Hydrogen-bonding strength is largely due to the high electronegativity of which elements?

Hydrogen-bonding strength is largely due to the high electronegativity of which elements?

• A. F, O, and N
• B. H, He, Li
• C. C, N, and O
• D. Na, Cl, and Mg

Answer: (A)

Hydrogen bonding arises from a bond polarity created when hydrogen is attached to a highly electronegative atom. That strong pull on the bonding electrons gives hydrogen a noticeable partial positive charge, while the lone pairs on another electronegative atom can carry a partial negative charge. When those conditions involve atoms with very high electronegativity, the attraction becomes a relatively strong, directional interaction known as a hydrogen bond. Among common elements, fluorine, oxygen, and nitrogen are the most electronegative, so they are the ones that most effectively support strong hydrogen bonding. This is why the strength of hydrogen bonds is largely tied to the high electronegativity of F, O, and N. Other elements present in the options are either far less electronegative or do not provide the same combination of polarity and lone-pair availability, so they contribute much less to hydrogen-bond strength.

Hydrogen bonding arises from a bond polarity created when hydrogen is attached to a highly electronegative atom. That strong pull on the bonding electrons gives hydrogen a noticeable partial positive charge, while the lone pairs on another electronegative atom can carry a partial negative charge. When those conditions involve atoms with very high electronegativity, the attraction becomes a relatively strong, directional interaction known as a hydrogen bond. Among common elements, fluorine, oxygen, and nitrogen are the most electronegative, so they are the ones that most effectively support strong hydrogen bonding. This is why the strength of hydrogen bonds is largely tied to the high electronegativity of F, O, and N. Other elements present in the options are either far less electronegative or do not provide the same combination of polarity and lone-pair availability, so they contribute much less to hydrogen-bond strength.