Essay On Polar Molecules
A polar molecule has a net dipole as a result of the opposing charges (i.e. having partial positive and partial negative charges) from polar bonds arranged asymmetrically.
Water (H2O) is an example of a polar molecule since it has a slight positive charge on one side and a slight negative charge on the other. In chemistry, polarity is a separation of electric charge leading to a molecule or its chemical groups having an electric dipole or multiple moment. Polar molecules interact through dipole–dipole intermolecular force and hydrogen bonds. Molecular polarity is dependent on the difference in the electro negativity between atoms in a compound. Not all atoms attract electrons with the same force.
The amount of "pull" an atom exerts on its electrons
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A molecule may be polar either as a result of polar bonds due to differences in electro negativity as described above, or as a result of an asymmetric arrangement of non polar covalent bonds and non-bonding pairs of electrons known as a full molecular orbital.
A polar molecule has a net dipole as a result of the opposing charges. Water (H2O) is an example of a polar molecule since it has a slight positive charge on one side and a slight negative charge on the other. The dipoles do not cancel out resulting in a net dipole. Due to the polar nature of water molecule itself, polar molecules are generally able to dissolve in water. Other examples include sugars (like sucrose), which have many polar oxygen- hydrogen (-OH) groups and are overall highly polar. If the bond dipole moments of the molecule do not cancel, the molecule is polar. For example, the water molecule (H2O) contains two polar O-H bonds in a bent (nonlinear) geometry. The bond dipole moments do not cancel, so that the molecule forms a molecular dipole with its negative pole at the oxygen and its positive pole midway between the two hydrogen atoms. In the figure each bond
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