In large molecules, the molecular polarity molecular polarity depends on both the bond shape and bond polarity. When there is a polar bond, it doesn't necessarily mean that the molecule is polar; the shape and the atoms around the central atom must be considered. Example for AX[tex]_{2}[/tex]: BeCl[tex]_{2}[/tex] - both Be-Cl bonds in this molecule are polar because of the difference in electronegativity, but the molecule has no polarity because the molecule shape is linear (180∘∘) and both polarities cancel each other.
Example for AXn (n >> 2):SO[tex]_{2}[/tex] (AX[tex]_{2}[/tex]E) - we can see that there is assymetric distribution of electron between S and O atoms; there are more electrons around more electronegative O atom. This makes permanent dipole moment, which makes SO[tex]_{2}[/tex] molecule. Polarities doesn't cancel because the molecule is V shaped.
When there is a lone electron pair around central atom, that changes the molecule shape in a way that polarities cannot cancel each other, then the molecule is polar - AXnEn
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