STRIKING IT RICH LAB
July 22, 2013
Abby, Jilly, Layla
Chemistry
Dr. Forman
b. Yes, the zinc coin looks like silver.2. I would say that the precious metal would be too expensive and rare to use in coins.3. The two uses would be telling temperature or in jewelry.4. a. The copper atoms changed their arrangement causing the color to change.
b. I don't think that the pennies could be converted back to ordinary coins.
RETRIEVING COPPER
July 19, 2013
Abby, Jilly, Layla
Chemistry
Dr. Forman
1. a. The
observational evidence was that the copper was all black but it was the oxygen
atoms surrounding the copper atoms.
b. We would
revise it by letting it heat for a longer time.
2. a. 1.07 grams of
copper reacted when heated.
b. 50% was
unconverted.
3. a. Zn: + Cu^2+
→ Zn^2+ + Cu:
ii. Cu was
reduced.
iii. Zn is the
reducing agent.
iv. Cu is the
oxidizing agent
4. a. The
color of the solution cleared and the zinc became dark red in color, and began
to break apart.
b. This is
because since zinc is more reactive than copper, the zinc caused copper to
reduce as it oxidized in the solution.
5. a. Although
the law of conservation of matter states that matter can neither be created or
destroyed, Cu^2+ ions and solid Zn were “used up” in this recovery process.
b. Cu^2+ reduced
into solid Cu and Zn was oxidized into Zn^2+ ions within the solution.
REACTIVITIES OF METALS LAB
MINI REPORT
July 16, 2013
Abby, Jilly, Layla
Chemistry
Dr. Forman
Chart:
Lab Questions #1-8 (pg. 143)
1. Magnesium
2. Copper
3. I would think that silver nitrate would react with all of the elements since it is less reactive than all elements.
4. Magnesium, Zinc, Copper, Silver
5. Copper is less reactive than zinc.
6. a. Silver might be a better choice since it is the least reactive element.
b. Silver is too expensive and hard to find
7. a. Copper
b. Zinc
8. a. Yes
b. Magnesium and zinc nitrate could've been eliminated since they didn't react with any of the elements.
METAL LAB REPORT
BERYLLIUM
July 15, 2013
Abby, Jilly, Layla
Chemistry
Dr. Forman
1. Beryllium is produced by extraction from beryl, however it is very difficult to extract since beryllium has a high attraction to oxygen. It is prepared by reducing beryllium fluoride with magnesium metal. Beryllium has many uses including springs, materials in crafting space shuttles, x-rays, computer parts, as well as others. It was discovered in 1798 by a man named Louis Nicholas Vauquelin from France.
2. Beryllium has a melting point of 1287+/-5°C, boiling point of 2970°C, specific gravity of 1.848 (20°C), and valence of 2. The metal is steel-gray in color, very light, with one of the highest melting points of the light metals. Its modulus of elasticity is a third higher than that of steel. Beryllium has high thermal conductivity, is nonmagnetic, and resists attack by concentrated nitric acid. Beryllium resists oxidation in air at ordinary temperatures. The metal has a high permeability to x-radiation. When bombarded by alpha particles, it yields neutrons in the ratio of approximately 30 million neutrons per million alpha particles. Beryllium and its compounds are extremely toxic.
3. Beryllium has good properties for uses like springs and materials used in spacecrafts since it has a high resistance to corrosion and doesn't usually react with many elements. Beryllium is very chemically similar to aluminum but not as similar to other elements so aluminum would be the best replacement if one was ever needed.
4. Beryllium is the most abundant in the United States, China, Mozambique, and Kazakhstan. It is usually found in up to 30 mineral species so the production needs are met for it's uses.
CONVERTING COPPER LAB
MINI REPORT
July 12, 2013
Abby, Jilly, Layla
Chemistry
Dr. Forman
Chart:
Lab Questions #1-4 (pg. 45)
1. a. The copper turned from a reddish gold to dark gray then black. The copper also become a solid but we were able to separate the particles by using a spatula.
b. Yes, the copper atoms remained in the crucible and we could tell since we kept the cap on during almost the entire procedure.
2. a. Physical changes
b. We said that we saw physical changes because we noticed changes in the texture and color of the copper.
3. a. There was more copper after we finished the lab procedure.
b. The amount of copper changed because it was oxidized. Since oxygen atoms weigh more the copper molecules, it caused the copper to weigh more and also caused the formation of copper oxide.
METAL OR NONMETAL LAB
July 9, 2013
Abby, Jilly, Layla
Chemistry
Dr. Forman
Abstract:
In this lab, the goal was to figure out if the elements given to us were metals, nonmetals, or metalloids. This lab was really interesting because we saw how some elements react to different liquids and how quickly some react, if they do. To figure out if an element given was a metal we typically looked at patterns in its appearance, durability (crushing test), and conductivity. If an element was a nonmetal, we looked to see whether the element reacted, if it was an insulator, and if it shattered when it was hit with a hammer. If the element was recorded as a metalloid, we noticed that it had properties of both the metals and nonmetals.
Procedure:
1. The first thing we did was make a chart for the elements and we would write down each element's appearance, conductivity, durability, HCl reactivity, and CuCl2 reactivity. Then after the lab, we thought about the results and decided which elements were metals, nonmetals, or metalloids.
2. We then recorded the appearance of the element and tested it's conductibility. We clipped each element to the electrodes of an electrical conductivity apparatus. If the light lit up, the element was a conductor. If the light didn't light up, the element was a nonconductor. We then recorded the data onto the chart.
3. The next step was to test the elements for durability and see if they would shatter when hit with a hammer. If the element was bendable and didn't shatter, it was malleable. If the element shattered, it was brittle.
4. Next, we placed all the sample elements in a well plate and poured Copper (II) Chloride in each well. After 5 minutes, we looked at how each sample reacted to the liquid and recorded it on our chart. We then got a new plate and did the same step except this time we added Hydrochloric acid and watched and recorded the results. (The Copper (II) Chloride is the blue liquid and the Hydrochloric acid is the clear liquid.)
Results:
We noticed that a lot more of the elements reacted to the Copper (II) Chloride than they did to the Hydrochloric acid, which we found interesting since the Hydrochloric acid is very dangerous. In the end, Elements A, C, and G were the only ones that reacted to the Copper (II) Chloride. (Element A rusted, Element C reacted right away and turned red, and Element G also reacted right away but turned black.) When the Hydrochloric acid was added only Element G reacted. It automatically began sizzling once the liquid was added. We concluded that all the elements that conducted electricity were metals, as well as the ones that reacted when the liquids were added into the wells.
1. Appearance - physical
Conductivity - chemical
Crushing - physical
Reactivity to CuCl2 - chemical
Reactivity to HCl - chemical
2. Chemical - A, C, G
Physical - B, D, E, F
3. Elements B and D could fit into the chemical properties group because they both conducted electricity.
4.
SOLUBILITY CURVE LAB
July 1, 2013
Abby, Jilly, Layla
Chemistry
Dr. Forman
Abstract:
This lab was to figure out the solubility of succinic acid and make a graph of the height of the crystals compared to the temperature of the water. It was really interesting to see how the crystals were formed and how they reacted at different temperatures. We noticed that as the temperature rose in the hot water bath, the acid dissolved more and more into the water. However, when the liquid was put in the cold water, even if it looked like there was no more substance in the water, even more crystals were there.
Procedure:
1. First, we warmed up some water in a beaker to 45 degrees C. At the same time, another person in the lab group got the succinic acid and added distilled water to it.
2. We then placed the test tubes in the hot water, mixing it with a stirring rod every 30 seconds for 7 minutes. Unfortunately, a test tube was shattered while we were mixing the solution so we skipped the data for 45 degrees and used the lab group Lithium's information.
3. After 7 minutes, we poured out the liquid into another test tube without getting any of the succinic acid into it and put the liquid into a cold-water bath for 2 minutes.
4. After 2 minutes we would stir the mixture a couple times to get the crystals to settle and measure the height of the crystals.
5. We then repeated this process for the temperatures of 55 and 65 degrees C and made a solubility curve measuring the height and temperature of the crystals.
Procedure:
1. First, we warmed up some water in a beaker to 45 degrees C. At the same time, another person in the lab group got the succinic acid and added distilled water to it.
4. After 2 minutes we would stir the mixture a couple times to get the crystals to settle and measure the height of the crystals.
5. We then repeated this process for the temperatures of 55 and 65 degrees C and made a solubility curve measuring the height and temperature of the crystals.
Results:
Since our 45 degree C experiment had a little setback and we ended up using data from another group, we don't have results for it. However, in the 55 and 65 degrees C tests, the crystals looked solid before settling so when we mixed the test tubes after being in a cold-water bath, we were surprised to see that the mixture was actually mushy like snow. Before mixing the liquid, we noticed the crystals were suspended in the liquid. In the 65 degree test, the crystals clumped together and dissolved into the liquid when they were in the hot bath. However, after being in the cold water, there was more crystals than the 55 degree test.
WATER TESTING LAB
June 25, 2013
Abby, Jilly, Layla
Chemistry
Dr. Forman
Abstract:
Throughout the process of testing the water to see what ions were in the solution, my group stayed focused and worked through any problems we had. There were four tests that we had to do: Calcium Ion Test, Iron Ion Test, Chloride Ion Test, and Sulfate Ion Test. The reference solution would always be cloudy to compare other solutions to and the distillation solution would always have a clear appearance to compare the other solutions to, as well. In the end, we noticed that a lot of the mixtures didn't look any different from what they looked like when we started. This shows that even though we put in another chemical, some of the substances dissolved into the mixture making it have a clear appearance although something was put in them.
Procedure:
For each test, we added 20 drops of distilled water, the reference solution, an unknown solution (control), tap water, and ocean water into a well plate. Then, into each of those liquids we added approximately 3 drops of sodium carbonate (Calcium test), potassium thiocyanate (Iron test), silver nitrate (Chloride test), and barium chloride (Sulfate test). Then we wrote down how the liquid changes (if it did). For every time the liquid changed, we said for each ion test, the ion was present.
Results:
1. Calcium Ion Test
- After adding sodium carbonate, the reference solution was the only mixture that had a cloudy appearance. However, the ocean water at the end turned slightly cloudy.
2. Iron Ion Test
- After adding potassium thiocyanate, the reference solution was the only mixture that changed greatly. At first, it was a yellow color but after adding potassium thiocyanate, the reference solution turned a very dark red.
3. Chloride Ion Test
- After adding silver nitrate, the control/unknown mixture was the only one that didn't change. All the other results became cloudy and the natural water (ocean) became a little chunky.
4. Sulfate Ion Test
- After adding barium chloride, the tap water was the only one that didn't change. In the reference solution, there was a light color before adding barium chloride but once it was added, it had a cloudy yellow appearance.
Lab Questions #1-4 (pg. 45)
1. A reference solution was used to compare it to other solutions. A reference solution would always have a reaction. A black solution was used to for comparison as well however there would never be a reaction.
2. Some problems that could be associated with qualitative tests are that there could be residue left over from the previous experiment which would change the chemical reaction.
3. Qualitative tests cannot always confirm the absence of an ion because sometimes the quality is changed by accidental addition of other chemicals.
4. If we didn't clean our wells and rods, the chemical reaction of the solutions would be different.
PURIFYING FOUL WATER
June 18, 2013
Abby, Jilly, Layla
Chemistry
Dr. Forman
Abstract
Purifying the foul water was a long process but simple to follow. There are 3 main steps: oil-water separation, sand filtration, and charcoal adsorption and filtration. Using these steps, substances that gave the water a bad small, an ugly color, and a rotten taste were removed, making the water clear, without an odor, although still not drinkable. In the end, the water came out as clear, no strong odor, as well as no visible substances, like oil and sand, as there was to begin with, proving our foul water lab successful!
Procedure
1. Oil-Water Separation
- Using a pipe, we removed as much of the top layer of oil as we could
- We put the oil in a test tube adding drops of distilled water seeing if the water would sink or float
~ The water ended up sinking bringing the oil to the top
2. Sand Filtration
- First, we poked holes in a cup to add moistened gravel/sand to get rid of solids in the water
- The foul water then was filtered into a beaker having a yellowish color rather than brown
3. Charcoal Adsorption and Filtration
- The first thing to do in this step is fold a piece of filter paper in a funnel and moisten it
- We then poured the foul water into the charcoal in a flask and swirled it until it seemed mixed
- After pouring the water/charcoal mix into the funnel, clear water came out the other end
~ Moistening the paper and adding charcoal will adsorb any substances making the water bad
Results
In the beginning, the water was brown and had a very strong, unpleasant odor. Using the filtration process created clear and more pure water. Once the negative substances were removed, the water become less dirty and odorless. However, as a result, approximately 23 milliliters of water was lost throughout the filtration process. Luckily, the lab was successful and our group ended up having clear water, the main goal of this experiment. Doing this lab, my group realized the tedious work of filtering water and how long the task can take. We also discovered that water is lost during the filtration process, making it harder to have a greater amount of water. We also found out that the water that we filtered was not 100% pure (no water can be 100% pure). Even though the water may not look dirty, there are still small particles of salt in the water since the salt can't be removed by the Foul Water Lab. Because of the salt leftover in the foul water, the final product is able to create electrical conductivity, unlike the distilled water where the salt was removed by boiling the water. There is also a wide variation of results of the percent of water left over from the final product. There are these different results because some groups may have removed more or less of the substances in the foul water.
good report!
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