Carbon tetrachloride, CCl4 is used as a solvent and a coolant. Its boiling point I s-22.9 degrees. By considering the intermolecular forces involved discuss whether you expect the boiling point of CHCL3 to be greater or lower than tis value. [6]
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Look at the intermolecular forces for each and remember that CCl4 is not polar while CHCl3 is.
To determine whether the boiling point of CHCl3 (chloroform) is greater or lower than that of CCl4 (carbon tetrachloride), we need to consider the intermolecular forces involved in both compounds.
Both CHCl3 and CCl4 are nonpolar molecules, meaning that they have only carbon-hydrogen (CH) or carbon-chlorine (CCl) bonds and no polar bonds. Nonpolar molecules generally exhibit weak intermolecular forces, such as London dispersion forces (also known as van der Waals forces).
In the case of CCl4, it is a larger molecule with more electrons, which results in stronger London dispersion forces. These forces hold the CCl4 molecules together and require more energy to overcome, resulting in a higher boiling point.
On the other hand, CHCl3 is a smaller molecule, so it has fewer electrons and weaker London dispersion forces compared to CCl4. This means that the intermolecular forces in CHCl3 are generally lower, leading to a lower boiling point.
Therefore, we expect the boiling point of CHCl3 to be lower than that of CCl4 based on the intermolecular forces involved.