UNIT 1–
Matter
What is matter anyway?
Matter is ANYTHING
that has MASS &
takes up SPACE
(has VOLUME)
Kinetic Molecular Theory
 KMT=Kinetic Molecular Theory
 Particles of matter are always in
motion.
 The kinetic energy (speed) of these
particles increases as temperature
increases.
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
Pure Substances: only TWO
types…element OR compound!
Element
 composed of identical atoms
 Found on the PERIODIC TABLE
 EX: copper wire, aluminum foil
Pure Substances: only TWO
types…element OR compound!
Compound
 composed of 2 or more
elements in a fixed ratio
 It has a chemical formula!!!
 properties differ from those
of individual elements
 EX: table salt (NaCl)
Pure Substances
 Law of Definite Composition
 A given compound always contains
the same, fixed ratio of elements.
 In other words, water is always H2O
with a 2:1 ratio of H to O and
hydrogen peroxide is always H2O2
with a 2:2 ratio of H to O.
C. Johannesson
Pure Substances
 Law of Multiple Proportions
 Elements can combine in different
ratios to form different compounds.
 Same as before, ratios matter. You
can have the same elements, such as
H & O combined in DIFFERENT
ratios. H2O (water) and H2O2
(peroxide) are two very different
compounds!!!
Pure Substances
 Additional example…
Two different compounds,
each has a definite composition.
A. 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
Mixtures
 Variable combination of 2 or more pure
substances. NOT chemically combined!
Heterogeneous
Homogeneous
Mixtures
 Homogeneous Mixtures are
called Solutions
 Appear the same throughout
 very small particles
 no Tyndall effect (light doesn’t
scatter)
 particles don’t settle; they are
dissolved
 EX: rubbing alcohol
Mixtures
 Heterogeneous Mixtures:
Two Types
 Colloid
 medium-sized particles
 Tyndall effect (will scatter
light)
 particles don’t settle
(they’re too small)
 EX: milk
Mixtures
 Suspension
 large particles
 Tyndall effect
 particles settle
(because they are so
large)
 EX: fresh-squeezed
lemonade; pond water
C. Mixtures
 You try…
 mayonnaise
colloid
 muddy water
suspension
 fog
colloid
 saltwater
solution
 Italian salad
dressing
suspension
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)
DENSITY
 Solving density problems involves using
math.
 Recall the formula Density =
MASS
VOLUME
 EX: A gold colored ring has a mass of 18.9 g
and a volume of 1.12 mL. Is the ring pure gold
(Au)? The density of pure gold is 19.3 g/mL.
18.9g/1.12mL= 16.9 g/mL
The ring is NOT pure gold because the
density is not the same as pure gold.
DENSITY
 Solving more advanced density
problems is easy using a method known
as DIMENSIONAL ANALYSIS.
 Dimensional analysis is known as the
“FACTOR-LABEL” Method:
 A method used to “factor” out
(cancel) labels (units)
g
cm 
g
3
cm
3
DENSITY
Solve the following: What volume would a
0.871 gram sample of air contain if the
density of the air is 1.29 g/L?
KNOWNS: 0.871 g and 1.29 g/L
UNKNOWNS: ? L
CALCULATIONS:
0.871 g
1L
= 0.68 L
1.29g
EXPLANATION: The air occupies a space
0.68L.
Significant Figures
 Figures (values) that indicate
precision of a measurement.
 Recording Sig Figs
Sig figs in a measurement include
the known digits plus a final
estimated digit
2.35 cm
Counting Sig Figs
Count all numbers EXCEPT:
Leading zeros:
0.0025  2 sig figs
Trailing zeros without
a decimal point:
 2,500  2 sig figs
Atlantic-Pacific Method
Pacific Ocean
PRESENT
“_________”
Atlantic Ocean
ABSENT
“ _______”
Atlantic-Pacific Method:
1. Decimal point is PRESENT:
 count significant figures from the
LEFT (Pacific side)
Decimal point is ABSENT:
 count significant figures from the
RIGHT (Atlantic side)
2. Start counting significant figures at
the first nonzero number and don’t
stop until there are no more digits.
Practice Counting Sig Fig
1. 23.50
4 sig figs
2. 402
3 sig figs
3. 5,280
3 sig figs
4. 0.080
2 sig figs
5. 0.006700
4 sig figs
Practice Counting Sig Fig
 Round the number at left to the
number of significant figures stated in
each column
Number
80.405
29,350
4 sig
figs
3 sig
figs
2 sig
figs
1 sig
fig
80.4
1
80.4
80.
80
29,00
0
30,00
0
29,35 29,40
0
0
Number vs. Quantity
 A number
without a unit
is a “naked”
number
 Quantity -
number + unit
UNITS MATTER!! EVERY # MUST
HAVE A UNIT!!!
Extensive vs. Intensive
 Extensive Property
 depends on the amount of matter
present
 Can be “extended” or changed
 Intensive Property
 depends on the identity of substance,
not the amount
A. Extensive vs. Intensive
 Examples:
 boiling point
intensive
 volume
extensive
 mass
extensive
 density
intensive
 conductivity
intensive
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
Percent Error
 Indicates accuracy of a
measurement
% error 
actual - experiment al
What you
calculate
actual
 100
What it should be
Small % = more accurate
Large % = less accurate
Percent Error
 A student determines the density of a
substance to be 1.40 g/mL. Find the %
error if the accepted value of the
density is 1.36 g/mL.
% error 
1.40 g/mL  1.36 g/mL
1.36 g/mL
% error = 2.9 %
 100
Proportions
Direct Proportion
y
X as Y
• Inverse Proportion
X as Y
x
y
x
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
Properties of Matter
 Conservation of mass: The mass of all
substances before a chemical change
equal the mass of all substances
remaining after the change.
 Exothermic—heat is released
 Exergonic—energy is released
 Endothermic—heat is absorbed
 Endergonic—energy is absorbed
EXO- means “out”
ENDO- means “in”
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
Calculating Rules:
Multiplying & Dividing :
The # with the fewest sig figs
determines the # of sig figs in the
answer.
(13.91g/cm3)(23.3cm3) = 324.103g
4 SF
3 SF
3 SF
324 g
Calculating Rules:
Adding & Subtracting:
 The # with the lowest decimal
value determines the place of the
last sig fig in the answer.
3.75 mL
+ 4.1 mL
7.85 mL  7.9 mL
224 g
+ 130 g
354 g  350 g
Significant Figures Practice
Problems
1. 2.066 g
2. 85.6 cm
3. 38 g
4. 1.13 g
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