Solids, Liquids, and Gases

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Solids, Liquids, and Gases
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Kinetic Theory

• The kinetic theory is an explanation of how
  particles in matter behave.
• The three assumptions of the kinetic theory are
  as follows
• All matter is composed of small particles (atoms,
  molecules, and ions).
• These particles are in constant, random motion.
• These particles are colliding with each other and
  the walls of their container.

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Kinetic Theory (2)

• These particles do lose some energy during
  collisions with other particles.
• But the amount of energy lost is very small and
  can be neglected in most cases.
• At higher temperature, particles move faster and
  bump into one another with more force.
• At lower temperatures, they move with less energy.

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States of Matter

• Basis of classification of the four states of
  matter
• Based upon particle arrangement.
• Based upon energy of particles.
• Based upon distance between particles.
• On Earth, matter is usually found as solids,
  liquids, or gases.
• Plasma is the most common state of matter in the
  universe, but it is rarely found on Earth.

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States of Matter (2)

• An everyday activity such as eating lunch may
  include solids, liquids, and gases.
• Can you identify the states of matter present in
  the photo shown?

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Solid

• Atoms in solids are held tightly in place by the
  attraction between the particles.
• This attraction between the particles gives
  solids a definite shape and volume. However, the
  thermal energy in the particles causes them to
  vibrate in place.
• Although the particles vibrate in place, they
  cannot change position. As a result, a solid
  retains its size and shape.

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Solids (2)
Particle Movement Examples
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Liquids

• Particles in a liquid have more kinetic energy
  than particles in a solid.
• This extra kinetic energy allows particles to
  partially overcome the attractions to other
  particles.
• Thus, the particles can slide past each other,
  allowing liquids to flow and take the shape of
  their container.
• However, the particles in a liquid have not
  completely overcome the attractive forces between
  them.
• This causes the particles to cling together,
  giving liquids a definite volume.

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Liquids (2)
Particle Movement Examples
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Gases

• Gas particles have enough kinetic energy to
  overcome the attractions between them.
• Gases do not have a fixed volume or shape.
• Therefore, they can spread far apart or contract
  to fill the container that they are in.

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Gases (2)
Particle Movement Examples
Br
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Plasma

• Plasma is matter consisting of positively and
  negatively charged particles.
• Matter enters the plasma state when it is heated
  to such a high temperature that some of the atoms
  begin to break apart.
• A type of plasma is used on Earth to make neon
  and fluorescent lights. Instead of heating the
  gases to an extremely high temperature, an
  electrical current is passed through them. The
  current strips the electrons from the atoms,
  producing plasma.

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Plasma (2)

• The negatively charged electrons (yellow) are
  freely streaming through the positively charged
  ions (blue).

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Plasma (3)

• Plasma can be found in stars, fluorescent light
  bulbs, Cathode ray tubes, neon signs, and
  lightening.

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Changes of State

• What happens to a solid when thermal energy or
  heat is added to it?
• The particles on the surface of the solid vibrate
  faster.
• These particles collide with and transfer energy
  to other particles.
• Soon the particles have enough kinetic energy to
  overcome the attractive forces.
• The particles gain enough kinetic energy to slip
  out of their ordered arrangement and the solid
  melts.

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Changes of State (2)

• This is known as the melting point, or the
  temperature at which a solid begins to liquefy.
• Energy is required for the particles to slip out
  of the ordered arrangement.
• The amount of energy required to change a
  substance from the solid phase to the liquid
  phase at its melting point is known as the heat
  of fusion.

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Changes of State (3)

• How does a liquid become a gas?
• The particles in a liquid are constantly moving.
• Some particles are moving faster and have more
  kinetic energy than others. The particles that
  are moving fast enough can escape the attractive
  forces of other particles and enter the gas
  state.
• This process is called vaporization.

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Changes of State (4)

• Vaporization can occur in two waysevaporation
  and boiling.
• Evaporation is vaporization that occurs at the
  surface of a liquid and can occur at temperatures
  below the liquids boiling point.

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Changes of State (5)

• The boiling point of a liquid is the temperature
  at which the pressure of the vapor in the liquid
  is equal to the external pressure acting on the
  surface of the liquid.
• Heat of vaporization is the amount of energy
  required for the liquid at its boiling point to
  become a gas.

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Heating Curve of a Liquid

• This type of graph is called a heating curve
  because it shows the temperature change of water
  as thermal energy, or heat, is added.
• Notice the two areas on the graph where the
  temperature does not change.
• At 0C, ice is melting.

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Heating Curve of a Liquid (2)

• The temperature remains constant during melting.
• After the attractive forces are overcome,
  particles move more freely and their average
  kinetic energy, or temperature, increases.
• At 100C, water is boiling or vaporizing and the
  temperature remains constant again.