Final answer:
NH3 (ammonia) is the compound that exhibits hydrogen bonding because the nitrogen atom can form hydrogen bonds with the hydrogen atoms of another NH3 molecule.
Step-by-step explanation:
The student is asking which of the given compounds exhibits hydrogen bonding. Hydrogen bonding typically occurs when a hydrogen atom is bonded to a highly electronegative atom such as oxygen (O), nitrogen (N), or fluorine (F), and this hydrogen is attracted to another electronegative atom with a lone pair of electrons.
Among the compounds listed:
- NH3 (ammonia) exhibits hydrogen bonding. The nitrogen atom has a lone pair of electrons, and it is electronegative enough to form hydrogen bonds with the hydrogen atoms of another NH3 molecule.
- CH3OCH3 (dimethyl ether) does not exhibit hydrogen bonding because there are no hydrogen atoms bonded directly to the oxygen atom.
- CH3Cl (methyl chloride) and HI (hydrogen iodide) also do not exhibit hydrogen bonding; the former has no H atoms bonded to O, N, or F, and the latter has a less electronegative atom, iodine, which is usually not strong enough to participate in hydrogen bonding.
Therefore, the compound that exhibits hydrogen bonding is NH3.