alchemy unit investigation v: building with matter lesson 1: you light up my life lesson 2: electron...

Alchemy Unit

Investigation V: Building with MatterLesson 1: You Light Up My LifeLesson 2: Electron Glue

Lesson 3: Nobel Gas EnvyLesson 4: Getting ConnectedLesson 5: Salty EightsLesson 6: As Good as Gold

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Alchemy Unit – Investigation V

Lesson 1:

You Light Up My Life


Unit 1 • Investigation V

© 2004 Key Curriculum Press.

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? What type of bonding does each substance have?



The Big Question

• What patterns do we see in the properties of substances?



You will be able to:

• Predict whether MgSO4(aq), epsom salts, will conduct electricity.



Activity

Purpose: This lesson allows you to collect evidence regarding some of the properties of substances, and look for patterns.

(cont.)



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



(cont.)

(cont.)



Substances that dissolve in water

Conduct Don’t conduct

(cont.)



Making Sense



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 NoNo

Conducts

Notes



Check-Out

• Predict whether MgSO4(aq), epsom salts, will conduct electricity. State your reasoning.

• If it is dangerous to take a bath with a blow dryer, what must also be true about the water in the bathtub?



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.


Lesson 2:

Electron Glue




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?



The Big Question

• How can we use bonding to explain the properties of substances we encounter?




• Classify the bonding that occurs in the making of brass.



• A chemical bond is an attraction between atoms that holds them together in space.

• The electrons in the outer shell determine how atoms bond. These are called valence electrons.

Notes: Chemical Bond and Valence Electrons



• 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.)



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.)



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.)



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.)



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.)



IonicCovalentNetwork Metallic

MolecularCovalent

(cont.)

(cont.)



Metalatoms

Non-Metalatoms

Metal &Non-Metal

atoms

MetallicCovalentNetwork

MolecularCovalent Ionic

Notes (cont.)



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.)



Ionic Covalent Network

Metallic Molecular Covalent

(cont.)



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.



Check Out

• On the very first day of class, you combined copper with zinc to form brass. How would you classify the bonding in brass? Ionic, Covalent or metallic?

• Would it dissolve in water? Why or why not?



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.


Lesson 3:

Noble Gas Envy




ChemCatalyst

• What type of bonding does this picture represent?

• What happens to the charge on each atom?




• Predict what would have to happen for potassium to obtain a noble gas configuration.



What happens when atoms bond?

1. Atoms can gain or loose electrons when they bond (covalent, ionic or metallic)

2. When this happens the atom is called an ion because it will have a charge. (positive or negative)



• A valuable piece of information helps 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.)



•When atoms bond they will gain or loose electrons to get closer to the configuration of their nearest noble gas.

What do atoms do when they bond?



How do we know which ones will gain and which ones will lose?

Metals tend to lose their electrons (becoming positive +) while nonmetals tend to gain electrons (becoming negative -)



What do they become when they gain or lose electrons?

• Cations :Atoms that loose electrons and have a positive charge.

• Ex. Sodium becomes Na+ _______________________________

• Anions: Atoms that gain electrons and have a negative charge.

• Ex. Bromine becomes Br-



Which is the cation and which is the anion?



Purpose: You will explore the ions that are formed when atoms give up and receive electrons from other atoms.



Make a picture for all of the elements in Period 2 ( skip Flourine)



Making Sense

• Why do you think the noble gas configuration is especially stable?



Check-Out

• Write the electron configuration for potassium, K.

• What would have to happen for potassium to have a noble gas configuration? Explain.



Wrap-Up

• 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.


Lesson 4:

Getting Connected




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.



The Big Question

• What determines how two elements will combine to form ionic compounds?




• Use the number of valence electrons to determine which ionic compounds can form.



• 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



ActivityElement 1

(metal)# of

valence electrons

Element 2(nonmetal)

# of valence

electrons

compound total # of valence

electrons

Na 1 F 7 NaF sodium fluoride

8

MgOmagnesium

oxide

MgCl2magnesium

chloride

Neneon

BeF2

beryllium fluoride



ActivityElement 1

(metal)# of

valence electrons

Element 2(nonmetal)

# of valence

electrons


electrons


8

Mg 2 O 6 MgOmagnesium

oxide

8

MgCl2magnesium

chloride

Neneon

BeF2

beryllium fluoride



ActivityElement 1

(metal)# of

valence electrons

Element 2(nonmetal)

# of valence

electrons


electrons


8


oxide

8

Mg 2 Cl 7 MgCl2magnesium

chloride

16

Neneon

BeF2

beryllium fluoride



ActivityElement 1

(metal)# of

valence electrons

Element 2(nonmetal)

# of valence

electrons


electrons


8


oxide

8


chloride

16

Ne 8 N/A 0 Neneon

8

BeF2

beryllium fluoride



ActivityElement 1

(metal)# of

valence electrons

Element 2(nonmetal)

# of valence

electrons


electrons


8


oxide

8


chloride

16

Ne 8 N/A 0 Neneon

8

Be 2 F 7 BeF2

beryllium fluoride

16



Element 1(metal)

# of valence

electrons

Element 2(nonmetal)

# of valence

electrons


electrons

MgSmagnesium

sulfide

CaCl2calcium chloride

Na Br

K Se

Al N

Al O Al2O3

aluminum oxide

Al F



Making Sense

• Can you make a rule that helps you predict the composition of compounds that form?



Check-In

• What elements will combine with Sr, strontium, in a one-to-one ratio?



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.


Lesson 5:

Salty Eights




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.



The Big Question

• What salts can be formed by combining a metal and a non-metal?




• Apply the octet rule.



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.)



• 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.)



• 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.)



• 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.)



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.)



• 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.)



Metal Nonmetal Compound

Formula

Compound Name Point

value

Total



Problem of the Day

What types of bonds are in these compounds?

(a) Na2S

(b) K2Mg

(c) AlBr2

(d) Na3N

(e) OCl

(f) CaMgO2



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.


Lesson 6:

As Good as Gold




ChemCatalyst

• Name three items that might be on an exam covering the entire Alchemy Unit.



The Big Question

• Can an element be turned into something else?




• Explain the relationship between compounds, atoms, elements, and the periodic table.



Activity

Purpose: This lesson provides you with end-of the-unit review and practice.

(cont.)



Element Symbol Atomic

No.

Group

No.

# of protons

Numberof valenceelectrons

Electron configuration

oxygen

iodine

iron

radon

tungsten

lead

(cont.)

(cont.)



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.)



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.



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.)



d) Investigation IV: How can gold be produced from copper in a nuclear reaction? Give a specific example.

e) 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.)



Check-In

• No Check-In.



Wrap-Up

• No Wrap-Up.

alchemy unit investigation v: building with matter lesson 1: you light up my life lesson 2: electron...

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