Flame+Test+Lab.

Flame Test Lab. Brittany St. John #17 Nicole West #21 December 2, 2009 Period 3



**__ Introduction: __**

This lab is about testing different metals in the Bunsen Burner to see the different spectrum/colors of light. This lab is also about finding the frequency and wavelength, and calculating energy in joules of a given solution. Mainly this lab is about testing the metals in the Bunsen Burner to see different colors of flame and determine which metal is used.

__ **Hypothesis:** __

If you change the metal under the Bunsen Burner, then the colors of the flame will change.

__ **Pre-Lab Questions:** __

Red, Orange, Yellow, Green, Blue, Indigo, Violet Frequency of a wave shows how many cycles the wave goes through. The units of frequency are Hertz; Hz equals 1/seconds. The relationship between frequency and wavelength is when wavelength increases, frequency decreases. When using a Bunsen Burner, you have to keep the flame away from your body. Also, if you are burning a test tube, you need to face the opening of the test tube away from everyone. Put your hair up and roll up your sleeves.
 * 1. List the colors of the visible spectrum in order of increasing wavelength.**
 * 2. What is meant by the term frequency of a wave? What are units of frequency? Describe the relationship between frequency and wavelength.**
 * 3. List the safety precautions associated with using a Bunsen Burner.**

__ **Materials:** __


 * Bunsen Burner
 * Tubing
 * Striker
 * Test Tube Rack with 8 Solutions
 * Nichrome Wires

__ **Procedures:** __


 * 1) Write out for all solutions and get teacher inital.
 * 2) Obtain solutions to be tested.
 * 3) Light Bunsen burner flame.
 * 4) Dip wire in one solution and place it in the edge of the burner flame.
 * 5) Record the color given off by the compound when placed in the flame.
 * 6) Repeat the above steps for the compounds to be tested.

__ **Results:** __

(description) || Color Sketch of Flame || Wavelength ||
 * Solution || Formula || Metal Ion Present || Color Emitted
 * Sodium Chloride || NaCl || Na + || yellow || ................................ || 6x10 -7 m ||
 * Sodium Nitrate || NaNO 3 || Na + || orange || ................................ || 6.25x10 -7 m ||
 * Potassium Chloride || KCl || K + || purple || ................................ || 4x10 -7 m ||
 * Potassium Nitrate || KNO 3 || K + || purple || ................................ || 4x10 -7 m ||
 * Copper (II) Sulfate || CuSO 4 || Cu ++ || green || ................................ || 5.50x10 -7 m ||
 * Potassium Chloride || Unknown1 || K + || purple || ................................ || 4x10 -7 m ||
 * Barium Chloride || BaCl 2 || Ba ++ || yellow/green || ................................ || 5.75x10 -7 m ||
 * Strontium Chloride || SrCl 2 || Sr ++ || red || ................................ || 7x10 -7 m ||
 * Copper (I) Chloride || CuCl || Cu ++ || green || ................................ || 5.50x10 -7 m ||
 * Sodium Nitrate || Unknown2 || Na + || bright orange || ................................ || 6.15x10 -7 m ||

__
 * Calculations:** __

600nm x 1m/ 1x10 -9 nm = 6x10 -7 m 625nm x 1m/ 1x10 -9 nm = 6.25x10 -7 m
 * NaCl**
 * NaNO** **3**

400nm x 1m/ 1x10 -9 nm = 4x10 -7 m
 * KCl**

400nm x 1m/ 1x10 -9 nm = 4x10 -7 m
 * KNO** **3**

550nm x 1m/ 1x10 -9 nm = 5.50x10 -7 m
 * CuSO** **4**

400nm x 1m/ 1x10 -9 nm = 4x10 -7 m
 * Unknown1(Potassium Chloride)**

575nm x 1m/ 1x10 -9 nm = 5.75x10 -7 m
 * BaCl** **2**

700nm x 1m/ 1x10 -9 nm = 7x10 -7 m
 * SrCl** **2**

550nm x 1m/ 1x10 -9 nm = 5.50x10 -7 m
 * CuCl** **2**

615nm x 1m/ 1x10 -9 nm = 6.15x10 -7 m
 * Unknown2 (Sodium Nitrate)**


 * __Energy in joules__** Energy = hv Frequency = c/ wavelength

v= 3.00 x 10 8 m/s / 6.00 x 10 -7 m = 5.0 x 1014 1/s E= 6.63 x 10 -34 j x s x 5.0 x 10 14 1/s = 3.315 x 10 -17 J
 * NaCl**

v= 3.00 x 10 8 m/s / 4 x 10 -7 m = 750 E= 6.63 x 10 -34 j x s x 750 = 4.97 J
 * KCl**

v= 3.00 x 10 8 m/s / 5.75 x 10 -7 m = 521.74 1/s E= 6.63 x 10 -34 j x s x 521.74 1/s = 3.46 x 10 -30 J
 * BaCl 2 **

v= 3.00 x 10 8 m/s / 7 x 10 -7 m = 545.45 1/s E= 6.63 x 10 -34 j x s x 545.45 1/s = 3.62 x 10 -30 J
 * SrCl 2 **

v= 3.00 x 10 8 m/s / 5.50 x 10 -7 m = 5.45 x 10 14 1/s E= 6.63 x 10 -34 j x s x 5.45 x 10 14 1/s = 3.51 x 10 -19 J
 * CuCl2**

Post-Lab Questions:

Yes we were able to see different colors for the metals because each metal was different which made the color of flames different. We discovered that the color of the flame was shown by the color of the dominant metal in the solution. The colors of the non-metals were yellow, orange, and red. The colors of the metals were purple, blue and green. Maybe there are different amounts of electrons that set off the different colors of light. They emit different colors of light because they are different solutions. The heat of the flame gives the solutions a reaction to make the different colored lights. We have seen other light emissions from everyday lights that you turn on and off in a room. These are related because something in the light bulb triggers the different reactions, so they are both making reactions. We could know the exact wavelength of the metal instead of estimating on a wavelength spectrum. Nano-meters to meters: 486 nm x 1m/ 1 x 10 -9 nm = 4.86 x 10 -7 m Frenquency: v= 3.00 x 10 8 m/s / 4.86 x 10 -7 m = 6.17 1/s Energy: E= 6.63 x 10 -34 J x s x 6.17 1/s = 4.09 x 10 -33 J We proved our hypothesis. Possible errors were not getting the previous chemical off the Nichrome wire before putting another chemical on.
 * 1. Were you able to see different colors for the metals? Why or why not?**
 * 2. What did you discover?**
 * 3. Was the color from the metal or the non-metals? How do you know?**
 * 4. What particles are found in the chemicals that may be responsible for the production of colored light?**
 * 5. Why do different chemicals emit different colors of light?**
 * 6. Why do you think the chemicals have to be heated in the flame first before the colored light is emitted?**
 * 7. Colorful light emissions are applicable to everyday life. Where else have you observed colorful light emissions? Are these light emission applications related? Explain why you think they are or are not.**
 * 8. Propose at least one possible method for improving the accuracy of the results in this lab experiment.**
 * 9. A green line of wavelength 486 nm is observed in the emission spectrum of hydrogen. Calculate the energy of 1 photon of this green light.**
 * 10. I (proved/ disproved) my hypothesis. Possible errors in this experiment were:**

Conclusion:

We proved our hypothesis because when we tested different metals under the Bunsen Burner, the colors of the flame were different.

|| Pts. Earned || Possible Pts. ||
 * Grade: - Nice Job! ||   ||   ||
 * Title Page || 2  || 2 ||
 * Introduction || 5  || 5 ||
 * Hypothesis || 3  || 3 ||
 * Pre-lab Questions || 5  || 5 ||
 * Materials || 5  || 5 ||
 * Procedures || 5  || 5 ||
 * Results / Data || 8  || 10 ||
 * Calculations || 10  || 10 ||
 * Post-lab Questions || 17  || 20 ||
 * Conclusion || 2  || 2 ||
 * Clean Lab bench || 3  || 3 ||
 * Lab work || 10  || 10 ||
 * Preparedness/ Collaboration/ Safety || 10  || 10 ||
 * Grammar / spelling / coolness || 7  || 10 ||
 * ** Total Points  ** ||  92  ||  100  ||