What happens to the molecules of liquid water when changing in gaseous water and what is the weakest force of attraction between molecules?
When liquid water changes into gaseous water (steam), several things happen to the molecules:
1. Increased Kinetic Energy: The primary change is in the kinetic energy of the molecules. As heat is applied to the liquid, the molecules gain energy and vibrate more rapidly. This increase in energy allows them to overcome the forces holding them together in the liquid state.
2. Weaker Intermolecular Forces: While the type of intermolecular forces present in water remains the same (hydrogen bonding), they become weaker due to the increased distance between molecules. This means the molecules are less tightly packed and experience less attraction to each other.
3. Increased Distance Between Molecules: The increased kinetic energy also causes the molecules to move farther apart, leading to a significant increase in volume. This is why steam takes up much more space than the same amount of liquid water.
4. Phase Transition: When enough molecules have gained enough energy to overcome the intermolecular forces completely, they break free from the liquid and enter the gas phase, forming steam.
The weakest force of attraction between molecules: Among the intermolecular forces present in water, the weakest is the London dispersion force. This force arises from temporary fluctuations in electron distribution within molecules, creating instantaneous attractive forces between nearby molecules. While it plays a role in liquid water, its contribution is overshadowed by the stronger hydrogen bonding.
In summary: The transition from liquid water to steam involves an increase in molecular kinetic energy, weaker intermolecular forces, increased distance between molecules, and ultimately, a phase change from liquid to gas. The weakest force of attraction in this case is the London dispersion force.
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