Hello friends, you might have many doubts regarding the polarity in some molecules in the chemistry world. Many of us have a doubt regarding the polarity of SO2 (sulfur dioxide). So, I will share my information with you to clear the doubt regarding the polarity of SO2.
Is SO2 polar or nonpolar? SO2 is polar in nature because of the difference in electronegativity between sulfur and oxygen atoms. The greater the difference in electronegativity more will be the polarity of the molecule. The bent shape of SO2 is because of the repulsion between the unbonded electrons present on the sulfur and oxygen atoms. The unsymmetrical shape also identifies whether a molecule is polar or not.
Why is SO2 Polar?
In the SO2 molecule, the Sulfur has 6 electrons in its vacant shell and Oxygen also has 6 electrons in its vacant shell. 4 electrons of sulfur bond with the two pairs of electrons from both oxygen atoms around sulfur.
And after bonding in the SO2 molecule, the unequal charge remains on Sulfur and Oxygen. 2 unbonded electrons remain on Sulfur and 4 electrons on both of the Oxygen atoms.
Therefore, unequal charge distribution occurs after the bonding of the SO2 molecule. The lone pair present on Sulfur and lone present on Oxygen atoms cause repulsion between each other.
Oxygen is more electronegative than Sulfur, as a result, the Oxygen-Sulfur bond shares unequal charge distribution, and the bond formed in it is polar.
According to the VSEPR theory, the repulsion between two lone pairs is greater than the repulsion between the lone pair and bond pair.
Similarly, in the SO2 case, the lone pair present on Sulfur and Oxygen atoms produces repulsion between them.
In such cases as SO2, where more than one lone pair group is present, the geometrical shape of the molecule is slightly different as compared to the molecule where all groups are bonds.
Factors affecting the polarity of a chemical compound
The polarity of a molecule is decided based on the unequal charge distribution of the atoms involved in the molecule. The unequal charge distribution results in the net dipole moment.
The molecule which has a non-zero value of net dipole moment is polar whereas the molecule which has net dipole moment equals zero is non-polar. The CO2, O2 is an example of non-polar molecules.
You can read out the article for the reason of the non-polarity of CO2.
The molecules that have zero net dipole moment is due to equal charge distribution on the atoms in the molecule. Therefore, the dipole moment gets canceled out and results in a net-zero dipole moment.
Dipole moment = Bond length * charge on each element
The calculated dipole moment of SO2 (sulfur dioxide) is 1.6 debyes.
It is better to understand that the difference in electronegativity is one of the main factors that affects polarity.
The polarity of a molecule is directly proportional to the difference between the electronegativities of the atoms involved in the molecule.
The polarity and non-polarity of a molecule depends on the various factors such as
- Molecular geometry of the molecule
- The number of identical atoms present.
- The number of lone pairs present in the molecule.
- The symmetry of the molecule.
In the world of chemistry, electronegativity is a measure of how strongly an atom can attract an electron towards itself.
More electronegative atom can strongly attract electron and low electronegative atom can weakly attract the electron.
SO2 Bond Angle
The SO2 molecule forms the shape of the trigonal planar. The lone pair repulsion among the Oxygen and Sulfur forms a bent shape and the angle between the bonds is found to be around 119-120 degrees.
The position of the atoms in the SO2 is such that the Sulfur atom is present in the center/between both of the Oxygen atoms.
However, the lone pair present on the Sulfur atom causes repulsion with the lone pair present on the Oxygen atoms resulting in the V-shape/bent-shaped SO2 molecule.
The bond angle in SO2 = 120 degrees.
For more detailed information regarding geometry, hybridization, and lewis structure of SO2, you should also refer to the article on the lewis structure of SO2.
Polar and Non-Polar Compounds
We all should understand that when two atoms form a bond, they basically share electrons from each other.
And also, it is important to keep in mind that two different atoms do not equally share the electron of each other. It is because of the electronegativity difference.
The atom with more electronegativity attracts the pair of bonded electrons toward itself as compared to the atom of lesser electronegativity.
As per the studies already done, the bond formed between two atoms is polar covalent if the electronegativity difference lies between 0.5 and 1.6.
In this bond, the center of negative charge does not lie in the center. It would be at the end of an atom with greater electronegativity.
And if the electronegativity difference is lesser than 0.5, the bond is non-polar covalent. Whereas, if the electronegativity difference is above 2, the bond is ionic.
For example, in the case of SO2, Oxygen has a higher electronegativity than Sulfur and it makes it polar. The electronegativity of Sulfur is 2.58 whereas the electronegativity of Oxygen is 3.44.
And in the case of NaCl, the Chlorine atom has a higher electronegativity than Sodium, due to which the Chlorine atom pulls the electron shared pair towards itself.
If you are a student of science, it is very helpful to remember that as you move right in the periodic table of chemistry, the electronegativity of elements gets higher.
Also, as you move up in the periodic table, the electronegativity of the elements gets higher.
Thus, if you want to check if a molecule is polar or not.
You should note down the value of electronegativity of atoms involved in the molecule, the number of lone pairs and bonds.
And the overall geometrical shape of the molecule. This information is sufficient to conclude whether the molecule is polar or non-polar.
In this article, I tried to cover the polarity of sulfur dioxide, and the factors that affect the polarity, how to check the polarity of a molecule with the information required to conclude.
I hope, I cleared your all doubts regarding the polarity of SO2 and also made you understand the fundamentals of the polar and non-polar bonds.