Properties of Matter
Andrew Jackson
Leeds Middle School
Lesson 1 –
Our Ideas About Matter
You will perform a circuit of eight
inquiries to observe how matter
behaves. The inquiries involve the
following: different states of matter,
changes of state, mass and volume,
floating and sinking, thermal
expansion, mixtures, solubility and
insolubility, and chemical reactions.
Lesson 1 –
• Matter - the physical material that has mass and
occupies space.
• 1.1 - Temperature change affects the volume of air.
• 1.2 - The shape of the object does not affect its volume
or mass.
• 1.3 - Air is a gas.
• 1.4 – Pure substance or mixture?
• 1.5 - Some matter is soluble in water.
• 1.6 - Some liquids do not mix (immiscible)
• 1.7 - Buoyancy
• 1.8 - Air and gases are forms of matter even though they
are invisible.
Lesson 1 –
(1-3)
1. matter - the physical material that has mass
and occupies space
2. expansion - the increase in the volume of
matter that occurs when matter is heated.
3. contraction - decrease in volume of matter
when matter is cooled
4. immiscible - liquids that are unable to
dissolve in one another.
5. miscible - liquids are able to dissolve in one
another.
Lesson 1 -
(2-3)
6. density - the mass of a known volume of a
substance; measured in g/cm3
7. mass - the amount of matter in an object;
measured in g or kg.
8. volume - the amount of space occupied
matter; measured in L, mL, cm3, or m3.
Lesson 2 – Determining Density
• You will use mass and volume
measurements to calculate the densities of
water, regular shaped objects, and
irregular shaped objects.
Lesson 2.1 –
•Does
Doeschanging
changingthe
thevolume
volumeofofwater
waterchange
change
the density
of water?
the density
of water?
Lesson 2.1
2.1 Calculating Mass
Volume
Mass of
Mass of
of
Graduated Graduated
Cylinder
Water
Cylinder
and Water
(cm3)
(g)
(g)
25
50
Mass of
1 cm3 of water
(density in
g/cm3)
Lesson 2.1 • Density is calculated by dividing the mass by the
volume; measured in grams per cubic
centimeter (g/cm3).
• Volume is the amount of space taken up by an
object; measured in mL or cm3. (space)
• Changing the amount of a substance does not
change the density of the substance.
• Density is a characteristic property of matter.
• Characteristic property - property that is
independent of mass, volume, and shape….
Lesson 2.2 –
• Do the substances making up different
regular-shaped objects have the same
density?
Lesson 2.2 –
2.2
Comparing the Densities of Different Substances
Substance
Wax
block
White
plastic
Clear
plastic
Aluminum
Length (l)
(cm)
Width (w)
(cm)
Height (h)
(cm)
Volume (v)
(cm3)
(v=l x w x h)
Mass
(m)
(g)
Mass of
1 cm3
(density
in
g/cm3)
(m/v)
Lesson 2.2 Conclusion
• The shape of an object does not change the
density of the substance of which it is composed.
• The volume of a regular shaped object is
found by measuring l x w x h; measured in
cm3(one mL = one cm3)
• The mass of a regular-shaped object is found
by using an electronic balance; measured in
grams.
• Density is a characteristic property of matter;
measured in g/cm3.
• Characteristic property - property that is
independent of mass, volume, and shape….
Lesson 2.3 –
• Do the substances making up different
irregular-shaped objects have the same
density?
Lesson 2.3 –
2.3
Comparing the Densities of Different Substances
Object/
substance
Mass
(g)
Volume of
water
without
object
(mL)
Volume of
water and
object
(mL)
Volume of
object
(mL)
Density
(g/cm3)
Lesson 2.3 • Different irregular-shaped objects made of
the same material will have the same
density (characteristic property). Different
materials have different densities.
Lesson 2 -
(1-2)
9. gram - a metric unit used to measure
mass
10. milliliter – unit used to measure
volume
11. cm3 – unit used to measure volume
12. g/cm3 – unit of measure of density
13. water displacement – method used to
find the volume of irregular-shaped
objects
Lesson 2 -
(2-2)
14. l x w x h - a method used to find
the volume of a regular-shaped object
15. 1.0 g/cm3 – the density of water
16. characteristic property - an attribute
that can be used to help identify a
substance; not affected by the mass,
volume, or shape of a substance;
refers to substances, not objects…..
Lesson 3 – Density Predictions
You will predict whether the blocks you
investigated in Inq. 2.2 and 2.3 will float or
sink. After finding the density of three
liquids, you will predict the order in which
the liquids will layer when you build a
density column. You will calculate and
predict whether objects will float or sink in
the density column.
Lesson 3.0 How can you determine if an object will float
or sink when placed in water?
Lesson 3.0 -
L3.0 Results of Floating & Sinking Observations
Substance
wax block
white plastic
block
clear plastic
block
aluminum block
steel (short nail)
copper rod
nylon spacer
(bolt)
Density
(g/cm3)
Floats or sinks?
Prediction
Results
Lesson 3.0 - Conclusion
• Solids have density.
• Density can be used to predict whether an
object will float or sink.
• An object floats when its’ density is less
than that of the liquid in which it is placed.
• An object sinks when its density is more
than that of the liquid in which it is
placed………..
Lesson 3.1 How can you determine if an object will float
or sink when placed in water?
Lesson 3.1 -
L3.1 Calculating Density
Liquid
Volume
(cm3)
Mass
(g)
Grad.
Cylinder
Vegetable
oil
Corn
syrup
Water
Grad.
Cylinder and
substance
Density
(g/cm3)
Substance
Lesson 3.1 • Liquids and solids have density.
• An object or substance floats when its density is
less than that of the liquid in which it is placed.
• An object or substance sinks when its density is
more than that of the liquid in which it is placed.
• Some liquids are immiscible (insoluble in one
another.)………
Lesson 3 17. solid – a state or phase of matter in which
a substance had definite shape and volume
18. liquid - a state or phase of matter in which
a substance has a definite volume but no
definite shape; takes shape of the container
it occupies.
19. floating - matter is less dense than
substance it is in
20. sinking - matter is more dense than
substance it is in…………..
Lesson 4 – Do Gases Have Density
You will determine the mass,
volume, and density of a bottle of
air.
Lesson 4 -
Do gases (air) have density?
Lesson 4 -
L4 Finding the Density of Air
Volume of
bottle
(mL or
cm3)
Mass of air,
bottle,
washer, &
rubber
valve
(g)
Mass of
bottle,
washer, &
rubber
valve after
removing
air (g)
Mass of air
(g)
Density of
air
(m/v)
(g/cm3)
Lesson 4 –
Gases have mass, volume, and
density.
Air is less dense than liquids and
solids……………
Lesson 4 21. vacuum - space without matter.
22. gas - a state or phase of matter in
which a substance has no definite
shape or volume……………
Lesson 5 – Temperature & Density
You will observe the effect of heat on a
bimetal strip. You will investigate how
temperature affects the volume of matter
by using a glass tube in a rubber stopper
placed in a test tube filled with water.
Lesson 5 –
What is the relationship between
temperature, heat, and density?
Lesson 5 -
Lesson 5 • Heat is a form of energy that can move from a
hot place to a cooler place (measured in joules).
• Temperature is a measure of kinetic energy of
particles of matter (measured by a thermometer
in degrees Celsius).
• Density changes with temperature:
– As temperature increases, density will decrease and
volume will increase (mass stays the same).
• expansion
– As temperature decreases, density will increase and
volume will decrease (mass stays the same).
• contraction
• Gas or liquid-filled thermometers work as the
result of expansion or contraction………….
Lesson 5 –
(1-3)
23. heat - a form of energy that can move
from a hot place to a cooler place; the
transfer of energy from one body to
another.
24. temperature - a measure of the kinetic
energy of the particles that make up
matter; the measurement of how hot
something is.
25. Celsius - a temperature scale with the
melting point of ice at 0 degrees and the
boiling point of water at 100 degrees.
Lesson 5 –
(2-2)
26. Fahrenheit - a temperature scale with the
melting point of ice at 32 degrees and the
boiling point of water at 212 degrees.
27. Kelvin - a temperature scale with the lowest
possible temperature at the zero point, which
is called absolute zero; ice melts at 273 K.
28. calibrate - set; measure to scale…………
Lesson 6 – Applying the Heat
You will heat pure substances (solids) and
observe and describe changes that occur.
Lesson 6 –
How does heat affect pure substances
(solids)?
Lesson 6 -
L6
Results - Heating substances
Substance
Potassium
permanganate
Ammonium
chloride
Copper sulfate
Sodium
chloride (I)
Sodium
chloride (NI)
Zinc oxide
Sulfur
Copper
carbonate
Appearance
before heating
Changes
observed
during heating
Appearance
after cooling
Lesson 6 –
• Physical and chemical changes result from the
application of heat.
• The way a substance behaves when it is heated is a
characteristic property of that substance.
• Evaporation and condensation results when heat energy
is greater than the forces that hold a solid together or
keep a liquid in a fluid state.
• Heating may cause a chemical change, phase change, or
no change at all.
• When cooling occurs after heating, changes in
substances may be reversible or irreversible.
• If a chemical reaction occurs, new substances with
different observable properties are formed.
• Chemical reactions have reactants and products………..
Lesson 6 –
(1-2)
29. chemical reaction - a change in which new
substances are formed; has reactants and
products.
30. reactant - the starting substances in a
chemical reaction.
31. product - a substance formed by a chemical
reaction.
32. physical change - reversible through physical
means and do not involve the formation of new
substances; no change in chemical properties.
33. chemical change - not readily reversible and
do involve the formation of new substances
with different properties.
Lesson 6 –
(2-2)
34. sublimation - physical change in which
a substance goes directly from a solid to
a gas and then back to a solid.
35. evaporation - the change of a
substance from a liquid to a gas
36. condensation - the change of state from
a gas to a liquid…..
Lesson 7 – Just A Phase
As ice is heated, you will observe the phase
changes that occur. You will also observe
melting and boiling points.
Lesson 7 –
How does heat affect phase changes?
Lesson 7
L 7.1 Temperature v. time
Time
(min. and s)
0
30 s
1 min
1 min, 30 sec
2 min
2 min, 30 sec
3 min
3 min, 30 sec
4 min
4 min, 30 sec
Temperature of
water (C degrees)
Observations
Lesson 7 –
•
•
•
Phase changes are dependent on temperature
and pressure.
Three phases or states of matter: solid, liquid,
gas
Phase changes take place when molecules
lose or gain kinetic energy (heat energy) and
can be related to a change in temperature.
• Lose kinetic energy – molecules move
closer – (gas > liquid > solid).
• Gain kinetic energy – molecules move
apart – (solid > liquid > gas)
•
A change of state is not the result of a
chemical reaction.
Lesson 7 The melting point and boiling point of a substance
is a characteristic property of the substance.
• Freezing and melting points are the same.
• An increased input of heat has no effect on the
boiling point of a substance, although it will
make a fixed mass of matter change state faster.
• Substances that boil are not always hot. Many
substances melt and boil below 0 degrees C…...
Lesson 7 –
(1-1)
37. melting - the phase change in which a solid turns into
a liquid.
38 . melting point - the temperature at which a solid turns
into a liquid; the same temperature as freezing point
(the temperature at which a liquid turns into a solid);
altered by changes in pressure.
39. boiling - the process by which a liquid changes into a
gas at its boiling point. .
40. boiling point - the temperature at which a liquid
changes into a gas; boiling point depends on air
pressure.……
Lesson 8 –
Changing Matter and Mass
You will determine what happens to the
mass of ice when it melts and water when
it freezes.
Lesson 8.1 What happens to the mass of water when it
changes from a solid to a liquid (ice to
water)?
Lesson 8.1
8.1 Determining a Change in Mass
Group #
Mass of Ice and
Bottle
Mass of Water and
Bottle
Change in Mass
( + or -)
Lesson 8.1 • Mass is conserved as matter goes through
phase changes………
Lesson 8.2 What happens to the mass of water when it
changes from a liquid to a solid (freezes)?
Lesson 8.2
L8.2 Determing a Change in Mass
Group
Mass of Bottle
and Water
Mass of Bottle
and Ice
Change in Mass
(+ or -)
Lesson 8.2 • Mass is conserved as matter goes through
phase changes………
Lesson 8 41. law of conservation of mass - mass is
neither created or destroyed; the total mass of
all substances remains the same regardless of
any changes in phase or chemical reactions
that occur.
42. phase - solids, liquids, and gases are three
phases or states of matter……….
Lesson 9
Lesson 9 43 . composite - a material made from two
or more substances
44. material - the substance from which
something is made
Lesson 10
Lesson 11 –
Pure Substance or Mixture
You will examine eight different substances
to determine if they are pure substances
or mixtures.
Lesson 11 –
How can you determine the difference
between pure substances and mixtures?
Lesson 11
L11 Identifying Pure Substances or Mixtures
Sample
A
B
C
D
E
F
G
H
Pure
Substance or
Mixture?
How did you reach your conclusion?
Lesson 11 –
• A pure substance has definite physical
and chemical properties.
• A mixture is made of two or more
substances with each substance keeping
its’ own properties.
• Solutions are mixtures.
• Compounds are not mixtures…..
Lesson 11 –
(1-1)
45. pure substance - matter that has definite
chemical and physical properties; either an
element or a compound
46. mixture - two or more elements or compounds
that are mixed together but are not chemically
combined; differ in physical and chemical
properties.
47. heterogeneous - different (poorly mixed)
48. homogeneous - same (well-mixed)
49. solution - a homogeneous mixture of a solvent
and a solute
Lesson 12 –
What Happens When Substances
are Mixed with Water?
You will mix several substances with water
and observe what happens.
Lesson 12 What property of matter determines what
type of mixture a substance will form when
mixed with water?
Lesson 12
L 12 What Happens to a Solid?
Name of Substance
added to water
Sugar
Sodium
chloride
Sulfur
Zinc oxide
Copper sulfate
Appearance after being
shaken 10 times
Does it
dissolve?
(Yes or No)
Lesson 12 –
• Solubility is a characteristic property of
matter.
• Solutions consist of a solvent and a solute.
• A solvent is the substance present in the
larger proportion in a solution.
• A solute is the substance present in the
smaller proportion.
• The components of a solution can be
solids, liquids, or gases.
• When a solid is passed into solution, it is
said to dissolve…………..
Lesson 12 -
(1-3)
50. soluble - substances that will dissolve
51. insoluble - substances that will not
dissolve
52. solubility - the amount of solute that will
dissolve in a solvent at a given
temperature and pressure; the ability of
one substance to dissolve in another.
53. solvent - the substance that the solute
is dissolved in; the substance present in
the larger proportion
Lesson 12 -
(2-2)
54. solute - the substance that dissolves in a
solvent; the substance in the smaller
proportion; may be solids, liquids, or
gases.
55. aqueous solution - solution in which
water is the solvent………
Lesson 13 –
How Much Solute Dissolves in a
Solvent?
You will make a saturated copper sulfate
solution. You will also conduct an
investigation to determine the solubility of
two different chemicals.
Lesson 13 –
Are different substances equally soluble in
water?
Lesson 13
L 13 - Determining Solubility
Volume of
water (mL)
Substance
10
Sodium
chloride
10
Sodium
nitrate
Initial mass of jar
& substance (g)
Final mass of jar
& substance (g)
Amount of
substance in
saturated
solution (g)
Lesson 13 –
• Solubility is the amount of a solute that will completely
dissolve in a given amount of a solvent.
• Solubility is a characteristic property of matter.
• Different substances are not equally soluble in water.
• A saturated solution has the maximum amount of solute
dissolved in it.
• When an unsaturated solution of a solid is cooled, it may
become saturated.
• Solubility is affected by temperature. Solids dissolved in
water may increase or decrease in solubility with the rise
in temperature. Gases always decrease in solubility with
increased temperature.
• Recrystallization occurs when a solution of a solid is
cooled and some solid solute precipitates out………….
Lesson 13 –
(1-1)
56. saturated solution - a solution that has the
maximum amount of solute dissolved in it at a
specific temperature and pressure.
57. exothermic - heat is given off (increase in
solubility with a decrease in temperature)
58. endothermic - heat is taken in (increase in
solubility with increase in temperature)
59. recrystallization - occurs when an
unsaturated solution of a solid is cooled and
becomes saturated and some solid solute
precipitates out, usually as crystals………..
Lesson 14 –
Mass, Volume, and Dissolving
You will use equal volumes of water and
alcohol (you will mass each one
separately) and will predict what will
happen to the mass and volume after
mixing the two substances.
You will also conduct an investigation to
determine what happens to the mass of
salt when it is dissolved in water.
Lesson 14.1 –
Is the volume and mass of a solution
different from the combined volume and
combined mass of the two separate
substances that make up the solution?
Lesson 14.1 -
14.1 Mixing Water and Alcohol
Liquid
Volume of
liquids (mL)
Water
50.0
Alcohol
50.0
Predicted
measurements
(water and alcohol)
Actual
measurements
(water and alcohol)
Differences
Mass of liquids and
cylinders
Lesson 14.1 –
• Water has space between the molecules
that allows soluble substances to occupy
that space.
• The combined volume of a separate
solvent and a solute is greater than that of
the solution they form.
• Mass, not volume, is conserved during
dissolving.
Lesson 14.2 –
What happens to the mass and volume of
one type of matter when it is dissolved in
another type of matter?
Lesson 14.2 -
14.2 Dissolving a Solid & Measuring Mass
Initial mass of
test tubes,
beaker, salt and
water (g)
Final mass of
test tubes,
beaker, and
dissolved salt
solution (g)
Difference/ change in
mass (g)
Lesson 14.2 –
• Water has space between the molecules
that allows soluble substances to occupy
that space.
• The combined volume of a separate
solvent and a solute is greater than that of
the solution they form.
• Mass, not volume, is conserved during
dissolving………….
Lesson 14
No new vocabulary
(solubility, volume, mass, solid..)
Lesson 15 Separating a Soluble and an
Insoluble Substance
You will focus on two separation techniques
that relate to solubility: filtration &
evaporation.
You will use a filter to determine which
substances will pass through.
Lesson 15 How can you separate soluble and insoluble
components of a mixture?
Lesson 15.1 -
15.1 Filtering a Solution
Mixture
Copper (II)
sulfate and
water
Zinc oxide
and water
Prediction
Result
Lesson 15.2 -
Lesson 15 • Filtration can be used to show that insoluble
substances will not pass through a filter.
• Solutions (the solvent and the solute) will pass
through a filter.
• Evaporation can be used to recover a solid from
a solution.
• The rate of evaporation could be increased by
heating, increasing the surface area, or
increasing airflow over the surface of the
solution. Dissolving the solute in the least
amount of solvent greatly reduces evaporation
time. …………..
Lesson 15 -
(1-1)
60. filtration - the process of separating a solid
and a liquid by passing a mixture of the two
through a mesh or filter paper.
61. residue - remains of a substance.
62. sedimentation - the process by which a solid
settles out from a solid/liquid mixture…..
Lesson 16 Researching Solvents
You will conduct an investigation to show
how solvents can remove stains.
Lesson 16 How effective are various solvents at
removing stains a variety of stains?
Lesson 16 -
Stain
Results
Solvent results
Water
Ketchup
Chocolate syrup
Vegetable oil
Marker pen ink
Ballpoint pen ink
Isopropyl Kerosene
alcohol
Lesson 16 • Water and other liquids can act as
solvents……….
Lesson 16 No new vocabulary.
Lesson 17 - Separating Solutes
You will use paper chromatography to
separate solutes and to compare the dyes
found in different colored inks.
17.0
Dip tip of green marker in 25 mL of water.
Lesson 17 What does the process of paper
chromatography indicate about an ink
solution?
17.1 - Analyzing Inks
Place a spot of green ink (2mm) on one
piece of chromatography paper.
Fold end of paper and hang the paper over
a pencil. Place the pencil and paper over
the beaker, with the tip of the paper in the
water.
Observe what happens over the next five
minutes.
Write conclusions on the student sheet.
Lesson 17
Lesson 17.3 (
RESULTS
Lesson 17 -
(1-2)
• Ink is made up of several dyes of different colors
that are dissolved in water.
• Chromatography is a technique used to analyze
solutions.
• Solutes in the ink must be soluble in the solvent
for the chromatogram to be produced.
• Different solutes move through paper at different
speeds. As the solution moves up the paper,
the various components of the solution separate
out and occupy distinct areas on the paper.
Lesson 17 -
(2-2)
• Less soluble dyes move slower that more
soluble dyes. The faster moving, more soluble
dyes will eventually separate.
• The characteristic properties of each solute
determine the way in which that solute
separated from a mixture of solutes in a solution.
• Chromatography does not separate colors; it
separates solutes.
• Chromatography is often used to separate
colorless substances……….
Lesson 17 -
(1-1)
63. chromatography - a process used to
separate different solutes from a solution
by passing them through a medium.
64. absorption - one substance penetrates
into the inner structure of another….
Lesson 18 - Changing Mixtures
You will investigate how adding salt affects
the melting and boiling points of water.
You will also investigate the melting points
of three different tin alloys.
Lesson 18.1 Does adding salt change the melting point of
ice?
Lesson 18.1 -
Lesson 18.1 • Adding salt to ice lowers the melting point.
The change in the melting point of a
solvent is directly proportional to the
amount of solute in the mixture.
Lesson 18.2 Does adding salt change the boiling point of
water?
Lesson 18.2 -
Lesson 18.2 • The boiling point of water rises when salt is
added to water because solute particles interfere
with the evaporation of a solvent.
Lesson 18.3 Do all metal alloys have the same melting
point?
Are the properties of a mixture different from
the properties of the individual
components that make up the mixture?
Lesson 18.3 -
Lesson 18.3 • The properties of a mixture can be very different
from the properties of the individual components
that make up the mixture.
• An alloy is a mixture that contains at least one
metal………………
Lesson 18 65. alloy - solutions of solid metals
66. freezing point - temperature at which a
liquid turns to a solid.
67. metal - group of elements; usually hard
solids; have common characteristics shiny, good conductivity, and
malleability…..
Lesson 19 Assessing Our Progress
You will investigate a mixture.
Lesson 19 What are the physical properties of
substances that make up a mixture?
Lesson 19 • Physical properties can be used to identify
the substances that make up a mixture.
Lesson 19 No new vocabulary.
Lesson 20 Breaking Down a Compound
You will use electrolysis to break down
water.
Lesson 20 Can compounds (such as water) be broken
down?
Lesson 20 -
Lesson 20 Use Student Sheet 20.1
Lesson 20 • Water is a compound made of the
elements hydrogen and oxygen.
• Compounds are pure substances made of
more than one element.
• Elements are pure substances that cannot
be broken down.
• Some pure substances are composed of
two or more pure substances combined.
• Compounds of pure substances can be
broken down by a chemical reaction…..
Lesson 20 -
(1-1)
68. element - a substance that cannot be
broken down into other substances by
chemical or physical means
69. compound - a pure substance
consisting of two or more elements
combined
Lesson 21 Examining and Grouping Elements
You will study the characteristics of 25
elements and look at how they are
grouped on the Periodic Table.
Lesson 21 What properties of elements can be used in
grouping elements?
Lesson 21 -
Lesson 21 -
Lesson 21 • Elements are grouped according to similar
chemical and physical properties.
• The Periodic Table is used in predicting
the chemical and physical properties of
elements.
• Each element can be identified by its
characteristic properties……….
Lesson 21 -
(1-1)
70. isotope - an atom that has the same number
of protons as other atoms of the same element
do but has a different number of neutrons; sum
of neutrons and protons.
71. reactivity - the readiness of a substance to
react chemically.
72. conductivity - able to allow electricity or heat
to pass through
73. conductor - carries electricity or heat
74. magnetic - a substance that is attracted to a
magnet…….
Lesson 22 - Combining Elements
You will examine four substances and
determine how they fit into two groups:
metals and nonmetals.
Lesson 22.1 What are the two main groups of elements?
Lesson 22.1 -
Lesson 22.1 • The two major groups of elements are metals
and nonmetals.
Lesson 22.2 What happens when elements combine?
Lesson 22.2 -
Lesson 22.2 • Elements combine to form new substances.
• Compounds are substances formed by a
chemical reaction between two or more
elements.
• Chemical reactions can be represented in the
form of equations.
• Iron + oxygen produces iron oxide……
Lesson 22 -
(1-2)
75. chemical equation - a representation
of a chemical reaction that uses symbols
to show the relationship between the
reactants and products.
Lesson 22 -
(2-2)
76. compound - a pure substance
consisting of two or more elements
combined by chemical bonds
77. element - a substance that cannot be
broken down into other substances by
chemical or physical means
78. reactant - the starting substances in a
chemical reaction.
79. product - a substance formed by a
chemical reaction…………..
Lesson 23 - Chemical Reactions
You will combine four different metals with
hydrochloric acid and look for the reactivity
of the metals. You will also compare the
corrosion of the four metals.
Lesson 23.1 Why are some elements more reactive than
others?
Lesson 23.1 - -
Lesson 23.1 Use Student Sheet 23.1.
Lesson 23.1 • Some metals are more reactive than others.
• The reactivity of metals determines how they
can be used.
• Metals on the right side of the periodic table are
less reactive than the other elements.
• Exothermic reactions give off heat……
Lesson 23.2 Do certain conditions prevent corrosion?
Lesson 23.2 -
Lesson 23.2 - -
Lesson 23.2 Use Student Sheet 23.2.
Lesson 23.2 • Corrosion is a chemical reaction that causes the
disintegration of a substance……
Lesson 23 80. reactivity - the readiness of a substance to
react chemically.
81. corrosion - a chemical reaction, usually
between a metal and the air.
Lesson 24 - Countering Corrosion
You will compare different substances that
prevent rusting from occurring.
Lesson 24 What causes rusting and how can it be
prevented?
Lesson 24 -
Lesson 24 -
24.1
Treatment
No treatment
Paint
Galvanizing
Petroleum jelly
Magnesium
wrapped
Stainless steel
nail
Appearance of Nail
Lesson 24 • Rusting occurs when iron is combined with
oxygen.
• Rusting is a chemical reaction with
reactants and products………
Lesson 24 No new vocabulary.
Lesson 25 Mass and Chemical Reactions
You will place an effervescent tablet in water
in an open container and in a closed
container. You will measure the mass
before and after adding the tablet to see if
the law of conservation of mass can be
applied to chemical reactions.
Lesson 25 What happens to the mass of matter in a
chemical reaction?
Lesson 25 -
Lesson 25 -
Lesson 25 -
Lesson 25 In a chemical reaction, the total mass of the
reactants and the products is the same.
The conservation of mass is demonstrated
in a closed system………
Lesson 25 82 . burning - a rapid chemical reaction between a
substance and a gas that produces heat and light;
most burning takes place in the air and has oxygen as
one of its reactants…..
Lesson 26