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Ethanol has a higher boiling point than dimethyl ether though they have the same molecular weight. This is due to :
- a)Resonance
- b)Coordinate bonding
- c)Hydrogen bonding
- d)Ionic bonding
Correct answer is option 'C'. Can you explain this answer?
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Ethanol has a higher boiling point than dimethyl ether though they hav...
⇒ due to intermolecular H-bond, it has higher b.p. than CH3OCH3
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Ethanol has a higher boiling point than dimethyl ether though they hav...
Introduction
Ethanol and dimethyl ether both have the same molecular weight, yet ethanol has a higher boiling point. The key reason for this difference lies in the type of intermolecular forces present in each substance.
Intermolecular Forces
- Ethanol (C2H5OH) contains an -OH (hydroxyl) group.
- Dimethyl ether (C2H6O) has an ether functional group (C-O-C) without the ability to form hydrogen bonds.
Hydrogen Bonding in Ethanol
- Ethanol can form hydrogen bonds due to the presence of the hydroxyl group.
- Hydrogen bonds occur when a hydrogen atom is attracted to a highly electronegative atom (like oxygen).
- These bonds create strong attractions between ethanol molecules, requiring more energy (higher temperature) to break them apart during boiling.
Lack of Hydrogen Bonding in Dimethyl Ether
- Dimethyl ether, while polar, cannot form hydrogen bonds as effectively because it lacks an -OH group.
- Instead, it relies on weaker dipole-dipole interactions and London dispersion forces.
- As a result, less energy is needed to overcome these forces, leading to a lower boiling point.
Conclusion
- The significant difference in boiling points between ethanol and dimethyl ether can be attributed to the presence of hydrogen bonding in ethanol.
- This interaction leads to stronger intermolecular forces compared to the weaker forces in dimethyl ether, thus resulting in a higher boiling point for ethanol.
Ethanol and dimethyl ether both have the same molecular weight, yet ethanol has a higher boiling point. The key reason for this difference lies in the type of intermolecular forces present in each substance.
Intermolecular Forces
- Ethanol (C2H5OH) contains an -OH (hydroxyl) group.
- Dimethyl ether (C2H6O) has an ether functional group (C-O-C) without the ability to form hydrogen bonds.
Hydrogen Bonding in Ethanol
- Ethanol can form hydrogen bonds due to the presence of the hydroxyl group.
- Hydrogen bonds occur when a hydrogen atom is attracted to a highly electronegative atom (like oxygen).
- These bonds create strong attractions between ethanol molecules, requiring more energy (higher temperature) to break them apart during boiling.
Lack of Hydrogen Bonding in Dimethyl Ether
- Dimethyl ether, while polar, cannot form hydrogen bonds as effectively because it lacks an -OH group.
- Instead, it relies on weaker dipole-dipole interactions and London dispersion forces.
- As a result, less energy is needed to overcome these forces, leading to a lower boiling point.
Conclusion
- The significant difference in boiling points between ethanol and dimethyl ether can be attributed to the presence of hydrogen bonding in ethanol.
- This interaction leads to stronger intermolecular forces compared to the weaker forces in dimethyl ether, thus resulting in a higher boiling point for ethanol.
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Ethanol has a higher boiling point than dimethyl ether though they have the same molecular weight. This is due to :a)Resonanceb)Coordinate bondingc)Hydrogen bondingd)Ionic bondingCorrect answer is option 'C'. Can you explain this answer?
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