M EMISSION SPECTROSCOPY ADVANCED STUDY ASSIGNMENT Name Section Date This assignm
ID: 566347 • Letter: M
Question
M EMISSION SPECTROSCOPY ADVANCED STUDY ASSIGNMENT Name Section Date This assignment MUST be completed before the laboratory period begins. Wavelength values for the hydrogen emission spectrum are required for the experiment. A few answers have been provided for you You may wish to verify some of these to ensure that your calculation methods and significant digits are 1. Calculate energy values for the first SIX hydrogen energy levels using En =-RH/n2 =-(2.179 ×10-18J/n2 where n=1,2,3,4 6 Express your answers in 10-20 exponential form as a convenience for later calculations -217.90 x 10-20J × 10-20J × 10-20J -13.6, × 10-201 x 10-20J -6.052, x 10-30J 2. Calculate all possible energy level DIFFERENCES between: a. Level 1 and levels 2 through 6 b, Level 2 and levels 3 through 6 c. Level 3 and levels 4 through 6 Calculate the corresponding wavelength for each possible SUMMARIZE the E values in the table below 3. value using: As hc/dE = (6.626 × 10-34J-s)(2.998 x1017 nm. s-1)/AE SUMMARIZE the wavelengths on the table below underneath their corresponding . n higher n lower 211.8, x 10-20J x10-20J 121.5, nm × 10-20] 204.2, x 10-20J ×10-20J | nm 97.24, nm nm nm 48.42, x 10-20] 410.23 nm × 10-201 30.26, x 10-20J nm 656.3, nm × 10-20J 434.1, nm 18.15, x 10-20J 15.49,x 10-2010.59, x 10-30] 1093-9 nm nm nm Diagram each energy level (E, thru E) on the reverse. Diagram all possible transitions betweern levels. Label each transition with its wavelength. Identify the ultra-violet, the visible, and the infrared wavelengths 4. 63Explanation / Answer
For hydrogen,
using the above formula,
1. energy levels
E1 = -2.179 x 10^-18/1^2 = -2.179 x 10^-18 J
E2 = -2.179 x 10^-18/2^2 = -5.45 x 10^-19 J
E3 = -2.179 x 10^-18/3^2 = -2.42 x 10^-19 J
E4 = -2.179 x 10^-18/4^2 = -1.36 x 10^-19 J
E5 = -2.179 x 10^-18/5^2 = -8.72 x 10^-20 J
E6 = -2.179 x 10^-18/6^2 = -6.05 x 10^-20 J
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2. Energy level differences
a. 1 to others,
1-->2 dE = -5.45 x 10^-19 - (-2.179 x 10^-18) = 1.63 x 10^-18 J
1-->3 dE = -2.42 x 10^-19 - (-2.179 x 10^-18) = 1.94 x 10^-18 J
1-->4 dE = -1.36 x 10^-19 - (-2.179 x 10^-18) = 2.04 x 10^-18 J
1-->5 dE = -8.72 x 10^-20 - (-2.179 x 10^-18) = 2.10 x 10^-18 J
1-->6 dE = -6.05 x 10^-20 - (-2.179 x 10^-18) = 2.12 x 10^-18 J
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2 to others,
2-->3 dE = -2.42 x 10^-19 - (-5.45 x 10^-19) = 3.03 x 10^-19 J
2-->4 dE = -1.36 x 10^-19 - (-5.45 x 10^-19) = 4.09 x 10^-19 J
2-->5 dE = -8.72 x 10^-20 - (-5.45 x 10^-19) = 4.58 x 10^-19 J
2-->6 dE = -6.05 x 10^-20 - (-5.45 x 10^-19) = 4.84 x 10^-19 J
--
3 to others,
3-->4 dE = -1.36 x 10^-19 - (-2.42 x 10^-19) = 1.06 x 10^-19 J
3-->5 dE = -8.72 x 10^-20 - (-2.42 x 10^-19) = 1.55 x 10^-19 J
3-->6 dE = -6.05 x 10^-20 - (-2.42 x 10^-19) = 1.81 x 10^-19 J
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3. Wavelengths (l)
l = hc/dE
So,
1-->2 l = 6.626 x 10^-34 x 3 x 10^8/1.63 x 10^-18 = 122 nm
1-->3 l = 6.626 x 10^-34 x 3 x 10^8/1.94 x 10^-18 = 102 nm
1-->4 l = 6.626 x 10^-34 x 3 x 10^8/2.04 x 10^-18 = 97 nm
1-->5 l = 6.626 x 10^-34 x 3 x 10^8/2.10 x 10^-18 = 95 nm
1-->6 l = 6.626 x 10^-34 x 3 x 10^8/2.12 x 10^-18 = 94 nm
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2 to others,
2-->3 l = 6.626 x 10^-34 x 3 x 10^8/3.03 x 10^-19 = 656 nm
2-->4 l = 6.626 x 10^-34 x 3 x 10^8/4.09 x 10^-19 = 486 nm
2-->5 l = 6.626 x 10^-34 x 3 x 10^8/4.58 x 10^-19 = 434 nm
2-->6 l = 6.626 x 10^-34 x 3 x 10^8/4.84 x 10^-19 = 434 nm
--
3 to others,
3-->4 l = 6.626 x 10^-34 x 3 x 10^8/1.06 x 10^-19 = 1875 nm
3-->5 l = 6.626 x 10^-34 x 3 x 10^8/1.55 x 10^-19 = 1282 nm
3-->6 l = 6.626 x 10^-34 x 3 x 10^8/1.81 x 10^-19 = 1093 nm
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