To determine which compound in each pair would have the higher boiling point, we need to consider the intermolecular forces present in each compound.

In the first pair, we have CH3CH2CH2OH (1-butanol) and CH3CH2OCH3 (diethyl ether). Both compounds have similar molecular weights, but 1-butanol has a higher boiling point. This is because 1-butanol can form hydrogen bonds between the oxygen atom and the hydrogen atoms of neighboring molecules. Diethyl ether, on the other hand, cannot form hydrogen bonds. The presence of hydrogen bonding in 1-butanol leads to stronger intermolecular forces, resulting in a higher boiling point.

In the second pair, we have CH3CH2CH2OH (1-butanol) and HOCH2CH2OH (ethylene glycol). Both compounds can form hydrogen bonds, but ethylene glycol has a higher boiling point. This is because ethylene glycol has two hydroxyl groups, allowing for more hydrogen bonding interactions compared to 1-butanol, which only has one hydroxyl group. The increased number of hydrogen bonds in ethylene glycol leads to stronger intermolecular forces and a higher boiling point.

In summary, the compound with stronger intermolecular forces, such as the ability to form hydrogen bonds, will generally have a higher boiling point.

Question

To determine which compound in each pair would have the higher boiling point, we need to consider the intermolecular forces present in each compound.

In the first pair, we have CH3CH2CH2OH (1-butanol) and CH3CH2OCH3 (diethyl ether). Both compounds have similar molecular weights, but 1-butanol has a higher boiling point. This is because 1-butanol can form hydrogen bonds between the oxygen atom and the hydrogen atoms of neighboring molecules. Diethyl ether, on the other hand, cannot form hydrogen bonds. The presence of hydrogen bonding in 1-butanol leads to stronger intermolecular forces, resulting in a higher boiling point.

In the second pair, we have CH3CH2CH2OH (1-butanol) and HOCH2CH2OH (ethylene glycol). Both compounds can form hydrogen bonds, but ethylene glycol has a higher boiling point. This is because ethylene glycol has two hydroxyl groups, allowing for more hydrogen bonding interactions compared to 1-butanol, which only has one hydroxyl group. The increased number of hydrogen bonds in ethylene glycol leads to stronger intermolecular forces and a higher boiling point.

In summary, the compound with stronger intermolecular forces, such as the ability to form hydrogen bonds, will generally have a higher boiling point.

Knowee AI · Accepted Answer

To determine which compound in each pair would have the higher boiling point, we need to consider the intermolecular forces present in each compound.

In the first pair, we have CH3CH2CH2OH (1-butanol) and CH3CH2OCH3 (diethyl ether). Both compounds have similar molecular weights, but 1-butanol has a higher boiling point. This is because 1-butanol can form hydrogen bonds between the oxygen atom and the hydrogen atoms of neighboring molecules. Diethyl ether, on the other hand, cannot form hydrogen bonds. The presence of hydrogen bonding in 1-butanol leads to stronger intermolecular forces, resulting in a higher boiling point.

In the second pair, we have CH3CH2CH2OH (1-butanol) and HOCH2CH2OH (ethylene glycol). Both compounds can form hydrogen bonds, but ethylene glycol has a higher boiling point. This is because ethylene glycol has two hydroxyl groups, allowing for more hydrogen bonding interactions compared to 1-butanol, which only has one hydroxyl group. The increased number of hydrogen bonds in ethylene glycol leads to stronger intermolecular forces and a higher boiling point.

In summary, the compound with stronger intermolecular forces, such as the ability to form hydrogen bonds, will generally have a higher boiling point.

Which compound in each of the following pairs would have the higher boiling point ? Explain your answers.CH3CH2CH2OHorCH3CH2OCH3CH3CH2CH2OHorHOCH2CH2OH

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Which compound in each of the following pairs would have the higher boiling point? Explain your answers.

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