Using the fact that electrons can only exist in certain energy "shelves," we can predict what wavelengths of light, or colors, are emitted when we add energy to the system. The following equation shows the energy levels for a hydrogen atom with only one electron (when dealing with multiple electrons and protons the math becomes far more complex and is outside the scope of this activity). = RH) Where: A is the wavelength of light RH is the Rydberg Constant for a Hydrogen atom, 1.0974 - 10 /m n2 is the final energy level ni is the starting energy level (n1 and n2 are always integers: 1, 2, 3, ..) 1. Using the formula above, what is the wavelength of light emitted between the 2nd and 1t energy levels? 121.5 nm 102.5 nm 121500 nm 102500 nm 5:56 acer % bac 3 8. 9. h
Using the fact that electrons can only exist in certain energy "shelves," we can predict what wavelengths of light, or colors, are emitted when we add energy to the system. The following equation shows the energy levels for a hydrogen atom with only one electron (when dealing with multiple electrons and protons the math becomes far more complex and is outside the scope of this activity). = RH) Where: A is the wavelength of light RH is the Rydberg Constant for a Hydrogen atom, 1.0974 - 10 /m n2 is the final energy level ni is the starting energy level (n1 and n2 are always integers: 1, 2, 3, ..) 1. Using the formula above, what is the wavelength of light emitted between the 2nd and 1t energy levels? 121.5 nm 102.5 nm 121500 nm 102500 nm 5:56 acer % bac 3 8. 9. h
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:Spectroscopy, or the study of how light interacts with matter, is an extremely powerful tool scientists use to identify unknown
substances. One branch of spectroscopy is the measurement of the interactions between gases and visible light.
Sending a very high voltage through a gas adds energy to the system causing some of the electrons to enter a more unstable, or
excited, state. To return to the stable state, the electron emits some of that energy in the form of light.
Using the fact that electrons can only exist in certain energy "shelves," we can predict what wavelengths of light, or colors, are emitted
when we add energy to the system. The following equation shows the energy levels for a hydrogen atom with only one electron (when
dealing with multiple electrons and protons the math becomes far more complex and is outside the scope of this activity).
= R#-)
Where:
X is the wavelength of light
RH is the Rydberg Constant for a Hydrogen atom, 1.0974 - 10 /m
n2 is the final energy level
ni is the starting energy level
(ni and n2 are always integers: 1, 2, 3, ..)
1. Using the formula above, what is the wavelength of light emitted between the 2nd and1t energy levels?
OV1 5:5
acer
crl

Transcribed Image Text:Using the fact that electrons can only exist in certain energy "shelves," we can predict what wavelengths of light, or colors, are emitted
when we add energy to the system. The following equation shows the energy levels for a hydrogen atom with only one electron (when
dealing with multiple electrons and protons the math becomes far more complex and is outside the scope of this activity).
= R#)
Where:
Xis the wavelength of light
RH is the Rydberg Constant for a Hydrogen atom, 1.0974 - 10/m
n2 is the final energy level
n1 is the starting energy level
(n1 and n2 are always integers: 1, 2, 3, .)
1. Using the formula above, what is the wavelength of light emitted between the 2nd and 1st energy levels?
121.5 nm
O 102,5 nm
121500 nm
102500 nm
OVI 5:56
acer
%24
0%
&
bac
6.
mi
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