Matter – Properties
and Changes
Chap. 3
Can you think of
anything that is
pure?
I. Substance
(Pure) Substance
Matter that has a
constant, unchanging
composition
I. Substance
II. Properties of matter
I. Substance
II. Properties of matter
A. Extensive vs. Intensive
Extensive
Property
Intensive
Property
Extensive
Property
Depends on amount
of substance
Intensive
Property
Extensive
Property
Depends on amount
of substance
Ex.
mass, length,
volume,
Intensive
Property
Extensive
Property
Depends on amount
of substance
Ex.
mass, length,
volume,
Intensive
Property
Independent of
the amount of
substance
Extensive
Property
Intensive
Property
Depends on amount
of substance
Independent of
the amount of
substance
Ex.
mass, length,
volume,
Ex.
density, boiling
point, color
I. Substance
II. Properties of Matter
A. Extensive vs. Intensive
B. Physical vs. Chemical
Physical
Property
Chemical
Property
Physical
Property
Property that can be
observed without
altering composition
Chemical
Property
Physical
Property
Property that can be
observed without
altering composition
Ex.
color, state, BP,
density
Chemical
Property
Physical
Property
Chemical
Property
Property that can be Property that
observed without
when measured
altering composition alters a substance
Ex.
color, state, BP,
density
Physical
Property
Chemical
Property
Property that can be Property that
observed without
when measured
altering composition alters a substance
Ex.
color, state, BP,
density
Ex.
Oxidizing ability,
reactivity
I. Substance
II. Properties of Matter
A. Extensive vs. Intensive
B. Physical vs. Chemical
C. State
Three States of Matter
Three States of Matter
1. Solid
2. Liquid
3. Gas
I. Substance
II. Properties of Matter
III. Changes in Matter
I. Substance
II. Properties of Matter
III. Changes in Matter
A. Physical vs. Chemical
Physical
Change
Change in macroscopic structure
without altering
composition
Chemical
Change
Physical
Change
Change in macroscopic structure
without altering
composition
Ex.
Crush, cut, grind,
phase change
Chemical
Change
Physical
Change
Chemical
Change
Change in macroscopic structure
without altering
composition
Ex.
Crush, cut, grind,
phase change
Change that alters
composition of
substance
Physical
Change
Chemical
Change
Change in macroscopic structure
without altering
composition
Ex.
Crush, cut, grind,
phase change
Change that alters
composition of
substance
Ex.
Corrode, explode,
oxidize, burn
I. Substance
II. Properties of Matter
III. Changes in Matter
A. Physical vs. Chemical
B. Conservation of Mass
Conservation of Mass
Massreactants = Massproducts
Self Check – Ex. 1
A 22.8-g sample of water is
decomposed. It produces
2.6-g of hydrogen. What
mass of oxygen is formed?
Self Check – Ex. 1
A 22.8-g sample of water is
decomposed. It produces
2.6-g of hydrogen. What
mass of oxygen is formed?
Moxygen = 20.6 g
IV. Mixtures
A. Homogenous vs.
Heterogeneous
Mixture
Combination of two or
more pure substances
IV. Mixtures
A. Homogenous vs.
Heterogeneous
Homogeneous Heterogeneous
Mixture
Mixture
has the same
composition
throughout.
Homogeneous Heterogeneous
Mixture
Mixture
has the same
composition
throughout.
Ex.
gatorade, radiator
fluid, saltwater
Homogeneous Heterogeneous
Mixture
Mixture
has the same
composition
throughout.
Ex.
gatorade, radiator
fluid, saltwater
mixture with
visibly different
parts.
Homogeneous Heterogeneous
Mixture
Mixture
has the same
composition
throughout.
mixture with
visibly different
parts.
Ex.
gatorade, radiator
fluid, saltwater
Ex.
salad, root beer
float, sandy water
Homogenous Mixture
=
Solution
some other solutions
• gas in gas – air
• gas in liquid – carbonated drink
• liquid in gas – water droplets in air
• solid in solid – alloy
IV. Mixtures
B. Separating
IV. Mixtures
B. Separating
1. filtration
IV. Mixtures
B. Separating
1. filtration
2. distillation
IV. Mixtures
B. Separating
1. filtration
2. distillation
3. crystallization
IV. Mixtures
B. Separating
1. filtration
2. distillation
3. crystallization
4. chromatography
Self Check – Ex. 2
A mixture of salt, sand and
water is created. How can
you recover the sand and
salt?
Self Check – Ex. 3
A mixture of red dye is
placed in water. How can
this mixture be separated?
V. Elements & Compounds
A. Element
Element
Pure substance that can’t
be broken down by
physical or chemical
means
elements
• organized on periodic table
• about 100 elements (90 occur naturally)
• they aren’t equally abundant
• abbreviated with 1 or 2 letter symbols
V. Elements & Compounds
A. Element
B. Compound
Compound
Combination of two or
more elements
compounds
• over 10 million and increasing
• can be decomposed into elements
• chemical formulas show which elements
compose compounds
VI. Laws of the Compounds
A. Law of Constant
Composition
Law of Constant
Composition
Every sample of a given
compound contains the same
mass ratio of elements.
Self Check – Ex. 4
ID
Carbon
Oxygen
A
1.56 g
2.07 g
B
2.25 g
2.99 g
C:O ratio
Are compounds A and B the
same substance?
Self Check – Ex. 4
ID
Carbon
Oxygen
C:O ratio
A
1.56 g
2.07 g
1.33
B
2.25 g
2.99 g
1.33
Are compound A and B the
same substance? Yes – they have the
same C:O ratio.
VI. Laws of the Compounds
A. Law of Constant
Composition
B. Law of Multiple
Proportions
Law of Multiple
Proportions
The ratio of mass ratios for
the elements in two different
compounds will be a whole
number
Self Check – Ex. 5
ID
Nitrogen Oxygen
N2O C
15.02 g 8.58 g
D
5.48 g
N:O ratio
6.26 g
Compound C is N2O. Suggest a
formula for compound D?
Self Check – Ex. 5
ID
Nitrogen Oxygen
N:O ratio
C
15.02 g 8.58 g
1.75
D
5.48 g
0.875
6.26 g
Compound B has half the nitrogen.
Could be NO (nitrogen monoxide).
The End