For each pair of compounds listed, check the box next to the one with the higher boiling point.compounds higher boiling pointSi3H8 Si2H6 CH3CH3 CH3CH22CH3 He Ne

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The boiling point of a compound is determined by the type and strength of the intermolecular forces present. These forces include London dispersion forces, dipole-dipole interactions, and hydrogen bonding.

1. Si3H8 vs Si2H6: Si3H8 has a higher boiling point. The more complex the molecule (more atoms), the higher the boiling point due to increased London dispersion forces.

2. CH3CH3 (Ethane) vs CH3CH2CH3 (Propane): Propane (CH3CH2CH3) has a higher boiling point. Again, the larger molecule has stronger London dispersion forces.

3. He vs Ne: Ne has a higher boiling point. As you go down the periodic table, boiling points increase due to increased London dispersion forces. Ne (Neon) is below He (Helium) on the periodic table.