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Transcript of Key Terms for Chapter 4 ViscosityBoiling point Absolute zeroCompressibility KelvinAmorphous solid...
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Key Terms for Chapter 4
Viscosity Boiling point
Absolute zeroCompressibility
KelvinAmorphous solid
SublimationCrystalline solid
Condensation Brownian movement
Bose-Einstein condensate Diffusion
EvaporationFreezing point
Melting pointCondensation point
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Chapter 4PROPERTIES OF MATTER
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Properties of Matter
Physical PropertiesA characteristic of the object/material (color, shape….)
Physical ChangesA change in a material that does not alter its identity
Chemical PropertiesDescribes how matter will react in the presence of other
matter Chemical Changes
Alters the identity of the material (iron rusting, burning wood)
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Physical Properties
Property that can be observed and measured without a change in the kind of matter being observed
Examples Color Density Shape Texture Hardness State or Phase Conductivity
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Physical Changes
Does not alter the identity of the material It is a change in a physical property It remains the same kind of matter Generally easy to reverse Atoms do not rearrange Ex.: cutting a piece of paper, freezing water…
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Chemical Properties
Describes how matter will react in the presence of other substances
Ex. The tendency of iron to rust
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Chemical Change
Alters the identity of the material and forms a new kind of matter
Generally called a chemical reaction Both physical and chemical properties change Atoms are rearranged: new chemical formula Generally not a reversible reaction Energy is often produced or absorbed Ex.: burning, rusting
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Physical or Chemical change?
Water evaporates into steam A piece of cork is cut in half A bicycle chain rusts A piece of apple rots on the ground
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Models
Ideas that represent what might be happening No model is perfect Models can change Good models
Organize ideas
Describe observations
Help us describe what we cannot see
Predict what will happen
Different types of models Solar system models
DNA
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Matter
Aristotle (and other Greek philosophers) believed that matter was continuous
It could be divided infinitely without changing it
This concept was generally accepted from about 500 B.C. for 1500 A.D
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Particle Model of Matter
Matter could only be subdivided to a certain point – eventually you would not be able to divide it any more
Ex. Water droplet Measure those particles in angstroms and
nanometers These particles are called atoms Two or more atoms joined together forms a molecule
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Particle Model
You can watch the diffusion of food coloring in water whether you stir it or let it sit
If you let it sit long enough, the solution will spread throughout the water without stirring. How?
Brownian Movement: describes the constant motion of particles in a liquid or gas1st introduced by a botanist Robert Brown
Diffusion: mixing by this particle motion
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Phases of Matter
4 phases of matterSolidLiquidGasPlasma
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Solid
Definite shape Definite volume Usually dense: particles are packed closely together Low compressibility Particles vibrating in fixed position Low kinetic energy: strong attractive force
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Solid
Occur in 2 basic forms:Crystalline: atoms are in a fixed, repeating
structure in solidAmorphous: atom arrangement is random
Ex. glass
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Liquid
Definite volume No definite shape Low compressibility Random particle movement: Brownian Motion Particles fairly close Fairly equal kinetic energy to attractive force Viscosity: the ease with which a liquid will flow
Low viscosity: liquid flows very easily (water) High viscosity: liquid does not flow easily (pancake syrup)
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Gas
Indefinite shape Indefinite volume High compressibility Particles are far apart More kinetic energy than attractive force Brownian motion Gas pressure: from the collisions of the gas particles with the
sides of the container (ex. Balloon) Heat gas = more kinetic energy
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Comparing Phases
Solid Liquid Gas
Volume Definite Definite Indefinite
Shape Definite Indefinite Indefinite
Compressibility Low Low High
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Bose-Einstein Condensate
Hypothetical phase of matter that exists at absolute zero
Particles of the object behave as a single atom Still being studied in labs to determine it’s uses
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Phase Changes of Matter
Temperature increases = energy increases Temperature decreases = energy decreases Adding and removing energy will result in a phase
change
The type of matter stays the same
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Phase Changes
Phase changes that add energy
MeltingVaporization
Boiling Evaporation
Sublimation
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Melting
Change from a solid to a liquid The temperature at which melting occurs is called
the melting point
Water: 0oC or 32oF
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Vaporization
Change from liquid to gas Boiling
Occurs very quicklyDepends on the air pressure aboveBoiling point: temperature at which substance boils
EvaporationOccurs very slowly
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Sublimation
Change from solid to gas (without becoming a liquid)
Solid particles gain enough energy to escape into the atmosphere
Ex. Dry ice, moth balls, snow
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Phase Changes
Phase changes that remove energyFreezingCondensingDeposition
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Freezing
Change from liquid to solid Liquid particles lose enough kinetic energy that the
attractive forces hold the particles in place Temperature at which this occurs is freezing point
Water: 0oC or 32oF
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Condensing
Change from gas to liquid Temperature at which this occurs is dew point
(condensation point)
Ex. Dew
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Deposition
Change from gas to solid (without becoming liquid)
Ex. Frost, Ice on wings of plane
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Measuring Energy
Temperature: Measure of average Kinetic energyDifferent than heat (total Kinetic energy)
Celsius: 0C Fahrenheit: 0F Kelvin: K Absolute zero: the temperature at which all
molecular motion would cease
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Conversions
C to K – add 273 K to C – subtract 273 C to F – (C x 1.8) + 32 F to C – (F – 32)/1.8
MEMORIZE THESE CONVERSIONS
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Conversions
Convert -182 oC to K
-182 + 273 = 91 K Convert 298 K to oC
298 – 273 = 25 oC Convert 68oF to oC
68-32 = 36/1.8 = 20 oC Convert 312 K to oF
312 – 273 = 39 oC
(39 x 1.8) +32 = 102.2 oF