* Increased kinetic energy: Heat energy is added to the water, causing the water molecules to vibrate and move faster.

* Weakening of hydrogen bonds: The increased kinetic energy overcomes the attractive forces (hydrogen bonds) that hold water molecules together in a liquid state.

* Phase change: As the molecules gain enough energy, they break free from the liquid structure and transition into a gaseous state, which is steam.

* Increased distance between molecules: In the gaseous state, the water molecules are much farther apart than in the liquid state.

Here's a more detailed explanation:

1. Liquid State: In liquid water, molecules are close together and constantly move around, constantly making and breaking hydrogen bonds. These bonds are relatively strong and hold the molecules together.

2. Heating: When heat is applied, water molecules absorb energy. This energy increases their kinetic energy, causing them to vibrate faster and move around more rapidly.

3. Breaking Bonds: As the molecules move faster, the hydrogen bonds between them begin to weaken.

4. Vaporization: When enough energy is absorbed, the molecules have enough kinetic energy to overcome the attractive forces completely. They break free from the liquid state and enter the gaseous state as steam.

5. Gaseous State: In the gaseous state, the water molecules are far apart and move freely. They collide with each other and the container walls, but the collisions are less frequent and less forceful than in the liquid state.

It's important to note: The boiling point of water is 100°C (212°F) at standard atmospheric pressure. At this temperature, the water molecules have enough energy to overcome the attractive forces and escape into the gas phase. However, the temperature at which water boils can vary depending on the pressure.