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A hydrogen bond can only occur between a hydrogen and a nitrogen, oxygen, and fluorine atom. For a hydrogen to undergo hydrogen bonding, the hydrogen must first be covalently bonded to very electronegative atom (only N, O, and F). The second parameter is that the hydrogen must be close to another electronegative atom (N, O, and F) that has available lone pairs. D is correct because the hydrogen is first covalently bonded to a nitrogen. Next it is attracted to a very electronegative atom, in this case oxygen.
Carbon and hydrogen atoms have similar electronegativity values and therefore would share electrons equally. This means they would not form hydrogen bonds because the atoms do not have partial charges. This eliminates B,C,E, and F. Answer choice A does not have a hydrogen atom so it would not form a hydrogen bond. This leaves Answer D as the correct choice because difference in electronegativity values between O and C, and N and H allows them to have partial positive and negative regions that can interact. Hope this helps!
The Hydrogen must be able to create a strong dipole moment to bond to an electronegative element therefore bonding to another electronegative element will allow for the electrons to be shared unequally and allow for Hydrogen bonding to occur.
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