Spectral Classification-- Procedure and Worksheet Note: In this lab all wovelengths are given in units of Angstroms. I Angstrom - 10" meters; Inm - 10 Angstroms. Write all answers in the space below each question. 1. Look at the energy level diagram below. The open circles on the figure represent electrons. The electron transitions that corespond to the first four absorption lines of the Lyman series are drawn for you as well as their identifying wavelengths (ie. the wavelength of the photons the atom must absorb to allow the electron to make each transition.) Also shown are the first 2 transitions of the Paschen series. a) Draw the first 3 transitions of the Balmer series on the energy level diagram below. b) Each Balmer series transition is associated with one of the following wavelengths: 4340, 6563 and 4861 Angstroms. On the diagram, label which wavelength corresponds to each transition. Energy Levels for Hydrogen A- 18756 X A- 12821 A Paschen Series (nfrared) na2 Balmer Series (Optical A- j216 A A- j026 A A- 973 A A- 950 A Lyman Series (Utra-Violeg 9 The doted line in the energy level diagram represents hydrogen's highest energy level. What happens if an electron absorbs a photon with enough energy to place the electron above the dotted line? Energy level (n)
Spectral Classification-- Procedure and Worksheet Note: In this lab all wovelengths are given in units of Angstroms. I Angstrom - 10" meters; Inm - 10 Angstroms. Write all answers in the space below each question. 1. Look at the energy level diagram below. The open circles on the figure represent electrons. The electron transitions that corespond to the first four absorption lines of the Lyman series are drawn for you as well as their identifying wavelengths (ie. the wavelength of the photons the atom must absorb to allow the electron to make each transition.) Also shown are the first 2 transitions of the Paschen series. a) Draw the first 3 transitions of the Balmer series on the energy level diagram below. b) Each Balmer series transition is associated with one of the following wavelengths: 4340, 6563 and 4861 Angstroms. On the diagram, label which wavelength corresponds to each transition. Energy Levels for Hydrogen A- 18756 X A- 12821 A Paschen Series (nfrared) na2 Balmer Series (Optical A- j216 A A- j026 A A- 973 A A- 950 A Lyman Series (Utra-Violeg 9 The doted line in the energy level diagram represents hydrogen's highest energy level. What happens if an electron absorbs a photon with enough energy to place the electron above the dotted line? Energy level (n)
Related questions
Question
Transcribed Image Text:4.5
Telkom-Monat.
9% - 14:12
K/s
Document View
Spectral Classification-- Procedure and Worksheet
Note: In this lab al wavelengths are given in units of Angstroms. 1 Angstrom = 10" meters; Inm = 10 Angstroms.
Write all answers in the space below each question.
1. Look at the energy level diaggram below. The open circles on the figure represent electrons. The electron
transitions that correspond to the first four absorption lines of the Lyman series are drawn for you as well as their
identifying wavelengths (i.e. the wavelength of the photons the atom must absorb to allow the electron to make
each transition.) Also shown are the first 2 transitions of the Paschen series.
a) Draw the first 3 transitions of the Balmer series on the energy level diagram below.
b) Each Balmer series transition is associated with one of the following wavelengths: 4340, 6563 and 4861
Angstroms. On the diagram, label which wavelength corresponds to each transition.
Energy Levels for Hydrogen
n5
n=4
n3
A- 18756
A- 12821 A
Paschen Serles (Infrared)
n=2
Balmer Series (Optical)
A- 1216 A
A- 1026 A
A- 073 A
A- 950 A
n=1
Lyman Series (Utra-Violet)
) The dotted line in the energy level diagram represents hydrogen's highest energy level. What happens if an
electron absorbs a photon with enough energy to place the electron above the dotted line?
ае 26
d) An atom must absorb an ultraviolet photon to produce a Lyman series absorption line, an optical photon for
the Balmer series, and an infrared photon for the Paschen series. Explain why the Lyman series requires
ultraviolet photons as opposed to optical or infrared. (Hint: Help yourself visualize the reason by looking at
the energy level diagram.)
Look at the six panels of spectra on the following pages. Each panel shows the optical spectrum of six different
stars. The top graph in each panel is the full spectrum; the bottom graph in each panel is a blowup of the Balmer
series absorption line located at 6563 Angstroms. Astronomers call this particular absorption line Ha (because it
is the first line in the Balmer series and a is the first letter of the Greek alphabert), and it is created when an
electron moves from the 2" to the 3 energy level. Note the difference between the scale on the wavelength axis
for the top and bottom graphs.
2.
a) In one well written sentence, explain why Lyman and Paschen series absorption lines are not seen in each
panel's spectrum.
b) In the top graph of each panel of spectra (starting on the next page), circle each of the 3 Balmer series
absorption lines you drew on the energy level diaram in the first question.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 2 images
