MatterProperties and
Changes
I will distinguish between physical and chemical properties
I will classify matter by composition: element, compound or mixture
I will identify observable characteristics of chemical reactions
I will explain the fundamental law of conservation of mass
Properties of Matter
 I will identify the characteristics of a substance
 I will distinguish between physical and chemical properties
 I will differentiate among the physical states of matter
Substances
 Matter that has a uniform and unchanging composition
 Aka pure substance
 Example 1
 Table Salt
 Always 100% sodium chloride
 Example 2
 Water
 H2O
 NOT AN EXAMPLE
 Sea water
 Samples vary by location
 Amount of salts, water, dissolved substances
Physical Properties
 A characteristic that can be observed or measured
WITHOUT changing the sample’s composition
 Density
 Color
 Odor
 Taste
 Hardness
 Melting point
 Boiling point
Examples-Physical Properties
 Salt (sodium chloride)
 Forms solid white crystals at room temperature
 Unique salty taste
 Oxygen
 Colorless
 Gas at 25 degrees Celsius
 Melting point -218 degrees Celsius
 Boiling point -183 degrees Celsius
 Density 0.0014 g/cc
Extensive Properties
 Dependent upon the amount of substance present
 Examples
 Mass
 Volume
 Length
 Weight
Intensive Properties
 Independent of the amount of the substance present
 Examples
Chemical Properties
 The ability of a substance to combine with or change into
one or more other substances
And/Or
 The inability of a substance to change into another
substance
 Example
 Iron forms rust when combined with air
 Iron + Nitrogen (at room temperature) = no chemical change
Observing Properties of Matter
 Every substance has its own unique set of physical and chemical
properties
 May vary depending on conditions of immediate environment
 Room temperature, standard pressure, etc.
 Example
Copper
Physical Properties
Chemical Properties
Reddish brown
Shiny
Malleable (easily shaped)
Ductile (drawn into wire)
Conducts heat/electricity
Density 8.92 g/cc
Melting Point 1085 ℃
Boiling Point 2570 ℃
Forms green copper
carbonate compound when in
contact w/ moist air
Forms new substances when
combined with nitric and
sulfuric acids
Forms a deep blue solution
when in contact with
ammonia
States of matter
 Solid
 Liquid
 Gas
 Plasma
 FUN FACT: (only occurs
naturally on Earth in the
form of lightening bolts!)
PHYSICAL PROPERTY!!!!!
Solids
 A form of matter that has its own
definite shape and volume.
 Will only expand SLIGHTLY when
heated
 Examples
 Wood
 Iron
 Does NOT conform to shape of
container
 Paper
 Sugar
 Particles are VERY tightly packed
 Incompressible
 Volume stays the same
 Example
 Wax (moldable) but volume doesn’t
change
Liquids
 A form of matter that flows, has
constant volume, and takes the
shape of its container
 Examples
 Water
 Blood
 Mercury
 Virtually incompressible
 Tend to expand when heated
 Liquid Particles
 NOT rigidly held in place
 less closely packed than solids
 Are able to move past each other
Gases
 A form of matter that flows to
CONFORM to the shape of its
container and fills the ENTIRE
volume of its container
 Examples
 Neon
 Lighted signs
 Methane
 Cooking
 Air
 Mixture of gases
 Particles are VERY far apart
 EASILY compressed
 A substance NATURALLY in the
gaseous state at room temperature
RELATED TERMS
 Vapor
 The gaseous state of a substance that
is a SOLID or LIQUID at room
temperature
 Example
 steam
Quick Think
 Describe the characteristics that
identify a sample of matter as being
a substance.
 Using what you know about
the compressibility of gases,
explain why the oxygen in a
SCUBA tank is compressed.
 Classify each of the following as a
physical or chemical property
 Iron and oxygen form rust
 Iron is more dense than aluminum
 Magnesium burns brightly when
ignited
 Oil and water do not mix
 Mercury melts at -39 ℃
 Create a table that describes
the three common states of
matter in terms of their shape,
volume, and compressibility.
Quick Think- Check
 The sample of matter must
have a uniform and
unchanging composition to be
a substance.
 Properties
 Chemical (rust)
 Physical (density)
 Chemical (burning)
 Physical (mixing)
 Physical (melting)
point)
 Particles of gas are spaced
apart and are easily
compressed. Therefore, it is
possible to put a significant
volume of oxygen in the tank,
which allows the diver to
remain under water longer!
Solid
Liquid
Gas
Definite volume
Definite volume
Fills volume of
container
Definite shape
Fills container
shape
Takes shape of
container
Incompressible
Virtually
incompressible
Compressible
Changes in Matter
 I will define physical change and list several common
physical changes
 I will define chemical change and list several indications
that a chemical change has taken place
 I will apply the law of conservation of mass to chemical
reactions
Physical CHANGES
 Alter a substance WITHOUT changing its composition
 Might result in dramatically different appearance
(yet leave the composition of the substance unchanged)
 Examples
 Crunching up a piece of aluminum foil
 Cutting a sheet of paper
 Breaking a crystal
 Phase changes (solid, liquid, gas)
Key words of Physical Changes
 Bend
 Grind
 Crumple
 Split
 Crush
Chemical CHANGES
 A process that involves one or more substances changing
into a NEW substance
 New substance
 Formed in reaction
 Different compositions — than original substance(s)
 Different properties — than original substance(s)
 Example
 Fermentation of juice, sugars, and other ingredients (making
wine)
 Rusting of iron (a chemical combo of iron and oxygen)
Chemical CHANGES
 Commonly referred to as a chemical reaction
 Reactants
 Starting substances
 Products
 New substances
 Example
 Reactants = Iron, Oxygen
 Product = rust
Key Words of Chemical Changes
 Explode
 Rust
 Oxidize
 Corrode
 Tarnish
 Ferment
 Burn
 Rot
The LAW of Conservation of Mass
 Mass is neither created nor destroyed during a chemical
reaction
 Mass is conserved
 Mass of Reactants = Mass of Products
Conservation of Mass Problem
 Known
 Mass mercury (II) oxide =
10.0g
 Mass liquid mercury = 9.26g
 Mass Reactants = Mass
Products
 Mercury (II) oxide = Mercury +
Oxygen
 Unknown
 Mass formed oxygen = ? g
 10.0g = 9.26g + ?
 0.740 g of Oxygen formed
Quick Think
 Describe the results of a
physical change and 3
examples. Repeat with
chemical change.
 A friend tells you, “because
composition does not change
during a physical change, the
appearance of a substance
does not change.” Is your
friend correct? Explain WHY?
 Solve each of the following
 In the complete reaction of
22.99 g of sodium with 35.35 g
chlorine, what is the mass of
the sodium chloride formed?
 A 12.2 g sample of X reacts
with a sample of Y to form 78.9
g XY. What way the mass of Y
that reacted?
Quick Think-Check
 During a physical change a
substance is altered but its
composition does not change.
EX melting, freezing, boiling,
bending, tearing
 During a chemical change the
composition of a substance IS
altered. EX color change, odor,
temperatures change,
formation of gas or solid from
a liquid.
 The statement is false.
Composition doesn’t change
but a change in appearance
often accompanies a physical
change.
 58.44g of sodium chloride
 66.7 g of Y