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Chemical polarity
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===Nonpolar molecules=== A molecule may be nonpolar either when there is an equal sharing of electrons between the two atoms of a diatomic molecule or because of the symmetrical arrangement of polar bonds in a more complex molecule. For example, [[boron trifluoride]] (BF<sub>3</sub>) has a trigonal planar arrangement of three polar bonds at 120Β°. This results in no overall dipole in the molecule. [[File:Boron-trifluoride-elpot-3D-vdW.png|thumb|right|In a molecule of [[boron trifluoride]], the trigonal planar arrangement of three polar bonds results in no overall dipole.]] [[File:Carbon dioxide structure.png|thumb|left|Carbon dioxide has two polar C-O bonds in a linear geometry.]] [[Carbon dioxide]] (CO<sub>2</sub>) has two polar C=O bonds, but the geometry of CO<sub>2</sub> is linear so that the two bond dipole moments cancel and there is no net molecular dipole moment; the molecule is nonpolar. [[File:Methane-CRC-MW-3D-balls.png|thumb|left|In [[methane]], the bonds are arranged symmetrically (in a tetrahedral arrangement) so there is no overall dipole.]] Examples of household nonpolar compounds include fats, oil, and petrol/gasoline. In the [[methane]] molecule (CH<sub>4</sub>) the four CβH bonds are arranged tetrahedrally around the carbon atom. Each bond has polarity (though not very strong). The bonds are arranged symmetrically so there is no overall dipole in the molecule. The diatomic [[oxygen]] molecule (O<sub>2</sub>) does not have polarity in the covalent bond because of equal electronegativity, hence there is no polarity in the molecule.
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