Phase Transition

Definition

A phase transition is a physical transformation of a substance from one state of matter (solid, liquid, or gas) to another, often accompanied by the absorption or release of energy. These changes in the fundamental structure of a material occur at specific temperature and pressure conditions.

5 Must Know Facts For Your Next Test

1. Phase transitions are driven by changes in the intermolecular forces and the arrangement of atoms or molecules within the substance.
2. The three main phase transitions are melting (solid to liquid), boiling (liquid to gas), and sublimation (solid to gas).
3. During a phase transition, the temperature of the substance remains constant until the transition is complete, as the energy absorbed or released is used to change the state of matter.
4. The critical point marks the conditions where the distinction between the liquid and gas phases disappears, and they become a single, continuous fluid phase.
5. Phase diagrams are used to predict the phase of a substance under different temperature and pressure conditions.

Review Questions

• Explain the relationship between phase transitions and the changes in the intermolecular forces and atomic/molecular arrangement within a substance.
  • Phase transitions occur when the intermolecular forces and the arrangement of atoms or molecules within a substance change significantly. For example, during the melting of a solid, the strong intermolecular forces that hold the atoms or molecules in a fixed, crystalline structure are overcome, allowing the atoms or molecules to move more freely and adopt a less ordered, liquid state. Similarly, the transition from a liquid to a gas involves the complete overcoming of intermolecular forces, resulting in a highly disordered, gaseous state. These changes in the fundamental structure of the material are what define a phase transition.
• Describe the role of latent heat in phase transitions and how it relates to the constancy of temperature during a phase change.
  • Latent heat is the energy released or absorbed by a substance during a phase transition at a constant temperature and pressure. During a phase transition, the temperature of the substance remains constant until the transition is complete because the energy absorbed or released is used to change the state of matter, rather than to increase or decrease the temperature. For example, when a solid is heated, the temperature remains constant at the melting point until all of the solid has melted, as the energy is used to break the intermolecular bonds and overcome the forces holding the atoms or molecules in a fixed, crystalline structure. The latent heat is the amount of energy required for this phase change to occur.
• Analyze the significance of the critical point in the context of phase transitions and its implications for the behavior of substances.
  • The critical point is the unique combination of temperature and pressure at which the distinction between the liquid and gas phases of a substance disappears, and they become a single, continuous fluid phase. At the critical point, the properties of the liquid and gas phases become indistinguishable, and the substance exhibits a unique and anomalous behavior. This has important implications for the behavior of substances, as the critical point marks the conditions where the substance can no longer be easily separated into distinct liquid and gas phases. Understanding the critical point is crucial for predicting the phase behavior of substances and for applications in fields such as thermodynamics, materials science, and chemical engineering.

Related terms

Latent Heat: The amount of energy released or absorbed by a substance during a phase transition at a constant temperature and pressure.

Critical Point: The unique combination of temperature and pressure at which the distinction between the liquid and gas phases disappears, and they become a single, continuous fluid phase.

Phase Diagram: A graphical representation of the relationships between the phases of a substance and the conditions (temperature, pressure) under which the phases exist.