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 * Welcome to your personal class wiki page. Only you should edit this wiki and no other page unless designated by Mr. Miller. It is very important that you follow protocol. If you edit another student's page it will show in the history of that page and you will be penalized or reprimanded appropriately. This should be a fun activity and will be part of your grade. If you have any questions feel free to email Mr. Miller at any time.**


 * Parts of the Earth Assignment**

1.What is the main composition of the Earth's core? Iron and Nickel 2.Which layer of the Earth is thinnest? The crust 3.Which layer of the Earth is the source of all of the materials that we use? The crust 4.What is the theory that describes the changes of the earth's surface over time? The plate tectonics theory. 5.Which layer of the Earth is described in question 4? The outer layer or lithosphere. 6.Which type of boundary marks the location where two plates move apart from one another? A divergent boundary 7.Give an example of a transform boundary.. The boundary between the pacific plate and the north american plate in california. 8.Define a subduction zone. The more dense oceanic crust bends and gets pulled under the continental crust. 9.What causes sea floor spreading? Plates made of oceanic crust pull apart, a crack in the ocean floor appears. Magma then goes up from the mantle to fill in the space between the plates. This creates a raised ridge called a mid-ocean ridge. The magma can also spread outward which forms a new ocean floor and a new oceanic crust. 10.Describe the formation of a rift. When two continental plates diverge. This creates a valleylike rift. Streams and rivers then flow into the valleys which can create long narrow lakes. The widening crust could become thin enough that it breaks and creates a new tectonic plate. Water then rushes in and forms a new sea or ocean basin. 1.Identify the 5 essential characteristics of a mineral. It must occur naturally, it must be inorganic, it must be a solid, its atoms must be arranged in a definite pattern, and it must have a definite chemical composition that may vary within specified limits 2.Identify three properties used to identify minerals. Hardness, optical properties, or crystal structure 3.Identify three examples a mineral. Identify the composition of each mineral by the formula of the compound and name of a compound.
 * What Are Minerals? **
 * 1) Calcite, CaCO3 is made of Calcium, Carbon, and Oxygen
 * 2) Ruby, Al2O3 is made of Aluminum and Oxygen
 * 3) Pyrite, Fe2S is made of Iron and and Sulfur


 * Life Cycle of Copper/BS4**

1.What factors make it worthwhile for a mining company to mine in a specific location for a particular ore? "The amount of useful ore at the site, the percent of metal in the ore, the type of mining and processing needed to exract the metal from its ore, the distance of the mine from the metal refining facility and markets, and the matal's supply-versus-demand status"

2.List and describe the seven steps in the copper cycle. The copper ore starts in the ground. Then the ore is reduced to only the copper. The Copper metal is then melted to make it be able to be molded. Then the copper metal is Molded into things we can use such as pipes, cords, and pots and pans. The products are then Distributed throughout the u.s. and are mainly permanent used, but some are discarded. The copper is then recycled that isn't being used and the recycled copper can be reused.

3.Answer questions #1-3 on pp.115-116 (Building Skills 4) 1. It can be used for pots, and pans, and food preperation machinery because it conducts heat well so it will get hot and cook food, and also it won't corrode so it will be able to be used for a long time. It is good for roofs and pipes because it is malleable and will not corrode. It is also good for jewelery and coins because it is relatively cheap to get, it is shiny, it doesn't corrode easily and and it is malleable.

2a. If you recycle more scrap metal, it can be melted into molten copper and be reused like any new copper ore. 2b. Yes, because eventually there won't be any copper left that anyone wants to recycle. It will all be in use.

3a. People are using debit and cards much more now instead of using bills and coins. Therefore the demand for copper for coins will go down. 3b. Many people use cordless house phones or cell phones now so there won't be a demand for copper for the cords of phones. 3c. Many power plants don't have a high demand for copper now because they already have what they need because the copper they have doesn't corrode quickly. 3d. Many things are becoming wireless so there will be a decreased demand for copper for wires and cords.

B.2 - Converting Copper Laboratory Mass Crucible alone 4.31 g Lid alone 3.68g Crucible+lid 7.99g Copper powder 1.10g crucible+copper 5.41g Crucible+lid +powder 9.09g

After Crucible+powder 5.42 g Crucible+powder+lid 9.10g Copper mass alone 1.11g

observations... After the first two minutes of heating, it turned gray and smells bad. It stayed the same until 8 minutes into the heating, then it had a red tint to it.

Questions 1a. Chemical 1b. It changed color when heat was applied to it 2a. It turned gray and the pieces started to stick together slightly, then the pieces started to get very hot and started to turn red a little. 2b. They stayed in the crucible because the lid was on and the pieces weren't at a liquid stage so it couldn't evaporate. 3a.The mass of the contents in the crucible increased. 3b. This was because heat was added and which caused there to be a reaction and the molecules created from the reaction were mixed in with the copper. ** (Consider that the oxygen atoms in the air "combined" with the copper.) **

= B.3 - Metal Reactivity =

1.Describe what happens to the penny when it is placed in the sliver nitrate solution. The coin's surface gets dark. After a while, the shiny crystals form on the penny. The solution turns a light blue as well. Underneath the crystals, the coin's surface shows that some copper has dissolved.

2.Describe how ions in solution play a role in chemical reactivity The ions have to have the same charge such as 1+ and 1-

3.Explain, in detail, why this is happening, If the ions have the same charge then they will react but if the have different charges then you need more of an ion to make them equal.

4.Define Oxidation. When atoms leave some of its electrons in a metal structure. Such as when copper ions leave two electrons in a metal structure and create a copper(II) ion.

5.Define Reduction. When an elements' ion gains an electron from another elements' atoms. Such as when a silver ion gains an electron from a copper atom.

6.Explain what happens to the copper atoms during the redox reaction. Copper atoms are losing electrons during the redox reaction.

7.Explain what happens to the silver ions during the redox reaction. For every two electrons lost by the copper atoms, two silver ions each gain an electron

8.What ultimately controls chemical reactivity? Valence Electrons

B.3 - Reactivity of Metals Laboratory

solution turned black || When dropping solution, fizz sound || No reaction || The metal turned black || Solution turned black || No reaction || No reaction || turned barely green || Little reaction, solution turned black || No reaction || No reaction ||
 * || CuNO3 || AgNO3 || MgNO3 || ZnNO3 ||
 * Cu || No reaction || Slight reaction
 * Mg || Solution turned green
 * Zn || Slight reaction, solution


 * Ag || No reaction || No reaction || No reaction || No reaction ||

1. Which metal reacted with most of the solutions? Zinc

2. Which metal reacted with the fewest solutions? Copper

3. With which of the solutions (if any) would you expect silver metal to react, if it were available to be tested? I wouldn't expect it to react with anything.

4. List the metals (including silver) in order, placing the most reactive metal first (the one reacting with the most solutions) and the least reactive metal ( the one reacting with the fewest solutions) Zinc, Magnesium, Copper, Silver

5. Refer to your "metal activity series" list in question 4. Write a brief explanation of why the outside surface of a penny is made of copper instead of zinc. If the outside of a penny were zinc, the penny would react with many everyday solutions we deal with because it is more reactive to acids than copper which doesn't react to many things.

6a. Which of the four metals mentioned in this laboratory activity might be an even better choice than copper for the outside surface of a penny? Why? Silver, because it reacted with the least solutions. It reacted to zero of the solutions which is even less than copper, which is the outside of a penny now.

6b. Why do you think that metal is not used for that purpose? I think it isn't used for that purpose because it can more expensive than copper. Also there are already many coins that have silver outsides so it can be confusing and everyone is used to a penny being copper colored as well so it would be very tough to get used to.

7a. Which metal is most likely to be found in an uncombined, or "free," (metallic) state in nature? Zinc

7b. Which metal is least likely to be found chemically uncombined with other elements? Copper

8a. Would it have been possible to eliminate one or more of the metal-solution combinations and still obtain all information needed to create chemical activity ratings for the metals? Yes.

8b. If so, which combinations could have been eliminated? Why? The copper metal with the copper nitrate solution, the magnesium metal with the magnesium nitrate, and the zinc metal with the zinc nitrate solution. This is because they have the same things in them so they won't react anytime.


 * Activity Series of Metals**

1.Answer the following questions about these pages. Move the oval up the post to watch the different videos. Watch the videos about Oxidation/Reduction in relation to Zn and Mg by clicking the play button at each level. Describe what happens to the size of the Magnesium atoms as they change into Magnesium ions. Do the same for Zinc. Describe what happens when Zn2+(aq) reaction with Mg(s). Describe what happens when Mg2+(aq) reacts with Zn(s). The magnesium atom stays the same but the area around it goes away and the area inside the atom gets smaller. The exact same thing happened for the zinc atom.

2.Go to page 2. Click the ? in the table. Watch the video for each reaction. Describe what is happening for each reaction. Identify if the reaction occurred or if there was No Reaction. No reaction occured between Cu and Zn2+. No reaction occured between Cu and Mg2+ either. There was a reaction between both Mg and Cu2+ and Zn and Cu2+.

3.Go to page 3. You should recognize this table from the reactions in the laboratory. Identify what happens during each of the prediction spaces.Answer the question at the bottom of the page.Continue to page 4. The Ag will not react with the Mg2+﻿ or the Zn2+. The Mg and the Zn will react with the Ag+ because they are more reactive than the Ag+. It will react because the zinc metal is more reactive than the silver ions so they will replace the silver ions and the silver will go out of the solution.

4.Now go to page 5. List the elements in order, from top to bottom (most reactive to least reactive), for the Activity Series of Metals. Go to page 6. Magnesium, zinc, copper, silver

ChemQuandry 1/Building Skills 5
1. Because they are in their most non reactive state so they are easier to recover.

Building Skills 5 1a. The left side is more reactive, and it keeps getting lower and lower as you go to the right. 1b. The left side 1c. The right side

2a. There will be a reaction. 2b. No it will not 2c. Because a more reactive metal will replace the less reactive metal in the solution. Therefore, the iron will replace the lead in the lead (II) nitrate solution.

3a. Yes, because all they do to recover the non reactive metals is pass electricity through them where when the metals are more reactive, they have to go through a much longer more expensive process to recover the metal.


 * Modeling Matter p.124**

1a. Zn: --> Zn2+ + 2e- 1b. Ag+ + e- ---> Ag.

2a. The atom of zinc went through reduction to become a Zn2+ ion. 2b. The silver ion is oxidized to a metallic silver atom.

3a. Ag+ 3b. Cu

4. Each copper loses two electrons. So the copper atoms are oxidized and the two lost electrons are replaced by the two Ag+ ions.

5a. Cu(s) 5b. The atom that provides the electrons in the reaction.

6. Zn.(s) + Cu: (aq) > Zn: (aq) + Cu.(s)

7a. Cu2+ (aq) 7b. Zn(s)

8. Oxidizing agent: Cu2+(aq) Reducing Agent: Zn(s)

9. You could tell by knowing which element was more reactive. That would be the reducing agent and the oxidizing agent would be the less reactive out of the reaction.

10a. Oxidized: Zn2+(aq) 10b. Reduced: Mg(s) 10c. Oxidizing agent: Zn2+(aq) 10d. Reducing agent: Mg(s)


 * C.5 Retrieving Copper Lab**

copper oxide turned red because the more reactive HCl is reducing the copper oxide.
 * || First Sample || Second Sample ||
 * Filter Paper Weight (in grams) || .70g || .69g ||
 * Filter Paper Weight with Copper After (in grams) || 1.80g || 1.61g ||
 * Total Copper Recovered (in grams) || 1.10g || .92g ||

Lab Questions 1a.I think it was incomplete because the only reaction happening was heating which takes a while to completely react. Because the copper wasn't completely exposed 1b.I would heat the original copper powder for a longer period of time if i were to do this again. I would scratch the outside of the copper because it would expose the copper inside 2a. 1.10 grams 1.10g - 1.10g= 0g 2b. About 99% about 0% 3a.Cu2+ Zn: -> Cu: + Zn2+ 3b. Zn: was oxidized 3c. Cu2+ was reduced 3d. The reducing agent was Zn: 3e. The oxidizing agent was Cu2+ 4a. The solution got dark. It turned a dark gray/ blackish color 4b. Because the zinc metal was replacing the copper in the solution 4c. It shows that copper was being removed from the solution and the zinc was replacing it. 5a. Zinc and acid 5b. Zinc went into the CuCl2 solution and the acid went into the air

** Reading Questionnaire **
 * Section C.6-C.7 pp.145-148 – Conservation in the Community**

1. Describe the main differences between renewable and nonrenewable resources and provide an example of each. Renewable resources can eventually be replenished by natural processes. Non renewable resources cannot be readily replenished. An example of a renewable resource is a plant. An example of a nonrenewable resource is coal.

2a) If atoms are always conserved why do some people say that a resource may be “running out”? b) Can a resource actually “run out”? Atoms are conserved in chemical processes while molecules aren't always. So if the the molecule production of something is lower than how fast we use it, it would be considered "running out." A resource's molecules can actually run out.

3.What are the requirements for minimum profitability levels for a metal in an ore? It has to have at least some minimum metal content. The levels depend on which metal is in the ore.

4.Identify and explain the two strategies for avoiding the depletion of metal ores. One is to slow down the rate at which the resources are used. This could involve changing some things in your life such as walking or riding a bike sometimes instead of always driving or reusing and recycling things. Another way is to replace a resource by finding different substances with similar properties, if possible using renewable resources. You could also refurbish materials instead of throwing them away and sending them to a landfill.

5.Can recycling also create environmental problems? If so, explain how this can happen.

Yes because the process to take metals out of some products could be harmful to the air and create pollution.

6.How much trash does the average person produce per day? 4 pounds (2kg)

7.Identify two ways that consumer products can become waste. If they have reached their initial purpose or get replaced by a newer model of that product.

8.Describe a way of dealing with recyclable waste that might be profitable good for energy use. The waste can be turned into energy by creating combustion and can be used and will produce about a third of the energy coal would.

9. What are the three options for the final step in the life cycle of a material?

Recycling, landfilling, and combustion.

10. Which waste category has the greatest weight before recycling? What is the weight of this waste produced? Paper, 83.8 million tons

11. Using waste category has the least weight before recycling? What is the weight of this waste? Wood, 11.6 million tons

12.Calculate the difference between the waste produced from your answer to question 11 and the amount of waste produced after recycling. Remember these values are in __millions of tons__, so make sure that you calculate correctly and label with the correct units of measure. (1 ton = 2000 lbs) 11.6 million tons x 2000pounds in ton= 23,200 million lbs before recycling 11.0 million tons x 2000pounds in ton= 22,000 million lbs after recycling 23,200million lbs - 22,000million lbs = 1,200 million lbs of waste

13.If we compare the Total Generation of Waste **(before recycling)** to the Total Discards of Waste **(after recycling)**, what percentage of waste is actually thrown away? What percentage of the Total Generation of Waste is actually recycled? Show your calculations below using the correct units of measure and labels.

217million tons x 2000lbs in a ton= 434,000 million lbs before recycling 156.3million tons x 2000lbs in a ton=312,600 million lbs after recycling 434,000million lbs -312,600 million lbs =121,400 million lbs not recycled 121,400million lbs/434,000 million lbs= .28 x 100%= 28% thrown away 312,600 million lbs/ 434,000 million lbs= .72 x 100% = 72% recycled

14.Draw the diagram in Figure 22, on page 148, in the space below. Compare this to Figure 20 on page 146. Match and Label the location of the steps in figure 20 to your diagram by connecting them with lines/arrows around the outside.



Building Skills 10 or start looking at the Making Decisions or work on the section assessment quesions questions. 4a,c,d, 6-8a, 9-18a-c (for NaCO3 • 10H2O only) 1a. Matter cannot be created nor destroyed 1b.Scientific laws are like facts that will always happen and never not be true 2a. 1 Sn 1 1 H 2 1 F 2 not balanced 2b. 1 Si 1 2 O 1 1 C 2 not balanced 2c. 1 Al 1 3 OH 3 H 6 3 Cl 3 O 3 not balanced 3. Because you can never get rid of all of a substance chemically. The only thing that you might not have are molecules and that's physically.

D.3 Lab Striking the Rich

Penny treated with Zn and ZnCl2 and heated with hot plate... Turned a goldish color also
 * Condition || Appearance ||
 * Untreated Penny || Regular copper color, shiny ||
 * Penny Treated with Zn and ZnCl2 || Turned silver ||
 * Penny Treated with Zn and ZnCl2 and heated in burner flame || Turns Gold then burned slightly and turned orange ||

Lab Questions p.159 1a. Untreated- copper color, shiny Treated with Zn and ZnCl2- turned silver Treated with Zn and ZnCl2 and heated in burner flame- turned gold Treated with Zn and ZnCl2 and heated on hot plate- turned gold 1b. First coin- copper Second coin- copper and zinc Third coin- copper and zinc Fourth coin- copper and zinc 2. You could put it in a solution that you know the reactivity of and if it reacts than it is more reactive than the solution and you can determine what substance it is from the reactivity. 3. To make pipes and musical instruments. 4a. They mixed with the zinc. 4b. Yes, because you can melt the pennies and seperate the two metals while they're liquids.\

D.6 Copper Plating Lab

Observations Before- The iron nail was silver. Copper was copper color. After-The iron nail turned copper when put into the solution. The copper got brighter

1. What was the anode in this electrochemical cell? Copper

2. Write an equation for the reaction that occurred at the anode. Cu: > Cu2+ + 2e-

3. What was the cathode in this cell? The nail

4. Write an equation for the reaction that occurred at the cathode. Fe2+ +2e- > Fe:

5. Does it matter what metal is used for the anode? Explain. Yes because the anode has to be the same as what you are coating with so when the solution runs out, the new source of what you are coating with is the anode.

6. Does it matter what metal is used for the cathode? Explain. Yes because you don't want to coat something with the same substance it already is. It would be a waste.

7. Do you think this method would be useful for large-scale copper plating? Why or why not? No, although it would coat correctly, it would take a lot of solution and something very big to put it in to do it on a large scale.


 * A.2 Separation by Distillation (42/42) **

1. Graph is on excel document. 2a. First distillate= 87 degrees c. Second distillate= 100 degrees c. 2b. It starts at the same time and the first "plateau" is flat for 5 five minutes so it is very consistant. The second distillate however, there isn't a clear plateau because after it starts to boil, the temperature continues to rise. 3. Propanol and Water. 4a. The mode for the first is 86, the mode for the second is 100 and 103. The mean for the water is 101.5, and the mean for the propanol is 85.75. the median for the first is 86 and the median for the second is 101.5. 4b. This is because the thermometers might have been off a couple degrees. Also each group might not have recorded exactly 30 seconds continuously. This could change the temperatures of each distillate and the times. 5. Iodine was more soluble in the propanol. This is because there was a bigger color change of the substance when iodine was added therefore the iodine mixed into it. Also because water is a polar molecule and iodine is not, the iodine will not dissolve in water very well. 6. You could take samples of the remaining liquid and mix substances into each one that you know how it should react ahead of time to both water and propanol and you can see if the color changes to what you were expecting. Also you could put water or propanol into a sample and if they don't react then it is just that substance and not a mix. 7. Propanol and Cyclohexane. This is because they have such close boiling points. They are only 1.7 degrees c. away from each other so if your thermometer is off you could get messed up. You could think you are boiling one of them but you're really boiling the other. 8a. It would be very similar to the original graph but instead of having 2 plateaus, there will be four plateaus. They would be around 82.4, 56.5, 100, and 80.7 degrees c. This is because while each substance is boiling, the temperature stays relatively the same. It then rises when the substance is done boiling. 8b. There will be four plateaus. They would be around 82.4, 56.5, 100, and 80.7 degrees c. My graph for this problem is on paper

1a. They are organized in alphabetical order and it has the boiling point for each substance. 1b. Yes it is because you don't have to know what the boiling point of the substance is that you are trying to find, you just have to use the name. 2a. You could organize it by boiling point from lowest boiling point to highest boiling point.
 * Building Skills 1 Hydro Carbon Boiling Points**

2b. Hydro Carbon / Boiling point (degrees C.) Methane -161.7 Ethane -88.6 Propane -42.1 Butane -0.5 Pentane 36.1 Hexane 68.7 Heptane 98.4 Octane 125.7 Nontane 150.8 Decane 174.0 3. Methane, Ethane, Propane, Butane 4. Pentane 5. Decane's molecules are much longer because it has a boiling point of 174 degrees c. where butane's boiling point is -0.5 degrees c. The higher the boiling point, the longer the molecule because there is more to boil and it takes more energy to separate the molecules.

Building Skills 3 p.191 1. As the number of branches increase, the boiling point will decrease a little as well. 1a.98.4 degrees c. 1b. 92 degrees c. 1c. 79.2 degrees c. 3a. It will have a lower boiling point than the first isomer, a lower boiling point than the one branch, and it will have a higher boiling point than the three branch isomer. 3b. It would be a much higher boiling point than both of the C5H12 isomers in figure 10. 4. The more carbon atoms in the isomer the higher the boiling point. The longer the parent chain is, the higher the boiling point is. This is because the parent chain has more bonds therefore the overall bond is greater which makes the isomer harder to boil.