In chemistry, the bonds will be shared between two atoms. There are many types of bonds available. But the two most commonly used bonds in chemistry for sharing electrons are covalent and the other one is polar covalent.
Key Takeaways
- Covalent bonds involve equal sharing of electrons between atoms, while polar covalent bonds have unequal electron distribution.
- Nonpolar covalent molecules are electrically neutral, whereas polar ones have partial positive and negative charges.
- Polar covalent bonds result in polar molecules interacting via dipole-dipole forces, while nonpolar covalent molecules experience weaker dispersion forces.
Covalent vs Polar Covalent
The difference between Covalent and Polar Covalent is that they have a shared pair of electrons, and the electrons are in an unpaired stage, which is called a covalent bond. Polar covalent bonds are used to name polar bonds in covalent bonds. In covalent bonds, you can either see the dipole moment or cannot. But in polar covalent, you can see the dipole moment.
Covalent bonds are formed with the atoms. A bond can be identified, whether it is covalent or non-covalent, by looking at the periodic table.
Some of the characteristics a non-polar covalent bond should possess are the electrons should be equally shared between the atoms. In non-polar covalent, you will be able to find that the electronegativity difference between them is 0.
Comparison Table
| Parameters of Comparison | Covalent | Polar Covalent |
|---|---|---|
| Definition | They are chemical bonds that are created by unpaired electrons between the atoms. | This is used to name the polar covalent bonds |
| Polarity | Covalent can sometimes be polar and sometimes non-polar | Polar covalent are always polar |
| Charge Separation | They can have either electronic charge separation or not | They show some slight electronic charge separation |
| Dipole moment | They either show or don’t | They can show the dipole moment |
| Electrons | Electrons are shared equally | Electrons are not shared equally |
What is Covalent?
It is an interatomic linkage when electronic pair is shared between two atoms. This will be formed when they have lower energy than the widespread atoms.
One of the best examples to describe covalent bonds is with the help of carbon dioxide molecules. This molecule has one carbon atom and two oxygen atoms, which makes it very stringer because two electron pairs are shared.
This, in turn, will create a long chain and will allow the much-needed complexity in life. Atoms will bond with other atoms in the covalent bond so that they will be able to gain stability.
What is Polar Covalent?
Atoms that share electrons even though they are from different electronegativities are called polar covalent. Partial negative sharing will happen when the bonding pairs are unequally shared.
The best example of polar covalent is water. We can even find whether the bond is polar or non-polar by checking its electronegativity difference. If the electronegativity difference is less than 0.4, they are considered non-polar.
A non-polar covalent bond will be formed when they have two hydrogen atoms, and the electrons will be equally shared. SO2 bond is considered a polar covalent bond because you can find the electronegativity difference between sulphur and oxygen atoms.
Main Differences Between Covalent and Polar Covalent
- Covalent bonds can either show dipole moments or cannot. On the other hand, polar covalent will always show dipole moment.
- In covalent bonds, electrons will be shared equally. On the other hand, in polar covalent, the electrons are not shared equally.
- https://pubs.acs.org/doi/abs/10.1021/jp8106183
- https://journals.aps.org/prl/abstract/10.1103/PhysRevLett.91.015502
Last Updated : 11 June, 2023
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Piyush Yadav has spent the past 25 years working as a physicist in the local community. He is a physicist passionate about making science more accessible to our readers. He holds a BSc in Natural Sciences and Post Graduate Diploma in Environmental Science. You can read more about him on his bio page.
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The explanation of how non-polar covalent bonds are formed and how the electronegativity difference determines polarity is very informative and thorough.
The detailed explanation of dipole moments in covalent and polar covalent bonds is helpful for understanding molecular behavior.
Understanding the nature of chemical bonds is essential in chemistry. The comparison table provided in the article is concise and helpful in differentiating between covalent and polar covalent bonds.
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The examples of carbon dioxide and water help illustrate the concepts of covalent and polar covalent bonds. It’s good to see real-world applications being used to explain these scientific principles.