Definition and properties of polar covalent bond

Before we can understand what a polar covalent bond is, we need to know what a covalent bond is. So the definition of a covalent bond is: “A covalent bond is formed by equal sharing of electrons from both the participating atoms.”

Bonding electrons are the ones that are between the two nuclei. Covalent bonds happen between two atoms that are the same or between two different atoms. Whose differences in electronegativity are not big enough to let electrons move from one atom to the other and form an ion.

Polar covalent bond

When different atoms share a covalent bond in different ways, the result is a polar covalent bond. In particular, when the difference between the electronegativity of the two atoms in the bond is between 0.4 and 1.7.

Most of the time, the terms polar bond and polar covalent bond are used the same way.

The polar covalent bond is defined as “the bond formed between two different atoms having different electronegativity.”

In a polar bond, one end of the molecule is slightly positive and the other slightly negative. Electric dipoles have less than a full unit charge. So they are called partial charges and are shown by the symbols delta plus (+) and delta minus (-).

Because the bond separates the positive and negative charges, molecules with polar covalent bonds can interact with dipoles in other molecules. This makes forces between the molecules that are dipole-dipole.

Polar covalent bonding is what keeps us alive. You drink water. A polar covalent bond is something like the H2O molecule. The electrons are not shared equally. The oxygen atom spends more time with electrons than the hydrogen atoms.

The oxygen atom has a partially negative charge because electrons spend more time with it.


Polar covalent bonds are formed between two nonmetal atoms with different electronegativity.

Let’s look at A and B, which have a covalent bond even though they have various proportions of electronegativity. The pair of electrons shared by A and B and make a bond between them move toward the more electronegative B.

Then B gets a partial negative charge, and ‘A’ gets a partial positive charge. This gives them two charges, or “poles,” and is called a “dipolar molecular” or “polar covalent.” Like H–Cl. In this molecule, the shared pair of electrons move toward the chlorine atom with the most negative charge.

Then the H atom gets a small amount of positive charge, and the Cl atom gets a small amount of negative charge. This makes a dipole.

Electronegativity is a chemical expression for how an atom tends to pull electrons toward itself. The electronegativity of an atom is affected by both its atomic number and the distance of its valence electrons from its charged nuclei.

Example of Polar Covalent bond

1. Water (H2O) is a molecule with polar bonds. Oxygen has an electronegativity of 3.44, while hydrogen has an electronegativity of 2.20. The molecule bend because the electrons are not all in the same place.

Two hydrogen atoms on the other “side” of the molecule have a net positive charge. At the same time, the oxygen atom has a net negative charge.

2. Another molecule with a polar covalent bond is hydrogen fluoride (HF). Electrons in the bond are closer to the fluorine atom than the hydrogen atom. Because fluorine is the more electronegative atom. The fluorine side has a net negative charge, and the hydrogen side has a net positive charge.

This makes a dipole. Hydrogen fluoride is a linear molecule because it only has two atoms. Which means it can’t have any other shape.

3. The polar covalent bonds between the nitrogen and hydrogen atoms in the NH3. Three positive charged hydrogen atoms are all on one side. While nitrogen atom is a negative charge.

Properties of a polar covalent compound

1. Melting and boiling point: These are more difficult to melt and boil than non-polar compounds.

2. Physical state: These compounds can form solids because their bonds are stronger.

3. Solubility: These dissolve very well in polar solvents such as water.

4. Conductivity: They conduct electricity in a solution because ions can move around.

Key points

1. A polar bond is a covalent bond where the electrons that comprise the bond are not all in the same place. Electrons spend more time on one side of the bond than on the other.

2. Polar bonds are a kind of intermediate between covalent and ionic bonds. The difference between the anion and cation in how negatively charged they are is between 0.4 and 1.7.

3. Water, hydrogen fluoride, sulfur dioxide, and ammonia are all examples of polar molecules.


Leave a Comment

Your email address will not be published. Required fields are marked *