Voshel


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Parts of Earth Assignment
 * 1) The liquid of Iron and Nickel
 * 2) Crust
 * 3) Crust
 * 4) Plate tectonics theory
 * 5) Lithosphere
 * 6) Divergent Boundary
 * 7) Transform Boundary. The boundary of between the Pacific Plate and the Australian plate, crossing New Zealand.
 * 8) Oceanic crust tends to be denser and thinner than continental crust, so the denser oceanic crust gets bent and pulled under, or subducted, beneath the lighter and thicker continental crust.
 * 9) As plates made of oceanic crust pull apart, a crack in the ocean floor appears. Magma then oozes up from the mantle to fill in the space between the plates, forming a raised ridge called a mid-ocean ridge.
 * 10) A dropped zone where the plates are pulling apart. As the crust widens and thins, valleys form in and around the area, as do volcanoes, which may become increasingly active.

What are Minerals? 1)

It must occur naturally. It must be inorganic (little or no carbon) It must be a solid It must possess an orderly internal structure, that is, its atoms must be arranged in a definite pattern. It must have a definite chemical composition that may vary within specified limits."

2)Hardness, Optical properties, and crystal structure

 3)Calcite: CaCO 3 (Calcium, Carbon Oxide), Diopside: CaMgSi 2 O 6 (Calcium, Maganesium, Silicon, and Oxygen) , Gyrolite: NaCa 16 AlSi 24 O 60 (OH) 8.14 H 2 O (Sodium, Calcium, Aluminum, Silicon, (Oxygen Hydroxide), Hydrogen, and Oxygen (Water).

// Life Cycle of Copper/BS4 // //﻿//

1) Amount of useful ore at the site, percent of metal in the ore, type of mining and processing needed to extract the metal from it's ore, distance of the mine from metal refining facility and markets, and metal's supple-versus-demand status.

2)

- Mine the copper up - Melts down into a liquid copper

- Molding/casting - At this stage, the copper creates certain electrical/nonelectrical uses - Chemically processed to produce metallic copper, which makes a variety of materials - Copper becomes either discarded or remain in permanent use in today's society - Copper becomes recycled and starts the process over again

Building Skills 4

1) The malleability and ductility are high in regards of copper, with the thermal and electrical conductivity being high as well. The chemical reactivity is low, meaning that it won't melt in your pocket when it's warming up. Corrosion resistance is high since it won't rust away easily. Alloys are formed of the bronze, brass etc while the color is a reddish color with a lustrous form.

2)

a. If copper continues to be used over and over again, or if they continue to find more copper as they use them for electrical/nonelectrical purposes, **it will always be recycled to gain the copper back once again.**

b. There will be a limit because copper has always been recycling. That just means that it's **going to be fully permanent to houses or descarded.**

3) B.2 - Converting Copper Laboratory Before:  Crucible alone: 4.31g  lid alone: 3.68g  Crucible + lid: 7.99g  Copper powder mass before heating: 1.10g  Crucible + copper: 5.41g  Crucible + lid+ copper: 9.09g
 * Coins: We could use a new element that almost has the same properties as copper to replace copper as the main element for this coin. **(Credit Cards or debt cards)**
 * Communications: The phones are becoming more of cellphones since they don't need copper to create wires for a cellphone, unless it's a cord to give the cellphone more power, but other than that, they're changing the phones into cellphones.
 * Power Generation: Find a new source to replace copper that has the same properties as copper. I'm sure if they replace the copper, then the demands will lower. (**Solar panel (Silicon)**
 * Indoor electrical wiring: If a lot of things were to become wireless, then there would be a lot less copper use of wires in the house or anywhere else for that matter. (**Use aluminum since it's cheap)**

After:

Crucible + copper + lid: 9.10g Crucible + copper: 5.42g Copper mass alone: 1.11g

Observations: After two minutes, the copper turned into a gray color. After another two minutes, nothing has changed. Another two minutes have pass and nothing has changed. After two minutes, there was a slight red color to it, but not much. After two minutes, there was still the same changes from the last two minutes ago.

> b. The color changed from orange/red to a gray color and remained the same color throughout the ten minutes. > b. Yes, the copper atoms remained in the crucible since there was still remains of the copper left. The lid was tilted a bit to let the oxygen out, and if it weren't tilted, then perhaps it might've melted since the energy inside would transfer into the copper. That or the crucible would become really hot and break. > b. The heat was being added to the crucible as we waited for a change of the copper. After we place the crucible to the side with the help of the crucible tongs, the heat started to slowly go down. After placing the crucible on the balance, it went up slightly since the energy still remained there.(**The oxygen has mass and probably added onto the copper)**
 * 1) a. Chemical Change
 * 1) a. After about two minutes, the color changed into a gray color. Throughout most of the 10 minutes, it started to slightly stick together like glue and towards the end there was a red tint mixture of the gray copper.
 * 1) a. There was a slightly increase of the mass, however not by much since it only went up by 0.01g of the mass.
 * (Even though energy was necessary to speed up the reaction, it's important to remember that the molecules in the air were the only possible reactants with the copper for this reaction.) **

B.3 - Metal Reactivity


 * 1) Describe what happens to the penny when it is placed in the sliver nitrate solution.
 * 2) Describe how ions in solution play a role in chemical reactivity
 * 3) Explain, in detail, why this is happening,
 * 4) Define Oxidation.
 * 5) Define Reduction.
 * 6) Explain what happens to the copper atoms during the redox reaction.
 * 7) Explain what happens to the silver ions during the redox reaction.
 * 8) What ultimately controls chemical reactivity?

1) "When a solution of silver nitrate is added to the copper coin, the reflective coin surface immediately turns dark. Over time, shiny crystals form on the surface, and the solution turns a light blue. Underneath the crystals the rough coin surface shows that some copper metal has dissolved."

2) When there is less electron cloud in the metal structure, one copper (II) ion is pulled out by some water molecules. Meaning, once an electron has been added to an ion, it becomes an atom.

3) One copper (II) ion leaves for every two silver atoms that form on the surface. The silver atoms tend to build up on parts of the copper surface, and the copper (II) ions tend to leave from another part of the surface.

4) Oxidation: Any process in which one or more electrons can be considered as lost by a chemical species.

5) Reduction: Any process in which one or more electrons can be considered as gained by a chemical species.

6) A copper atom leaves it's two electrons in the metal structure, forming a copper (II) ion.

7) A silver ion gaining an electron from one of the copper atoms. Every two electrons lost by a copper atoms, two silver ions gain one electron each.

8) Valance Electrons

B.4 RELATIVE REACTIVITIES OF METALS


 * Metals || CuNO3 || AgNO3 || MgNO3 || ZnNO3 ||
 * Cu || N/A || Turned to a black color || N/A || N/A ||
 * Mg || Green color and it looked like it fizzed a little || Turned to a black color || N/A || **There was a fizz and there was bubbles around the metal.** ||
 * Zn || There is a green color of liquid and black substance on the bottom || Black color || N/A || N/A ||
 * Ag || N/A || N/A || N/A || N/A ||

1. Which metal reacted with the most solutions?


 * Magnesium

2. Which metal reacted with the fewest solutions?


 * Silver has the least reaction

3. With which of the solutions (if any) would you expect silver metal to react, if it were available to be tested?


 * There would be none **(Any element that would be less reactive to Silver)**

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 last (the one reacting with the fewest solutions).


 * Magnesium, Zinc, Copper, and 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.


 * Zinc is more reactive to acids rather than Copper. Zinc could also melt in your pants if heat/energy is being added when being in close contact of your pockets.

6. a. 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 would be a better choice because there wasn't a reaction to any of the solutions (or what's shown on the data table). Silver is also implied onto other coins and they have not melted off if it's being left in your pocket. Silver would be non reactive to acid as it says so on the table from above.

b. Why do you think that metal is not used for that purpose?


 * Silver is used for other coins and it would create a confusion for the other coins since the American's are use to seeing a brown/orange penny. **(It's expensive)**

7. Given your new knowledge about the relative chemical activities of these four metals, a. which metal is most likely to be found in an uncombined, or �free,� (metallic) state in nature?


 * Silver

b. which metal is least likely to be found chemically uncombined with other elements?


 * Magnesium

8. Reconsider your experimental design for this activity.

a. 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

b. If so, which combination(s) could have been eliminated? Why?


 * The same solutions that match the metals since they won't react at all because they are the same.

**Activity Series of Metals Assignment** (Oxidation/Reduction Part I)
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).

1) The cloud that was around the Magnesium atom has decreased and vanished without being seen. The size decreased to say the least.

2) As to Magnesium, the Zinc is the same since it decreased as well since the cloud around the blue ball disappeared.

3) The surrounding red plus white objects disappear from view and a blue ball comes flying down (Zinc). As soon as it appears beside the left side of the green ball with the surrounding green area, it shifts onto the blue ball which created a blue cloud around it and the second right green ball did the same to the left green ball. The green ball without the cloud surrounding it floats up.

4) When the green ball (Mg) came down towards the blue balls (Zn), there was no reaction at all. It remained still for a while before it floats right back up into the air.

Reactions of the (?):

Mg+2 (Cu): No reaction at all. Zn+2 (Cu): No reaction. Cu+2 (Mg): Reaction. When Cu+2 migrate to the surface of magnesium metal they gain two electrons each becoming two Cu atoms. Cu+2 (Zn): Reaction: When Cu+2 migrate to the surface of Zinc metal, they gain two electrons each to become Cu atoms.

Page 3 answer:

Mg+2 (Ag): No Reaction Zn+2 (Ag): No Reaction Ag+ (Mg): Reaction (Turned to a black color) Ag+ (Zn): Reaction (Turned to a black color)


 * Activity Series of Metals**

Mg Zn Cu Ag

ChemQuandry 1
They all largely non-reactive metals that exist widely in their free state in nature. The ancients that discovered these metals did not yet have the chemical know-how to separate other more-reactive metals from their compounds, so they only metals they knew about were the ones they could find in their uncombined state.
 * Answer:** Gold, silver, and copper, are among a few that appear as native elemental metals. Most others have combined with other elements.

Building Skills 5
1) a. When it goes from left to right, on Figure 16, it shows that from the highest reactive metal decreases as is continues to go to the right on the periodic table. b. The left side of the periodic table where the metals are **(Alkani-Metal)** c. The right side of the periodic table where the nonmetals are **(Transition Metals)**

2) a. The Iron will react with the lead Nitrate. b. No c. For 2a, Iron will react with lead Nitrate because the iron electrons will transfer onto lead Nitrate, creating a reaction. For 2b, the lead Nitrate is more reactive then that of plantium.

3) a. No they are not the cheapest because since they don't really react, it would cost a lot to make certain properties (such as penny) and make sure that they don't melt or anything that involves some kind of acid that would melt. b. Factors would be heat (if it would melt), acid that will react to the metal, how malleable they would be, and so on. **(Supply and Demand)**


 * Modeling Matter Questions**

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

2) Oxidation: Loss of one or more electrons Reduction: Gain of one or more electrons Zinc was the oxidation since it lost two electrons, while Silver gain an electron which is reduction.

3) a. Copper was oxidated since it lost two electrons b. Silver was reduced since it gained two electrons

4) To keep the equation balance, the copper must lose two electrons and for the Silver ions to replace the lost electrons. To put the copper electrons onto each Silver.

5) a. Copper is the one who has to be the reducing agent. b. The atom that gives away it's electrons during the reaction

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

7) a. Zinc is the oxidation since it lost two electrons. b. Copper is reduced since it gained two electrons

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

9) You could look at the reactions to see if it was less or more reactive to solutions, since if it's more reactive the atom would lose it's electrons and become an ion. The +2 that transfers to another ion and the (s) & (aq)

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


 * ~  || First Sample || Second Sample ||
 * Filter Paper Weight (in grams) || 0.70 g || 0.69g ||
 * Filter Paper Weight with Copper after (in grams) || 1.80g || 1.61g ||
 * Total Copper Recovered (in grams) || 1.10g || .92g ||

Observations: Nothing happened when adding the HCl to the beaker with the copper (II) oxide. When heating the beaker, the copper oxide is turning red because the more reactive hydrochloric acid is reducing the copper oxide. Overnight when we have 8 minutes left of heating it, the solution turned to a teal color.

Zinc Reaction: After covering it with the dish, the zinc metal started to bubble. Some of the metal particles are coming up to the surface and away from the metal that are clinging to the metal. It's rapidly reacting to the solution and bubbling extremely. The zinc metals are covered with black substance of the solution. The dish glass has water molecules in the middle (condensation). Over night, the zinc reaction turned to a orange color and looked rusted. Also, it almost looks like copper.

Questions from Lab:

1) a. There was only a single element and if it's by itself, then it wouldn't react strong enough to the air. Petite is involved since it was covering the copper and the inside of the black substance is still copper. b. Perhaps you can add another substance to the copper to form a better copper oxide(II). Clean the copper metal with steal wool with enough force to make sure it's petite surrounding the copper will be away.

2) a. 1.1 grams b. There was no percentage since there was zero grams in our group.

3) a. Cu + CuCl2 --> Cu2+ + Cl Zn(s): + Cu+2(aq) > Zn+2(aq) + Cu:(s) bi. Cu Zn bii. Cl Cu+2 biii. Chloride Zinc biiii. Zinc Cu+2

4) a. Once we put the zinc in the HCl where Copper was reacted to, the zinc metal started to bubble immediately. Over night, however, it stopped bubbling, but the color on the zinc was orange. The same color as copper.

b. Due to the chemical reaction of the solution, it changed the color of the zinc metal. (C)

c. The zinc metal had drawn the Cu+2 ions from the solution, as if it was a sponge of sorts. When adding the zinc(since it's more reactive), it was still blue. However, overnight the solution wasn't blue anymore, but a clear solution.

5) a. I am unsure of what resources that we used that may have been dispensed. (Zinc and acid) b. Same as above. (ZInc went into the solution and the acid went into the air, as the bubbles)

Reading Questionaire

1) Some resources such as fresh water, air, fertile soil, plants, and animals can eventually be replenished by natural processes. These resources are called renewable resources. Other materials such as metals, natural gas, coal, and petroleum are considered nonrenewable resources because they cannot be readily replenished.

2) a. Atoms are conserved in chemical processes, but molecules might not be. For example, the current production of new petroleum molecules in nature is very much slower than the current rate at which petroleum molecules are being burned to produce carbon dioxide, water, and other molecules. Thus the total inventory of petroleum on Earth is declining. b. Resources can run out since there might not be anymore minerals whenever we continue to mine from the bottom of the mines. There is also the possibility of water running out and the sea is where we cannot get the water from since if we indulge too much salt, then we will die.

3) Profitable mining depends on finding an ore with at least some minimum metal content. This minimum level depends on the metal and its ore: from as low as 1% for copper or 0.001% for gold to as high as 30% for aluminum.

4) One strategy for conservation is to slow down the rate at which the resources are used. Part of this strategy includes rethinking personal and societal habits and practices involving resource use. Such rethinking can involve decisions such as whether it is better to use paper or plastic bags in grocery stores, as well as whether, as is done in some parts of the world, it is even better to encourage customers to bring their own reusable bags. Another approach is to replace a resource by finding substitute materials with similar properties, preferably materials from renewable resources. In addition, some manufactured items can be refurbished or repaired for reuse rather than sent to a landfill.

5) However, even the recycling process can create environmental problems. For example, aluminum scrap, excluding cans, may contain up to one percent magnesium. The magnesium must be removed before the aluminum is processed into other products. Conventional removal of magnesium requires the addition of chlorine gas, which requires special handling in the workplace and can contribute to air pollution.

6) Each person in this country throws away an average of about 2 kg (4 lb) of unwanted materials (or waste) daily.

7) Some products, such as yesterdays newspaper, become waste after they fulfill their initial purpose. Others, such as telephones and computers, become waste when they are discarded for newer models. Combined, materials directly discarded by U.S. citizens would fill the New Orleans Superdome from floor to ceiling twice each day.

8) A high proportion of combustibles in the waste stream, waste-to-energy plants have become an attractive option. More than 120 waste-to-energy plants currently operate in the United States, burning about 97 000 tons of solid waste per day. Each ton of garbage that serves as fuel in these plants produces about a third of the energy released by a similar quantity of coal.

9) Recycling, landfilling, and combustion for energy production are three options for the final step in the life cycle of a material.

10) Paper; the weight is 83.3 million ton. Percent of waste is 38.6%.

11) Wood; the weight is 11.6 million ton.

12) 11.6 waste before recycling - 11 waste after recycling = .6 million tons

13) 156.3 million tons/217 million tons X 100% = 72.0% Wasted 100% - 72% = 28%


 * Building Skills 11 **

1)

Each carbon-carbon linkage in diamond is a covalent bond involving the sharing of a pair of electrons. Thus “bending” or “denting” a diamond crystal would be extremely difficult because it would involve breaking a network of strong chemical bonds that locks each carbon atom in a fixed position.

2)

The diamond has a melting point that is the highest of any element. Both natural and synthetic diamonds exist. Also, the diamond contains a pure carbon where it is not recommended to use it as a heating fuel. (The bonds are hard to break and they are repeating pattern in which that makes it's structure.)

3)

Graphite has a pure carbon, where it can burn in oxygen to produce carbon dioxide gas and thermal energy. (Has layers of bonds that have rubbed off easily)

4)

The particular fullerene described here is buckminsterfullerene, a 60-carbon hollow sphere (C60), which resembles a soccer ball. Other fullerene molecules with formulas such as C70, C240, and C540 are known, as are structures composed of “rolled up” layers of carbon atoms in the form of hollow tubes termed nanotubes. (Due to the fact that they are spheres, they cannot connect with each and roll away from each others)

5)

Use in the medicine as capsules (pills) and pain killers. Use this material inside of the blood stream to use as a painkiller. Use this material to identify the cancer cells or destroy them.


 * ~ Condition ||~ Appearances ||
 * Untreated Penny || Copper color shiny ||
 * Penny with Zn & ZnCl2 || Silver ||
 * Penny treated with burner with Zn and ZnCl2 || The flame was green, the penny turned gold, then orange and got burnt ||
 * Penny treated on hot plate with Zn and ZnCl2 || Turn gold color ||


 * I redid the table to make it my table rather than Morgan's table.**


 * Lab Questions from Lab**

1)

a. The control was just a regular shiny copper penny that we see everyday in the society. The penny treated with Zn and ZnCl2 turned to a silver color. The penny treated with Zn and ZnCl2 while being putting under a flame turned into a gold color, before orange and then got burned. The last penny treated that has Zn and ZnCl2 was heated onto a hot plate and the color changed into a gold color.

b. Yes, the pennies that we have tested in this lab contain Copper and Zinc, which makes the two metals together likes a mixture. (But don't they "look" like "silver" and "gold"?) -1

2)

If they claim that a precious metal was produced, than we would have to see if the metal reacts to anything, the color (depending on what kind of precious metal it is), and to see if it contains the same properties as a precious metal. (What about the Law of Conservation of Matter?) -2

3)

The metals would be used for pipes and buildings that contain the metals. (Pipes I can see but buildings? Not sure what you mean there?) -1

4)

a. The Copper atoms were covered with Zinc due to the fact that the copper pennies were put into the ZnCl2 solution and reacted.

b. Take the Zn covered pennies that were tested in the labs and melt them down completely. If we do this, we can mold the pennies back to normal. (Why not just scratch the coating off or use acid like we did in the Retrieving Copper lab?) -2


 * Copper Plating Lab**

Observations: After setting up the procedure and putting the iron nail and copper plate into the acid, we saw that the nail started to change into a copper color from the bottom up from the gray color. The copper plate doesn't change at all. The copper coated the iron nail like paint. After a little bit of time has passed, the copper plate turned brighter than before as if being coated once again. More time has passed by and the Iron nail with the coating copper has started to fall off starting at the bottom.

Questions:

1) Copper Plate

2) Cu: ---> Cu2+ + 2e-

3) The Iron Nail

4) Fe2+ + 2e- ---> Fe:

5) Yes, because the copper connects to the positive battery and if it were to be an iron, it would create a shock since the iron nail has electrons while the positive contains protons.

6) Yes, because the iron nail is a a main source of the negative (electrons) that is connected to the battery. If it were to be on the copper plate, it would not work if it was the main source of the electrons.

7) If we were to use a bigger large-scale copper, it would require more solution to create a coating. Also, the electrons that are being pushed off of the iron nail would require a bigger nail to make the copper ions into a neutral copper atoms.


 * A.2 Separation by Distillation**

1) Excel has the graph

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 consistent. The second distillation isn't as consistent since the temperature continues to increase every couple of minutes(30 seconds) or so.

3. Water and Propanol

4a.

Mode a: 86 Mode b: 100 and 103

Mean for water: 101.5 Mean for Propanol: 85.75

Median a: 86 Median b: 101.5

4b.

Not everyone is the same since the starting point of the time could have been different in each lab group. The thermometers could also have been off by a couple of degree's.

5.

Since water is a polar molecule and Iodine is not, they will not mix very well when Iodine is added into the water. However, Iodine does mix very well with Propanol since there was a color change, thus making it more soluble.

6.

You can take two of the samples that we gathered and use a match to see if the fire would react with the samples or not. Like for water, it'll go out immediately. However, if it's with propanol, then it will probably light up since it's alcohol.

7.

Cyclohexane and propanol because they have such close boiling points. If you were to do the same lab procedures with these two substances and use a thermometer, you would have to be careful because if you were to screw up, you wouldn't know which substance is which since they're almost the same in terms of boiling points.

8a.

The making of the graph would be similar, however there would be four plateaus instead of two. They would be around 82.4, 56.5, 100, and 80.7 degrees c. While each substance is boiling, the temperature will be the same making it consistent.

8b. The graph for this problem is on a sheet of paper.


 * Building Skills 1 (Hydro Carbon Boiling Points)**

1a.

They are in alphabetical order while having boiling points for each substance.

1b.

I would think so because instead of trying to find the boiling point of a substance, you can just look at the name since they will contain the information you are looking for.

2a.

Instead of laying the table in alphabetical order, you can just arrange the data from greatest to least or least to greatest.

2b.

Hydro Carbon / Boiling point (degrees C.)

Decane 174.0 Nontane 150.8 Octane 125.7 Heptane 98.4 Hexane 68.7 Pentane 36.1 Butane -0.5 Propane -42.1 Ethane -88.6 Methane -161.7

3. Ethane, Butane, Propane, Methane

4. Pentane

5.

Compared to Butane, Decane has larger molecules than Butane due to it's boiling point being a lot higher. Decane has 174.0 degrees C while butane has a -0.5 degrees C. The higher the boiling point, the larger the molecules since it takes more energy to separate the molecules.