Electronegativity differences explain Polar bonds in covalent compounds

Polar bonds are the result of two atoms having a substantial difference in electronegativity values. Electronegativity is a measure of an atom's ability (strength) to pull bonding electrons towards itself.  Fluorine is the most electronegative atom with a value of 4.0.  If the electronegativity difference is greater than 0.4 or 0.5, the difference is enough to cause the bond to be "polar" or lopsided.  This lopsided bond, or distorted electron density, causes the bond to behave similarly to a magnet (with a north pole & south pole).  If the polar bonds to not cancel each other out, then the entire molecule will be polar, which has many implications in its solubility, its boiling point, etc.

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