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Polar molecules (such as water) carry 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 tend to move toward a certain element of the [[Molecule|molecule]] (in order to complete its outer shell and [[ | 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) leaving for example the [[Hydrogen|hydrogens]] of water lacking in [[Electrons|electrons]] (delta +ve) and the [[Oxygen|oxygen]] of the water slightly gaining in [[Electrons|electrons]] (delta -ve). | ||
Revision as of 12:23, 14 November 2011
Polar molecules (such as water) carry 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 floating around the molecule tend to move toward a certain element of the molecule (in order to complete its outer shell and bonding requirements) leaving for example the hydrogens of water lacking in electrons (delta +ve) and the oxygen of the water slightly gaining in electrons (delta -ve).