Download - Matter: Properties & Change
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Matter: Properties & ChangeMatter: Properties & ChangeChapter 3
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MatterMatter
Matter – anything that has mass and takes up space
Everything around us
Chemistry – the study of matter and the changes it undergoes
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Four States of MatterFour States of Matter
Solidsparticles vibrate but can’t move
aroundfixed shape fixed volumeincompressible
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Four States of MatterFour States of Matter
Liquidsparticles can move
around but are still close together
variable shapefixed volumeVirtually incompressible
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Four States of MatterFour States of Matter
Gasesparticles can separate and
move throughout containervariable shapevariable volumeEasily compressedVapor = gaseous state of a
substance that is a liquid or solid at room temperature
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Four States of MatterFour States of Matter
Plasmaparticles collide with enough energy
to break into charged particles (+/-)gas-like, variable
shape & volumestars, fluorescent
light bulbs, TV tubes
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Physical PropertiesPhysical Properties
Physical Propertycan be observed without changing the
identity of the substance
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Physical PropertiesPhysical Properties
Physical properties can be described as one of 2 types:
Extensive Propertydepends on the amount of matter
present (example: length)
Intensive Propertydepends on the identity of substance, not
the amount (example: scent)
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Extensive vs. IntensiveExtensive vs. Intensive
Examples:boiling point
volume
mass
density
conductivity
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Density – a physical propertyDensity – a physical property
Derived units = Combination of base units
Volume (m3 or cm3 or mL) length length length Or measured using a
graduated cylinder
D = MV
1 cm3 = 1 mL1 dm3 = 1 L
Density (kg/m3 or g/cm3 or g/mL)mass per volume
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DensityDensity An object has a volume of 825 cm3 and a
density of 13.6 g/cm3. Find its mass.
GIVEN:
V =
D =
M = ?
WORK:
V
MD
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DensityDensity A liquid has a density of 0.87 g/mL. What
volume is occupied by 25 g of the liquid?
GIVEN:
D =
V =
M =
WORK:
V
MD
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DensityDensityM
ass
(g)
Volume (cm3)
Δx
Δyslope D
V
M
= g/cm3units of yunits of x
Units of the slope
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ProportionsProportions
Direct Proportion
Inverse Proportion
xy
xy
1
y
x
y
x
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Percent ErrorPercent Error
Indicates accuracy of a measurement
100literature
literaturealexperimenterror %
your value
accepted value
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Percent ErrorPercent Error
A student determines the density of a substance to be 1.40 g/mL. Find the % error if the accepted value of the density is 1.36 g/mL.
100g/mL 1.36
g/mL 1.36g/mL 1.40error %
% error = 0.04/1.36 = 3 %
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Chemical PropertiesChemical Properties
Chemical Propertydescribes the ability of a substance to
undergo changes in identity
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Physical vs. Chemical PropertiesPhysical vs. Chemical Properties
Examples:melting point
flammable
density
magnetic
tarnishes in air
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Physical ChangesPhysical Changes
Physical Changechanges the form of a substance without
changing its identity
properties remain the same
Examples: change in shape or size, dissolving, change in color by dying, all phase changes,
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Phase Changes – PhysicalPhase Changes – Physical
Evaporation =
Condensation =
Melting =
Freezing =
Sublimation =
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Chemical ChangesChemical Changes
Process that involves one or more substances changing into a new substanceCommonly referred to as a chemical
reactionNew substances have different
compositions and properties from original substances
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Chemical ChangesChemical Changes
Signs of a Chemical Changechange in color or odor (not by dying)
formation of a gas (bubbling)
formation of a precipitate (solid)
change in light or heat
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Physical vs. Chemical ChangesPhysical vs. Chemical Changes
Examples:rusting iron
dissolving in water
burning a log
melting ice
grinding spices
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What Type of Change?What Type of Change?
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Matter FlowchartMatter Flowchart
MATTER
Can it be physically separated?
yes no
Can it be chemically decomposed?
noyesIs the composition uniform?
noyes
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Pure SubstancesPure Substances
Elementcomposed of identical atomsEX: copper wire, aluminum foil
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Pure SubstancesPure Substances
Compoundcomposed of 2 or more
elements in a fixed ratio
properties differ from those of individual elements
EX: table salt (NaCl)
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MixturesMixtures
Variable combination of 2 or more pure substances.
Heterogeneous Homogeneous
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MixturesMixtures
Solutionhomogeneousvery small particlesparticles don’t settleEX: rubbing alcohol
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MixturesMixtures
Heterogeneousmedium-sized to
large-sized particles
particles may or may not settle
EX: milk, fresh-squeezed
lemonade
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MixturesMixtures
Examples:tea
muddy water
fog
saltwater
Italian salad dressing