Polar covalent bond

Definition

A polar covalent bond is a type of chemical bond where electrons are shared unequally between atoms due to differences in electronegativity. This results in a molecule with a partial positive charge on one end and a partial negative charge on the other.

5 Must Know Facts For Your Next Test

1. Polar covalent bonds occur between atoms with an electronegativity difference between 0.4 and 1.7.
2. Water (H2O) is a classic example of a molecule with polar covalent bonds.
3. The unequal sharing of electrons in polar covalent bonds creates dipoles, which influence the physical properties of substances.
4. Polar covalent bonding can lead to hydrogen bonding, which is crucial for many biological molecules.
5. Molecules with polar covalent bonds tend to be soluble in water due to their ability to interact with water's polarity.

Review Questions

• What is the primary characteristic that defines a polar covalent bond?
• Why do polar covalent bonds result in molecules having partial charges?
• Can you name an example of a molecule that contains polar covalent bonds and explain its significance in biology?

Related terms

Electronegativity: A measure of an atom's ability to attract and hold onto electrons.

Dipole: A pair of equal and oppositely charged or magnetized poles separated by a distance.

Hydrogen_Bonding: A weak bond between two molecules resulting from an electrostatic attraction between a proton in one molecule and an electronegative atom in the other.