. Advertisement .
..3..
. Advertisement .
..4..
......... ADVERTISEMENT ......... ..8..
Which of these molecules are polar? Check all that apply.
......... ADVERTISEMENT .........
..8..
A. PCl3
B. SO2
C. CO2
D. CH2Cl2
♦ Relevant knowledge
When two different atoms create chemical bonds and share electrons, the bond is in the direction of the atom with the greater electronegative. The chemical bond is thought to be an polar bond. Molecules with dipole moments that are permanent are considered to be Polar and are regarded as dipoles.
If the electronegativity between the bonded atoms is different, then the bond may be polar. Some molecules may contain polar bonds but others might not. If all the bonds in the molecule have opposite polarities, then the molecule is considered non-polar.
If an atom in a bond is more electronegative than another atom, the highly electronegative one attracts more electrons than its share. Partial negative charge is created on the highly-electronegative atom, and partial positive charge on the less electronegative.
These are the structures and directions of the dipolemoment bonds:
These are the results of all dipolemoments in the molecules.
The polar molecules are therefore [katex]{\rm{PC}}{{\rm{l}}_3}{\rm{,}}\,\,{\rm{S}}{{\rm{O}}_2}\,\,{\rm{and}}\,\,{\rm{C}}{{\rm{H}}_2}{\rm{C}}{{\rm{l}}_2}[/katex]
Ans
The polar molecules therefore are [katex]{\rm{PC}}{{\rm{l}}_3}{\rm{,}}\,\,{\rm{S}}{{\rm{O}}_2}\,\,{\rm{and}}\,\,{\rm{C}}{{\rm{H}}_2}{\rm{C}}{{\rm{l}}_2}[/katex]