Polar molecules
Chemical bonding is the result of either an atom sharing one or more outer orbit electrons with another atom or an atom taking outer orbit electrons from the atom with which it is bonding. Normally, an atom has an even distribution of electrons in the orbits or shells, but if more end up on one side that the other in a molecule, there can be a resulting electrical field in that area.
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Water
Water is a polar molecule because of the way the atoms bind in the molecule such that there are excess electrons on the Oxygen side and a lack or excess of positive charges on the Hydrogen side of the molecule.
Water is a polar molecule with positive charges
on one side and negative on the other
Gases
Examples of polar molecules of materials that are gases under standard conditions are: Ammonia (NH3), Sulfur Dioxide (SO2) and Hydrogen Sulfide (H2S).
Non-polar molecules
A non-polar molecule is one that the electrons are distributed more symmetrically and thus does not have an abundance of charges at the opposite sides. The charges all cancel out each other.
The electrical charges in non-polar Carbon Dioxide are evenly distributed
Liquids
Most hydrocarbons are non-polar molecules. Examples include Toluene and Gasoline. (SeeHydrocarbon Bonding for more information.)
Gases
Common examples of non-polar gases are the noble or inert gases, including Helium (He), Neon (Ne), Krypton (Kr) and Xenon (Xe). Other non-polar gases include the Hydrogen (H2), Nitrogen (N2), Oxygen (O2), Carbon Dioxide (CO2), Methane (CH4) and Ethylene (C2H4) molecules.