Chapter 10
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Transcript of Chapter 10
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Chapter 10States of Matter
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10.1 Kinetic Molecular Theory (KMT)
“Particles of Matter are always in motion”
States of MatterWe will discuss the KMT in terms of :
1. Gases2. Liquids3. Solids
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KMT - GasesO Ideal gas- follows all of the tenets of
the KMT.O 1. Gases consist of large numbers of
atoms/molecules that are in continuous, random motion.
O 2. The combined volume of all the atoms/molecules of the gas is negligible relative to the total volume in which the gas is contained.
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Gases Cont.O 3. Attractive and repulsive forces between
gas particles is negligible.O 4. Energy can be transferred between
particles during collisions, but the average kinetic energy of the particles does not change with time (assuming temperature is constant) = collisions are elastic
O 5. The average kinetic energy of the particles is proportional to the absolute temperature.O K.E. = ½ mv2
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Properties of GasesO Expansion-gases occupy the volume
of the container they are enclosed in.O Fluidity- gas particles move like
liquids because there are no attractive or repulsive forces among them
O Density- gases have low densities because of the large amounts of space between the particles.
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Properties of Gases Cont.
O Compressibility- Gases can be easily condensed with an increase in pressure due to the large space between the particles.
O Diffusion- the random mixing of particles due to their constant motion.
O Effusion- gas particles pass through a tiny opening.O Rate is directly proportional to the velocities
of the particles. (Smaller particles move faster and vice-versa)
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Real GasesO Those that do not conform to the 5 parts
of the KMT.O When gases are held at high pressure
and low temperatures they deviate from their expected behavior.
O Noble gases conform the most to the KMT and act like ideal gases.
O The more polar the gas molecule the more it deviates from the KMT and acts like a real gas.
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10.2 LiquidsO Have a definite volume and take the
shape of its containerO Particles are closer together so their
attractive forces are stronger than in gases
(think strength of intermolecular forces)O Fluid – the ability to flow and occupy
the shape of its container.
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Liquids Cont.O Density – fairly high considering the
closer arrangement of the particlesO Incompressibility- because of the
close proximity to one another, the particles in a liquid can’t be pushed much closer together.
O Diffusion- liquids move easily among other liquids. Attractive forces and temperature of the particles lends to a slower diffusion rate of the liquid particles.
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Liquids Cont.O Surface Tension- a force that attracts
adjacent particles on a liquids’ surface together enough to decrease the surface area.O The higher the intermolecular forces
the higher the surface tension. O Water has a fairly high surface
tension.
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Liquids Cont.O Capillary Action – the attraction of
the surface of a liquid to the surface of a solid.O MeniscusO ChromatographyO Phloem tubes in plants
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Liquids Cont.O Vaporization – liquid changing to a
gasO Evaporation – vaporization at the
surface of a liquid O Individual particles gain enough
kinetic energy to break the I.F. and escape as a gas.
O Freezing – liquid changing to a solidO Due to the increased intermolecular
attractions among the particles
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10.3 SolidsO Highly ordered arrangement with
minimal movement among the particles
O I.F. exert stronger forces due to this proximity
O Types:O Crystalline- geometric, repeating
pattern of particlesO Amorphous- random arrangement of
particles O Glass, obsidianO “without shape”
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Solids Cont.O Melting- changing a solid to a liquid by
applying heat energyO Overcome I.F. and break apart from the
crystalline structureO Supercooled liquids (amorphous solids) –
retain some liquid properties due to their lack of a uniform, organized pattern
O High DensityO Low diffusion rate
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Solids Cont.O Types of Crystals (p. 340)
O 1. Ionic - NaClO 2. Covalent Network – SiO2O 3. Metallic - CuO 4. Covalent Molecular – NH3
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Changes of StateO Phase – when a substance has
uniform composition and propertiesO Melting, freezing, vaporization,
condensation, sublimation, depositionO Equilibrium – when two phases occur
at the same rate. E.g., melting freezing
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Changes of State Cont.O Equilibrium Vapor Pressure – the pressure
exerted by a vapor in equilibrium with its liquid at a given temp. O Proportional to the concentration of
molecules in the vapor phase.O Increases with an increase in temperatureO Volatile liquids (those that evaporate
easily) have higher V.P. because they tend to have weaker I.F. between the molecules.
O Vapor Pressure Animation
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Changes of State Cont.O Boiling – change of a liquid to vapor
at the surface and within the liquid.O Boiling point – when the V.P. equals
the atmospheric pressure.O Normal B.P. of water = 100oC, (normal
atmospheric pressure of 1 atm, 760 torr, 101.3 kPa)
O B.P. Animation
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Vapor Pressures of Various Substances
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Identity of SubstancesO A – Diethyl etherO B – BenzeneO C - water
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Phase Diagrams
O Phase Diagram Explanation
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Phase Diagram for Water