Key:11. Put the following intermolecular forces in order of increasing strength: dipole-induced dipole, London dispersion, hydrogen bonding, dipole dipolea.dipole-induced dipole < dipole dipole < London dispersion < hydrogen bondingb.hydrogen bonding < dipole-induced dipole < dipole dipole < London dispersionc.London dispersion < hydrogen bonding < dipole-induced dipole < dipole dipoled.London dispersion < dipole-induced dipole < dipole dipole < hydrogen bondinge.dipole-induced dipole < London dispersion < dipole dipole < hydrogen bondingOne way to understand intermolecular forces is to think of magnets. The reason a magnet sticks to another magnet is because the magnet has a positive pole and a negative pole. The positive side of one magnet is attracted to the negative side of the next magnet and vice versa. This is like a polar molecule – one side is somewhat positive and the other is somewhat negative. This difference in charge is called a dipole. With that in mind, consider the following types of intermolecular forces.
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