One of the attractive features of ionic liquids is their low vapor pressure, which in turn tends to make them nonflammable. Why do you think ionic liquids have lower vapor pressures than most room-temperature molecular liquids?

Verified step by step guidance

1. Step 1: Understand the nature of ionic liquids. Ionic liquids are composed of ions, which are charged particles. These ions are held together by strong electrostatic forces known as ionic bonds.
2. Step 2: Compare the forces in ionic liquids to those in molecular liquids. In molecular liquids, the molecules are held together by weaker intermolecular forces such as hydrogen bonds, dipole-dipole interactions, or London dispersion forces.
3. Step 3: Consider the energy required to vaporize the liquid. For a liquid to vaporize, the particles must overcome the forces holding them together. Since ionic bonds are much stronger than the intermolecular forces in molecular liquids, more energy is required to vaporize ionic liquids.
4. Step 4: Relate the energy requirement to vapor pressure. Vapor pressure is a measure of a liquid's tendency to evaporate. Because ionic liquids require more energy to overcome their strong ionic bonds, they have a lower tendency to evaporate, resulting in a lower vapor pressure.
5. Step 5: Conclude with the implications of low vapor pressure. The low vapor pressure of ionic liquids contributes to their nonflammability, as there are fewer vapor molecules available to ignite.