Bonding electrons = 2 double bonds = 2(4) = 8 electrons
• Non-bonding electrons = 1 lone pair = 2 electrons
• Formal charge = 6-2-8/2 =6-2-4 = 6-6 = 0

For each oxygen atom

• Valence electrons of oxygen = 6
• Bonding electrons = 1 double bond = 4 electrons
• Non-bonding electrons = 2 lone pairs = 2(2) = 4 electrons
• Formal charge = 6-4-4/2 = 6-4-2 = 6-6 = 0

Zero formal charges on all three bonded atoms denote that there is no overall charge present on the SeO₂ Lewis structure; thus, it is the most stable and correct Lewis representation of the selenium dioxide molecule.

Also check –

• How to draw a lewis structure?
• Formal charge calculator
• Lewis structure generator

The ideal electron pair geometry of SeO₂ is trigonal planar. However, it is due to the presence of a lone pair of electrons on the central Se-atom that SeO₂ adopts a different shape or molecular geometry, i.e., bent, angular, or V-shaped.

Molecular geometry of SeO₂

The selenium dioxide (SeO₂) molecule has a bent shape or molecular geometry. The presence of a lone pair of electrons on the central Se-atom leads to strong lone pair-bond pair repulsions in addition to a Se=O bond pair-bond pair repulsive effect in the molecule.

The strong electronic repulsions distort the shape and geometry of the molecule. The Se=O bond pairs tilt inwards, away from the lone pair at the top, to minimize the electron repulsive effect. It thus results in a bent, angular, or V-shape, as shown below.

Always keep in mind that the molecular geometry or shape of a molecule gets strongly influenced by the different number of lone pairs and bond pairs around the central atom.

Contrarily, the ideal electron pair geometry only depends on the total electron domains around the central atom (lone pairs and bond pairs inclusive).

A double covalent bond such as Se=O is considered a single electron domain while determining the electronic geometry of SeO₂.

Electron geometry of SeO₂

According to the valence shell electron pair repulsion (VSEPR) theory of chemical bonding, the ideal electron geometry of a molecule containing 3 regions of electron density around the central atom is trigonal planar.

In SeO₂, there are two Se=O bonds and one lone pair around the central Se-atom that makes a total of 3 electron density regions or electron domains. Thus, the ideal electron pair geometry of SeO₂ is trigonal planar.

A shortcut to finding the electron and the molecular geometry of a molecule is by using the AXN method.

AXN is a simple formula to represent the number of atoms bonded to the central atom in a molecule and the number of lone pairs present on it.

It is used to predict the shape and geometry of a molecule based on the VSEPR concept.

AXN notation for SeO₂ molecule

• A in the AXN formula represents the central atom. In SeO₂, a selenium (Se) atom is present at the center, so A = Se for SeO₂.
• X denotes the atoms bonded to the central atom. In SeO₂, there are two Se=O bonds; thus, X=2.
• N stands for the lone pairs present on the central atom. As per the Lewis structure of SeO₂,there is one lone pair of electrons on the central selenium atom, so N = 1.

Hence, the AXN generic formula for the selenium dioxide molecule isAX₂N₁.

Now, you may have a look at the VSEPR chart given below.

The VSEPR chart confirms that the molecular geometry or shape of an AX₂N₁-type molecule is bent or V-shaped while its ideal electron pair geometry is trigonal planar, as we already noted down for the selenium dioxide (SeO₂) molecule.

Hybridization of SeO₂

The central Se-atom and both O-atoms are sp² hybridized in SeO₂.

The electronic configuration of a selenium atom is 1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p⁴.

During SeO₂ chemical bonding, one 4p electron of selenium shifts to its empty 4d atomic orbital. Two 4p atomic orbitals of selenium then hybridize with its 4s atomic orbital to produce three sp² hybrid orbitals.

The sp² hybrid orbital containing paired electrons is situated as a lone pair on the central Se-atom in SeO₂. The other two sp² hybrid orbitals containing a single electron each form Se-O sigma (σ) bonds by overlapping with the sp² hybrid orbitals of terminal O-atoms.

The unhybridized p and d atomic orbitals of selenium then form the required pi bonds by overlapping with the p-orbitals of oxygen atoms in each Se=O covalent bond.

Refer to the figure drawn below.

A shortcut to finding the hybridization present in a molecule is by using its steric number against the table given below.

The steric number of central Se-atom in SeO₂ is 3, so it hassp² hybridization.

The SeO₂bond angle

It is due to the distortion present in the SeO₂ molecular shape and geometry that the O=Se=O bond angle decreases slightly from the ideal.

The ideal bond angle in a symmetrical trigonal planar molecule is 120° while the O=Se=O bond angle is approx. 119° in the selenium dioxide molecule. Each Se=O bond length is about 162 pm in SeO₂.

Also check:-How to find bond angle?