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Tyler Stanley #18 Sean Miller # 10** Period 3**
 * Flame Lab
 * 12/1/09

**__Introduction__ In a metal when an atom is heated the electrons in it are excited and move away from the nucleus. They eventually fall back and emit light. Different metals release different colors. Due to this difference in flame color a it is possible to discover the metal located in a solution. The color of the flame is due to the amount of energy release. A red flame means the metal releases the lowest amount of energy while a violet flame has the most energy. **


 * __Hypothesis__ **
 * I hypothesize that when the solutions are heated they will emit a colored light that will enable us to conclude what metal is in the solution. **

1. List the colors of the visible spectrum in order of increasing wavelength. Violet 380-450 nm Indigo 420-450 nm Blue 450-495 nm Green 495-570 nm Yellow 570-590 nm Orange 590-620 nm Red 620-750 nm  2. ** **What is meant by the term frequency of a wave? What are the units of frequency? Describe the relationship between frequency and wavelength.**
 * __Pre Lab Questions__** **
 * A frequency of a wave is the number of wave cycles to pass a given point per unit of time. The unit of a frequency is called a hertz (Hz). The higher the frequency the shorter the wavelength because if the frequency is higher there are more wave cycles making the distance between the crests smaller . **

**3** . ** List the safety precautions associated with using a Bunsen Burner. When using a Burner make sure no flammable materials are by it. Roll up sleeves and raise hair. Always wear your safety glasses while using the Burner. Always make sure the Burner is being supervised. **

**__Equipment__** ** Burner & tubing, striker, Test tube rack with 8 solutions, Nichrome wires.

__Procedures__ 1. Write out formulas for all solutions and get teacher initial 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. **

(description) ||= Colored Sketch of Flame ||= Wavelength (m) ||
 * __Result: (Data Table)__ **
 * = Solution ||= Formula ||= Metal Ion Present ||= Color Emitted
 * = Sodium Chloride ||= NaCl ||= Na+ ||= Light Orange ||= _ ||= 570nm ||
 * = Sodium Nitrate ||= NaNO3 ||= Na+ ||= Orange ||=  _ ||= 600nm ||
 * = Potassium Chloride ||= KCl ||= K+ ||= Purple Blue ||= _ ||= 440nm ||
 * = Potassium Nitrate ||= KNO3 ||= K+ ||= Yellow Orange ||=  _ ||= 630nm ||
 * = copper (II) sulfate ||= CuSO4 ||= Cu+ ||= Blue Green ||= _ ||= 540nm ||
 * = ||= Unknown1 ||= K+ ||= Violet ||=  _ ||= 470nm ||
 * = Barium Chloride ||= BaCl2 ||= Ba+ ||= Yellow ||= _ ||= 530nm ||
 * = Strontium Chloride ||= SrCl2 ||= Sr+ ||= Red Orange ||=  _ ||= 640nm ||
 * = Copper Chloride ||= CuCl2 ||= Cu+ ||= Light Blue Green ||= _ ||= 530nm ||
 * = ||= Unknown2 ||= Na+ ||= Yellow Gold ||=  _ ||= 570nm ||



**__Calculations__**

__**NaCl**__-575 x 1m/1x10^9nm= 5.75x10^-7m v=3.00 x 10^8 m/s / 5.75 x 10^-7 = 5.22x14 1/s E=6.63x10^-34 JxS x 5.2x10^14 1/s = **3.45x10^-19 J

__KCl-__**440nm x 1m/1x10^9nm=4.40x10^-7m v=3.00x10^8m/s / 4.4x10^-7m=6.82x10^141/s E=6.63x10^-34 JxS x 6.82x10^14= **4.52x10^-19 J

__BaCl2-__** 530nm x 1m/1x10^9=5.30x10^-7m v=3.00x10^8m/s / 5.30x10^-7m= 5.66x10^14 1/s E=6.63x10^-34 JxSx 5.66x10^14 1/s = **3.75x10^-19 J**

v=3.00x10^8 m/s/ 6.40x10^-7m=4.69x10^14 1/s E=6.63x10^-34 JxS x 4.69 x 10^14 1/s = **3.11x10^-19 J
 * __SrCl2__**- 640nm x 1m/1x10^9nm = 6.40x10^-7m

__CuCl2-__**530nm x 1m/1x10^9=5.30x10^-7m v=3.00x10^8m/s /5.30x10^-7m=5.66x10^14 1/s E=6.63x10^-34 JxS x 5.66x10^14 1/s= **3.75x10^-19 J**

__** Post Lab Questions **__ **1. Were you able to see different colors for the metals? Why or why not? Yes, we were able to see the colors because we heated the metal so the energy was released. ** We discovered that certain metals released a different color light when heated. It was from the metal because the energy comes from electrons from the metals. ** Electrons  The energy released is sometimes larger or smaller. ** 6.Why do you think the chemicals have to be heated in the flame first before the colored light is emitted. ** The electrons have to excited in order to release the energy. ** 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 why not. ** Rainbows are also emissions of light, but are not like the flames because it doesn't have to do with electrons. **8.Propose at least one possible method for improving the accuracy of the results in this lab experiment.** A color spectrum diagram during the lab would have been helpful to look at colors. ** 9.A green line of wavelength 486 nm is observed in the emission spectrum of hydrogen. Calculate the energy of one photon of this green light. **
 * 2.What did you discover?**
 * 3. Was the color from the metal or the non-metal? 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? **


 * 10. I proved my hypothesis. Possible errors in this lab were: a few misplacement of substances, no idea how to do the calculations. **