The boiling points of haloalkenes are lower than those of haloalkanes. What could be the cause(s) of this trend? Choose all that apply. Deductions will be made for incorrect answers.

A) The pi bond lowers the polarity of the C–Cl bond which weakens the dipole-dipole forces in the molecules.

B) The pi bond increases the polarity of the C–Cl bond which weakens the dipole-dipole forces in hydrocarbons.

C) The pi bond lowers the polarity of the C–Cl bond which strengthens the dipole-dipole forces in the molecules.

D) The pi bond increases the polarity of the C–Cl bond which strengthens the dipole-dipole forces in the molecules.

E) The presence of more H atoms makes the London dispersion forces more extensive in the alkane counterparts due to an increased surface area and mass.

F) The presence of more H atoms makes the London dispersion forces stronger in alkane counterparts since it makes the molecules more polar.

G) The presence of more H atoms allows the alkane counterparts to be more tightly packed affecting their relative boiling points.