Final answer:
The ordering from lowest to highest boiling point is C₂H₆, C₃H₈, C₄H₁₀.
Step-by-step explanation:
All of these compounds are nonpolar and only have London dispersion forces: the larger the molecule, the larger the dispersion forces and the higher the boiling point. The ordering from lowest to highest boiling point is therefore C₂H₆ C₃H₈ < C₄H₁₀.
To arrange the compounds from lowest to highest boiling point, we need to take into account the forces between the molecules. The attractive forces between molecules that determine their boiling points are known as intermolecular forces.
For this situation, we have four mixtures: He, Cl2, CH3OH, and HF.
1. He (helium) has the most reduced limit. It exists as a respectable gas with powerless van der Waals powers between its molecules. These powers are extremely feeble, and helium bubbles at an exceptionally low temperature of - 268.93°C (- 452.07°F).
2. Diatomic molecule Cl2 (chlorine) has stronger van der Waals forces than helium. These powers result from the transitory shift of electron thickness, making a dipole communication. Chlorine has a limit of - 34.04°C (- 29.27°F).
3. CH3OH (methanol) is a polar particle that shows more grounded intermolecular powers contrasted with chlorine. The oxygen atom in another molecule of methanol and the hydrogen atom in methanol form a hydrogen bond. Van der Waals forces are inferior to hydrogen bonding as intermolecular forces. At 64.7°C (148.46°F), methanol boils.
4. HF (hydrogen fluoride) is likewise a polar particle, like methanol. It likewise shows hydrogen holding. Nonetheless, hydrogen fluoride has a higher limit contrasted with methanol because of the more grounded connection among hydrogen and fluorine. Hydrogen fluoride bubbles at 19.5°C (67.1°F).