Why does hydrogen fluoride (HF) form stronger hydrogen bonds than water (H₂O) even though water has more hydrogen bonding sites?
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A.
Water has a symmetrical structure that reduces hydrogen bonding strength.
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B.
Fluorine is the most electronegative element, creating a stronger dipole.
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C.
The H–F bond is weaker than the H–O bond, allowing better hydrogen bonding.
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D.
HF has a lower molecular mass, making it more reactive.
Correct Answer:
B. Fluorine is the most electronegative element, creating a stronger dipole.
Explanation:
Hydrogen fluoride (HF) forms stronger hydrogen bonds than water (H2O) primarily because fluorine is more electronegative than oxygen. Although a water molecule can form up to four hydrogen bonds while HF typically forms only two, the extreme electronegativity of fluorine creates a more significant partial positive charge on the hydrogen atom and a more substantial partial negative charge on the fluorine atom. This result in a much stronger dipole-dipole attraction in HF compared to H2O, making the individual hydrogen bonds in HF significantly more robust. Therefore, the strength of the hydrogen bond is determined more by the intensity of the molecular dipole than by the total number of available bonding sites.
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