Question

the data below shows the change in temperature when 4 compounds are exposed to room temperature air over 2 minutes. which compound has the strongest intermolecular forces? \

$$\begin{tabular}{|c|c|c|} \\hline compound & temperature change (°c) & type of imf \\\\ \\hline a & -12.5 & df \\\\ \\hline b & -9.2 & df \\\\ \\hline c & -7.6 & df, dd \\\\ \\hline d & -4.8 & df, dd, hb \\\\ \\hline \\multicolumn{3}{|c|}{df -- dispersion forces, dd -- dipole-dipole,} \\\\ \\multicolumn{3}{|c|}{hb -- hydrogen bonding} \\\\ \\hline \\end{tabular}$$

\

$$\begin{tabular}{|c|} \\hline compound d \\\\ \\hline compound c \\\\ \\hline compound a \\\\ \\hline compound b \\\\ \\hline \\end{tabular}$$

Explanation:

Evaporation is endothermic—compounds with stronger intermolecular forces (IMFs) require more energy to overcome forces, so they evaporate less, causing a smaller temperature drop. Compound D has the smallest temperature change (-4.8°C) and the most IMFs (dispersion, dipole-dipole, hydrogen bonding), indicating the strongest IMFs.

Answer:

compound D