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Report (any type)/Brief report
22/09/2021
Here’s why that happens.
Carbon tetrachloride, ##”CCl”_4##, is a nonpolar molecule because of its .
In order for a molecule to be polar, it must have a net dipole moment. In the case of carbon tetrachloride, that net dipole moment is equal to zero.
Here’s why that is the case.
The ##”C” -“Cl”## bond is indeed quite polar. Chlorine is more electronegative than carbon, which means that it will attract the electrons more.
Consequently, a partial negative charge, ##delta^(-)##, will appear on the chlorine atom and a partial positive charge, ##delta^(+)##, will appear on the carbon atom.
A bond dipole moment will thus appear for each of the four ##”C”-“Cl”## bonds that exist in a molecule of carbon tetrachloride. Because these four bonds are identical, theese dipole moments will also be identical in magnitude.
Now, carbon tetrachloride has a tetrahedral molecular geometry. This means that the resultant of any three ##”C”-“Cl”## bonds will always
with the fourth. In other words, no net dipole moment will exist because the four bond dipole moments that arise from the polar ##”C”-“Cl”## bonds will cancel each other out.
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I want to thank your team (Jeff) for finding a new writer when you were unable to reach my existing writer to revise my paper. I appreciate your professionalism and efforts. Thanks
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