Monday, March 2, 2020

SCH 3U/4C - Molecular Dipole

Molecular Dipole

We have learned that a bond between two atoms can be polar or non-polar (pure covalent).  We have also learned that molecules are 3-D entities.  Combining these two ideas helps us to arrive at the concept of molecular dipole.  So, entire molecules can either be polar or non-polar as well.

 

Determine Polarity

For a molecule to be polar, both of the following stipulations must be met:

1.  there must be at least one polar bond in the molecule

2.  the molecule must be asymmetrical

But, how do you know if a molecule is asymmetrical?  Let's take a look-see:

A molecule is asymmetrical if the ẟ+ and ẟ- can be separated by a straight line.  In the examples below, I have indicated whether stipulation 1 and stipulation 2 have been met.  Remember - both stipulations must be met for a molecule to be considered to be polar (ie, to have a molecular dipole).


ex. H2O


 Homework 


Answer Key: