states of matter newport high school academic chemistry modified from a powerpoint found at
TRANSCRIPT
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States of MatterStates of MatterStates of MatterStates of Matter
Newport High SchoolAcademic ChemistryNewport High SchoolAcademic Chemistry
Modified from a PowerPoint found at http://www.nisd.net/communicationsarts/pages/chem/
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Lesson 1 – Kinetic Molecular TheoryLesson 1 – Kinetic Molecular Theory
Essential Questions:• How does the kinetic-molecular theory
describe the properties of gases that include: expansion, fluidity, low density, compressibility, diffusion, and effusion?
Vocabulary: kinetic-molecular theory, ideal gas, elastic collision, diffusion, effusion, real gas
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Lesson 1 – The Kinetic Molecular Theory
Lesson 1 – The Kinetic Molecular Theory
Kinetic-molecular theory is based on the idea that particles of matter are always in motion.
Can be applied to solids, liquids, and gases.
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Assumptions of GasesAssumptions of Gases
Ideal gas – one that behaves in a way to fit all 5 assumptions of the kinetic-molecular theory of gases.
5 Assumptions• Gases consist of large numbers of tiny particles that
are far apart.• Collisions between particles are elastic.• Gas particles are in continuous, rapid, random motion.• There are no forces of attraction between gas particles.• The temperature of a gas depends on the average
kinetic energy of the particles of the gas.
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ExpansionExpansion
Gases do not have a definite shape or volume.
Completely fill any container they occupy.
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FluidityFluidity
Gas particles glide past each other because attractive forces are insignificant.
They are considered fluid, because they flow.
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Low densityLow density
Density is about 1/1000 the same substance in the liquid or solid state.
Reason is that gas particles are very far apart.
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CompressibilityCompressibility
Gas particles become more crowded when compressed.
Volume can be decreased due to large amount of space between particles.
Examples of compression of gases?
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Diffusion and EffusionDiffusion and Effusion
Diffusion – spontaneous mixing of the particles of two substances caused by random motion
http://www.indiana.edu/~phys215/lecture/lecnotes/diff.html
Effusion – process where gas particles pass through a tiny opening
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Lesson 2 - LiquidsLesson 2 - Liquids
Essential Question:• How does the kinetic-molecular theory of
liquids describe the motion of particles and the properties of liquids?
Vocabulary: Fluid, surface tension, capillary action, vaporization, evaporation, freezing
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Kinetic Molecular Theory & Liquids
Kinetic Molecular Theory & Liquids
Liquid = definite volume and takes the shape of its container
Particles are closer togetherAttractive forces do existMore ordered than gasesParticles have lower mobility, but are
fluids
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Properties of LiquidsProperties of Liquids
DensityCompressibilityDiffusionSurface TensionCapillary actionEvaporation and BoilingFormation of Solids
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DensityDensity
Substances are hundreds of times denser in the liquid state than in the gaseous state
Water is one of the few substances that because less dense when it solidifies. • Most become more dense.
Densities differ so much between liquids that they can form layers.
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CompressibilityCompressibility
They are relatively incompressibile.
• Particles are more closely packed.
• Volume only decreases by 4% at very high pressures.
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DiffusionDiffusion
Liquids diffuse in the same way as gases.• Due to random motion of particles.• Is slower than gases since particles are closer together
and attractive forces exist.• Increase temperature, increase diffusion
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Surface TensionSurface Tension
Surface tension – force that pulls adjacent parts of a liquid’s surface together, consequently decreasing surface area to the smallest possible size• This is why they form a sphere shape
Higher force of attraction = higher surface tension
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Capillary actionCapillary action
Capillary action – attraction of the surface of a liquid to the surface of a solid
Attraction tends to pull the liquid molecules upward along the surface – reason for the meniscus
Responsible for the transportation of water in plants.
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Evaporation & BoilingEvaporation & Boiling
Vaporization – process by which a liquid changes to a gas• Evaporation – vaporization without boiling• Boiling – energy is added in the form of heat
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Formation of SolidsFormation of Solids
When a liquid is cooled, the average energy of the particles decreases.• This is called freezing or solidification.• Each substance has its own freezing
temperature.
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Lesson 3 - SolidsLesson 3 - Solids
Essential Question:• How does the kinetic-molecular theory of
solids describe the motion of particles in solids and the properties of solids?
Vocabulary: Crystalline solids, crystal, amorphous solids, melting, melting point, supercooled liquids, crystal structure, unit cell
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Kinetic Theory & SolidsKinetic Theory & Solids
Crystalline and amorphous solids Definite shape and Volume
• Shape stays due to arrangement of particles.• Volume only changes slightly with change in temperature.
Definite Melting Point• When particles overcome the forces holding them together.
High Density• Results from the fact that the particles of a solid are more closely packed
than liquids or gases
Incompressibility Low Rate of Diffusion
• Millions of times slower than liquids
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Crystalline SolidsCrystalline Solids
Crystal structure – 3D arrangement of particles• Unit cell – smallest portion of a crystal lattice
that shows 3D structure
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Four Types of CrystalsFour Types of Crystals
Ionic• Positive and negative ions arranged in a regular pattern
• High melting points, hard and brittle, good conductors
Covalent network• Each atom is covalent bonded to its nearest neighbor.
• Very hard and brittle, high melting point, nonconductors or semiconductors
Metallic• Metal cations surrounded by a sea of valence electrons
• High melting point, good conductors
Covalent molecular crystals• Held together by intermolecular forces
• Low melting points, easily vaporized, soft, insulators
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Amorphous SolidsAmorphous Solids
Particles not arranged in an orderly pattern
Most are cooled in ways that do not let them crystallize.
Glass, plastic, rubber, and asphalt are examples.
Have no definite melting point
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Lesson 4 – Phase ChangesLesson 4 – Phase Changes
Essential Questions: • How do phase diagrams show the relationship
between the physical states of a substance and its temperature and pressure?
Vocabulary: phase, condensation, equilibrium, vapor pressure, volatile liquid, boiling, boiling point, molar enthalpy of vaporization, freezing point, molar enthalpy of fusion, sublimation, deposition, phase diagram, triple point, critical point, critical temperature, critical pressure
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Phase ChangesPhase Changes
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Phase ChangesPhase Changes
EvaporationEvaporation• molecules at the surface gain enough
energy to overcome IMF
VolatilityVolatility• measure of evaporation rate• depends on temp & IMF
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Phase ChangesPhase Changes
Kinetic Energy
# o
f P
art
icle
s
p. 477
Boltzmann Distribution
temp
volatility
IMF
volatility
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Phase ChangesPhase Changes
EquilibriumEquilibrium• trapped molecules reach a balance
between evaporation & condensation
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Phase ChangesPhase Changes
Vapor PressureVapor Pressure• pressure of vapor above
a liquid at equilibrium
IMF v.p.temp v.p.
• depends on temp & IMF• directly related to volatility
temp
v.p
.
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Phase ChangesPhase Changes
Boiling Point• temp at which v.p. of liquid
equals external pressure
IMF b.p.Patm b.p.
• depends on Patm & IMF
• Normal B.P. - b.p. at 1 atm
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Which has a higher m.p.?• polar or nonpolar?• covalent or ionic?
Phase ChangesPhase Changes
Melting Point• equal to freezing point
polar
ionic
IMF m.p.
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Phase ChangesPhase Changes
Sublimation
• solid gas
• v.p. of solid equals external pressure
EX: dry ice, mothballs, solid air fresheners
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Heating CurvesHeating Curves
Melting - PE
Solid - KE
Liquid - KE
Boiling - PE
Gas - KE
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Heating CurvesHeating Curves
Temperature Change• change in KE (molecular motion) • depends on heat capacity
Heat Capacity• energy required to raise the temp of 1
gram of a substance by 1°C• “Volcano” clip - water has a very high
heat capacity
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Heating CurvesHeating Curves
Phase Change• change in PE (molecular arrangement)• temp remains constant
Heat of Fusion (Hfus)
• energy required to melt 1 gram of a substance at its m.p.
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Heating CurvesHeating Curves
Heat of Vaporization (Hvap)
• energy required to boil 1 gram of a substance at its b.p.
• usually larger than Hfus…why?
EX: sweating, steam burns, the drinking bird
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Phase DiagramsPhase Diagrams
• Shows the relationship among the solid, liquid, and vapor states.
• Each region represents a pure phase
• Line between regions is where the two phases exist in equilibrium
• Triple point is where all 3 curves meet, the conditions where all 3 phases exist in equilibrium!
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Phase Diagrams cont.Phase Diagrams cont.
Critical temperature – temperature above which a substance cannot be in a liquid state
Critical pressure – lowest pressure at which the substance can exist as a liquid at the critical temperature
Critical point – critical temperature and pressure
Normal freezing point – point at which liquid freezes at sea level
Normal boiling point – point at which liquid boils at sea level
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Lesson 5 - WaterLesson 5 - Water
Essential Questions:
• How are the properties of water determined by its structure?
• What happens to the energy of water when it changes state?
Vocabulary: Heat, energy
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Structure of WaterStructure of Water
Two hydrogen atoms and one oxygen atom
Molecules in water are linked by hydrogen bonding
Why is water not a gas at room temperature?
Empty space between molecules is why ice has lower density.
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Physical Properties of WaterPhysical Properties of Water
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Works CitedWorks Cited
Modern Chemistry Textbookwww.nclark.nethttp://mrsj.exofire.net/chem/http://www.unit5.org/chemistry/