Arrange the following in order of increasing boiling points.

(A) Bromomethane
(B) Bromoform
(C) Chloromethane
(D) Dibromomethane

Choose the correct answer from the options given below:

(C), (A), (D), (B)

The correct answer is Option (1) → (C), (A), (D), (B)

Boiling point of haloalkanes increases with:

• Molecular mass
• Number of halogen atoms
• Strength of intermolecular (London dispersion) forces

Let’s compare:

• (C) Chloromethane (CH₃Cl) → lowest molar mass
• (A) Bromomethane (CH₃Br) → heavier than CH₃Cl
• (D) Dibromomethane (CH₂Br₂) → two Br atoms → higher b.p.
• (B) Bromoform (CHBr₃) → three Br atoms → highest b.p.

Increasing order of boiling points: $(C) < (A) < (D) < (B)$

(C) Chloromethane < (A) Bromomethane < (B) Bromoform <(D) Dibromomethane