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The Gas State and Kinetic Molecular Theory (KMT)
Lesson 1Unit 5 Gases and Atmospheric Chemistry
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Most substances can exist in the solid, liquid or gas states. Recall that the attractions between particles influence the state each substance is in at room temperature:
The States of Matter
Ionic Compounds: contain strong electrostatic attractions and are therefore found in the solid state at room temperature. They have high boiling points (e.g. NaCl (s))
Polar Molecules: These compounds contain permanent dipoles and form strong dipole-dipole intermolecular bonds. They are found in the liquid or solid state but have a lower boiling point. (e.g. H2O (l))
Non-polar Molecules: These have no dipoles and contain very weak intermolecular bonds. They are usually gases. (e.g. H2 (g), Cl2 (g) , CO2 (g)).
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The States of MatterGas, Liquid, and Solid - there is also a
fourth; it is called a plasma which has charged particles that can conduct electricity and are influenced by magnetic fields. It is similar to a gas in its properties
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Vibrational Motion: back-and-forth motion of particles.
Rotational Motion: spinning motion of particles.
Translational Motion: straight-line motion from place to
place.
The Motion of Particles:
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Phase Structure Movement of Particles
Shape and Volume
Ability to Pour
Compressibility
Solid - particles closely packed -particles in fixed positions
- vibration -definite shape -definite volume
-cannot be poured
-cannot be compressed significantly
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Phase Structure Movement of Particles
Shape and Volume
Ability toPour
Compressibility
Liquid -particles closely packed -particles not fixed in position
-vibration -rotation -translation (slower)
- takes shape of container - Definite volume
-can be poured
- cannot be compressed significantly
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Phase Structure Movement of Particles
Shape and Volume
Ability to Pour
Compressibility
Gas - particles widely spaced - particles not fixed in position
-vibration - rotation-translation (faster)
-occupies entire volume of container
- can be poured
- can be easily compressed
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Kinetic Molecular Theory of Gases1. A gas consists of particles in constant,
random, straight-line motion; they collide with each other and with the walls of the container
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2. Gas particles influence each other only by collision; they exert no other forces on each other.
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3. All collisions between gas particles are perfectly elastic; all kinetic energy (energy of motion) is conserved.
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4. The volume actually occupied by the particles of a gas is negligible; the vast majority of the volume of the gas is empty space through which the gas particles are moving.
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5. Particles of different gases have equal kinetic energies at the same temperature.
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Therefore, according to this theory, an ideal gas behaves much like billiard balls on a pool table.
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Gas PressuresIn the KMT, pressure is the force exerted
against the wall of a container by the continual collision of molecules against it. THE COLLAPSING CAN DEMO
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HomeworkRead 416 – 422# 1, 2, 3 (a,b), 4, 5 on pg. 422.