alchemy unit investigation v: building with matter · rules for salty eights: the point of the game...
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Alchemy Unit
Investigation V:
Building with Matter
Lesson 1: You Light Up My Life
Lesson 2: Electron Glue
Lesson 3: Nobel Gas Envy
Lesson 4: Getting Connected
Lesson 5: Salty Eights
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Alchemy Unit – Investigation V
Lesson 1:
You Light Up My Life
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
ChemCatalyst
• If you were to drop a spoonful of salt,
NaCl, into a glass of water, what would
happen? If you were to drop a gold
ring into a glass of water, what would
happen?
• What do you think is different about the
atoms of these two substances? Why
wouldn’t the individual gold atoms
come apart?
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
The Big Question
• What patterns do we see in the
properties of substances?
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
You will be able to:
• Predict whether MgSO4(aq), epsom
salts, will conduct electricity.
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Activity
Purpose: This lesson allows you to
collect evidence regarding some of the
properties of substances, and look for
patterns.
(cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Predictions Test Results
Substances Conduct?
Yes/No
Dissolve?
Yes/No
Conduct?
Yes/No
Dissolve?
Yes/No
H2O(l), water Yes
Al(s), foil aluminum
C12H22O11(s), sucrose
(sugar)
NaCl(s), salt,
sodium chloride
SiO2(s), sand,
silicon dioxide
C20H42(s), paraffin (wax)
C2H6O(l), ethanol
Cu(s), copper
CaCl2(s),
calcium chloride
CuSO4(s), copper
sulfate
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
(cont.)
(cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Substances that dissolve in water
Conduct Don’t conduct
(cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Making Sense
• If it is dangerous to take a bath with a
blow dryer, what must also be true
about the water in the bathtub?
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
NaCl – salt
CuCl2 – calcium
chloride
CuSO4 – copper
sulfate
H2O – water
C12H22O11 –
sugar
C2H6O – ethanol
Au – gold
Cu – copper
Al – aluminum
SiO2 – sand
C20H42 – paraffin
Dissolves
Yes No
Conducts
Yes Yes No No
Conducts
Notes
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Check-In
• Predict whether MgSO4(aq), epsom
salts, will conduct electricity. State your
reasoning.
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Wrap-Up
• Not all substances conduct electricity.
• Substances that do conduct electricity
involve either solid metals, or metal-
nonmetal compounds dissolved in
water.
• Not all substances dissolve in water.
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Alchemy Unit – Investigation V
Lesson 2:
Electron Glue
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
ChemCatalyst
A gold ring is made up of individual gold
atoms.
• What keeps the atoms together?
• Why don’t the atoms just fall apart from
each other?
• What parts of the atom do you think
are responsible for keeping the atoms
together in a solid?
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
The Big Question
• How can we use bonding to explain
the properties of substances we
encounter?
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
You will be able to:
• Classify the bonding that occurs in the
making of brass.
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
• A chemical bond is an attraction
between atoms that holds them
together in space.
Notes
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Activity
Purpose: This lesson helps to explain
the physical properties of basic
substances by examining the types of
bonds that exist between the atoms of
these substances.
(cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Ionic Covalent
Network Metallic Molecular
Covalent
(cont.)
(cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Ionic Covalent Network
Metallic Molecular Covalent
(cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Making Sense
• If you have the chemical formula of a
substance, how and what can you
figure out about it’s properties?
Explain. Use the compound silver
nitrate, AgNO3, as an example.
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Model 1: IONIC
Properties:
Made of metal and non-metal atoms
Dissolves in water
Conducts electricity when dissolved but not when
solid
Brittle solids
Description of drawing: Spheres without gray
areas represent metal atoms. Spheres with gray
areas are non-metal atoms. Metal atoms “give up”
their valence electrons to non-metal atoms.
Notes
(cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Model 2: COVALENT NETWORK
Properties:
Made entirely of nonmetal atoms
Does not dissolve in water
Does not conduct electricity
Very hard solids
Description of drawing: Valence electrons
connect atoms with each other in all directions
– like a grid or network.
(cont.)
Notes (cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Model 3: METALLIC
Properties:
Made entirely of metal atoms
Do not dissolve in water
Conduct electricity
Bendable solids
Description of drawing: Valence electrons
are free to move throughout the substance like
a “sea” of electrons. (cont.)
Notes (cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Model 4: MOLECULAR COVALENT
Properties:
Made of nonmetal atoms
Some dissolve in water, some do not
Do not conduct electricity
Tend to be liquids or gases or softer solids
Description of drawing: Valence electrons
are shared between some atoms. This creates
small stable units within the substance.
(cont.)
Notes (cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
• Atoms which are connected into many
identical units are called molecules.
They units may be composed of only
two atoms or of dozens of atoms.
(cont.)
Notes (cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
NaCl – salt
CuCl2 – calcium
chloride
CuSO4 – copper
sulfate
H2O – water
C12H22O11 –
sugar
C2H6O – ethanol
Au – gold
Cu – copper
Al – aluminum
SiO2 – sand
C20H42 – paraffin
Dissolves
Yes No
Conducts
Yes Yes No No
Conducts
Ionic Molecular
Covalent
Metallic Covalent
Network
Notes (cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Metal
atoms
Non-Metal
atoms
Metal &
Non-Metal
atoms
Metallic Covalent
Network
Molecular
Covalent Ionic
Notes (cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Check-In
• On the very first day of class, you
combined copper with zinc to form
brass. How would you classify the
bonding in brass? Explain.
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Wrap-Up
• A chemical bond is an attraction
between atoms involving the valence
electrons.
• There are four types of bonds: ionic,
extended covalent, molecular covalent,
and metallic.
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Alchemy Unit – Investigation V
Lesson 3:
Noble Gas Envy
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
ChemCatalyst
• What type of bonding does this picture
represent?
• What happens to the charge on each
atom?
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
The Big Question
• What ion charges are formed when
atoms attain a noble gas electron
configuration?
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
You will be able to:
• Predict what would have to happen for
potassium to obtain a noble gas
configuration.
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Notes
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Activity
Purpose: You will explore the ions that
are formed when atoms give up and
receive electrons from other atoms.
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Making Sense
• Why do you think the noble gas
configuration is especially stable?
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
• A valuable piece of information that
can help us predict which ions might
be encountered in chemistry: Atoms
tend to lose or gain electrons to
attain the electron configuration of
the noble gas nearest to it on the
periodic table.
Notes
(cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
• Atoms with a positive charge are called
cations.
• Atoms with a negative charge are
called anions.
(cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Check-In
• Write the electron configuration for
potassium, K.
• What would have to happen for
potassium to have a noble gas
configuration? Explain.
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Wrap-Up
• Noble gases are stable with filled
outermost electron shells.
• Atoms can gain or lose electrons to
end up with a noble gas configuration.
• When atoms lose electrons, they have
a positive charge and are called
cations.
• When atoms gain electrons, they have
a negative charge and are called
anions.
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Alchemy Unit – Investigation V
Lesson 4:
Getting Connected
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
ChemCatalyst
• Only certain combinations of elements
result in the formation of compounds.
Li, lithium, will react with F, fluorine, to
form LiF, but it won’t form LiF2 or LiF3.
Mg, magnesium will react with F to
form MgF2, but it won’t form MgF or
MgF3. Explain what you think is going
on.
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
The Big Question
• What determines how two elements
will combine to form ionic compounds?
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
You will be able to:
• Use the number of valence electrons
to determine which ionic compounds
can form.
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Activity
Element 1
(metal)
# of valence
electrons
Element 2
(nonmetal)
# of valence
electrons
compound total # of valence
electrons
Na 1 F 7 NaF
sodium
fluoride
8
Mg O MgO
magnesium
oxide
Mg 2 Cl 7 MgCl2
magnesium
chloride
16
Ne Ne
neon
Be F BeF2
beryllium
fluoride
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Element 1
(metal)
# of valence
electrons
Element 2
(nonmetal)
# of valence
electrons
compound total # of valence
electrons
MgS
magnesium
sulfide
CaCl2
calcium
chloride
Na Br
K Se
Al N
Al O Al2O3
aluminum
oxide
Al F
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Making Sense
• Can you make a rule that helps you predict the composition of compounds that form?
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Unit 1 • Investigation V
• Rule of Eight: Ionic compounds tend
to form from atoms that together have
a total of 8 (or a multiple of 8) electrons
in their outermost (valence) shells.
This gives each ion a valence electron
configuration identical to a noble gas
and makes them very stable.
Notes
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Unit 1 • Investigation V
Check-In
• What elements will combine with Sr,
strontium, in a one-to-one ratio?
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Unit 1 • Investigation V
Wrap-Up
• Elements react to form compounds in
such a way as to result in 8 electrons in
their outermost (valence) shell (or a
multiple of eight).
• Compounds with eight valence electrons
are very stable.
• Noble gases already have eight valence
electrons and don’t combine with other
elements to make new compounds. They
are already very stable.
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Alchemy Unit – Investigation V
Lesson 5:
Salty Eights
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
ChemCatalyst
• List the compounds you can make with
pairs of cards of two different elements.
• List the compounds you can make with
three cards and only two different
elements.
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
The Big Question
• What salts can be formed by
combining a metal and a non-metal?
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
You will be able to:
• Apply the octet rule.
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Activity
Rules for Salty Eights:
The point of the game is to make
compounds and to be the first to play all
of the cards in your hand. These
compounds can have two or three or
more cards in them, but they can only
have two different elements. The game
ends when a player uses up all of the
cards in his or her hand making
compounds. (cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
• Shuffle the deck as best as possible.
• Deal eight cards to each player.
• The player to the left of the dealer plays first.
• Using at least two cards from your hand, try
to make one compound – the valence
electrons must add up to eight or a multiple
of eight. You must have at least one pink
card and one blue card with each compound
(the noble gases—green cards—are an
exception and can be played singly). (cont.)
(cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
• You must play every turn. In other words
you must make one compound each time
it is your turn. If you cannot make a
compound you must draw from the draw
pile until you can put down a compound.
• When you form a compound during your
turn simply place those cards on the
table in front of you. As soon as you put
down a compound you must name it and
then your turn is over. (cont.)
(cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
• Play proceeds around the circle until a
player uses up all of his or her cards.
• A player gets 20 points for going out
first.
• Wild cards can be used as any element
in that particular group (Wild cards only
exist for Groups 1 and 7). The player
must identify which element a wild card
represents at the time it is played. (cont.)
(cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Scoring:
Every compound played on the table is
worth points. The cards left in a person’s
hand are subtracted.
• 5 points for every noble gas.
• 10 points for every compound made
out of two cards.
• 40 points for every compound made
out of three cards. (cont.)
(cont.)
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Unit 1 • Investigation V
• 70 points for every compound made
out of four cards.
• 100 points for every compound made
out of five cards.
• 20 points for going out first.
Any player with cards left in his or her
hand must count up the number of
valence electrons and subtract them from
his or her total. (cont.)
(cont.)
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Unit 1 • Investigation V
Metal Nonmetal Compound
Formula
Compound Name Point
value
Total
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Check-In
Which of the following compounds are
likely to form?
(a) Na2S
(b) K2Mg
(c) AlBr2
(d) Na3N
(e) OCl
(f) CaMgO2
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Wrap-Up
• Ionic compounds tend to form from
atoms that together have a total of 8 (or
a multiple of 8) electrons in their
outermost (valence) shells
• Compounds with eight valence electrons
are highly stable.
• Noble gases already have eight valence
electrons and don’t combine with other
elements to make new compounds. They
are already highly stable.
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Alchemy Unit – Investigation V
Lesson 6:
As Good as Gold
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
ChemCatalyst
• Name three items that might be on an
exam covering the entire Alchemy
Unit.
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
The Big Question
• Can an element be turned into
something else?
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
You will be able to:
• Explain the relationship between
compounds, atoms, elements, and the
periodic table.
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Activity
Purpose: This lesson provides you with
end-of the-unit review and practice.
(cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Element
Symbol
Atomic
No.
Group
No.
# of
protons
Number of valence electrons
Electron
configuration
oxygen
iodine
iron
radon
tungsten
lead
(cont.)
(cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Substance Conducts?
Yes/No
Dissolves in
H2O?
Yes/No
Conducts
after
dissolving?
Type of
bonding
CuxZnx – brass
CSi – silicon
carbide
C3H8 – propane
CuCl2 – copper
chloride
(cont.)
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
Making Sense
It is not possible to convert copper into
gold in chemical reactions. This can only
be done by nuclear reactions, which
require the energy of a supernova. Thus,
we must resort to using chemistry to
create things that are as good as gold.
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© 2004 Key Curriculum Press.
Unit 1 • Investigation V
a) Investigation I: How do the mass and
volume of copper and gold compare?
b) Investigation II: Copper and gold have
similar properties, but gold is more
bendable than copper. Is this consistent
with their locations on the periodic table?
c) Investigation III: How are copper atoms
different from gold atoms? Be specific
about the difference in the numbers of
atomic particles. (cont.)
Notes (cont.)
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Unit 1 • Investigation V
d) Investigation V: The golden penny
produced on the first day of this Unit was
brass, CuZn. If you wanted to make a
substance that is as good as gold, would
you choose any elements on the right
side of the periodic table? Why or why
not?
Notes (cont.)
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Unit 1 • Investigation V
Check-In
• No Check-In.
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Unit 1 • Investigation V
Wrap-Up
• No Wrap-Up.