Textbook Question
For each pair of compounds, circle the compound you expect to have the higher boiling point. Explain your reasoning.
(d) HOCH2—(CH2)4—CH2OH or (CH3)3CCH(OH)CH3
(e) (CH3CH2CH2)2NH or (CH3CH2)3N
(f)
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2. Molecular Representations
Intermolecular Forces
Multiple Choice
Which of these phenomena result from hydrogen bonding?
A
Nonpolar nature of
B
High boiling point of
C
Weak van der Waals forces in noble gases
D
Low melting point of
Verified step by step guidance1
Identify the nature of hydrogen bonding: Hydrogen bonding is a type of dipole-dipole interaction that occurs between molecules where hydrogen is covalently bonded to a highly electronegative atom, such as oxygen, nitrogen, or fluorine.
Consider the properties of water: Water (H₂O) is a polar molecule with hydrogen atoms bonded to oxygen, which is highly electronegative. This allows for hydrogen bonds to form between water molecules.
Analyze the effect of hydrogen bonding on boiling points: Hydrogen bonds are relatively strong intermolecular forces, which require more energy to break. This results in a higher boiling point for substances like water, where hydrogen bonding is prevalent.
Evaluate the other options: Methane (CH₄) is nonpolar and does not exhibit hydrogen bonding. Noble gases have weak van der Waals forces due to their full electron shells and lack of polarity. Iodine (I₂) is a nonpolar molecule with low melting points due to weak intermolecular forces.
Conclude which phenomenon is due to hydrogen bonding: The high boiling point of water is a direct result of hydrogen bonding, as it requires significant energy to overcome these strong intermolecular forces.
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