Help Sign Out Mastering Chemistry Course Home My Courses KHomework 7 Chap 7 Course Home Energy of an Electron in a Hydrogen Atom 2 of 4 Syllabus I Review I Constants I Periodic Table Scores How much energy does the electron have initially in the n=4 excited state? The electron from a hydrogen atom drops from an excited state into the ground state. When an electron drops into a lower-energy orbital, energy is released in the form of electromagnetic radiation. (Figure 1) Express your answer with the appropriate units. eТext View Available Hint(s) Document Sharing Hint 1. Use the equation relating energy to orbital User Settings The energy of an electron (En) in an orbital of the hydrogen atom with the principal quantum number n is given by Course Tools -18 En =-2.18 x 10 This equation can be derived from the Rydberg equation Figure 1 of 1 1.10 x 10 m-1( -wavelength (m)- where 1/A has been substituted with hc/E be rearranging the equation E hc/A: 10-1 10-11 10-9 10-7 10-5 10-3 101 micro- radio gamma rays Uvinfrared I I X rays - 1.10 x 10 m1) hc waves waves Е 1018 1016 visible 1010 1020 10 1012 106 where -frequency (s-1) 6.626x1034 J.s (Planck's constant) h 400 nm 515 nm 750 nm and c 3.00x108 m/s (the speed of light in a vacuum) Visible region II
Help Sign Out Mastering Chemistry Course Home My Courses KHomework 7 Chap 7 Course Home Energy of an Electron in a Hydrogen Atom 2 of 4 Syllabus I Review I Constants I Periodic Table Scores How much energy does the electron have initially in the n=4 excited state? The electron from a hydrogen atom drops from an excited state into the ground state. When an electron drops into a lower-energy orbital, energy is released in the form of electromagnetic radiation. (Figure 1) Express your answer with the appropriate units. eТext View Available Hint(s) Document Sharing Hint 1. Use the equation relating energy to orbital User Settings The energy of an electron (En) in an orbital of the hydrogen atom with the principal quantum number n is given by Course Tools -18 En =-2.18 x 10 This equation can be derived from the Rydberg equation Figure 1 of 1 1.10 x 10 m-1( -wavelength (m)- where 1/A has been substituted with hc/E be rearranging the equation E hc/A: 10-1 10-11 10-9 10-7 10-5 10-3 101 micro- radio gamma rays Uvinfrared I I X rays - 1.10 x 10 m1) hc waves waves Е 1018 1016 visible 1010 1020 10 1012 106 where -frequency (s-1) 6.626x1034 J.s (Planck's constant) h 400 nm 515 nm 750 nm and c 3.00x108 m/s (the speed of light in a vacuum) Visible region II
Help Sign Out Mastering Chemistry Course Home My Courses KHomework 7 Chap 7 Course Home Energy of an Electron in a Hydrogen Atom 2 of 4 Syllabus I Review I Constants I Periodic Table Scores How much energy does the electron have initially in the n=4 excited state? The electron from a hydrogen atom drops from an excited state into the ground state. When an electron drops into a lower-energy orbital, energy is released in the form of electromagnetic radiation. (Figure 1) Express your answer with the appropriate units. eТext View Available Hint(s) Document Sharing Hint 1. Use the equation relating energy to orbital User Settings The energy of an electron (En) in an orbital of the hydrogen atom with the principal quantum number n is given by Course Tools -18 En =-2.18 x 10 This equation can be derived from the Rydberg equation Figure 1 of 1 1.10 x 10 m-1( -wavelength (m)- where 1/A has been substituted with hc/E be rearranging the equation E hc/A: 10-1 10-11 10-9 10-7 10-5 10-3 101 micro- radio gamma rays Uvinfrared I I X rays - 1.10 x 10 m1) hc waves waves Е 1018 1016 visible 1010 1020 10 1012 106 where -frequency (s-1) 6.626x1034 J.s (Planck's constant) h 400 nm 515 nm 750 nm and c 3.00x108 m/s (the speed of light in a vacuum) Visible region II
The electron from a hydrogen atom drops from an excited state into the ground state. When an electron drops into a lower-energy orbital, energy is released in the form of electromagnetic radiation.
How much energy does the electron have initially in the n=4 excited state?
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Mastering Chemistry
Course Home
My Courses
KHomework 7 Chap 7
Course Home
Energy of an Electron in a Hydrogen Atom
2 of 4
Syllabus
I Review I Constants I Periodic Table
Scores
How much energy does the electron have initially in the n=4 excited state?
The electron from a hydrogen atom drops from an
excited state into the ground state. When an electron
drops into a lower-energy orbital, energy is released in
the form of electromagnetic radiation. (Figure 1)
Express your answer with the appropriate units.
eТext
View Available Hint(s)
Document Sharing
Hint 1. Use the equation relating energy to orbital
User Settings
The energy of an electron (En) in an orbital of the hydrogen atom with the principal
quantum number n is given by
Course Tools
-18
En =-2.18 x 10
This equation can be derived from the Rydberg equation
Figure
1 of 1
1.10 x 10 m-1(
-wavelength (m)-
where 1/A has been substituted with hc/E be rearranging the equation
E hc/A:
10-1
10-11
10-9
10-7 10-5 10-3
101
micro-
radio
gamma
rays
Uvinfrared
I I
X rays
- 1.10 x 10 m1)
hc
waves
waves
Е
1018 1016 visible
1010
1020
10
1012
106
where
-frequency (s-1)
6.626x1034 J.s (Planck's constant)
h
400 nm
515 nm
750 nm
and
c 3.00x108 m/s (the speed of light in a vacuum)
Visible region
II
Interaction between an electric field and a magnetic field.
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