Download - Matter & Its Properties
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Matter & Its PropertiesCh 1: Lesson 3 Honors Chemistry K. Davis
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Matter
Matter – anything that has mass and takes up spaceEverything around us
Chemistry – the study of matter and the changes it undergoes
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SubstancesAtoms: the building blocks of all
matter Ions: atoms that become negatively
or positively charged Element: matter containing only one
type of atom; ex. hydrogen and oxygen
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Four States of Matter
Solidsparticles vibrate but can’t move
aroundfixed shape fixed volumeincompressible
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Four States of Matter
Liquidsparticles can move
around but are still close together
variable shapefixed volumeVirtually incompressible
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Four States of MatterGases
particles can separate and move throughout container
variable shapevariable volumeEasily compressedVapor = gaseous state of a
substance that is a liquid or solid at room temperature
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Four 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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Four States of Matter
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Physical PropertiesPhysical Property
can be observed without changing the identity of the substance
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Physical PropertiesPhysical properties can be described
as one of 2 types:
Extensive Propertydepends on the amount of matter
present (example: length) Intensive Property
depends on the identity of substance, not the amount (example: scent)
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Intensive Physical PropertiesThe intensive physical properties for a
sample of a pure substance remain constant. ex. pure water- always a colorless liquid
that boils at 100ºC at sea level; doesn’t matter if you have 10 mL or 1 L
Melting and boiling point are examples of these constant physical properties. can be used to help identify a substance
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Extensive vs. IntensiveExamples:
boiling pointvolumemassdensityconductivity
intensiveextensiveextensiveintensiveintensive
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Density – 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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DensityM
ass
(g)
Volume (cm3)
ΔxΔyslope D
VM
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Density An object has a volume of 825 cm3 and a
density of 13.6 g/cm3. Find its mass.
GIVEN:V = 825 cm3
D = 13.6 g/cm3
M = ?
WORK:M = DV
M = (13.6 g/cm3)(825cm3)
M = 11,220 g
M = 11,200 gVMD
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Density A liquid has a density of 0.87 g/mL. What
volume is occupied by 25 g of the liquid?
GIVEN:D = 0.87 g/mLV = ?M = 25 g
WORK:V = M D
V = 25 g 0.87 g/mL
V = 29 mLVMD
= 28.736 mL
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Chemical PropertiesChemical Property
describes the ability of a substance to undergo changes in identity
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Physical vs. Chemical PropertiesExamples:
melting pointflammabledensitymagnetictarnishes in air
physicalchemicalphysicalphysicalchemical
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Physical ChangesPhysical Change
changes the form of a substance without changing its identity
properties remain the sameEx: cutting a sheet of paper, breaking
a crystal, all phase changes
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Some Physical ChangesBoilingCondensationDissolvingEvaporationFreezingMeltingSublimation
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Phase Changes – Physical Evaporation =
Condensation =
Melting =
Freezing =
Sublimation =
Liquid -> Gas
Gas -> Liquid
Solid -> Liquid
Liquid -> Solid
Solid -> Gas
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Chemical ChangesProcess 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 ChangesSigns of a Chemical Change
change in color or odorformation of a gasformation of a precipitate (solid)change in light or heat
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Change of Energy
All physical & chemical changes involve a change of energy.
• Endothermic – energy absorbed• a positive number (+) means endothermic• feel cold to the touch
• Exothermic – energy released • a negative number (-) means exothermic• feel warm or hot to the touch
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Some Chemical Changes Combustion Corrosion Electrolysis Fermentation Metabolism Photosynthesis Bubble formation Temperature change Smell Rust
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Tip for Distinguishing Is the change permanent? Can I get
the original substance back after the change?” If so, it is a physical change. If not, it is a chemical change.
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Physical vs. Chemical ChangesExamples:
rusting irondissolving in waterburning a logmelting icegrinding spices
chemicalphysicalchemicalphysicalphysical
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What Type of Change?
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What Type of Change?
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Law of Conservation of MassAlthough chemical changes occur,
mass is neither created nor destroyed in a chemical reaction
Mass of reactants equals mass of products
massreactants = massproducts
A + B C
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Conservation of Mass In an experiment, 10.00 g of red mercury (II) oxide powder is
placed in an open flask and heated until it is converted to liquid mercury and oxygen gas. The liquid mercury has a mass of 9.26 g. What is the mass of the oxygen formed in the reaction?
Mercury (II) oxide mercury + oxygenMmercury(II) oxide = 10.00 gMmercury = 9.26Moxygen = ?
GIVEN:Mercury (II) oxide mercury + oxygenMmercury(II) oxide = 10.00 gMmercury = 9.86 gMoxygen = ?
WORK:10.00 g = 9.86 g + moxygen
Moxygen = (10.00 g – 9.86 g)
Moxygen = 0.74 g
massreactants = massproducts
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Matter Flowchart
MATTERCan it be physically
separated?
Homogeneous Mixture
(solution)
Heterogeneous Mixture Compound Element
MIXTURE PURE SUBSTANCE
yes no
Can it be chemically decomposed?
noyesIs the composition uniform?
noyes
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Matter FlowchartExamples:
graphitepeppersugar (sucrose)paintsoda
elementhetero. mixturecompoundhetero. mixturesolution
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Pure SubstancesElement
composed of identical atomsEX: copper wire, aluminum foil
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Pure SubstancesCompound- ex. table salt (NaCl)
composed of 2 or more elements in a fixed ratio
properties differ from those of individual elements
Molecule smallest particle of a compound
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Mixtures Variable combination of 2 or more pure substances that
is physically combined. There is no particular ratio and each part of the mixture
keeps its own properties. Ex. Perfume, potting soil, salad dressings, and tea.
Heterogeneous Homogeneous
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MixturesSolution
Homogeneous mixturevery small particlessubstances are in the same amount in all
parts of the mixtureparticles don’t settleex. rubbing alcohol, perfume
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MixturesHeterogeneous
medium-sized to large-sized particles
substances in the mixture are not evenly mixed
particles may or may not settle
ex. milk, fresh-squeezed lemonade, salad
dressing, potting
soil
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Heterogeneous Mixtures
Colloid: a heterogeneous mixture with larger particles that never settle; scatter light in the Tyndall effect. Ex. Milk
Suspension: a heterogeneous mixture containing a liquid in which visible particles settle
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MixturesExamples:
teamuddy waterfogsaltwaterItalian salad dressing
Answers:SolutionHeterogeneousHeterogeneousSolutionHeterogeneous
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Separating Mixtures Substances in a mixture are physically
combined, so processes based on differences in physical properties are used to separate component
Numerous techniques have been developed to separate mixtures to study components
FiltrationDistillationCrystallizationChromatography
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Filtration Used to separate
heterogeneous mixtures composed of solids and liquids
Uses a porous barrier to separate the solid from the liquid
Liquid passes through leaving the solid in the filter paper
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DistillationUsed to separate
homogeneous mixtures
Based on differences in boiling points of substances involved
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Crystallization Separation technique resulting in
the formation of pure solid particles from a solution containing the dissolved substance
As one substance evaporates, the dissolved substance comes out of solution and collects as crystals
Produces highly pure solids Ex. Rocky candy
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Chromatography Separates components of a mixture based on
ability of each component to be drawn across the surface of another material
Mixture is usually liquid and is usually drawn across chromatography paper
Separation occurs because various components travel at different rates
Components with strongest attraction for paper travel the slowest