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Chapter 2 Overview
Chapter 2 Overview
Three Basic States of Matter
Solids, Liquids, and Gases
Gas
Particles have little or no attraction
Gas
Vapor
The gas state of a substance that is normally a solid or a liquid at room temperature
Vapor
Liquid
Particles have some attraction to each other and can flow past one another
Liquid
Viscosity
The ability of a liquid to resist flow
Viscosity
Solid
Particles are attracted and held close together
Solid
Changes in State
Changes in State
State Changes
Terms for State Changes
Deposition
The change of state of a gas to a solid without going through the liquid state
Deposition
Sublimation
The change of state from a solid to a gas without going through the liquid state
Sublimation
Condensation
The change of state from a gas to a liquid
Condensation
Evaporation
Vaporization that occurs only at the surface of a liquid
Evaporation
Vaporization
The change in state of a liquid into a gas
Vaporization
Types of Energies
Types of Energy
Thermal Energy
The total potential and kinetic energies of an object
Thermal
Potential Energy
Stored energy due to the interactions between particles or objects
Potential
Kinetic Energy
The energy an object has due to its motion
Kinetic
The behavior of Gases
The Behavior of Gases
Pressure
The amount of force applied per unit of area
Pressure
Kinetic Molecular Theory
An explanation of how particles in matter behave
Kinetic Molecular Theory
Basic concepts of kinetic molecular theory
- Small particles make up all matter
- These particles are in constant, random motion
- The particles collide with other particles, other objects, and the walls of their container
- When particles collide, no energy is lost
Boyle's Law
States that pressure of a gas increases if the volume decreases and pressure of a gas decreases if the volume increases, when temperature is constant
Charles's Law
The volume of a gas increases with increasing temperature, if the pressure is constant