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Definition, States,
Change of State, Types
of Matter, and Properties and
Changes
Unit 1B p. 2-5.
MATTER, Definition, States, and
Change of State
At the conclusion of our time
together, you should be able to:
1. Define matter
2. Define the various states of matter and
draw an example of each state
3. Recognize that particle motion
determines the state of matter
Matter:
 Anything that has mass and takes up
space
Matter is made up of building blocks:
atom – smallest unit of an element.
element – a pure substance made of
only one kind of atom.
compound – made of two or more atoms
that are chemically combined.
FYI
 90% of the Earth’s crust is made up of
only 5 elements:
Oxygen
49.2%
Silicon
25.7 %
Aluminum
7.5%
Iron
4.7%
Calcium
3.4%
States of Matter
 Solid Definite volume and shape
 Particles are tightly packed
 Slight expansion when heated
 Incompressible
Solid
Vibration
around fixed
points
States of Matter
 Liquid Has definite volume, but no definite
shape
(assumes the shape of the container)
 Particles are loosely packed
(can flow by sliding over each other)
 Easily expand when heated
 Considered incompressible
Liquid
Vibration
around
sliding
points
States of Matter
 Gas No definite shape or volume
 Expand to fill the container
 Particles are spaced far apart
 Compressible
Gas
Vibration
around
moving
points
States of Matter
 Plasma Consists of electrically charged
particles
 It’s an ionized gas
 Common in space, but very rare on
Earth
 Found in lightning, fluorescent lights
and neon signs
Plasma
When atoms
are so hot,
they lose ALL
of their
electrons.
“Super-heated
Gas”
Energy Amounts in States of Matter
 Solid- little energy, particles vibrate and
rotate
 Liquid- more energy, they move freely
by sliding over each other
 Gas- even more energy, move quickly
 Plasma- most energy, move extremely
fast
All You Really Need To Know
You Can Learn From Noah's Ark
 5. Plan ahead. It wasn't raining when
Noah built the ark.
 6. Build your future on high ground.
Solid
Made of
Atoms
Holds
its shape
Atoms move
past each
other
Liquid
Gas
Plasma
States of Matter
Changes of State
Energy
Gas
Energy
Liquid
Energy
Solid
Names of Phase Changes






Solid to Liquid
Liquid to Gas
Gas to Liquid
Liquid to Solid
Solid to Gas
Gas to Solid
=
=
=
=
=
=
Melting
Boiling/evaporation
Condensation
Freezing
Sublimation
Deposition
D
e
p
o
s
i
t
i
o
n
Boiling
Melting
Condensation
Freezing
Sublimation
When a solid
turns directly
into a gas.
Dry ice is
solid CO2
Moisture that collects on the
outside of a cold glass results
from the process of…
1. evaporation.
2. condensation.
3. sublimation.
4. vaporization.
Matter,
Classify Matter
At the conclusion of our time
together, you should be able to:
1. Classify a mixture of matter based on
their physical and chemical properties
2. Characterize various types of matter
Types of Matter
 Pure Substance Matter with a fixed composition
 It has distinct properties
 Examples =
elements
compounds
Types of Matter
 Mixtures Most matter is a mixture
 The composition is not fixed (changes
from sample to sample)
 Two Types –
Homogeneous
Heterogeneous
Homogeneous Mixtures
 Composition is uniform throughout
 Solution Particle size = 0.01 – 1 nm
 Doesn’t settle out upon standing
 Can’t be separated by filtering
 Doesn’t scatter light
 Example = salt water
Homogeneous Mixtures
 Colloid Particle size = 1 – 1000 nm
 Doesn’t settle out upon standing
 Can’t be separated by filtering
 Scatters light (Tyndall Effect)
 Examples = milk, gelatin, smoke
Heterogeneous Mixtures - Suspension
 The sample varies in composition,
properties and appearance
 No uniformity
 If a suspension:
 Particle size is greater than 1000 nm
 Particles settle out upon standing
 Can be separated by filtration
 Might scatter light
 Examples = soil, trail mix, pond water
Let’s Look at Some Examples:
 Mixtures are variable combinations of 2
or more pure substances.
Heterogeneous –
visibly separate phases
Homogeneous –
Same throughout
Pure substance
Only ONE element
or compound.
(distilled water)
vs.
Mixture
has 2 or more
elements/
compounds.
Distilled Water is
a compound.
an element.
a solution.
a mixture.
Air is a mixture of several gases.
Name
Formula
amount
Nitrogen
N2
78 %
Oxygen
O2
21 %
Argon
Ar
1%
Carbon
CO2
Dioxide
0.03 %
Air is a mixture of several gases
Name
Formula
Amount
Neon
Ne
0.002 %
Methane
CH4
0.0002 %
Helium
He
0.000524 %
Krypton
Kr
0.000114 %
Hydrogen
H2
0.00005 %
Xenon
Xe
0.0000087 %
Atoms are NOT the same as molecules.
Air and oxygen are NOT the same.
Helium and hot air are NOT the same.
Helium and hot air are NOT the same.
What’s the MATTER
Classify Matter
Let’s Put it All Together in
a Chart!!
This is on p. 5
Yes
MATTER
No
Can it be physically
separated?
MIXTURE
PURE SUBSTANCE
Yes
No
Can it be chemically
Is the composition
uniform?
decomposed?
Yes
HomoNo
Heterogeneous
geneous
Mixture
Compound
Element
Mixture
(solution)
Colloids &
Putting sand and salt together
makes
a compound.
an element.
a mixture.
a solution.
Pure Water is
a compound.
an element.
a solution.
a mixture.
Tap Water is
a compound.
an element.
a solution.
a mixture.
An atom is to an element, as a
molecule is to a
metal.
nonmetal.
metalloid.
compound.
If different kinds of atoms are
represented by different colored
dots, which picture represents a
sample of a compound?
If different kinds of atoms are
represented by different
colored dots, which picture
below represents a mixture?
Which of the following illustrations
represents a pure substance?
Salt (NaCl) is a common
substance. Salt is which of these?
atom
element
compound
mixture
A chocolate chip cookie is an
example of a __________,
because ______________.
a. compound, the ingredients are chemically
bonded.
b. compound, it is the same throughout.
c. mixture, you can separate out the chips.
d. mixture, you cannot distinguish between
the ingredients.
Which of the following is a
compound?
• oxygen
• water
• nitrogen
• air
Physical Change
Physical
A change in matter from one form
to another without changing its
chemical properties
(most can be reversed)
No change in atoms/molecules
Physical Change
 Examples =
 Change in state or phase change
 Dissolving
 Compressing
 Light emission/absorption
 Electrons passing through metals
Physical Change
More Examples =
 boiling of a liquid
 melting of a solid
 dissolving a solid in a
liquid to give a
homogeneous mixture
 making a solution
Properties
 Every substance has a unique set of
properties (characteristics that identify
that substance)
 Physical Properties Properties that can be measured
without changing the identity and
composition of the substance
Physical Property Examples






Color
Odor
Density
Melting Point
Boiling Point
Hardness
Solubility
Chemical Change
2
1
Chemical
A change in matter from one form to
another by changing its composition (most
cannot be reversed)
Bonds are made / broken
Chemical change or chemical reaction —
transformation of one or more atoms or molecules into
one or more different molecules.
Sure Signs of a Chemical Change
“Chemists Get Practice Trying Labs”
 Color Change
 Gas Produced (not from
boiling!)
 Precipitate – a solid
formed by mixing two
liquids together
 Temperature Change
 Light
Chemical Properties
 Properties that describe the way a
substance may change to form other
substances
 Only observed when a chemical reaction
takes place
Chemical Properties
 Properties that describe the way a
substance may change to form other
substances
 Only observed when a chemical reaction
takes place
Chemical Property Examples





Combustible
Reactive with water or acid
Flammable
Corrosive
Decomposes in air
Remember the Law of Conservation
of Mass
 In a physical change or a chemical
reaction, mass is neither created or
destroyed
(Antoine Lavoisier)
Physical vs. Chemical Change
 Examples:
 melting
physical
 flame produced
chemical
 paper cut
physical
 dissolving salt
physical
in water
 tarnishes in air
chemical
Physical vs. Chemical Change
 Examples:
 rusting iron
chemical
 mixing mud and
physical
water
 burning a log
chemical
 freezing water
physical
 grinding spices
physical
Physical vs. Chemical Properties
 Physical Properties Properties that can be measured
without changing the identity and
composition of the substance
 Chemical Properties Properties that can be measured by
changing the identity and composition
of the substance
Physical vs. Chemical Property
 Examples:
 melts at 55oF
physical
 flammable
chemical
 will tear easily
physical
 will dissolve in
physical
water
 will tarnish
chemical
Physical vs. Chemical Properties
 Examples:
 will rust
chemical
 mixture can be
physical
separated by boiling
 burns
chemical
 freezes at -20oC
physical
 can be crushed
physical