Respuesta :
The H-F bond is the strongest because the F atom has the highest electronegativity and the smallest size; breaking the H-F bond would need the greatest energy.
H-bond strength
All three compounds were created using elements from Period 2 of the Periodic table, and they are all distinct hydrides. It is well known that the atomic radii decrease over the period starting with C,N,O.
The electronegativity also rises as the number of electrons increases. Due to their vastly different electronegativities from the H atom, all of these atoms—C, N, and O—form a H bond.
However, the electron density of the atom grows from C,N,O as the atomic radii (and, consequently, the atomic size) drop over the period with rising electronegativity.
Therefore, H is more drawn to the neighboring molecule with higher electron densities.
The bond energy (29 kJ/mol for HF) confirms that F would form the strongest hydrogen bond because it is the least electronegative and smallest in size.
Similar to OO, the H bond strength would be a little bit lower due to O's weaker electronegativity and somewhat larger size.
Water would therefore have a lower bond energy, 22 kJ/mol for H2O. The bond energy estimate for NH3 17 kJ/mol confirms that N has the lowest energy.
Overall, the H-F bond would require the greatest energy to break because it has the strongest H-bond.
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