Polar And Nonpolar Covalent Bonds: Easy Explanation With Examples - Chemistry Basics

The video introduces the concept of polarity in chemistry, specifically in covalent bonds. It clarifies that polarity relates to how valence electrons are shared: equally for non-polar bonds and unequally for polar bonds. This unequal sharing is due to differences in electronegativity.

Electronegativity is defined as an atom's tendency to gain electrons or its strength in pulling on electrons. An atom with higher electronegativity pulls electrons with more strength than one with lower electronegativity.

A polar bond occurs when two covalently bonded atoms have different electronegativities, leading to unequal sharing of electrons. The atom with higher electronegativity pulls the electrons closer. This is compared to a strong polar bear and a weak polar bear sharing ice cream, where the stronger one gets more.

A non-polar bond occurs between two atoms with the same electronegativity, resulting in equal sharing of electrons. An exception is the carbon-hydrogen bond, which is considered non-polar despite a slight electronegativity difference due to its negligible impact. This is likened to two equally strong polar bears sharing ice cream.

The video provides examples: a bond between two chlorine atoms is non-polar because they have the same electronegativity, leading to equal sharing. A bond between carbon and oxygen is polar because oxygen has higher electronegativity, pulling the electrons more towards it, resulting in unequal sharing and a dipole.