Unit 2 Properties of Matter

2.1 Matter
I will be able to…
• Define matter.
• Describe the qualities of
solids, liquids, and gases.
• Describe what happens when
energy is added/removed
from matter.

2.1 Matter
•Matter – anything that has mass and
takes up space.
• The “stuff” of which the universe is made
of.
•We classify matter into the three states
of matter.
• Solids
• Liquids
• Gases

2.1 Matter
•Solids
• Shape = fixed
• Volume = fixed
• Particles are held together tightly.

2.1 Matter
•Liquids
• Shape = shape of the container
• Volume = fixed
• Particles are not held together as
tightly as a solid.

2.1 Matter
•Gases
• Shape = shape of the container
• Volume = volume of the container
• Particles move independently.

2.1 Matter
2.1 Assignments
•2.1 Matter WS

2.2 Physical and
Chemical Properties
and Changes
• Define and differentiate
between physical and
chemical properties.
between physical and
chemical changes.

2.2 Physical and Chemical
Properties and Changes
•Physical Properties – a characteristic of a
substance that can change without the
substance becoming a different substance.
• Examples: Color, Shape, Texture, Mass, State,
Volume, Density, Freezing/Boiling/Melting Points
Gallium has a melting point of ~85 °F.

•Chemical Properties – the ability of a
substance to change to a different
substance.
• Examples: Reactivity, pH, Flammability, Corrosiveness
Iron is very reactive with oxygen. Aluminum is unreactive with oxygen.

EXAMPLES
• Classify each of the following as a physical or
chemical property.
• The boiling point of a certain substance is 78°C.
• Diamond is very hard.
• Sugar ferments to form alcohol.
• Baking soda reacts with vinegar when they are placed
into a container.

• Physical Change – a
change of matter from
one form to another,
without a change in
chemical properties.
• The substance you start with is
the substance you end with.
• Chemical formulas stay the
same.
• Examples: state changes,
dissolving a substance, change
in size, color, or shape

• Chemical Change – a
change that occurs
when one or more
substances change
into entirely new
substances, with
different properties.
• The substance you start with is
different than the substance
you end with.
• Chemical formulas are changed.
• Examples: light and/or heat is
produced, formation of gases or
solids.

•Evidence of a
Chemical Change
• Production of Gas
• Production of a Solid
• Precipitate
• Release or Absorption
of Energy
• Temperature Change
• Creation of Light
• A Change in Color

EXAMPLES
• Classify each of the following as a physical or
chemical change.
• Iron metal is melted.
• Iron reacts with oxygen to form rust.
• Wood burns.
• A rock is smashed into small pieces.

2.2 Assignments
•2.2 Physical and Chemical
Properties and Changes WS
•Physical and Chemical
Properties and Changes WS

2.3 Density
• Define and provide
appropriate units for mass,
volume, and density.
• Solve density problems.

2.3 Density
•Volume – the space an object occupies.
• Base Unit = Liter (L)
• Volume of Rectangular Prism = l * w * h
• Volume of a Cylinder = π * r2 * h
• Volume of a Sphere =
4
3
* π * r3
Rectangular Prism Cylinder
Sphere

2.3 Density
•Mass – a measure of the amount of
matter in an object.
• Base Unit = Gram (g)
• Mass ≠ Weight

2.3 Density
•Density - the amount of
matter present in a given
volume of substance.
• The density of a substance
always remains constant.

2.3 Density
EXAMPLE
•The five liquids in the
table were added to a
graduated cylinder.
Identify each liquid
based on the
densities provided in
the table.

2.3 Density
EXAMPLE
•A mason is trying to determine the density
of bricks to determine their quality. Each
brick has a mass of 3.00 x 103 g. Each brick
measures 15 cm x 8 cm x 45 cm. What is
the density (g/cm3) of each brick?

2.3 Density
EXAMPLE
•A shot put has a density of 7.86
grams/cm3. A shot put has a mass of
7.260 kg. What is the volume (cm3) of the
shot put? What metal is the shot put
made of?

2.3 Density
EXAMPLE
•A sample of metal has
a density of 2.699
grams/cm3. The
sample also has a
volume 18.20 cm3.
What is the mass (g)
of the metal sample?
What metal is the
sample made of?

2.3 Density
2.3 Assignments
• 2.3 Density WS
• Volume Practice WS
• Density Problems WS
• Density Cube LAB
• Density of Liquids LAB
• Vernier Caliper and Graduated Cylinder Practice WS
• Density Identification LAB

2.4 Elements and
Compounds
between element, atom,
molecule, and compound.

•Element – a substance
that cannot be broken
down into simpler
substances by physical
or chemical means.
• All atoms of an atom
have the same atomic
number.
• Elements are found on
the periodic table.
2.4 Elements and Compounds

•Atom – smallest unit of an element that
maintains the properties of that
element.
• Atoms can be physically mixed or
chemically joined together to make up
different types of matter.

•Molecule – the smallest unit of a
substance that keeps all of the physical
and chemical properties of that
substance.
• It can consist of one atom or two or more
atoms bonded together.

•Compound – a substance made up of
atoms of two or more different
elements joined by chemical bonds.
• Compounds have chemical formulas.

EXAMPLES
• Are the following elements or compounds?
• Water
• Oxygen
• Carbon Dioxide
• Silver

Scale of the Universe

2.4 Assignments
• 2.4 Elements and Compounds WS
• Elements, Compounds, & Mixtures WS

2.5 Mixtures and
Pure Substances
between pure substances
and mixtures.
between homogenous
mixtures and heterogenous
mixtures.

•Pure Substance – a sample
of matter that has definite
chemical and physical
properties.
• Constant physical and
chemical composition.
• Single Elements
• Single Compounds
2.5 Mixtures and Pure Substances

•Mixture – a combination of two or more
substances that are not chemically
combined.
• Two or more pure substances mixed
(not bonded) together.

EXAMPLES
• Are the following mixtures or pure substances?
• Tap water
• Distilled water
• Oxygen
• The air

•Homogeneous Mixture – a mixture that
has the same composition or structure
throughout.
• Pure substances are in the same
proportions throughout.
• Sometimes called solutions.

•Heterogeneous Mixture – a mixture
that has different properties in different
regions of the mixture.
• Pure substances are not in the same
proportions throughout.

EXAMPLES
•Are the following homogenous or
heterogeneous mixtures?
• A glass of milk
• A bowl of cereal with milk
• Air
• Olive oil and water

2.5 Assignments
• 2.5 Mixtures and Pure Substances WS

2.6 The Elements
• Memorize the first 20
elements.
• Identify common elements
by their element symbols.

2.6 The Elements
•All matter can be
broken down
chemically into 118
different elements.
• Everything is made
of matter, and all
matter can be
broken down into
the elements found
on the periodic
table.

2.6 The Elements
•Elements 1-98 occur
naturally in nature.
• This has been updated since your
textbook was written.
•All other elements are
created by scientists in
the lab and only last for
very small amounts of
time.
• They are too unstable to last in
nature.

2.6 The Elements
•The names of the elements come from
many sources.
• Many are described from Greek, Latin, or
German words that describe some of the
properties of the element.
• Gold (Au) was named aurum, the Latin word
meaning “shining dawn”
• Lead (Pb) was named plumbum, the Latin word
meaning “heavy”
• Bromine (Br) was named after the Greek word
meaning “stench”

2.6 The Elements
•The names of the elements have come
from many sources.
• The place where the element was discovered.
EXAMPLES

2.6 The Elements
•The names of the elements have come
from many sources.
• The element was named after a famous
scientist.
EXAMPLES

2.6 The Elements
•Just like the states have abbreviations (MI),
elements have abbreviations.
•Element Symbols – abbreviations for the
chemical elements.
EXAMPLES

2.6 The Elements
2.6 Assignments
•2.6 The Elements WS
•Elements WS

2.7 Formulas
of Compounds
• Describe a compounds
composition based on its
chemical formula.
• Determine simple chemical
compounds from a word
problem.

2.7 Formulas of Compounds
•Compound – a substance made up of
atoms of two or more different
elements joined by chemical bonds.
• Compounds have chemical formulas.

•Chemical Formula – a representation of
a molecule in which the symbols for the
elements are used to indicate the types
of atoms present and subscripts are
used to show the relative number of
atoms.

•Rules for writing chemical formulas.
1. Each atom present is represented by its
elements symbol.
2. The number of each type of atom is
indicated by a subscript written to the
right of the element symbol.
3. When only one atom of a given type is
present, the subscript one is not written.

EXAMPLES
• Each molecule of a compound contains one
atom of sulfur and three atoms of oxygen.
• Each molecule of a compound contains two
atoms of nitrogen and five atoms of oxygen.
• Each molecule of glucose contains six atoms
of carbon, twelve atoms hydrogen, and six
atoms of oxygen.

2.7 Assignments
•2.7 Formulas of Compounds WS

2.8 Chemical Reactions
• Define chemical reaction and
chemical equation.
between reactants and
products
• Explain the Law of
Conservation of Mass

•Chemical Reaction – a process in which
one or more substances are changed
into one or more new substances by the
reorganization of component atoms.
• Chemical Changes

•Chemical Equation – a representation
of a chemical reaction showing the
relative numbers of reactant and
product molecules.

•Reactants – the starting substances in a
chemical reaction. It appears to the left
of the arrow in a chemical equation.
• “Ingredients”

•Products – a substance resulting from a
chemical reaction. It appears to the
right of the arrow in a chemical
equation.
• “Finished Product”

•Law of Conservation of Mass – mass
cannot be created or destroyed in
ordinary chemical and physical reactions.
• Atoms in Reactants = Atoms in Products

2.8 Assignments
•2.8 Chemical Reactions WS

Unit 2: Properties of Matter
Unit 2 Test Review ASSIGNMENT
•Unit 2 Test Review WS

Unit 2 Properties of Matter

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