Chemistry Chapter 12 Flashcards

Viscosity and Phase Changes

• Viscosity: Measures resistance of liquids to flow; influenced by particle size, shape, temperature, and intermolecular forces.
• Phase Changes: Occur when energy is added or removed, leading to transitions between solid, liquid, and gas states.
• Freezing Point: Temperature at which a liquid becomes a crystalline solid; melting point is the opposite.

Intermolecular Forces and Properties

• Intermolecular Forces: Includes dispersion forces, dipole-dipole forces, and hydrogen bonds; essential for determining states of matter at specific temperatures.
• Surface Tension: Energy needed to increase liquid surface area; affected by intermolecular forces.
• Cohesion and Adhesion: Intermolecular forces also impact these phenomena, influencing how substances interact with each other.

Types of Solids

• Crystalline Solids: Characterized by orderly geometric arrangements of atoms, ions, or molecules; can be classified by shape and composition.
• Amorphous Solids: Lack regular patterns; formed when molten material cools quickly, preventing crystal formation.
• Allotropes: Different structural forms of the same element in the same state, exhibiting distinct properties.

Gas Behavior and Kinetic Molecular Theory

• Kinetic Molecular Theory: Describes the behavior of solids, liquids, and gases based on particle movement and energy. Explains properties like expansion, diffusion, and pressure in gases.
• Vaporization: An energy-requiring process in which a liquid transitions to a gas; evaporation occurs specifically at the liquid's surface.
• Vapor Pressure: Pressure exerted by vapor above a liquid; increases with temperature.

Phase Diagrams and Critical Points

• Phase Diagram: Graph depicting phases of a substance (solid, liquid, gas) related to pressure and temperature.
• Triple Point: Specific conditions where solid, liquid, and gas phases coexist.
• Condensation and Deposition: Energy-releasing processes transforming gas to liquid (condensation) or gas to solid (deposition) without passing through the liquid phase.

Additional Key Terms

• Surfactant: Compounds, like soap, that reduce surface tension in liquids by disrupting hydrogen bonds between water molecules.
• Unit Cell: Smallest repeating structural unit in a crystal lattice that reflects the symmetry of the whole crystal.
• Barometer: Instrument for measuring atmospheric pressure, often used to understand weather patterns.
• Dalton's Law of Partial Pressures: Relates to the behavior of gases and how different gases exert their own pressures within a mixture.
• Atmospheric Pressure (atm): Standard unit for reporting air pressure.

Strength of Forces

• Intramolecular vs. Intermolecular Forces: Intramolecular forces, which hold atoms together within a molecule, are stronger than intermolecular forces.

Explore essential concepts from Chemistry Chapter 12 with our flashcards. Learn key terms like viscosity and the Kinetic Molecular Theory, which explain the behavior of solids and liquids. Perfect for students looking to reinforce their understanding of these important chemistry topics.