1. Properties of Matter (solid, Liquid, and gases).ppt

properties of solid, liquid and, gases

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In this lesson, you
will learn how
properties can be
used to classify
and identify
matter.
CHEMISTRY&YOU
Why are windows made of glass?

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Describing Matter
Why do all samples of a substance
have the same intensive properties?
Describing Matter

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What you observe when you look at a
particular sample of matter is its properties.
•Is a solid shiny or dull?
•Does a liquid flow quickly or slowly?
•Is a gas odorless, or does it have a smell?
Describing Matter

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Properties used to describe matter can be
classified as extensive or intensive
properties.
Describing Matter

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Recall that matter is anything that has
mass and takes up space.
•The massof an object is a measure of the
amount of matter the object contains.
Extensive Properties
Describing Matter
–The mass of a
basketball is greater
than the mass of a golf
ball.

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The volumeof an object is a measure of
the space occupied by the object.
•The volume of a basketball is greater than the
volume of a golf ball.
Extensive Properties
Describing Matter

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Mass and volume are both examples of
extensive properties.
•An extensive propertyis a property that
depends on the amount of matter in a
sample.
Extensive Properties
Describing Matter

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There are properties to consider when
selecting a basketball besides mass and
volume.
•The outer covering may be made of
leather, rubber, or a synthetic composite.
–Each of these materials has different
properties that make the basketballs
suitable for different playing
situations.
Intensive Properties
Describing Matter

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For example, leather balls are suitable for
indoor play but not outdoor play.
•Leather balls absorb water and dirt more
than rubber balls do.
Intensive Properties
Describing Matter

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Absorbency is an example of an intensive
property.
•An intensive propertyis a property that
depends on the type of matter in a sample,
not the amount of matter.
Intensive Properties
Describing Matter

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Each object in this figure has a
different chemical
makeup, or
composition.
Identifying a Substance
Describing Matter
•The soda can is mainly
aluminum.
•The watering can is
mainly copper.

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Matter that has a uniform and definite
composition is called a substance.
•Aluminum and copper are examples of
substances, which are also referred to as
pure substances.
Identifying a Substance
Describing Matter

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Every sample of a given substance
has identical intensive properties
because every sample has the same
composition.
Identifying a Substance
Describing Matter

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Aluminum and copper have some properties in
common, but there are differences besides their
distinctive colors.
•Aluminum is highly reflective and is often used in silver
paint.
•Pure copper can scratch the surface of aluminum
because copper is harder than aluminum.
•Copper is a conductor of heat or electric current.
•Copper and aluminum are both malleable, which means
they can be hammered into sheets without breaking.
Identifying a Substance
Describing Matter

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Hardness, color, conductivity, and
malleability are examples of physical
properties.
•A physical propertyis a quality or
condition of a substance that can be
observed or measured without changing the
substance’s composition.
Identifying a Substance
Describing Matter

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Physical Properties of Some Substances
Substance StateColor Melting point
(°C)
Boiling point
(°C)
Neon Gas Colorless –249 –246
Oxygen Gas Colorless –218 –183
Chlorine Gas Greenish-yellow –101 –34
Ethanol LiquidColorless –117 78
Mercury LiquidSilvery-white –39 357
Bromine LiquidReddish-brown –7 59
Water LiquidColorless 0 100
Sulfur SolidYellow 115 445
Sodium chlorideSolidWhite 801 1413
Gold SolidYellow 1064 2856
Copper SolidReddish-yellow 1084 2562
InterpretData
This table lists physical properties for some substances.
•The states of the substances are given at room temperature.

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Physical properties can help chemists
identify substances.
•For example, a colorless substance that
was found to boil at 100˚C and melt at
0˚C would likely be water.
•A colorless substance that boiled at 78˚C
and melted at –117˚C would definitely not
be water. It would likely be ethanol.
Identifying a Substance
Describing Matter

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Glass is often used to make windows,
while copper is often used in electrical
wires. What properties of glass make it
a desirable material to use for
windows?
CHEMISTRY&YOU

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Glass is often used to make windows,
while copper is often used in electrical
wires. What properties of glass make it
a desirable material to use for
windows?
Glass is transparent, so it can be seen through;
hard, so it stays in place within window frames;
and heat resistant, so it helps prevent the
transfer of heat between outside and inside.
CHEMISTRY&YOU

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You want to compile a list of
properties of a substance, but you
don’t have a way to measure mass or
volume. What kinds of properties can
you determine without knowing the
amount of matter in the sample?

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You want to compile a list of
properties of a substance, but you
don’t have a way to measure mass or
volume. What kinds of properties can
you determine without knowing the
amount of matter in the sample?
You can determine the sample’s intensive
properties.

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States of Matter
What are three states of matter?
States of Matter

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Depending on the circumstances, you use
three different words to refer to water—
water, ice, and steam.
•Water, which is a common substance, exists in
three different physical states.
–So can most other substances.
States of Matter

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Three states of matter are solid, liquid,
and gas.
States of Matter

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A solidis a form of matter that has a definite
shape and volume.
•The shape of a solid doesn’t depend on the
shape of its container.
Solids
States of Matter

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A solidis a form of matter that has a definite
shape and volume.
•The shape of a solid doesn’t depend on the
shape of its container.
Solids
States of Matter
•The particles in a
solid are packed
tightly together, often
in an orderly
arrangement.

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A solidis a form of matter that has a definite
shape and volume.
•As a result, solids are almost incompressible;
that is, it is difficult to squeeze a solid into a
smaller volume.
•In addition, solids expand only slightly when
heated.
Solids
States of Matter

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The particles in a liquid are in
close contact with one
another, but the arrangement
of particles in a liquid is not
rigid or orderly.
Liquids
States of Matter

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The particles in a liquid are in
close contact with one
another, but the arrangement
of particles in a liquid is not
rigid or orderly.
Liquids
States of Matter
•Because the particles in a
liquid are free to flow, a liquid
takes the shape of the
container in which it is placed.

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The particles in a liquid are in
close contact with one
another, but the arrangement
of particles in a liquid is not
rigid or orderly.
Liquids
States of Matter
•However, the volume of the
liquid doesn’t change as its
shape changes.

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The volume of a liquid is fixed or constant.
•Thus, a liquidis a form of matter that has
an indefinite shape, flows, and yet has a
fixed volume.
Liquids
States of Matter

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The volume of a liquid is fixed or constant.
•Thus, a liquidis a form of matter that has
an indefinite shape, flows, and yet has a
fixed volume.
Liquids
States of Matter
–Liquids are almost incompressible.
–However, they tend to expand slightly when
heated.

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•Like a liquid, a gas takes the shape of
its container.
•But, unlike a liquid, a gas can expand to
fill any volume.
Gases
States of Matter

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A gasis a form of matter that
takes both the shape and
volume of its container.
Gases
States of Matter

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A gasis a form of matter that
takes both the shape and
volume of its container.
Gases
States of Matter
•The particles in a gas are usually
much farther apart than the
particles in a liquid.

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A gasis a form of matter that
takes both the shape and
volume of its container.
Gases
States of Matter
•The particles in a gas are usually
much farther apart than the
particles in a liquid.
•Because of the space between
particles, gases are easily
compressed into a smaller volume.

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The words vaporand gasare sometimes used
interchangeably. But there is a difference.
•The term gasis used for substances, like
oxygen, that exist in the gaseous state at
room temperature.
•Vapordescribes the gaseous state of a
substance that is generally a liquid or solid
at room temperature, as in water vapor.
Gases
States of Matter

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A substance is in a state in which it
takes the shape of its container. What
state or states could it be in?

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A substance is in a state in which it
takes the shape of its container. What
state or states could it be in?
The substance could be either a liquid or a gas,
as each takes the shape of its container.

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Physical Changes
How can physical changes be
classified?
Physical Changes

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The melting point of
gallium metal is 30˚C.
The figure at left
shows how the heat
from a person’s hand
can melt a sample of
gallium.
Physical Changes

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The shape of the sample changes during
melting as the liquid begins to flow, but
the composition of the sample does not
change.
•Melting is a physical change.
•During a physical change, some properties
of a material change, but the composition of
the material does not change.
Physical Changes

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•Words such as boil, freeze, melt,and
condenseare used to describe
physical changes.
•So are words such as break, split,
grind, cut, and crush.
–There is a difference between these
two sets of words. Each set describes
a different type of physical change.
Physical Changes

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Physical changes can be classified
as reversible or irreversible.
•Melting is an example of a reversible
physical change.
–If a sample of liquid gallium cools
below its melting point, the liquid
will become solid.
Physical Changes

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All physical changes that involve a
change from one state to another are
reversible.
•Cutting hair, filing nails, and cracking
an egg are examples of irreversible
physical changes.
Physical Changes

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Water boils and becomes water vapor.
Is this a reversible or irreversible
physical change?

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Water boils and becomes water vapor.
Is this a reversible or irreversible
physical change?
It is a reversible physical change because it
involves a change from one state to another.

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Alters the chemical composition or identity of a
substance and makes new substances.
Burning paper
Digesting food
Rotting
Iron reacting with oxygen gas
A chemical change is also called a chemical
reaction.
Chemical Changes

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Is it Physical or Chemical?
Change Physical Chemical
Melting cheese
Burning wood
Milk souring
Wadding up paper
Bicycle rusting

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Is it Physical or Chemical?
Change Physical Chemical
Melting cheese
Burning wood
Milk souring
Wadding up paper
Bicycle rusting

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Every sample of a given substance has
identical intensive properties because
every sample has the same
composition.
Three states of matter are solid, liquid,
and gas.
Physical changes can be classified as
reversible or irreversible.
Key Concepts

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Glossary Terms
•mass: a measure of the amount of matter that
an object contains; the SI base unit of mass is
the kilogram
•volume: a measure of the space occupied by
a sample of matter
•extensive property: a property that depends
on the amount of matter in a sample
•intensive property: a property that depends
on the type of matter in a sample, not the
amount of matter

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Glossary Terms
•substance: matter that has a uniform and
definite composition; either an element or a
compound; also called pure substance
•physical property: a quality or condition of a
substance that can be observed or measured
without changing the substance’s composition
•solid: a form of matter that has a definite
shape and volume
•liquid: a form of matter that flows, has a fixed
volume, and has an indefinite shape

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Glossary Terms
•gas: a form of matter that takes the shape
and volume of its container; a gas has no
definite shape or volume
•vapor: describes the gaseous state of a
substance that is generally a liquid or solid at
room temperature
•physical change: a change during which
some properties of a material change, but the
composition of the material does not change

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Physical Property-A trait of
matter that can be observed or
measured without changing the
chemical composition of the
matter.
No chemical reactions allowed!

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1. Color–how the object
absorbs and reflects light

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2. Texture–how the
substance looks and feels.

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3. Temperature
A measure
of the
average
kinetic
energy
(energy of
motion) of
particles in a
substance.

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4. Mass
The amount
of matter in
an object
(in g or kg).

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5. Volume
The amount
of space an
object
occupies
(in mL, L,
cm
3
, m
3
,
etc.)

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6. Density–the ratio of mass to
volume; reflects the degree of
packing of particles in matter.
D = m/v

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Lowest density element:
Hydrogen
0.0009 g/cm
3

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Highest density element:
Osmium
23 g/cm
3

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7. Luster
The way
that a
substance
reflects
light
(metallic,
non-
metallic,
glassy,

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8. Ductility
Ability of a
substance
to be
stretched
into a wire.

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9. Malleability
Ability of a
substance to
be
hammered
flat and to
retain the
new shape.

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10. State(phase) of matter
What is the 4
th
state of
matter (rare on Earth)?

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11)Melting Point/Freezing
Point -
The exact temperature at
which a solid becomes a
liquid or a liquid becomes
a solid.
For H
2O, what
temperature is this?
12) Boiling Point/
Condensation Point -
The exact temperature at
which a liquid becomes a
gas or a gas becomes a
liquid.
For H
2O, what
EVERY PURE
SUBSTANCE HAS AN
EXACT
MELTING/FREEZING

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Chemical Property-A trait of
matter that can only be observed if a
substance has the property. In the
process of testing the chemical
property, the substance changes
composition if it has that property.
i.e. Does the substance chemically
“react with”something else?

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1)Reactivity with oxygen :
rusting (iron)
tarnishing (silver, copper, brass, etc)

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2) Reactivity with water:

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3) Reactivity with acids or bases:

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4)Combustibility or Flammability:

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5) Chemical formula (chemical composition):
What something is made of is alwaysa chemical
property.
Ex: rust is Fe
2O
3
water is H
2O
diamond is C

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Allchemical
properties are
intensive. None
are extensive.
Why?

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Allchemical
properties are
intensive. None
are extensive.
Why?
Because chemical properties never depend on
how much of a substance is present, but only
on what kind of particles make up the
substance.