Understanding
Matter
Georgia Performance Standards
SPS2. Students will explore the nature of matter, its
classifications, and its system for naming types of matter.
a. Calculate density when given a means to determine a substance’s
mass and volume.
SPS5. Students will compare and contrast the phases of matter as
they relate to atomic and molecular motion.
a. Compare and contrast the atomic/molecular motion of solids, liquids,
gases and plasmas.
b. Relate temperature, pressure, and volume of gases to the behavior
of gases.
SPS6. Students will investigate the properties of solutions.
a. Describe solutions in terms of …solute / solvent, conductivity,
concentration
b. Observe factors affecting the rate a solute dissolves in a specific
solvent.
c. Demonstrate that solubility is related to temperature by constructing
a solubility curve.
How
How is the density of
an object determined?
How
Density is the
comparison of
how much matter
(mass) is in a
certain amount of
space (volume).
Density
depends
on
an
How
objects mass and its volume.
Density = mass / volume
Determined
from the mass
balance.
Determined by
measurement
using a ruler or
water
displacement.
The units of density are
3
g/cm or g/ ml.
Bubba has a rectangular solid that
measures 2 cm wide by 3 cm high by 5 cm
long. He places the rectangular solid on a
mass balance and determines the mass to
be 60 grams. Determine the density of the
solid?
Density Problems
Bubba has a rock that has a mass of 22
grams. How would he determine the volume
of the rock if he can not measure it with a
ruler?
By Water
HowDisplacement
How
Classification of Matter
How can the physical and
chemical properties of matter
help us describe it?
A physical property of matter is
one that is How
unique to that element
or substance. They do not change
the chemical identity of matter.
Examples are…density (mass and
volume)…viscosity…texture…color…
melting point…freezing
point…boiling point…
Chemical properties always
How
alter the identity of a
substance. Something new is
always produced.
Examples are: flammability, heat
of combustion, reactivity with
other substances, and pH.
Physical changes in a substance do not
change what the substance is.
How
For example, if a piece of paper is
cut up into small pieces it still is
paper. If water boils and makes
Physical changes can be reversed
steam (vapor) it is still water.
Physical changes
can be reversed
In a chemical change where there is a
chemical reaction, a new substance is
How
formed and energy is either given off
or absorbed.
If the same piece of paper is
burned, it is broken up into
different substances that are not
paper.
Chemical changes cannot be
reversed with the substance
changed back without
extraordinary means.
Signs of a
How
Chemical Change
Color change
Property change
Energy change
Precipitate forms
Gas produced
A precipitate is a solid that is formed
when 2 liquid reactants are combined.
How
How does the motion of
particles explain the physical
properties of matter?
Particle Motion in Solids, Liquids, and Gases
HowTheory of Matter:
The Particle
1. Matter is made up of tiny particles (Atoms & Molecules)
2. Particles of Matter are in constant motion.
3. Particles of Matter are held together by very strong electric
forces
4. There are empty spaces between the particles of matter that are
very large compared to the particles themselves.
5. Each substance has unique particles that are different from the
particles of other substances 1
6. Temperature affects the speed of the particles. The higher the
temperature, the faster the speed of the particles.
Summary
PROPERTY
SOLID
LIQUID
GAS
shape
fixed
volume
definite
same as
container
(indefinite)
definite
no
yes
same as
container
(indefinite)
fills entire
container
(indefinite)
yes
very slightly
very slightly
yes
very small
small
large
ability to
flow
can be
compressed
volume
change with
heating
th state of matter
Plasma, the
4
How
A plasma is a phase of matter that has enough
energy for the electrons to separated from the
nucleus. It consists of independently moving
electrons and nuclei, and thus has some rather
interesting properties, such as very good
magnetic shielding. It can be found in places
such as the center of the sun, and also, in small
quantities, surrounding a lightening bolt.
Particles of a
How
typical Solid
Particles of solids
are held in place by
strong electrostatic
forces and are
densely packed
together. Particles
of solids vibrate
constantly due to
their internal energy
but they cannot move
from one place to
another.
Particles of a
typical Liquid
Particles of liquids are
kept together by
forces of attraction
that are weaker than
those of solid
particles. Within the
walls of the container
they can move from
place to place bumping
into the sides of the
container and into
other particles.
Particles of gases are more
Particles of a distant than either liquids or
How
solids. The forces of
typical Gas
attraction that hold them
together are very weak and
that the spaces between
them are much larger than
the spaces between solid and
liquid particles. Particles of
gases move from place to
place within a container
bumping against the container
walls and against other gas
particles.
Relationships
How
between
temperature,
pressure, and
volume of gases.
Boyle’s Law
A relationshipHow
between pressure and volume
Boyle's Law states the volume
of a definite quantity of dry
gas is inversely proportional to
the pressure, provided the
temperature remains constant.
Mathematically Boyle's law can
be expressed as P1V1 = P2V2
How
How
How
Charles’s
Law
Charles’ Law
A relationship between volume and temperature
How
How
Charles's Law can be stated as
the volume occupied by any
sample of gas at a constant
pressure is directly proportional
to the absolute temperature.
Gay-Lussac’s Law
How
Why may your soda
can burst open if you
leave it in your car
too long on very hot
days? Why do closed
jars or aerosol cans
explode when they
are tossed into a
fire? These unruly
behaviors are
manifestations of
Gay-Lussac's Law at
work.
Identify the Gas Law
How
How
Reminder
Changes
of State
are
Physical
Changes
Changes of State for Water
Changes of State for Water
Gas
Boiling Point
T
E
E
N
M
E
P
R
E
G
R
A
Y
T
U
R
E
Condensation
Freezing or
Melting Point
Vaporization
Freezing
Liquid
Energy
Absorbed
Melting
Energy
Released
Solid
ENERGY
Solutions
How
A solution is a homogenous
mixture of two or more
substances that exist in a
single phase.
Two main parts
How of any solution
The solute is the component of a solution
that is dissolved in the solvent; it is usually
present in a smaller amount than the
solvent. The solvent is the component into
which the solute is dissolved, and it is
usually present in greater concentration.
For example, in a solution of salt water, salt
is the solute and water is the solvent.
How
Solution
Conductivity
Conductivity is the ability of a solution to
conduct and electric current.
Electrolytes are solutions that conduct
electricity due to ions in the solution.
Non-electrolytes are solutions that do not
conduct electric current. These solutions
do not contain ions.
How
Solution
Concentration
The concentration of a solution
represents the amount of solute dissolved
in a unit amount of solvent or of solution,
and can be expressed in a variety of ways
(qualitatively and quantitatively).
Solution Concentration
How
Qualitative Expressions of Concentration
A solution can be qualitatively described as …
dilute: a solution that contains a small proportion
of solute relative to solvent, or
concentrated: a solution that contains a large
proportion of solute relative to solvent.
Solution Concentration
Semi-Quantitative
Expressions of Concentration
How
A solution can be semi-quantitatively described as…
unsaturated: a solution in which more solute will
dissolve, or
saturated: a solution in which no more solute will
dissolve.
supersaturated: a solution that contains more solute
than it can dissolve at that temperature.
Solution Concentration
How
The solubility of a solute is the amount of solute
that will dissolve in a given amount of solvent to
produce a saturated solution.
For example, at 0oC, we can dissolve a maximum of
35.7 g of solid NaCl in 100 mL of water (a
saturated solution). Any additional solid NaCl that
we add to the saturated solution simply falls to
the bottom of the container and does not dissolve.
Solution Concentration
How
Quantitative Expressions of Concentration
There are a number of ways to express the
relative amounts of solute and solvent in a
solution. Which one we choose to use often
depends on convenience. For example, it is
sometimes easier to measure the volume of a
solution rather than the mass of the solution.
One way to measure the concentration of a
solution is in grams of solute / liter of solution.
Factors Affecting the Rate a
Solute Dissolves in a Solvent
How
Stirring-brings more fresh solvent into contact
with more solute.
Grinding the solute into smaller size particles.
Smaller particles have more surface area than
larger size particles. Since dissolving occurs at
the surface of the solute, this allows more
solvent to come in contact with more solute.
Increase the temperature. This speeds up the
particles and increases the rate of
contact between solvent and solute particles.
How
Factors Affecting Solubility
What is a solubility curve?
How
A graph
showing the
concentration
of a substance
in its saturated
solution in a
solvent as a
function of
temperature.
How
When called
upon, please
answer the
instructor’s
questions
How much
NH4Cl will
dissolve in
100g of water
at 50 C?
Does the
solubility of
SO2 in 100g of How
water increase
or decrease as
the
temperature of
the solvent
increases?
About 40 g of
NH4Cl will
How
dissolve in 100g
of water at 30 C.
What solvent
temperature is
needed to
dissolve 55 g?
Which solid
shows a
How
decrease in
solubility as the
temperature of
the water is
raised?
Ten grams of
KClO3 produces a
How
saturated solution
at 20 C. If 10
additional grams
of KClO3 were
added, what
temperature would
be required to
produce a
saturated
solution?
How
The End
How much NH4Cl will dissolve in 100g
of water at 50 C?
How
Does the solubility of SO2 in 100g of
water increase or decrease as the
temperature of the solvent increases?
About 40 g of NH4Cl will dissolve in
100g of water at 30 C. What solvent
temperature is needed to dissolve 55 g?
Which solid shows a decrease in
solubility as the temperature of the
water is raised?
Ten grams of KClO3 produces a
saturated solution at 20 C. If 10
additional grams of KClO3 were added,
what temperature would be required to
produce a saturated solution?
How
How
How