Which of the following bonds is not associated with hydrogen bonding?

Hydrogen bonding is a particularly strong type of dipole-dipole interaction that occurs when hydrogen is directly bonded to highly electronegative elements such as oxygen, nitrogen, or fluorine. In the case of the choices given, the bonds involving hydrogen and either oxygen (H-O), nitrogen (H-N), or fluorine (H-F) will all exhibit significant hydrogen bonding due to the high electronegativity of these elements, which creates a strong dipole when bonded to hydrogen.

The bond between carbon and hydrogen (C-H) is relatively non-polar because carbon is not highly electronegative compared to oxygen, nitrogen, or fluorine. As a result, while there is some polarity to the C-H bond, it is not sufficient for hydrogen bonding to occur. The hydrogen atom in a C-H bond cannot effectively interact with lone pairs on electronegative atoms, as is required for hydrogen bonding. This lack of appropriate electronegativity in the carbon atom means that the C-H bond cannot participate in hydrogen bonding like the other bonds listed, making it the only bond in this context that is not associated with hydrogen bonding.