Intermolecular Forces Question 1

\begin{array}{|l|c|c|} \hline \text{Name} & \text{Molecular} & \text{Molar Mass} \\ & \text{Formula} & \text{(g/mol)} \\ \hline \text{Ethane} & \ce{C2H6} & 30 \\ \hline \text{Butane} & \ce{C4H10} & 58 \\ \hline \end{array}

The molecular formula and molar mass of two straight-chain hydrocarbons are listed in the table above. Based on the information in the table, which compound has the higher boiling point, and why is that compound's boiling point higher?

\ce{C4H10}

, because it has more hydrogen atoms, resulting in more hydrogen bonding

\ce{C4H10}

, because it has more electrons, resulting in greater polarizability and stronger dispersion forces

\ce{C2H6}

, because its molecules are smaller and they can get closer to one another, resulting in stronger dispersion forces

\ce{C2H6}

, because its molecules are more polar, resulting in stronger dipole-dipole attractions