Enter the observed scale values for each of the observed lines listed below and indicate the corresponding wavelength. (Enterscale values to the nearest 0.1. Enter computed values to the correct number of significant figures.)Scale Values of Observed Lines (as observed through spectroscope)Discharge TubeObserved Line ColorScale Value (fromspectroscope)4.05.7 XCalculated Wavelength(nm)4.0redgreen/bluehydrogenbluetoo low4.05.14.04.04.04.34.04.0indigo (violet)4.0red4.05.64.04.04.0argongreen5.5blue4.0 4.54.0red4.0 6.04.04.0neonorange6.34.0green4.05.54.0

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Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter9: Pre-quantum Mechanics

Section: Chapter Questions

Problem 9.7E: Draw, label, and explain the functions of the parts of a spectroscope.

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Similar questions

Draw, label, and explain the functions of the parts of a spectroscope.
Convert a a wavelength of 218A to cm1, b a frequency of 8.0771013s1 to cm1, c a wavelength of 3.31m to cm1.
The maximum in the blackbody radiation intensity curve moves to shorter wavelength as temperature increases. The German physicist Wilhelm Wien demonstrated the relation to be max1/T . Later, Planck’s equation showed the maximum to be max=0.20hc/kt . In 1965, scientists researching problems in telecommunication discovered “background radiation” with maximum wavelength 1.05 mm (microwave region of the EM spectrum) throughout space. Estimate the temperature of space.
What is the threshold frequency for sodium metal if a photon with frequency 6.661014s1 ejects an electron with 7.741020 J kinetic energy? Will the photoelectric effect be observed if sodium is exposed to orange light?
6.10 Define the term refraction.
6.9 If a string of decorative lights includes bulbs with wave-lengths of 480, 580, and 700 mm, what are the frequencies of the lights? Use Figure 6.6 to determine which colors are in the set.
In a FranckHertz experiment on hydrogen atoms, the first two excitation thresholds occur at 10.1 and 11.9 eV. Three optical emission lines are associated with these levels. Sketch an energy-level diagram for hydrogen atoms based on this information. Identify the three transitions associated with these emission lines. Calculate the wavelength of each emitted line.
State how many radial, angular, and total nodes are in each of the following hydrogen-like wavefunctions. a 2s b 3s c 3p d 4f e 6g f 7s
There are an infinite number of allowed electronic transitions in the hydrogen atom. Why dont we see more lines in the hydrogen emission spectrum?
What is a rotating frame of reference?
A particular transition of the rubidium atom emits light whose frequency is 3.84 1014 Hz. (Hz is the abbreviation for hertz, which is equivalent to the unit/s, or s1.) Is this light in the visible spectrum? If so, what is the color of the light? (See Figure 7.5.)
Using Table 5.2, write down the mathematical expression for the 2px wave function for an electronically excited H atom. Estimate the probability of finding the 2px electron if you look in a cubical box of volume of 0.8(pm)3 centered at a distance of 0.5001010m in the =/2 , =0 direction. Does this probability change as you change ? At what angles is the probability of finding the electron smallest and at what angles is the probability the largest? (Note that =2 is the same location as =0 , so don’t double count.)

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