Specific Heat Capacity of Water:
The specific heat capacity of water is approximately 4.18 J/g°C. This means that it takes 4.18 joules of energy to raise the temperature of 1 gram of water by 1 degree Celsius.

Specific Heat Capacity of Ice:
The specific heat capacity of ice is approximately 2.09 J/g°C. This value is lower than that of water, indicating that it takes less energy to raise the temperature of ice compared to water.

Specific Heat Capacity of Water Vapor:
The specific heat capacity of water vapor is approximately 1.996 J/g°C. This value is even lower than that of ice, suggesting that it takes even less energy to raise the temperature of water vapor compared to ice or water.

Explanation:
The specific heat capacities of water, ice, and water vapor differ due to the different molecular arrangements and bonding states of each substance.

Water:
Water molecules are held together by hydrogen bonds, which are relatively strong and require a significant amount of energy to break. When heat is added to water, it not only raises the temperature but also breaks these hydrogen bonds. This results in water having a relatively high specific heat capacity. Furthermore, water has a high boiling point, which means that it requires significant energy to convert it from a liquid to a gas.

Ice:
In ice, water molecules are arranged in a crystal lattice structure held together by hydrogen bonds. While heat can still increase the temperature of ice, it primarily breaks the hydrogen bonds to allow the water molecules to move more freely. The energy required to break these hydrogen bonds is lower than that of liquid water, resulting in a lower specific heat capacity for ice.

Water Vapor:
Water vapor consists of individual water molecules that are not held together by hydrogen bonds. The energy required to raise the temperature of water vapor is primarily used to increase the kinetic energy of the molecules, allowing them to move faster. Since there are no hydrogen bonds to break, the specific heat capacity of water vapor is the lowest among the three states.

Conclusion:
In summary, the specific heat capacities of water, ice, and water vapor differ due to the different molecular arrangements and bonding states of each substance. Water has a higher specific heat capacity compared to ice and water vapor because of the energy required to break hydrogen bonds. Ice has a lower specific heat capacity than water because it has a more ordered molecular arrangement. Water vapor has the lowest specific heat capacity as it consists of individual water molecules with no hydrogen bonds to break.