The kinds of interactions that exist between CH3COOH molecules
include dipole-dipole (including hydrogen bonding) interactions and London forces.True or False
Its false there are no hydrogen bonds?
Yes, there are hydrogen bonds (between the O of the COOH of one molecule and the H of the COOH of another molecule).
To determine the kinds of interactions that exist between CH3COOH (acetic acid) molecules, we need to consider the molecular structure and functional groups present.
CH3COOH contains both a carbonyl group (C=O) and a hydroxyl group (OH) attached to a carbon atom.
The carbonyl group and the hydroxyl group can both participate in hydrogen bonding. Hydrogen bonding occurs when a hydrogen atom is bonded to a highly electronegative atom (such as oxygen in this case) and is attracted to another electronegative atom. In acetic acid, the carbonyl oxygen atom can act as the hydrogen bond acceptor, while the hydrogen atom in the hydroxyl group can act as the hydrogen bond donor. Therefore, dipole-dipole interactions, including hydrogen bonding, are present in CH3COOH molecules.
Apart from hydrogen bonding, CH3COOH also exhibits London dispersion forces (also known as Van der Waals forces). This type of interaction results from temporary fluctuations in electron distribution, leading to temporary dipoles. These temporary dipoles induce similar temporary dipoles in neighboring molecules, resulting in attractive forces between them.
Hence, the statement that the kinds of interactions between CH3COOH molecules include dipole-dipole (including hydrogen bonding) interactions and London forces is true. Therefore, the statement is not false, and hydrogen bonds are present between CH3COOH molecules.