The energy-level diagram for the atomic emission spectra of an unknown gas is presented in the diagram below. a) Initially, electrons are only in the ground state (n=1). A beam of red light hits the gas. This beam is a continuous spectrum of red light (from 620 nmnm to 750 nmnm) How many absorption line/s will there be in the spectra? 1 b) Initially, electrons are only in the ground state (n=1). A beam of red light hits the gas. This beam is a continuous spectrum of red light (from 620 nmnm to 750 nmnm) Calculate the wavelength of the absorption line λa = 690 nm c) After absorption of the red light, the electrons are now in the n = 3 energy level. How many possible line/s will there be in an emission spectra after absorption of the red light? 3 d) Calculate the wavelength of the emission lines. Enter from smallest wavelength to largest wavelength (or highest energy to lowest energy). Separate each answer by a comma. Please solve for D.
The energy-level diagram for the atomic emission spectra of an unknown gas is presented in the diagram below. a) Initially, electrons are only in the ground state (n=1). A beam of red light hits the gas. This beam is a continuous spectrum of red light (from 620 nmnm to 750 nmnm) How many absorption line/s will there be in the spectra? 1 b) Initially, electrons are only in the ground state (n=1). A beam of red light hits the gas. This beam is a continuous spectrum of red light (from 620 nmnm to 750 nmnm) Calculate the wavelength of the absorption line λa = 690 nm c) After absorption of the red light, the electrons are now in the n = 3 energy level. How many possible line/s will there be in an emission spectra after absorption of the red light? 3 d) Calculate the wavelength of the emission lines. Enter from smallest wavelength to largest wavelength (or highest energy to lowest energy). Separate each answer by a comma. Please solve for D.
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The energy-level diagram for the atomic emission spectra of an unknown gas is presented in the diagram below.
a) Initially, electrons are only in the ground state (n=1). A beam of red light hits the gas. This beam is a continuous spectrum of red light (from 620 nmnm to 750 nmnm)
How many absorption line/s will there be in the spectra?
1
|
b) Initially, electrons are only in the ground state (n=1). A beam of red light hits the gas. This beam is a continuous spectrum of red light (from 620 nmnm to 750 nmnm)
Calculate the wavelength of the absorption line
λa =
|
690
|
nm
|
c) After absorption of the red light, the electrons are now in the n = 3 energy level. How many possible line/s will there be in an emission spectra after absorption of the red light?
3
d) Calculate the wavelength of the emission lines. Enter from smallest wavelength to largest wavelength (or highest energy to lowest energy). Separate each answer by a comma.
Please solve for D.
![The energy-level diagram for the atomic emission spectra of an unknown gas is presented in the diagram below.
n= 4
4.0 ev
n = 3
1.8 ev
n= 2
1.5 ev
n = 1
O ev
Calculate the wavelength of the emission lines. Enter from smallest wavelength to largest wavelength (or highest energy to lowest energy). Separate each answer by a comma.
A2
nm](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F43abe65f-7e5f-4ca7-a91c-ab097f3acb86%2Fb3de35f0-4077-4086-87be-40e3d2ccb3f0%2Fscs45no_processed.png&w=3840&q=75)
Transcribed Image Text:The energy-level diagram for the atomic emission spectra of an unknown gas is presented in the diagram below.
n= 4
4.0 ev
n = 3
1.8 ev
n= 2
1.5 ev
n = 1
O ev
Calculate the wavelength of the emission lines. Enter from smallest wavelength to largest wavelength (or highest energy to lowest energy). Separate each answer by a comma.
A2
nm
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