Answer :
CBr4 has a higher boiling point than CCl4 because it is more massive, which contributes to stronger London dispersion forces and a resulting higher boiling point. Option 2) is correct.
The higher boiling point of CBr4 compared to CCl4 can be attributed to the strength of the intermolecular forces between their molecules. The strength of these forces often increases with the number of electrons present in the molecules, thereby increasing as the molecular mass increases. Out of the given options, this explains why Option 2: 'CBr4 molecules have stronger London dispersion forces' is the correct answer.
The London dispersion forces are the weakest type of van der Waals force, but they become significant in larger and heavier atoms. Since bromine atoms are heavier than chlorine atoms, CBr4 is more massive than CCl4, leading to stronger London dispersion forces, a higher boiling point, and hence a lower vapor pressure at a given temperature.
The answer is Option 2: CBr4 molecules have stronger London dispersion forces.
What's the boiling point?
London dispersion forces are the weakest of the intermolecular forces, but they are also the most prevalent. They are caused by the temporary uneven distribution of electrons in a molecule, which creates a temporary dipole. This temporary dipole can then induce a dipole in a neighboring molecule, resulting in a weak attractive force.
The strength of London dispersion forces increases with the size and polarizability of the molecule. Since bromine is larger and more polarizable than chlorine, CBr4 molecules have stronger London dispersion forces than CCl4 molecules. This is why CBr4 has a higher boiling point than CCl4.
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