Answer the problem below:

Answer:1. List the following compounds from highest boiling to lowest boiling: The order of the compounds from highest boiling point to lowest boiling point is determined by the strength of their intermolecular forces. Stronger intermolecular forces lead to higher boiling points. The compounds shown contain hydrogen bonding, dipole-dipole interactions, and London dispersion forces. Hydrogen bonding is the strongest of these, followed by dipole-dipole interactions, and then London dispersion forces. Here's the ranking, with reasoning: 1. CH_3CH_2CH_2OH: This molecule has a hydroxyl group (-OH), allowing for strong hydrogen bonding, resulting in the highest boiling point. 2. CH_3CH_2COOH: This molecule also has a hydroxyl group (-OH) capable of strong hydrogen bonding, but the presence of the carbonyl group (C=O) reduces the overall strength of hydrogen bonding compared to the previous molecule. 3. CH_3CH_2CH_2NH_2: This molecule has an amino group (-NH2), which also allows for hydrogen bonding, but generally weaker than the hydroxyl group. 4. CH_3CH_2CH_2CH_3: This molecule is a nonpolar alkane. It only exhibits weak London dispersion forces, resulting in a low boiling point. 5. CH_3CH_2CHO: This molecule has a carbonyl group (C=O), which is polar and leads to dipole-dipole interactions. However, it lacks hydrogen bonding, resulting in a lower boiling point compared to the molecules with -OH or -NH2 groups. 6. (CH_3)_2NH: This molecule has a secondary amine group, which can participate in hydrogen bonding, but less effectively than a primary amine or a hydroxyl group. The steric hindrance from the two methyl groups also reduces the effectiveness of hydrogen bonding. Therefore, the final order is: CH_3CH_2CH_2OH > CH_3CH_2COOH > CH_3CH_2CH_2NH_2 > (CH_3)_2NH > CH_3CH_2CHO > CH_3CH_2CH_2CH_3

Answered by rosalyncarillo29 | 2025-04-24