Water,Ethanol,and Ether are all liquids at ro | vedclass

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(B) The boiling point of a liquid depends on the strength of the intermolecular forces holding the molecules together. $1$. Water $(H_2O)$ exhibits st

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Due to differences in the strength of intermolecular forces.

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(B) The boiling point of a liquid depends on the strength of the intermolecular forces holding the molecules together. $1$. Water $(H_2O)$ exhibits strong hydrogen bonding,leading to a high boiling point of $100 \ ^\circ C$. $2$. Ethanol $(C_2H_5OH)$ also exhibits hydrogen bonding,but it is weaker than in water due to the presence of the hydrophobic ethyl group,resulting in a boiling point of $78 \ ^\circ C$. $3$. Diethyl ether $((C_2H_5)_2O)$ lacks hydrogen bonding and is held together by weaker dipole-dipole interactions,resulting in a much lower boiling point of $34.6 \ ^\circ C$. Therefore,the difference in boiling points is primarily due to the varying strength of intermolecular forces.

Water,Ethanol,and Ether are all liquids at room temperature; why do their boiling points differ?

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