Question

Which statement below matches the correct response with the proper reasoning when comparing the volatility of CH2Cl2 with CH2Br2? a. CH2Cl2 is more volatile than CH2Br2 because the dipole-dipole interactions in CH2Cl2 are greater than the dipole-dipole interactions in CH2Br2. b. CH2Cl2 is more volatile than CH2Br2 because of the large dispersion forces in CH2Br2. c. CH2Br2 is more volatile than CH2Cl2because because the dipole-dipole interactions in CH2Br2 are greater than the dipole-dipole interactions in CH2Cl2d. CH2Br2 is more volatile than CH2Cl2 because of the large dispersion forces in CH2Br2

Answer 1

b. CH₂Cl₂ is more volatile than CH₂Br₂ because of the large dispersion forces in CH₂Br₂

Step-by-step explanation:

CH₂Cl₂ is more volatile than CH₂Br₂ (b.p of CH₂Cl₂ = 39,6 °C; b.p of CH₂Br₂ = 96,95°C). Thus, c. and d. are FALSE

Dipole-dipole interactions in CH₂Cl₂ are greater than the dipole-dipole interactions in CH₂Br₂ because Cl is more electronegative that Br (Cl = 3,16; Br = 2,96). But this mean CH₂Cl₂ is less volatile than CH₂Br₂ but it is false.

There are large dispersion forces in CH₂Br₂ because Br has more electrons and protons than Cl. Large disperson forces mean CH₂Br₂ is less volatile than CH₂Cl₂ and it is true.

I hope it helps!