Respuesta :
Answer:
D) CH₃OH
Explanation:
Hydrogen bonding is due to the electrostatic force of attraction between the hydrogen atom which is bounded to a electronegative atom covalently which has high value of electronegativity as compared to hydrogen. Particularly, second-row elements which are nitrogen , oxygen and fluorine forms hydrogen bonding with the hydrogen connected to these elements.
A) CH₄ and E) CO₂ cannot form hydrogen bonding.
B) C₅H₁₁OH and C) C₆H₁₃NH₂ - have more number of carbon atoms and steric factor will come into picture and thus hydrogen bonding is not the significant component of intermolecular forces.
D) CH₃OH - molecule is small and hydrogen bonding is likely to be the most significant component of the total intermolecular forces in this molecule.
The hydrogen bonding in the compound is most likely dominated between atoms with more electronegativity difference with hydrogen. Significant hydrogen bonding is found in methanol.
What are intermolecular forces?
The intermolecular forces are the interactions and the force that attaches the two atoms together in a compound. The intermolecular force of hydrogen bonding is found between hydrogen and the more electronegative atom.
The methane and carbon dioxide with the absence of high electronegative atoms and oxygen results in the absence of hydrogen bonding.
The molecules of pentanol and hexylamine had consisted of steric hindrance, and thus the hydrogen binding has not been a significant force.
The molecule of methanol has the hydrogen atom bound to the oxygen atom and consisted of significant hydrogen bonding Thus, option D is correct.
Learn more about hydrogen bonding, here:
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