Question

Statement 1 : Bromine has a higher boiling point than chlorine.
Statement 2 : Bromine has stronger dispersion forces than chlorine.

• A. Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.
• B. Both Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1.
• C. Statement 1 is correct but Statement 2 is not correct.
• D. Statement 1 is not correct but Statement 2 is correct.
• E. Both the Statement 1 and Statement 2 are not correct.

Answer 1

Answer: (A)

Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.

Statement 1 : Bromine has a higher boiling point than chlorine. This is due to the fact that the Bromine has higher , molar mass than the Chlorine.
Statement 2:
Dispersion forces are present between all molecules, whether they are polar or nonpolar.
Larger and heavier atoms and molecules $\left(Br\right)$ exhibit stronger dispersion forces than smaller and lighter ones $\left(Cl\right)$
In a larger atom or molecule, the valence electrons are, on average, farther from the nuclei than in a smaller atom or molecule. They are less tightly held and can more easily form temporary dipoles.
The ease with which the electron distribution around an atom or molecule can be distorted is called the polarizability.
London dispersion forces tend to be:
1. stronger between molecules that are easily polarized.
2. weaker between molecules that are not easily polarized.

In short "The more electrons a molecule has, the stronger the London dispersion forcesare. For example, bromine, Br2, has more electrons than chlorine, Cl2, sobromine will have stronger London dispersion forces than chlorine, resulting in a higher boiling point for bromine, 59 oC, compared to chlorine, –35 oC."