View source for Polar

Polar molecules (such as [[Water|water]]) carry [[Dipole charge|dipole charges]] (slight positives and negatives) meaning that they tend to be very good solvents and have higher than predicted boiling points. The polar ends of the molecule are created because the [[Electrons|electrons]] floating around the [[Molecule|molecule]] tend to move toward a certain element of the [[Molecule|molecule]] (in order to complete its outer shell and [[Bonding|bonding]] requirements)&nbsp;leaving for example the [[Hydrogen|hydrogens]] of water lacking in&nbsp;[[Electrons|electrons]] (delta +ve) and the [[Oxygen|oxygen]] of the water slightly&nbsp;gaining in [[Electrons|electrons]] (delta -ve). 

<br> 

Polarity is determined by the [[Electronegativity|electronegativity]] of the elements within the molecule. For example in [[Water|water]], [[Oxygen|Oxygen]] has a higher [[Electronegativity|electronegativity]] than [[Hydrogen|Hydrogen]] so the shared [[Electrons|electrons]]&nbsp;within the molecule are drawn to the [[Oxygen|oxygen]] atom more than two [[Hydrogen|hydrogen]] atoms. Since the negatively charged electrons have moved towards the oxygen it becomes slightly negative and the hydrogen slighlty positive.