4, 3. Excited Ground state 1(ground state) state 4. 4.85E-19 J 4.42E-19 J 3.98E-19 J 3. 1. 3.03E-19 J 2. 1. 1 (ground state) Energy Energy paquosqe emitted 2) [30] Energy Levels Above is a schematic of a Hydrogen atom with its first 5 energy levels. On the right is the energy emitted from the transitions (lines pointing down on the diagram). Using the knowledge that energy and wavelength are hc, connected ( E =) you will figure out the wavelength for each of these %3D transitions. %3D E. h = Planck constant = 6.63E-34 J*s c = speed of light = 3E8 m/s 2 = wavelength in meters E = energy in Joules (J) %3D hc %3D E will be in meters! Divide by 10-9 for nm If you need help converting this to a color easier, try this website once you get the wavelength in nm: https://academo.org/demos/wavelength-to- colour-relationship/ For the following give the wavelengths in nanometers (nm) and no decimal points needed. The above equation is in meters! A nanometer is 10° meters. ALL ANSWERS ARE IN VISUAL, so they should all be between 400- 700 nm range. This is important to be able to do on your calculator, so hopefully knowing the range helps double check your answer! a) The electron can absorb energy to go to any of the higher energy levels. If it gets absorbed to the 4th excited state (the top line labeled 5), what wavelength does the atom emit if it goes from this state (5) back to the ground state (1)? What color is this? tariw (1)eti2 bruong ard of S) 9a betioxe orh mol yltes (b froloo tadw bns rignslovsw Sagan mea We are matle of star b) The electron can go to any state depending on the energy absorbed. What wavelength does the atom emit if it goes from the 3rd excited state (4) to the ground state (1)? What color is this? about finding planets an poasibly e an young sten?

4, 3. Excited Ground state 1(ground state) state 4. 4.85E-19 J 4.42E-19 J 3.98E-19 J 3. 1. 3.03E-19 J 2. 1. 1 (ground state) Energy Energy paquosqe emitted 2) [30] Energy Levels Above is a schematic of a Hydrogen atom with its first 5 energy levels. On the right is the energy emitted from the transitions (lines pointing down on the diagram). Using the knowledge that energy and wavelength are hc, connected ( E =) you will figure out the wavelength for each of these %3D transitions. %3D E. h = Planck constant = 6.63E-34 J*s c = speed of light = 3E8 m/s 2 = wavelength in meters E = energy in Joules (J) %3D hc %3D E will be in meters! Divide by 10-9 for nm If you need help converting this to a color easier, try this website once you get the wavelength in nm: https://academo.org/demos/wavelength-to- colour-relationship/ For the following give the wavelengths in nanometers (nm) and no decimal points needed. The above equation is in meters! A nanometer is 10° meters. ALL ANSWERS ARE IN VISUAL, so they should all be between 400- 700 nm range. This is important to be able to do on your calculator, so hopefully knowing the range helps double check your answer! a) The electron can absorb energy to go to any of the higher energy levels. If it gets absorbed to the 4th excited state (the top line labeled 5), what wavelength does the atom emit if it goes from this state (5) back to the ground state (1)? What color is this? tariw (1)eti2 bruong ard of S) 9a betioxe orh mol yltes (b froloo tadw bns rignslovsw Sagan mea We are matle of star b) The electron can go to any state depending on the energy absorbed. What wavelength does the atom emit if it goes from the 3rd excited state (4) to the ground state (1)? What color is this? about finding planets an poasibly e an young sten?

Related questions

Question

4,
3.
Excited
Ground
state
1(ground state)
state
4.
4.85E-19 J
4.42E-19 J
3.98E-19 J
3.
1.
3.03E-19 J
2.
1.
1 (ground state)
Energy
Energy
paquosqe
emitted
2) [30] Energy Levels
Above is a schematic of a Hydrogen atom with its first 5 energy levels. On
the right is the energy emitted from the transitions (lines pointing down on
the diagram). Using the knowledge that energy and wavelength are
hc,
connected ( E =) you will figure out the wavelength for each of these
%3D
transitions.
%3D
E.
h = Planck constant = 6.63E-34 J*s
c = speed of light = 3E8 m/s
2 = wavelength in meters
E = energy in Joules (J)
%3D
hc
%3D
E
will be in meters! Divide by 10-9 for nm
If you need help converting this to a color easier, try this website once you
get the wavelength in nm: https://academo.org/demos/wavelength-to-
colour-relationship/

For the following give the wavelengths in nanometers (nm) and no decimal
points needed. The above equation is in meters! A nanometer is 10°
meters. ALL ANSWERS ARE IN VISUAL, so they should all be between 400-
700 nm range. This is important to be able to do on your calculator, so
hopefully knowing the range helps double check your answer!
a) The electron can absorb energy to go to any of the higher energy levels.
If it gets absorbed to the 4th excited state (the top line labeled 5), what
wavelength does the atom emit if it goes from this state (5) back to the
ground state (1)? What color is this?
tariw (1)eti2 bruong ard of S) 9a betioxe orh mol yltes (b
froloo tadw bns rignslovsw
Sagan mea
We
are matle of star
b) The electron can go to any state depending on the energy absorbed.
What wavelength does the atom emit if it goes from the 3rd excited
state (4) to the ground state (1)? What color is this?
about finding planets an poasibly e an
young sten?

Expert Solution

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Blurred answer

Follow-up Questions

Read through expert solutions to related follow-up questions below.

Follow-up Question

c) How about the 2rd excited state (3) to the ground state (1)? What
wavelength and what color?
d) Lastly, from the 1st excited state (2) to the ground state (1), what
wavelength and what color?

Solution

by Bartleby Expert