UNIT 1–
Matter
What is matter anyway?
Matter is ANYTHING
that has MASS &
takes up SPACE
(has VOLUME)
Four States of Matter
 Solids
 very low KE (kinetic energy) particles vibrate but can’t
move around
 fixed shape
 fixed volume
Four States of Matter
 Liquids
 low KE - particles can
move over & around
each other but are still
close together
 variable shape
 fixed volume
Four States of Matter
 Gases
 high KE - particles have
enough energy to separate
and move throughout
container; so much so that
gases are mostly empty
space!
 variable shape
 variable volume
Four States of Matter
 Plasma
 Highest KE - particles collide with
enough energy to break into
charged particles (+/-)
 gas-like, variable
shape & volume
 stars, fluorescent
light bulbs
Fluids
 What is a fluid?
 a substance that can FLOW & has
particles that are able to move
around each other.
 What 2 phases of matter are
considered FLUIDS?
 Liquids & Gases
Properties of Fluids
 What is viscosity?
 The ability of a liquid to flow or the
resistance to flow. (Honey is
MORE viscous than water)
 What is buoyancy?
 The upward force a fluid exerts on
an object.
Properties of Fluids
 What 3 properties allow an object to
be “buoyant”?
1. The buoyant force exerted upward on the
object is ______________________ than the
force downward of the object’s weight.
2. The ___________________ of the object is
less than the _____________________ of the
fluid.
3. The weight of the water displaced by the
object is _________________ than the
_____________ of the object.
States of Matter…Test YOUR knowledge! 
Type of
Matter
Solid
Liquid
Gas
Plasma
Kinetic
energy
Shape
Volume
States of Matter…Test YOUR knowledge! 
Type of
Matter
Kinetic
energy
Shape
Volume
Solid
Very low
Definite/fixed
Definite/fixed
Liquid
Low
Indefinite/
not fixed/
variable
Definite/fixed
Gas
High
Indefinite/
Not fixed/
variable
Indefinite/
Not fixed/
variable
Plasma
Very high
Indefinite/
Not fixed/
variable
Indefinite/
Not fixed/
variable
Matter Flowchart
MATTER
yes
MIXTURE
yes
Is the composition
uniform?
Homogeneous
Mixture
(solution)
PURE SUBSTANCE
no
Heterogeneous
Mixture
Colloids
no
Can it be physically
separated?
yes
Can it be chemically
decomposed?
Compound
C. Johannesson
Suspensions
no
Element
Matter Flowchart
 Test yourself…
 graphite
element
 pepper
hetero. mixture
 sugar (sucrose)
compound
 paint
hetero. mixture
 soda
solution
Properties of &
Changes in Matter…
Density
Intensive vs. Extensive
Physical vs. Chemical
DENSITY
 Density is the measure of the MASS of a
substance to the VOLUME of a
substance at a given temperature.
 Density is expressed in g/mL or kg/L for
liquids and g/cm3 for solids.
 Density of a SUBSTANCE will determine
if the substance will SINK or FLOAT in
another substance. (recall buoyancy)
Accuracy vs. Precision
 Accuracy - how close a measurement
is to the accepted value
ACCURATE = CORRECTNESS
• Precision - how close a series of
measurements are to each other
PRECISE = CONSISTENT or
REPRODUCIBLE
Accurate
& Precise
Accurate,
not
Precise
Precise,
not
accurate
Neither
Accurate
nor
Precise
Example Problem
To determine the density of a
certain metal alloy, a chemist
measures the mass and volume
of each of four different samples
of the alloy. The chemist obtains
the density values shown in the
following:
Example Problem
Sample
Density
(measured)
1
5.87 g/cm3
2
5.89 g/cm3
3
5.83 g/cm3
4
5.92g/cm 3
Example Problem
Later, the chemist learns that the true
density of the alloy is 5.62 g/cm3.
Describe the chemist’s results in
terms of accuracy and precision.
a. accurate and precise
b. accurate, but not precise
c. precise, but not accurate
d. neither accurate nor precise
PHYSICAL CHANGES
 Physical Change
 changes the form of a substance without
changing its identity
 EX: cutting, dissolving, grinding
PHASE CHANGES
Changes of state
(phase changes) are
physical changes that
involve changes of
energy.
Phase Changes
(ARE physical change)
sublimation
melting
SOLID
vaporization
LIQUID
freezing
condensation
deposition
GAS
CHEMICAL CHANGES
 Chemical Change
 changes the identity of a substance
 products have different properties
 EX: tarnishing, burning, corroding
Physical vs. Chemical
 Indicators or Signs of a Chemical
Change (*important…you will need to
know this for the rest of the year!!!)
NEW substance formed
Change of color or odor
Release or formation of a gas
formation of a precipitate (solid
that settles…yes, a suspension)
change in light or heat
Physical vs. Chemical CHANGE
 You try it…(not in notes)
 rusting iron
chemical
 dissolving in water
physical
 burning a log
chemical
 melting ice
physical
 grinding spices
physical
Physical vs. Chemical
 Physical Property
 can be observed without changing the
identity of the substance
 Chemical Property
 describes the ability of a substance to
undergo changes in identity
Physical vs. Chemical
PROPERTY
 You try it…
 melting point
physical
 flammable
chemical
 density
physical
 magnetic
physical
 tarnishes in air
chemical
Other properties
 Conductivity- the ability of energy to
flow through something.
 Reactivity- how likely a substance is
to react with other substances
 Boiling Point- the point when a liquid
becomes a gas
 Freezing/Melting Point- the point
when a liquid becomes
a solid
Mine 
Scientific Notation
 In science, numbers can be very
small & very large (confusing!)
 Numbers can be expressed in
Scientific Notation:
Mx
n
10
1 ≤ M < 10
+n:
large #
Scientific Notation
 To convert into Sci. Notation:
Move decimal until there’s 1 digit to
its left. (# of places moved =
exponent)
Large # (>1)  positive exponent
Small # (<1)  negative exponent
Only include sig figs.
65,000 kg 
6.5 × 104 kg
Scientific Notation Practice
Problems
1. 2,400,000 mg 2.4 
6
10
mg
2. 0.00256 kg
2.56 
3. 7  10-5 km
0.00007 km
4. 6.2  104 mm
62,000 mm
-3
10
kg
Calculating with Scientific
Notation
(5.44 × 107 g) ÷ (8.1 × 104 mol) =
Type on your calculator:
5.44
2nd
EE
7
÷
8.1
2nd
EE
4
ENTER
= 671.6049383 = 670 g/mol = 6.7 × 102 g/mol