Properties of Matter
What is matter?
Matter is anything that has
mass and volume.
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Measuring Matter
Volume of a liquid
– Graduated cylinder- read from bottom of meniscus
Volume of solid
– Length X Width X Height
Volume of Irregular Shaped Objects
– Water Displacement
Indirect Measuring
– Large objects-take a core sample and use a formula
– Small objects-weigh 100 and then divide weight by
100 to get one small objects weight
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Classification of Matter
MATTER
Has mass and
volume
PHASES
Solid, liquid,
gas or plasma
PROPERTIES
PHYSICAL
CHEMICAL
MADE UP OF
Element, compound
or mixture
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Phases of Matter
SOLID, LIQUID, GAS, or PLASMA
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Phases of Matter
Solids - definite shape and volume
Atoms are held close together by strong bonds
 Movement is slow
 Crystalline Solids (crystals) - atoms are
arranged in regular fashion (geometric)
• Ex. - ice, salt, diamonds


Amorphous Solids - atoms LACK a regular
arrangement
• Ex. - rock, glass, wax
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Phases of Matter - Continued
Liquids - NO definite shape but definite
volume
Bonds are weaker and atoms are spaced
apart
 They take the shape of container they
are in
Examples: oil, water, syrup, OJ, milk

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Phases of Matter - Continued
Gases - NO definite shape OR volume

Bonds are weakest and atoms far apart

Expands to fill the container they are in
• Examples - air, oxygen, smoke
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Phases of Matter - Continued
Plasma
• Gas like mixture of + and – charged particles

Movement very rapid (10,000˚C)

99% of mass of our solar system

Examples: Sun, Stars and Lightning
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Classifying Matter
• Physical
Properties are
those that can be
observed without
changing the
identity of the
substance
• Chemical
Properties are
those that describe
how a substance
changes into other
new substances
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PROPERTIES OF MATTER
PHYSICAL
CHEMICAL
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Size
Shape
Texture
Color
Phase
Conductor
Ductile
Malleable
Shiny/luster
Density
Mass
Tasteless
Dissolves
Odorless
Hardness
Brittle
Tensile strength
Fluid
Viscosity
Elasticity
Buoyant
Melting point
Freezing point
Boiling point
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Flammability
Changes color
Reacts with
Combustible
Corrosive
Volatile
Explosive
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Physical Properties of Matter
• Viscosity –
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• Measure of the material’s resistance to flow
• High-viscosity liquids take longer to flow
• Example: Ketchup when comparing to
water
• Low-viscosity liquids flow easier
• Example: Tomato Juice flows
easier than ketchup
• Temperature raising-viscosity decreases
except in gases.
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Physical Properties of Matter – Cont.
• Elasticity –
• Measure of ability to be stretched and
then return to its original size.
• Example:Rubber Bands, Elastic, and
Playground Balls
Question: Which ball would you rather play
basketball?
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Physical Properties of Matter – Cont.
• Malleability –
• Ability to be hammered into sheets
• Example: Gold &Silver Coins, Aluminum
Foil and Soda Cans
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Physical Properties of Matter – Cont.
• Brittleness –
• measures a material’s tendency to
shatter upon impact
• Example: Sulfur, Calcium and Glass
• Hardness –
• Resistance to breaking or scratching
• Example: diamonds
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Physical Properties of Matter – Cont.
• Luster –
• shininess
• Example: Gold, Silver, Mercury
• Ductility –
• ability to be pulled into wires
• Example: Most metals (Copper, Silver)
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Physical Properties of Matter –
Cont.
Tensile Strength• Measure of how much
pulling, or tension, a
material can
withstand before
breaking
• Property of fibers,
ropes, cables, girders
• DuPont Kevlar-5
times tensile strength
of steel
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Physical Properties
Melting Point –
• Temperature at which a solid changes
to a liquid
• Example: Ice  water
Freezing Point –
• Temperature at which a liquid changes
to a solid
• Example: Water  Ice (0°C)
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Physical Properties
Boiling Point –
• Temperature at which a liquid changes
into a gas
• Example: Water  vapor (100˚ C)
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Physical Properties of Matter – Cont.
• Density –
• The amount of mass in a given volume
• How tightly packed the atoms or molecules
are in a substance
• Formula to calculate density is:
Density = Mass
Volume
• Units are expressed as:
• g/mL or g/L for liquids (remember the graduated
cylinder)
• g/cm3 for solids
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Density of a Fluid
Fluid• Any matter that is able to flow
• Liquids and gases
• Density of a liquid might be different from the
density of the same solid
• Most materials are denser in solid phase
than their liquid phase
• Exception- Water-freezes with air spaces so
it is less dense and floats.
• Density of liquid water is 1 g/ml
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Physical Properties of Matter – Cont.
• Buoyancy –
• Upward force a fluid exerts on an object
•Determines whether the object will sink
or float
• Example: Buoyancy of water keeping
you afloat while swimming
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Buoyancy
Buoyancy force is LESS
then object’s weight,
object will SINK
Buoyancy force is EQUAL
to the object’s weight,
object will FLOAT
Buoyancy force is MORE
then object’s weight,
object will FLOAT IN
AIR
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Archimedes's Principle
• Greek mathematician, 3rd century BC
• Principle states-The buoyancy force on an object
in a fluid is equal to the weight of the fluid
displaced by the object
Buoyancy of Gasses
• Balloon floats because it displaces a very large
volume of air
• Volume of air displaced weighs more than the
balloon
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Classification of Matter
MATTER
Has mass and
takes up space.
SUBSTANCES
Definite Composition
ELEMENT
Only 1 Kind
of Atom
COMPOUND
Two or More
Kinds of
Atoms
MIXTURES
Variable Composition
HOMOGENEOUS
Solution evenly
mixed
HETEROGENEOUS
Solution
Unevenly mixed
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Classification of Matter
Matter can be divided into 2 categories:
SUBSTANCES & MIXTURES
• Substances can NOT be separated into
different kinds of matter by physical means.
• Mixtures can be separated into different
kinds of matter by physical means.
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Classification of Matter
What are substances?
In science, substances are limited to elements
and compounds.
– Elements
• Any substance in which all the atoms in a
sample are alike, one kind of matter
• Examples: Carbon, Sodium and Oxygen
– Compounds
• 2 or more elements chemically
combined in a fixed ratio (subscript)
• Usually has different appearance from
elements that make it up
• Examples: Water – H2O and Salt - NaCl
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Classification of Matter
• Atom-smallest
possible particle of
an element
• Molecule- smallest
possible particle of
a compound
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Classification of Matter
What are mixtures?
2 or more substances that can be separated by
physical means
Do not always contain the same amounts of the
different substances that make them up
–Homogeneous
• same throughout, particles so tiny that cannot
be seen, don’t settle out or scatter light
• Examples: milk, salt water and cola
–Heterogeneous
• a mixture in which different materials can be
easily distinguished
•Suspension-visible particles settle-muddy water
• Examples: Sand/water, Italian salad dressing,
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pizza and dry soups
Changes in Matter
MATTER
PHYSICAL
CHANGES
CHEMICAL
CHANGES
NUCLEAR
CHANGES
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Changes in Matter
Physical
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Melting
Freezing
Boiling
Evaporation
Cutting
Splitting
Chopping
Sublimation
Chemical
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Chemical reaction
Photosynthesis
Respiration
Digestion of food
Nuclear
•Fission
•Fusion
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Physical vs. Chemical Change
Physical Change Does NOT create a new substance, affects only the
physical properties.
A change in size, shape or form (phases of matter).
Appearance changes – not chemical makeup
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Physical Change
Vaporization• process at which a liquid
changes to a gas by
increasing the
temperature to the liquids
boiling point
• Example: water boils to
form steam at 100° C
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Physical Change
Evaporation• process at which a liquid
changes to a gas. The
liquid is not boiling.
Example: A puddle drying
up or sweat drying
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Physical Change
Condensation –
• Process at which a gas becomes a liquid
•Gas cooled below its boiling point
• Example: water vapor  water, dew in the
morning, glass of ice tea in hot weather.
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Physical change
Sublimation –
• When a solid changes directly to a gas
•The matter doesn’t melt
• Example:snow, dry ice
and glaciers
Deposition-
•Gas changes directly into a solid
•Ex. Fire extinguisher
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Chemical Change
Chemical Change A change in which a NEW substance is created
End products are chemically different from the
original.
Corrosive-dissolving away of a metal-rusting
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Four Signs or Evidence of a
Chemical Change
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Gas forms
Permanent color change
Heat/or light energy is given off
Precipitate forms. A precipitate is an
insoluble substance that forms out of
solution.
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Physical vs. Chemical Change
Identify the following as physical or chemical change.
Ice cube melting.
People eating.
Wood burning.
Slicing an apple into pieces.
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Changes in Matter - Continued
Exotic Super Hot
• Nucleus of atom
comes apart
• Particle accelerates
Exotic Super Cold
• Below -270˚ C
• Superfluids from gases
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Charles’ Law
Jacques Charles, French scientist (1742-1823)
• Law states-volume of a gas increases when
temperature increases and reverse, volume
of gas decreases when temperature
decreases.
• V1 / T1 = V2 / T2
– Temperature must be in Kelvin degrees (+273)
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Boyle’s Law
Robert Boyle-British scientist (1627-1691)
• Law states-as pressure of a gas increases,
its volume decreases proportionately and
reverse pressure of gas decreases, its
volume increases proportionately.
• P1 V1 = P2 V2
• Pascal-unit for pressure (Pa) (kPa)
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