CM 1: MATTER

• What is the main concept behind the Kinetic Molecular Theory?

  All matter is made up of moving particles
• In higher temperatures, particles move faster
• How do particles behave in solids based on the Kinetic Molecular Theory?

  They hardly move and hold a regular pattern.
• What are the characteristics of liquids according to the Kinetic Molecular Theory?

  Particles have more energy than solids and can flow
• How do particles behave in gases according to the Kinetic Molecular Theory?

  They are sparse and move freely
• How does the Kinetic Molecular Theory describe the behavior of particles within matter?

  Moving randomly with kinetic energy
• Why do gases have the ability to expand and compress?

  Due to high energy
• Temperature is the main factor that influences the energy of particles according to the theory.
• Atoms and molecules - the particles that hold kinetic energy and move around in random directions according to the Kinetic Molecular Theory
• In low temperatures, particles have less energy
• kinetic energy - the energy needed for the particles to keep moving
• solid - have a definite shape and a definite volume
• crystalline solids - molecules are arranged in a geometric pattern
• amorphous solids - molecules do not have a set pattern of arrangement
• table salt is a type of crystalline solid
• gels are a type of amorphous solid
• liquid - have an indefinite shape and a definite volume
• Basis of Classification of the Four States

  • particle arrangement
  • energy of particles
  • distance between particles
• Why are liquids denser than gases?

  Molecules are closer together
• How do you boil liquid without increasing the temperature?

  By lowering the atmospheric pressure
• plasma - an ionized gas
• Molecules in the solid phase have the least amount of energy, while gas particles have the greatest amount of energy
• The temperature of a substance is a measure of the average kinetic energy of the particles
• A change in phase may occur when the energy of the particles is changed.
• Intermolecular Forces - attractive forces that become stronger as the particles move closer together
• phase change - a change from one state of matter to another
• exothermic - heat energy is released
• endothermic - heat energy is absorbed
• melting - solid to liquid
• freezing - liquid to solid
• sublimation - solid to gas
• deposition - gas to solid
• boiling - liquid to gas
• condensation - gas to liquid
• ionization - gas to plasma
• recombination - plasma to gas
• phase diagram - illustrates the changes in the phase of a matter under varying temperature and pressure conditions
• critical point - at a certain pressure and temperature, the substance is indistinguishable if liquid or gas
• triple point - at a certain temperature and pressure, the substance may be solid, liquid, or gas