Melting is the process by which a solid becomes a liquid when heat is applied. The energy breaks the bonds between the particles, leading to a change in state without changing the substance's composition.

Boiling is the rapid vaporization that occurs when a liquid is heated to its boiling point, turning it into a gas. This process occurs throughout the liquid, forming bubbles.

Latent heat is the energy absorbed or released by a substance during a phase change at constant temperature. It is used to change the state without increasing the temperature.

Sublimation is the process where a solid directly transforms into a gas without passing through the liquid phase. Dry ice is a common example of sublimation.

Sensible heating refers to a rise in temperature without a change of state, whereas phase changes involve transformations such as melting, freezing, or condensation. No state change occurs during sensible heating.

During a phase change, the energy input is used to break intermolecular bonds rather than increasing the kinetic energy of the particles. This energy is known as latent heat, which results in a constant temperature until the phase transition is complete.

The latent heat of fusion is the energy required for a solid to change into a liquid at its melting point. This energy is used to overcome the forces holding the solid particles together without increasing the temperature.

Deposition is the process in which a gas transforms directly into a solid without becoming a liquid first. The formation of frost on cold surfaces is a clear example of deposition.

A plateau on a temperature versus heat graph indicates that the added energy is being used for a phase change. During this period, the energy is absorbed as latent heat, meaning the temperature remains constant until the transition is complete.

Latent heat of vaporization is usually much higher than latent heat of fusion because converting a liquid to a gas requires a greater amount of energy to overcome stronger intermolecular forces. This contrast highlights the energy differences between the two phase changes.

Ambient pressure is a key factor that influences the boiling point of a liquid. Lower atmospheric pressure lowers the boiling point, while higher pressure raises it.

At higher altitudes, the atmospheric pressure is reduced, which in turn lowers the boiling point of liquids. This is why liquids require a lower temperature to boil on a mountain compared to sea level.

Superheating occurs when a liquid is heated above its normal boiling point but does not boil due to the absence of nucleation sites. This results in a metastable state until a disturbance triggers rapid boiling.

Adding salt to water reduces its vapor pressure, meaning that a higher temperature is needed for the water molecules to escape into the gas phase. This effect, known as boiling point elevation, is a colligative property of solutions.

During the vaporization process, the absorbed energy is primarily utilized to overcome the intermolecular forces that hold the liquid together. This energy is known as the latent heat of vaporization, and it is not used to increase the temperature.

The energy absorbed by the ice during its phase change from solid to liquid, without a temperature increase, is called latent heat. This energy is used to break the intermolecular bonds in the ice structure.

The triple point is the unique set of pressure and temperature conditions at which all three phases (solid, liquid, and gas) coexist in equilibrium. It is a fundamental concept in phase diagrams and thermodynamics.

During a phase change, the added heat energy is utilized to break intermolecular bonds rather than to increase the kinetic energy of the molecules. This absorbed energy, known as latent heat, results in a constant temperature until the phase change is complete.

The boiling point of a liquid is strongly influenced by its intermolecular forces. Water's higher boiling point is due to its strong hydrogen bonding compared to ethanol's relatively weaker intermolecular attractions.

For most substances, increasing external pressure favors the phase with the lower volume, typically the solid, thereby raising the melting point. This behavior is explained by Le Chatelier's principle, which predicts that a system in equilibrium will adjust to counteract changes imposed on it.