In which of the following pure compounds is hydrogen bonding most likely to be a dominant intermolecular force? A. Dimethyl ether, CH3OCH3 B. Hydrogen bromide, HBr C. Difluoromethane, CH2F2 D. Ammonium iodide, NH4I E. Dimethylamine, (CH3)2NH
Question
In which of the following pure compounds is hydrogen bonding most likely to be a dominant intermolecular force? A. Dimethyl ether, CH3OCH3 B. Hydrogen bromide, HBr C. Difluoromethane, CH2F2 D. Ammonium iodide, NH4I E. Dimethylamine, (CH3)2NH
Solution
The compound in which hydrogen bonding is most likely to be a dominant intermolecular force is E. Dimethylamine, (CH3)2NH.
Here's why:
Hydrogen bonding is a special type of dipole-dipole attraction between molecules, not a covalent bond to a hydrogen atom. It results from the attractive force between a hydrogen atom covalently bonded to a very electronegative atom such as a N, O, or F atom and another very electronegative atom.
A. Dimethyl ether, CH3OCH3: This molecule does not have a hydrogen atom bonded to a N, O, or F atom, so it cannot exhibit hydrogen bonding.
B. Hydrogen bromide, HBr: This molecule does not have a hydrogen atom bonded to a N, O, or F atom, so it cannot exhibit hydrogen bonding.
C. Difluoromethane, CH2F2: This molecule does not have a hydrogen atom bonded to a N, O, or F atom, so it cannot exhibit hydrogen bonding.
D. Ammonium iodide, NH4I: This is an ionic compound, not a molecule, so it does not exhibit hydrogen bonding.
E. Dimethylamine, (CH3)2NH: This molecule has a hydrogen atom bonded to a nitrogen atom, so it can exhibit hydrogen bonding. Therefore, hydrogen bonding is most likely to be a dominant intermolecular force in this compound.
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