Name: ________________________ Period ___ Assign. # ____
Matter Notes
Vocabulary
Particle Diagrams – particle diagrams allow
us to visualize the various types of matter.
Examples:
Ne(g)
Ne(l)
Ne(s)
Elements –
substances that
cannot be broken
down into simpler
substances by
chemical means.
Listed on the
periodic table.
H2(g)
Diatomic Molecule –
A molecule
containing two
identical atoms.
The diatomic
elements are:
Br2, I2, N2, Cl2, H2,
O2, F2
(sounds like
"Brinklehoff)
1 - Matter Notes
Br2(l)
I2(s)
Compounds – a
substance composed
of two or more
elements that are
chemically combined
in definite
proportions.
CO2(g)
CH4(g)
H2O(s)
Pure Substance - compounds and elements. Composition and
properties are fixed (stay the same).
Mixtures – Combinations of two or more pure substances that can
be separated by physical means.
Air
O2(aq)
Ne(g) and
N2(g)
Sand in
H2O(l)
Oil/Water
Soil
Homogeneous – a
mixture in which the
particles are
uniformly mixed.
Heterogeneous - a
mixture in which the
particles are not
uniformly mixed.
(Has pebbles, plant matter
and sand)
2 - Matter Notes
Classification of Matter:
Matter
Everything that has mass.
Pure Substances
Mixtures
 Composition, as well as physical and
 A blend of two or more pure substances.
 Variable composition and properties.
 Can be separated by physical means such
chemical properties do not vary.
as filtration, evaporation and distillation.
Elements
 Found on Periodic
Table.
 Cannot be broken
down by a
chemical change.
 Diatomic
elements consist
Compounds
 Composed of two or more
elements chemically
 Can only be separated by
chemical change into their
component elements.
the same element
Examples: H2O
more pure substances.
 When a substance dissolves in
a liquid the resulting
homogeneous mixture is called
 Can be expressed as a
chemical formula.
bonded together.
 Uniform mixture of two or
bonded in a fixed ratio.
of two atoms of
Homogeneous Mixture
a solution.
CO
C6 H O
 A homogeneous mixture of
metallic elements is called an
12 3 -2Matter Notes
alloy.
Heterogeneous
Mixture
 A non-uniform
mixture of two
or more pure
substances.
 Components are
distinguishable.
Practice: Classify each of the following as an element, compound,
homogeneous or heterogeneous mixture.
1. Chlorine - element
2. Distilled water - compound
9. Soil - heterogeneous
mixture
10. C2H5OH(l) - compound
3. Sugar water - homogeneous
mixture
4. Copper - element
11. C2H5OH(aq) - homogeneous
mixture
12. NaCl(s) - compound
5. NaCl(aq) - homogeneous
mixture
6. Salad dressing heterogeneous mixture
7. Carbon dioxide - compound
13. Air - homogeneous
mixture
14. Tin - element
8. CuCl2(s) - compound
15. Steel (iron + other metals) homogeneous mixture
16. CuCl2(aq) - homogeneous
mixture
Phases of Matter
Solids:
 Attractive forces between particles are strong which
holds them together in a rigid form.
 Solids have a definite shape and volume.
 Indicated by placing a (s) after the formula or symbol.
 True solids have a crystalline structure
4 - Matter Notes
Particle Diagrams:
Ar(s)
N2(s)
H2O(s)
Liquids:
 Liquid phase particles are able to move past one another.
 Definite volume but non-definite shape.
 Indicated by placing a (l) after the formula or symbol.
Particle Diagrams:
Ar(l)
N2(l)
H2O(l)
5 - Matter Notes
Gases:
 Particles are separated by large distances.
 No defined shape or volume.
 Indicated by placing a (g) after the formula or symbol.
 A vapor is the gaseous phase of a substance that is a
liquid or solid at normal conditions.
Particle Diagrams:
Ar(g)
N2(g)
H2O(g)
6 - Matter Notes
Picture examples of Elements, Compounds and Mixtures
7 - Matter Notes
Practice: Identify each of the following as an element, compound
or mixture.
If the diagram indicates a mixture identify the
components as elements and/or compounds:
Element
Compound
Mixture of 2 elements
Mixture of an element
and a compound
8 - Matter Notes
Sketch a particle diagram for each substance indicated.
Use
the following key:
Hydrogen atom
The element
hydrogen at STP.
Oxygen atom
H2O(l)
(diatomic H2 gas)
A mixture of
A mixture of H2O(g)
hydrogen and oxygen
and Ar(g)
as elements at STP.
(gas)
9 - Matter Notes
Argon atom
The element argon
at STP.
(gas)
H2O(s)
Physical and Chemical Properties:
A physical property is observed with the senses and can be
determined without altering the object. Color, shape, mass,
volume, density, solubility and odor are all physical properties.
A chemical property indicates how a substance reacts with
another substance. The original substance is changed when
observing a chemical property.
Indicate whether the following are physical or chemical properties:
1. Blue color - physical
9. Luster - physical
2. Hardness - physical
10. Corrosive - chemical
3. flammable - chemical
11. Odor - physical
4. Dissolves in water
(solubility) - physical
12. Melting point - physical
5. Density - physical
6. Reacts with acids chemical
7. Supports combustion chemical
8. Boiling point - physical
13. Decomposes in air chemical
14. Can neutralize a base chemical
15. Releases H2 when
exposed to acid chemical
10 - Matter Notes
Density
The density formula is given in Reference Table T. For all of
the following problems show a correct numerical set-up and
express the answer to the correct number of significant
figures.
1. A block of aluminum occupies a volume of 15.0 mL and
has a mass of 40.5 g. Determine the density.
2. Mercury metal is poured into a graduated cylinder to a
level of exactly 22.5 mL. The mercury used to fill the
cylinder weighs 306.0 g. Determine the density of
mercury.
3. Determine the mass of 200.0 mL ethyl alcohol. The
density of ethyl alcohol is 0.789 g/mL.
11 - Matter Notes
4. A rectangular block of copper metal weighs 1896 g. The
dimensions of the block are 8.4 cm by 5.5 cm by 4.6 cm.
Determine the density of copper.
5. A graduated cylinder that weighs 345.8 g is filled with
225 mL of carbon tetrachloride. The weight of the flask
and carbon tetrachloride is found to be 703.55 g. From
this information, determine the density of carbon
tetrachloride.
6. Determine the mass of 250.0 mL of benzene. The
density of benzene is 0.8765 g/mL.
7. A block of lead has dimensions of 4.50 cm by 5.20 cm
by 6.00 cm. The block weighs 1587 g. From this
information, calculate the density of lead.
12 - Matter Notes
8. A 28.5 gram piece of iron is added to a graduated
cylinder containing 45.50 mL of water. The water level
rises to the 49.10 mL mark. From this information,
determine the density of iron.
9. The density of silver is 10.50 g/cm3. Determine the
volume of a piece of silver having a mass of 31.57 grams.
10. A sample of iron occupies a volume of 10.0 cm3. The
density of iron is 7.87 g/cm3.
the sample.
13 - Matter Notes
Determine the mass of
Physical/Chemical Changes
Physical change – a change that does not alter the chemical
properties of the substance. The original substance still
exists, it has only changed forms.
Chemical change – a reaction in which the composition of the
substance is changed. A new substance is produced.
Identify the following as either physical or chemical changes:
1. Melting ice. Physical change
2. Hydrochloric acid reacts with sodium hydroxide. Chemical
change
3. Sodium hydroxide is dissolved in water. Physical change
4. Iron rusts. Chemical change
5. Water evaporates. Physical change
6. Potassium chlorate decomposes. Chemical change
7. Sugar is mixed with water. Physical change
8. Liquid sodium is solidified. Physical change
9. Water freezes. Physical change
10. A filter removes dust from air. Physical change
14 - Matter Notes
Mixture Separation Techniques:
Mixtures are physical combinations of two or more
Substances. Since they are physically combined, they can be
physically separated.
Distillation:
 A method of separating a mixture of two liquids by their
differences in boiling points.
 The liquid with the lower boiling point will be concentrated
in the vapor phase.
Residue – the liquid that remains behind; it has a higher
boiling point.
Distillate – the liquid that boils first, it has a lower boiling
point.
15 - Matter Notes
Filtration: A process that separates a solid from a liquid
or a gas in a heterogeneous mixture.
Residue – the solid that remains on the filter
paper.
Filtrate – Liquid (or gas) and any dissolved
particles. They pass through the filter paper.
Note: Filtration cannot be used to separate
dissolved substances from solution. For
example, NaCl cannot be separated from water
by filtration.
Evaporation:
 A process that can be used to separate a dissolved
substance from solution.
 The liquid, usually water, is evaporated leaving the solid
behind.
16 - Matter Notes
Chromatography:
A method of separation relying on the components of a
mixture having different attractions with the transporting
medium.
There are other methods of separating mixtures, but all are
based upon physical properties. For example, magnetic metals
can be removed from mixtures by magnets.
Practice: Identify a method for separating each of the
mixtures below. Use the following choices: distillation,
filtration, evaporation, chromatography, magnets.
1. A homogeneous mixture of CuSO4 dissolved in water.
Use Evaporation to separate the dissolved CuSO4 from
the water.
17 - Matter Notes
2. A heterogeneous mixture of Iron filings and powdered
sulfur.
Use magnets to separate the metal iron from the powered
sulfur.
3. A mixture of Al(OH)3(s) and water.
Use Filtration to separate solid Al(OH)3 from the
water
4. A homogeneous mixture of C6H14(l) and C8H18(l).
Separate using Distillation because the mixture of liquid
compounds have different boiling points.
5. A heterogeneous mixture of NaCl(aq) and sand.
Use filtration to separate NaCl(aq) from sand.
Then use Evaporation to separate NaCl from the water it’s
dissolved in.
6. A homogeneous mixture of ethanol (boiling point 76°C) and
water (boiling point 100°C).
Distillation to separate two liquids that have different boiling
points.
7. An aqueous solution of KCl.
Use Evaporation to separate the KCl from the water.
18 - Matter Notes