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Properties of Matter
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Essential QuestionsHow does the state of matter define its properties?What are the real-life examples of molecules, atoms & ions?How are atoms, molecules & ions alike and how are they different?How can matter be classified?What are the essential components of solutions?Why is water the universal solvent?In what ways can matter be quantified?What units should be used to quantify matter?What are the chemical & physical properties of pure substances?How can chemical and physical changes be determined in a laboratory setting?
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The Breakdown of Matter
Matter
Anything with MASS & VOLUME
(solid, liquid, gas)
Pure Substanc
esMixtures
EQ: How can matter be classified?
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MIXTURES
Mixtures = two or more substances PHYSICALLY combined.
Can be PHYSICALLY separated
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Heterogeneous Mixtures
Hetero = different Geneous = origin or beginning has separations and/or boundaries can see to different parts Are ALL mixtures
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Heterogeneous MixturesHeterogeneou
sMixtures
MixturesPhysically combined
substances
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HomogeneousMixtures
Homeo = same Geneous = origin or beginning matter of the SAME make-up (no boundaries)
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Homogeneous Mixtures
Homogeneous
Mixtures
SolutionsOthers alloys,
colloids, etc.
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Homogeneous Mixtures
Homogeneous
Mixtures
Solutions
Solute Solvent
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SolutionsEQ: What are the essential components
of solutions?
Homogeneous mixtures Physically NOT chemical
combined Solute = the substance BEING
dissolved Solvent = the substance DOING
the dissolving
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Examples of Solutions Alloys = solid mixture or solution
(brass, 14K gold, steel) Air = gas mixture or solution Liquid solutions = sweet tea,
coffee, milk, tap water
EQ: Why is water the universal solvent?
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Solution Properties
Soluble = the solute is able to dissolve in the solvent
Insoluble = the solute is NOT able to dissolve in the solvent
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Descriptions of a Solution
Diluted Solutions = small amount of solute and/or a large amount of solvent
Concentrated Solutions = large amount of solute and/or a small amount of solvent
Saturated Solution = a solution that will NOT dissolve any more solute
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An increase in temperature will allow more solute to dissolve in a solvent. The molecules of the solvent move faster and further apart allowing more room for more solute molecules.
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3
21
Name three properties of solutions:
1. __________________________________
2. __________________________________
3. __________________________________
Name two types of mixtures & two types of pure substances.
1. ____________________________________
2. ____________________________________
What is the one key in distinguishing between homogeneous and heterogeneous mixtures
1. _____________________________________
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Pure Substances
Pure Substance
s
ElementsCompoun
ds
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Pure Substances
chemically pure substances only one part or one kind of
matter Elements = found on the
periodic table Compounds = 2 or more
elements that have combined CHEMICALLY EQ: How are atoms, molecules & ions alike
and how are they different?
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Elements EQ: What are the real-life examples of
molecules, atoms & ions? 90 natural occurring elements found on the periodic table Atoms = smallest part of an
element represented by symbols
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Compounds
2 or more elements that have combined CHEMICALLY
Molecules = smallest part of a compound
represented by formulas
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Elements & Compounds
Pure Substance
s
Elements
Atoms
Symbols
Compounds
Molecules
Formulas
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States of Matter Also called Phases of Matter Solids Liquids Vapors (gases)
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Solids
Have a definite shape Have a definite volume Particles VIBRATE in place
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Liquids
Have NO definite shape
Have definite volume particles SLIDE freely
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Gases (vapor)
Have NO definite shape Have NO definite volume particles fill the volume of
the container
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Solids, Liquids & Gases Solids = can form
crystals = solid where the particle are arranged into repeating patterns.
Liquids = physical property of Viscosity = “thickness” – the resistance to flow.
Gases = volume of gases depend greatly on pressure and temperature.EQ: How does the state of matter define its properties?
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Phase Changes
Melting Freezing Vaporization Condensatio
n Sublimation physical
changes
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Melting
the process of changing from a solid to a liquid
energy is being put into the substance
melting point = the temperature at which melting occurs – physical property
the melting point of water is 0ºC
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Freezing
the process of changing from a liquid to a solid
energy is being pulled out of the substance
freezing point = same temperature as the melting point
(used mainly in weather)
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Vaporization
the process of changing from a liquid to a gas
energy is being put into the substance
evaporation boiling
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Evaporation
vaporization that occurs at the surface of the liquid
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Boiling vaporization that occurs
throughout the liquid boiling point = the temperature
at which boiling occurs the boiling point of water is
100ºC
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Condensation
the process of changing from a gas to a liquid
energy is being pulled out of the substance
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Sublimation
the process of changing from a solid to a gas
energy is being put into the substance
ex: dry ice (CO2)
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3
21
Name three phases of matter:
1. __________________________________
2. __________________________________
3. __________________________________
Name two types of vaporization.
1. ____________________________________
2. ____________________________________
What is the so different about sublimation?
1. _____________________________________
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Properties of Matter
characteristics that can identify and describe matter.
Physical Properties Chemical Properties
EQ: What are the chemical & physical properties of pure
substances?
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Physical Properties
observable properties physical change = changes that
occur while the substance remains the same.
ex: phase change
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Examples of Physical Properties
density (d=m/v) color melting point & boiling
point hardness phase of matter malleable ductile taste conductivity luster texture solubility
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Chemical Properties
properties that describes how the substance interacts with other substances or will act chemically
chemical change = an actual chemical reaction takes place and a NEW substance is formed
ex: combustion
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Examples of Chemical Properties
flammability reactivity combustion oxidation reacts with _____ endothermic exothermic forms a
precipitate
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Chemical ChangeEQ: How can chemical and physical changes be
determined in a laboratory setting?
Color change Temperature change = reaction is
either endothermic or exothermic Gas given off Precipitate formed = solid formed in
the reaction of two liquids
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Energy (temperature) Changes in Reactions
Endothermic reactions– Energy is put into the
reaction– Reaction stops as soon
as energy is no longer put into the reaction
– Ex: cooking Exothermic reactions
– Energy is given off in the reactions
– Ex: burning
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Exothermic Reactions
May require energy to be put into to the reaction in order to start or activate the reaction
Activation Energy = energy required to start an exothermic reaction
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Reducing Activation Energy
Catalysts are often used to reduce the activation energy required to start an exothermic reaction
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Chemical change vs. Physical change
ask the question, “Has a new substance been formed?”
“yes” = chemical change
“no” = physical change
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Examples of Problems
ex: 2H2 + O2 2H2O hydrogen gas combines with
oxygen gas to form water a new substance is formed a chemical reaction occurs
EQ: How can chemical and physical changes be
determined in a laboratory setting?
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Examples of Problems
: N2 + O2 + CO2 = air nitrogen gas combines with
oxygen gas and carbon dioxide gas and a few other gases mix
NO chemical reaction takes place physical change has taken place
in the gases
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Examples of Problems
Ice melting Phases change Solid Liquid No new substance is
formed…it is still water Physical change
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Malleable
A physical property that describes being able to be flatten or pounded onto sheets
This property is associated with metals.
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Ductile
A physical property that describes being able to be drawn into a wire.
This property is associated with metals.
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Luster
A physical property that describes how a substance reflects light
This property is often associated with minerals, gem stones, metals and nonmetals.
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Oxidation
A chemical property describing a substance reaction with oxygen
slow oxidation = rusting, tarnish, corrosion
fast oxidation = burning, exploding, combustion
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Density The amount of matter in a
given amount of space Density = mass ÷ volume D = m/v D = ?
Mass = m = 96.5 gramsVolume = v = 5 cm3
D = 96.5 g / 5 cm3 = 19.3 g/cm3
19.3 g/cm3 is the density of gold
The density of water = 1.0 g/mL
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BUOYANCEThe ability of a fluid (liquid or gas) to exert an upward force on an object immersed in it.If buoyant force = object’s weightthe object will float
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GAS LAWS
Boyle’s Law: pressure and volume
Volume decreases as Pressure increases
Pressure decreases as Volume increases
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Gas Laws
Charles’s Law: temperature & volume
Volume increases as Temperature increases
Volume decreases as Temperature decreases