Classification Test for Organic Halides

3. Carefully felt the sides of the test tube and observed the resulted chemical reaction for about 30 seconds.

The mixture was heated at 120°C using an aluminum block and was stirred gently. After all of the solid dissolved, it was heated for 20 additional minutes to ensure the reaction was complete.

The experiment can also be done to compare the burn rate of different colored candles.

Prior to conducting this lab, it was known that flame colors are produced from the electronic transitions in the metallic ions present in the salt compounds. When heated, the electrons absorb energy, jumping from ground states of lower energy to higher-energy, excited states. The electrons must return to their lower energy levels as energy is emitted in specific amounts in the form of light. Each energy emission correlates to a certain color, and since the transitions of metallic ions vary from each other, each ion produces a unique pattern of spectral lines, therefore creating an equally unique flame color.

Examine a piece of nichrome wire. On the data sheet, record the color and the luster of the metal. Use a forceps to hold the wire in the flame of your burner for about two minutes (recall where the hottest part of the flame is located). Describe the appearance of the wire while held in the hottest part of the flame. Allow the wire to cool and reexamine it. From your observations, determine if there was a physical or a chemical change. Give specific reasons for your conclusions. Save the nichrome wire for step #2.

Purpose: To use indicators to test for the presence of organic compounds in certain substances.

The reaction will be complete after approximately 60 seconds. Observe where color develops, and consider what these results indicate. Record your results in Table 1.

The SN1 mechanism leads to substitution products, and the E1 mechanism leads to formation of alkenes, therefore in this case, it is shown that this mechanism leads to a substitution of products since the Cl- ion is replacing the OH group by the addition of a strong acid (HCl). When the nucleophile

What Is The Unknown White Compound By Alexander Medina Lab Partners Maxwell Yurs, Eugene Floersch, Mesih Harri Abstract A white compound is found, but its identity is unknown.

Ethyl acetate is highly flammable so all nearby fire hazards should be avoided during the experiment. No naked flame should be near the source of acetate during experimentation and all gas taps must be shut off.

For the first part of this experiment, six dry test tubes were obtained and labeled accordingly to test the following halides: 2-chlorobutane, 2-bromobutane, 1-chlorobutane, 1-bromobutane, 2-chloro-2-methylpropane, and bromobenzene. To each of the six test tubes 2ml of 15% sodium iodide in acetone was added. 4 drops of the appropriate halide was added to the test tube labeled for that specific halide. After adding the halide, the test tube was then shaken to mix thoroughly. If a precipitate formed the time it took was recorded. Since none of the solutions formed a precipitate at room temperature after five minutes, the test tubes were placed inside of a hot bath at about 50°C. After one minute, the test tubes were taken out of the hot bath and allowed to cool. If any test tubes formed a precipitate, the time it took was recorded on a table.

However, based on the data obtained in Table 1, Figure 1 shows that all of the chemical substances formed a precipitate, while the tertiary substrate 2-chloro-2-methylpropane formed a precipitate the fastest. This makes sense because as a rule in SN1 reactions, the more stable the carbocation is the faster the reaction will occur. Also, SN1 reactions will prefer tertiary substrates to secondary substrates and secondary substrates to primary substrates. The next substrates to form a precipitate were 2-bromobutane followed by 1-bromobutane. However, it was expected that 2-chlorobutane would form a precipitate before 1-bromobutane because 2-chlorobutane is a secondary substrate, and therefore has a more stable carbocation. The reason that this occurred is because bromine is a better leaving group than chlorine, which allows it to bind easier with the silver ion. The reactions that formed the heaviest precipitate were 2-bromobutane, 1-bromobutane, and 2-chloro-2-methylpropane. This is because these reactions occurred at a faster rate and therefore, generated more of a product than 2-chlorobutane and 1-chlorobutane, which only formed a precipitate upon cooling from the warm water bath.

For instance, pentan-1-ol, the alcohol utilised to synthesis 1-pentyl ethanoate, is relatively flammable due to the hydroxyl functional group attached to the molecule. Therefore, in order to prevent severe burns, a laboratory coat and safety glasses were worn. The experiment was additionally performed whilst standing up, so that if the aliquot of pentan-1-ol ignited,

4) Try and propose a mechanism for the reaction using the orders of reaction taking into account the iodine, propanone and sulphuric acid.

An ice bath was prepared in a large beaker and a small cotton ball was obtained. 0.5 g of acetanilide, 0.9 g of NaBr, 3mL of ethanol and 2.5 mL acetic acid was measured and gathered into 50mL beakers. In a fume hood, the measured amounts of acetanilide, NaBr, ethanol and acetic acid were mixed in a 25mL Erlenmeyer flask with a stir bar. The flask was plugged with the cotton ball and placed in an ice bath on top of a stir plate. The stir feature was turned on a medium speed. 7mL of bleach was obtained and was slowly added to the stirring flask in the ice bath. Once all the bleach was added, stirring continued for another 2 minutes and then the flask was removed from the ice bath and left to warm up to room temperature. 0.8mL of saturated sodium thiosulfate solution and 0.5mL of NaOH solution were collected in small beakers. The two solutions were added to the flask at room temperature. The flask was gently stirred. Vacuum filtration was used to remove the crude product. The product was weighed and a melting point was taken. The crude product was placed into a clean 25mL Erlenmeyer flask. A large beaker with 50/50 ethanol/water