Currently Internet Explorer is not working properly with our website. Please use the Chrome, Firefox or Safari browsers for a better user experience.

Polar Bond

You do not have access to this lesson.

The following is a limited nonfunctional preview of the actual lesson.


Hydrogen; oxygen

Preview mode...

Chemical bond

Preview mode...

Polar bond

Preview mode...

Polar Bonds

Since the atoms of most elements do not have full outer electron shells, they tend to react with one another to form compounds with a more noble gas like electron configuration. Not all chemical bonds fall fully under ionic or covalent, as there are many that lie somewhere between the two extremes. A polar bond is a covalent bond in which the individual atoms exert different attractions for the shared electrons. This results in an uneven distribution of charge and a molecule with one slightly positively charged end and one slightly negatively charged end.


The prime example of polar bonding is water. The Oxygen end has a slightly positive charge, while the Hydrogen ends are slightly negative. Other polar molecules dissolve readily in water, while non-polar molecules do not.

Demonstration mode. Purchase course to view.

This is the default dialog which is useful for displaying information. The dialog window can be moved, resized and closed with the 'x' icon.