Carolina Wasinger
Chemistry I
Ms. Bowser
11/17/2015

Pre-lab

Purpose:

To create different smells within a lab experiment. 

Procedure:

1. Fill 50 mL beaker with 30 mL of water. 
2. Drop into the beaker, a boiling stone. 
3. Put the beaker on a hot plate and bring water to a boil.
4. Label test tubes with the following numbers: 1, 2 and 3
5. Using the wafting technique, smell the acids and record in a data table. Add 5 drops of the respective carboxylic acids to each of the test tubes. 
6. Again, using the wafting technique, smell the alcohols and record in the data table. Add ten drops of each alcohol to to each tube (look in the following table). 

Test tube:             Carboxylic Acid                Alcohol

1                             acetic acid                       isopentanol

2                             acetic acid                       butanol

3                             butyric acid                     ethanol

1. Add 1 drop of the sulfiric acid (H2SO4) to each test tube.
2. Place a boiling stone into each test tube. 
3. Carefully smell each compound by using the wafting technique. 
4. Slice a plastic pipette to a length that is shorter than that of the test tube. Put the pipette into the test tube so that the bulb somewhat seals off the test tube. 
5. Put the test tubes into boiling water n heat for 5 minutes, or until the compund no longer smells putrid. 
6. After, remove the test  tubes from the water and turn off the hot plate. 
7. Take the pipette out from the test tube. There should only be vapors in it. 
8. squeeze the pipette and waft the vapors, Record the smell on the data sheet.
9. Dispose properly of chemicals. 

Materials:

• 50 mL beaker
• Hot plate. 
• 3 microscale test tubes. 
• Boiling stones. 
• 3 plastic pipettes. 
• scissors 
• pencil 
• organic acids and alcohols ( Acetic Acid, Butyric Acid, concentrated Sulfiic acid, Ethanol, Isopentanol, Butanol.)

Safety:

Hot Plate; Hot plate can burn. Do not  directly touch the heated surface of the hot plate and use tongs to move items on and off the hot plate. 

Boiling Stones: Be sure to handle with tongs. Boiling stones can cause burns. 

Acetic Acid, can be erosive to the skin. Keep out of eyes and off skin and clothing. 

Butyric Acid, Is corrosive to skin, combustible and flammable. Keep away from open flames. 

Sulfiric Acid. Is corrosive to skin and can cause burns to skin. 

Ehanol: 

Carolina Wasinger
Ms. Bowser
11/2/2015

The Conductor has lost his train of thought...

Procedure:

• Test the conductivity of each of the substances when dry. 
• After that, put each of the substances in water and observe whether or not the substance dissolves. 
• If the substance dissolved in the water, test whether or not the water is conducting electricity. 

Materials:

-Conductivity tester. 

-Beakers to hold distilled water. 

-Distilled water. 

-Aluminum Foil. 

-Sucrose (sugar). 

-Sodium chloride (salt). 

-Silicon Dioxide (sand). 

-Paraffin (wax). 

-Ethanol. 

-Copper.

-Calcium Chloride. 

-Copper (II) Sulfate. 

Background:

   

             Whether or not an element conducts electricity is largely dependent on the type of bonding the atoms make with each-other. For instance, Network Convalent bonds tend to be extremely strong and very hard to break, The toughness of a diamond comes from this type of bond. 

             An Ionic bond is when the metal valence electrons move to the nonmetal atoms atoms. Molecular Covalent bonds occur when some atoms but not all share valence electrons. Metallic bonds occur when  the valence electrons are free to move throughout the substance

Hypothesis:

Substance:                            Conduct? Yes/No                       Dissolve? Yes/No

-Distilled water.                    No                                                Yes

-Aluminum Foil.                   Yes                                                No

-Sucrose (sugar).                    No                                                Yes

-Sodium chloride (salt).         No                                                Yes

-Silicon Dioxide (sand).        No                                                 No

-Paraffin (wax).                     No                                                 No

-Ethanol.                                No                                                 No

-Copper.                                Yes                                                 No

-Calcium Chloride.               No                                                  Yes

-Copper (II) Sulfate.             Yes                                                No


Actual Data:


Substance:                        Conduct? Yes/No             Dissolve? Yes/No           Conduct when Dissolved

-Distilled water.                    No                                          Yes                               No

-Aluminum Foil.                   Yes                                         No                                N/A

-Sucrose (sugar).                    No                                         Yes                               No

-Sodium chloride (salt).         No                                          Yes                              Yes

-Silicon Dioxide (sand).        No                                           No                               N/A

-Paraffin (wax).                     No                                            No                               N/A

-Ethanol.                                No                                           Yes                              No

-Copper.                                Yes                                           No                              N/A

-Calcium Chloride.               No                                            Yes                             Yes

-Copper (II) Sulfate.             Yes                                           Yes                              Yes

Analysis. 

For the experiment, the class used a conductivity tester to see whether of not a substance could be a conductor. If so, the class tested if the substance could dissolve in water. If the substance could dissolve in water, the class tested the substances' ability to conduct in water. 

5.) The substances that could light up the bulb were metals, copper, aluminium Both these substances were conductors. 

6.) The substances that did not light up the bulbs were not pure metals. 

The types of bonding predicted for each substance:

Ionic - Sodium Chloride, Copper (II) Sulfate, Calcium Chloride. 

Molecular Covalent-Water, Ethanol. 

Metallic-Aluminum and Copper. 

Network Covalent- Sucrose, Paraffin, Silicon Dioxide. 

The only substances that conducted electricity were in either the Ionic group or the Metallic group. The substances had to have contained metals in order to conduct. 

Discussion:

There were a few instances were the results of our group were different from those of other groups. This was largely due to (we suppose) the condition the conductivity testers were in. The Substances chosen to test would have to be carefully picked because if not, us students could possibly get electrocuted.

Conclusion:

For this lab, my hypotheses were mostly right.  I was wrong in some cases though: I did not predict that Ethanol would dissolve. I did not correctly predict that Copper (II) Sulfate would dissolve. The reasons for my incorrect decisions is mostly due to that I did not know what either of the substances were and I could therefore, not make a reasonable prediction. 

Questions:

1.) 

• Glass Water Bottle- Network Covalent. 
• Plastic binder-Network Covalent. 
• Metal Lamp-Metallic. 
• Thumb-tacks- Mettallic. 
• Orange Juice-Molecular Covalent. 
• Water-Molecular Covalent. 
• Salt- Ionic
• -Ionic 

2.) 

1. Copper Jewelry- Metallic. 
2. Glass Jewelry-Network Covalent. 
3. Jewelry made from rocks -Molecular Covalent. 
4. It is impossible to make jewelry from an Ionic compound because it would dissolve in water and be very brittle. 

Works Cited:

You Light Up My Life. Classifying Substances. Lesson 25 lab Packet. Handed out by; Lindsey Bowser. October 26th, 2015  Chemistry I. Period A. Foxcroft School.