Flame+Test+Lab

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Flame Test Lab


Nicole Mazzilli #9 Kelsey Sell #15 December 2 Period 3

= Purpose: = ** To predict the identity of an unknown metal ion from a flame test and to find the color and wavelengths of different solutions. **

**Introduction:** In this lab we will test the reactions of different solutions by heating them over the flame and seeing what color they appear. Doing this will show us what color is emitted from each metal that makes up the solutions.

= Hypothesis: = // If you put a solution on the nichrome wire and place it over the Bunsen burner, then the emitted chemicals burning will change the color of the flame. //

= Pre- Lab Questions: = Red, orange, yellow, green, blue, and violet
 * 1**. **Q. //List the colors of the visibnle spectrum in order of increasing wavelength//.**

The frquency of a wave is the number of wave cycles to pass at a given point per unit of time. The unit used for frequency is shown as 1/s. The relationship between frequency and wavelength is as the wavelength increases, the frequency decreases.
 * 2**. **Q. //What is meant by the term frequency of a wave? What are units of frequency? Describe the relationship between frequency and wavelenght.//**

Never leave the flame unattended, someone must be watching it at all times. Put your hair back and dont lean near the flame. Keep the flame low and be careful not to burn anything. Also, when you put something over top of the flame, point it away from any people.
 * 3.** **Q. //List the safety precautions associated with using a Bunsen Burner//.**

= Equipment: =
 * Bunsen Burner and tubing
 * Safety Goggles
 * Striker
 * Nichrome wires
 * Eight chemical solutions and two unknown solutions

= Procedures: =
 * 1) Write out formulas for all solutions and get teacher initial.
 * 2) Obtain solutions to be tested.
 * 3) Light Bunsen burner flame.
 * 4) Record the color given off by the compound when placed in the flame.
 * 5) Repeat the above steps for the other compounds to be tested.

= R esults: = 

Present ** ||= ** Color Emitted ** Flame ** ||= ** Wavelength **
 * = ** Solution ** ||= ** Formula ** ||= ** Metal Ion
 * (description) ** ||= ** Color Sketch of
 * (m) ** ||
 * = Sodium

Chloride
||= NaCl ||= Na + ||= Dark Yellow ||= abcdefghi  ||=  570 nm 5.70x10 11 m  || 6.0x10 11 m || 4.80x10 11 m || chloride ||= CuCl 2 ||=  Cu2+  ||= Blue-green ||= abcdefghi ||=   492 nm   4.92x10 11 m || 5.65x10 11 m   ||
 * = Sodium Nitrate ||= NaNO 3 ||=   Na+   ||= Orange ||= abcdefghi ||= 600 nm
 * = Potassium Chloride ||= KCl ||=  K+   ||= Pale Pink ||= abcdefghi ||= 400 nm 4.0x10 11 m ||
 * = Potassium Nitrate ||= KNO 3 ||= K + ||= Light pink/Orange ||= abcd efghi ||= 615 nm 6.15x10 11 m ||
 * = Copper (II) Sulfur ||= CuSO 4 ||=   Cu2+   ||= Greenish ||= abcdefghi ||=   530 nm   5.30x10 11 m ||
 * = Potassium ||= Unknown 1 ||= K + ||= Light Purple ||= abcdefghi ||=  420 nm   4.20x10 11 m ||
 * = Barium Chloride ||= BaCl 2 ||=   Ba2+   ||= Pale Green ||= abcdefghi ||= 480 nm
 * = Strontium Chloride ||= SrCl 2 ||=   Sr+   ||= Red ||= abcdefghi ||=   780   nm   7.80x10 11 m ||
 * = Cooper (II)
 * = Cooper ||= Unknown 2 ||= Cu ||= Light Yellow ||= abcdefghi ||=  565 nm

= C alculations: =

**Wavelength**
**wavelength / 1 x 109**



NaCl
 E=HV V= 3.00 x 10 8m/s / 5 .70 x 10 11m = E= 6.63 x 10 -34 /s x 5.26 x 10 -4 m = E= 3.48 x 10 -37 J
 * V= C/ Wavelength**
 * V =** 5.26 x 10 -4s

**CuCl**


492nm x 1m / 1 x 10 9 nm = 4.92x10 11 m V= 3.00 x 10 8 m/s / 4.92x10 11  m = V= 6.09 x 10 -4 s E= 6.63 x 10 -34 j/s x 6.09 x 10 -4 s = E= 4.03 x 10 -37 J


 * BaCl2 **


480nm x 1m / 1 x 10 9 nm = 4.80 x 10 11 m V= 3.00 x 10 8 m/s / 4.80 x 10 11 m = V= 6.25 x 10 -4 s E= 6.63 x 10 -34 j/s x 6.25 x 10 -4 s = E = 4.14 x 10 -37 J

KCl 400nm x 1m / 1 x 10 9 nm = 4.0x10 11 m V= 3.00 x 10 8 m/s / 4.0x10 11  m = V= 7.50 x 10 -4 s

E= 6.63 x 10 -34 j/s x 7.50 x 10 -4 s = E= 4.97 x 10 -37 J

SrCl 780nm x 1m / 1 x 10 9 nm = 7.80x10 11 m V= 3.00 x 10 8 m/s / m = <span style="border-collapse: collapse; webkit-border-horizontal-spacing: 2px; webkit-border-vertical-spacing: 2px;">7.80x10 11  m = V= 3.85 x 10 -4 s E= 6.63 x 10 -34 j/s x 3.85 x 10 -4 s = E= 2.55 x 10 -37 J

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[[image:http://www.stagespot.com/Images/wavelength.jpg width="684" height="326" align="center"]]
= Post lab questions: = **1**//**.Where you able to see different colors for the metals? Why or why not?**//

Yes we were able to see different colors because different types of metals have different types of properties

 * 2//.What did you discover?//**


 * 3.//Was the color from the metal or the non metal? How do you know?//**

The color came from the metals. We know this because that is what the solutions with similar colors have in common.

 * 4.//What particles are found in the chemicals that may be responsible for the production of colored light?//**

The particle that is found in the chemicals, that is most likely responsible for the color is Photons.
<span style="font-family: Tahoma,Geneva,sans-serif;"> //** 5 .Why do different chemicals emit different colors of light? **//

Different chemicals emit different colors of light because each chemical is made up of different particles which show off 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?**//

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I think the chemicals have to be heated in the flame before the light is emited because it needs to be able to get the light needed. They then return to ground state, emitting a photon of light. To determine the color, what matters is the amount of energy in the photon. The energy in the photon gives off the light, making it a color. =====

//** 7 .Colorful light emissions are applicable to everyday life. Where else have you observed colorful light emissions? Are these light emission applications relates? Explain why you think they are or are not.**//

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Colorful light emissions that are applicable you could see in everyday life are in city and in a rainbow. The light emissions are not related because lights in a city are powered by electricity and rainbows are lights from the sun .=====

One way you could improve the accuracy of the results in this lab would be using a separate nichrome wire for each different chemical. This way you wouldn't have multiple chemicals burning at the same time.<span style="font-family: Georgia,serif;">
 * 8.//Propose at least one possible method for improving the accuracy of the results in this lab experiment.//**

Where v= frequency, c= speed of light (3.00 x 108 ** m/s), h= Plank's Constant (6.63 x 10-34 J*s), <span style="color: #000000; font-family: Tahoma,Geneva,sans-serif;">486nm x 1m / 1 x 109nm = 4.86 x 1011m V= 3.00 x 108 m/s / 4.86 x 1011m = 6.17 x 1018s E= 6.63 x 10-34 j/s x 6.17 x 1018s = 4.09 x 10-15 J
 * 9. //A green of wavelength 486 nm is observed in the emission spectrum of hydrogen. Calculate the energy of one photon of this green light.//

We proved our hypothesis because when we tested each chemical by placing it over a flame, the color that was emitted changed.
 * 10. //I (prove/disprove) my hypothesis. Possible errors in this experiment.//**

= C onclusion: =