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CHEM101 Study Guide - Final Guide: Copper(Ii) Sulfate, Bunsen Burner, Incandescent Light Bulb

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24 Nov 2016

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CHEM101 Full Course Notes

CHEM101 Full Course Notes

Document Summary

Flame test- identifies the presence of certain elements by observing their flame colour. A spectrophotometer is used to measure the absorbance of a certain colour. Larger a value means that more of the incident light was absorbed. Plot of a against the wavelength of the light is the atomic spectrum. Use a spectroscope to measure the colours and wavelengths of various light around the lab, such as the incandescent light bulb, fluorescent lights in the lab, and white side of tory building. Use the same spectroscope to measure the colour and wavelength of light emitted by the he, ne, and h discharge tubes that are set up on the lab bench. Iii) use a platinum wire, clean it in the bunsen burner at the fume hood with. Hcl, set up bunsen burner at lab bench, observe the colour of the flame with. Licl along with the colour of the other salt. Dissolve smarties of various colours in distilled water.

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Related Questions

The above is what we did in the lab

Down is the question

Today you are going to take a closer look at the light emitted from a wide variety of different types of matter. Before experimenting with these different light sources, make a large table in your lab notebook with columns listing the major regions of the visible spectrum (ROYGBIV). As you collect data by looking at different light sources, you will keep adding rows of observations into this table. The general layout should look something like this: Once you have your lab notebook ready, collect some observations about these different systems by performing the following experiment: At your bench, you should find a small handheld spectroscope through which you can split the visible spectrum apart and carefully observe each color region in the spectrum. For the first light source, set up and light the votive candle inside the metal pan (the metal pan is just to keep wax from dripping all over the benchtop). Then, look through the spectroscope at the burning candle. In your lab groups, predict what you think the emission spectrum will look like from a light source (flame) that is made by burning the ionic compound SrCI_2. With your prediction, provide a molecular-level justification that supports why you think the emission will look the way you predicted. Write the predictions and explanations down in your lab notebook (with a heading/label for your TA - as you should be doing for every activity). Fill a 400mL beaker about % of the way full with tap water and keep it near your area to use as a waste beaker for used matches and burning applicators. You should have a second beaker containing cotton-tipped applicators soaking in deionized (Dl) water (be sure the applicators are NOT placed in tap water). Into the 24-well microplate, add enough of the solid test samples that have been provided in the lab so that the solid just barely covers the bottom of each well. Be sure to record the identity of each solid you test. Note - be very careful not to cross-contaminate between wells as this will significantly skew results (even a single small crystal can cause a large contamination issue). Remove the candle and place the Bunsen burner in the center of the metal baking pan (the pan will help catch any burning solids that drip or spatter from the flame tests you will be performing). Your TA will demonstrate how to light and adjust the burner being used in our labs here at CSU (avoid fireballs in your face or your lab partner- listen to the TA's directions). To observe the flame colors, you will be placing the salts on the end of water-soaked wooden applicators. When placing the applicators into the burner flame, you only have a limited amount of time before the color will disappear and the applicator begins burning so you should be prepared to make observations as soon as you place the applicator into the burner flame. Also, while performing these steps, one member of your lab group should be observing the flame with the spectroscope while another group member handles the actual burning and observes just with their eye. You should record as much information as you can about the burning behavior including color, intensity, and any other details you notice. In your groups, predict what you think the spectrum would look like for a light-emitting diode (LED) light source. LEDs are made up of solid-state materials. What do you expect to see in the spectroscope while looking at a lit LED? Write this prediction down in your lab notebook and be sure to include a heading so your TA can find this prediction while reviewing your lab notebook pages later. Test your prediction by performing the following experiment: Setup the 9V battery and wire leads as shown below - the foam card that the LEDs are mounted may be clamped into a ring stand to hold it upright for easier viewing. Connect the alligator clips coming from the battery one LED at a time. The red alligator clip should be connected to the longer (+) lead of the LED bulb. The black alligator clip is connected to the shorter (-) lead of the LED bulb. If you reverse the wire leads, the LED will not light. Once connected to the battery, note the macroscopic color of the LED bulb that you can see with your eye, then look through the spectroscope at the lit LED bulb. As you examine the LED with the spectroscope, carefully note and rate the relative appearance/intensity of each of the color regions in the visible spectrum (ROYGBIV). After you have collected all your observations, your TA will demonstrate how to use a different type of spectroscope attached to the laptop computers (SpectroVis Plus). After your TA has demonstrated how to use the instrument, collect spectra for all the LED bulbs by following these Identify and write three (3) new and well-thought-out scientific questions related to the light emitted from a firework. For credit, these new questions MUST follow these guidelines: Questions must be molecular-level and focused on the behavior of the chemical components within fireworks Questions should be directly related to the light emission concepts covered in this lab