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What is the dominant intermolecular force or bond that must be overcome in converting liquid CH3CH2OH to vapours?
- a)H-bonding
- b)Dipole-dipole interactions
- c)Covalent bonds
- d)London dispersion force
Correct answer is option 'A'. Can you explain this answer?
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What is the dominant intermolecular force or bond that must be overcom...
CH3CH2OH is in liquid state due to association as a result of intermolecular H-bonding.
Most Upvoted Answer
What is the dominant intermolecular force or bond that must be overcom...
In alcohols there is presence of hydrogen bonding between molecules which makes it able to lose electrons if compared to corresponding alkanes which have the presence of Van dar Waals forces.
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What is the dominant intermolecular force or bond that must be overcom...
Intermolecular Forces in CH3CH2OH
Intermolecular forces are the forces of attraction or repulsion that exist between molecules. In the case of converting liquid CH3CH2OH (ethanol) to vapors, the dominant intermolecular force that must be overcome is hydrogen bonding.
Hydrogen Bonding
Hydrogen bonding is a strong type of dipole-dipole interaction that occurs when hydrogen is attached to a highly electronegative atom such as oxygen, nitrogen, or fluorine. In the case of ethanol (CH3CH2OH), the hydrogen atom attached to the oxygen atom forms hydrogen bonds with other ethanol molecules.
Overcoming Hydrogen Bonding
In order to convert liquid ethanol to vapors, these hydrogen bonds must be broken. This requires additional energy input to overcome the strong attraction between the hydrogen atom and the electronegative oxygen atom in neighboring molecules.
Other Intermolecular Forces
While dipole-dipole interactions, London dispersion forces, and covalent bonds also play a role in the overall behavior of ethanol molecules, hydrogen bonding is the dominant force that must be overcome in the process of converting liquid ethanol to vapors.
In conclusion, hydrogen bonding is the primary intermolecular force that must be disrupted in order to vaporize liquid ethanol. This requires additional energy input to break the strong attractions between ethanol molecules.
Intermolecular forces are the forces of attraction or repulsion that exist between molecules. In the case of converting liquid CH3CH2OH (ethanol) to vapors, the dominant intermolecular force that must be overcome is hydrogen bonding.
Hydrogen Bonding
Hydrogen bonding is a strong type of dipole-dipole interaction that occurs when hydrogen is attached to a highly electronegative atom such as oxygen, nitrogen, or fluorine. In the case of ethanol (CH3CH2OH), the hydrogen atom attached to the oxygen atom forms hydrogen bonds with other ethanol molecules.
Overcoming Hydrogen Bonding
In order to convert liquid ethanol to vapors, these hydrogen bonds must be broken. This requires additional energy input to overcome the strong attraction between the hydrogen atom and the electronegative oxygen atom in neighboring molecules.
Other Intermolecular Forces
While dipole-dipole interactions, London dispersion forces, and covalent bonds also play a role in the overall behavior of ethanol molecules, hydrogen bonding is the dominant force that must be overcome in the process of converting liquid ethanol to vapors.
In conclusion, hydrogen bonding is the primary intermolecular force that must be disrupted in order to vaporize liquid ethanol. This requires additional energy input to break the strong attractions between ethanol molecules.
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What is the dominant intermolecular force or bond that must be overcome in converting liquid CH3CH2OH to vapours?a)H-bondingb)Dipole-dipole interactionsc)Covalent bondsd)London dispersion forceCorrect answer is option 'A'. Can you explain this answer?
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