Kinetic Theory and a Model for Gases

• energy an object has bc of its motion = kinetic energy.
• kinetic theory describes all matter as tiny particles that are in constant motion
• Gases in Kinetic Theory small,

  hard spheres, insignificant volume. They are all in motion

  and colliding at room temperature
• no attractive forces between particles, all

  collisions are elastic,

  (no loss of kinetic energy in the collision)
• motion of the particles rapid, constant, random, particles move in straight lines until they collide with other particles or the container walls.
• particles in a gas can be individual atoms, or complex
• Standard temperature and pressure (STP)
• STP = standard set of conditions used for comparing properties of different gases / corresponds to a temperature abt 0°C and atmospheric pressure at sea level (100 kPa).
• (gas ) Helium = monatomic each particle single helium atom.
• ionic bonding = attraction between oppositely charged ions.
• metalic bonding is when the positive metal ions are attracted to the negative electrons in the outer shell of the atoms
• covalent bonding = sharing of e- between atoms
• Particles in steam are molecules of water at/above 100°C (becomes gas
• forces between molecule of gas and the container walls = gas pressure
• collsions = bumb together
• psi = pound per square inch