A hydrogen atom emits a photon of wavelength 486 nm. From what energy orbit to what lower energy orbit did the electron jump?
ninitial=
nfinal=
A hydrogen atom emits a photon of wavelength 486 nm. From what energy orbit to what...
A hydrogen atom emits a photon of wavelength 656 nm. From what energy orbit to what lower-energy orbit did the electron jump?
A certain atom emits a photon of wavelength 520 nm (1 nm = 10-9 m) when an electron jumps from a higher allowed orbit to a lower orbit. What is the frequency of the photon? What is the photon energy in Joules? What color in the visible light spectrum does it correspond to?
8. An exited hydrogen atom emits a photon having a wavelength of 388.9049 nm and the electron relaxes down to the n=2 level. What was the initial higher energy level of the electron? - hc 388.9049x10 nm -9 = -2.184x102 (12)
"If a hydrogen atom emits a photon of light with a wavelength of 102.6 nm when an electron returns to n = 1 , what n-value was the atom in originally?"
Part A What is the change in energy ?E of the hydrogen atom as the electron makes the transition from the n=3 energy level to the n=1 energy level? Express your answer numerically in electron volts. Part B When an atom makes a transition from a higher energy level to a lower one, a photon is released. What is the wavelength of the photon that is emitted from the atom during the transition from n=3 to n=1? Express your answer...
An atom (not a hydrogen atom) absorbs a photon whose associated wavelength is 234 nm and immediately emits a photon whose associated wavelength is 550 nm. How much net energy is absorbed by the atom in this process?
In a hydrogen atom, an emission line is observed at a wavelength of 486 nm. If the electron was excited to an energy state n = 4, from what state was the electron excited? What was the minimum energy of the excitation light source to cause the initial absorption event? Note: The Rydberg constant is 1.097373 × 107 m
What photon wavelength is emitted when an electron in a hydrogen atom drops from an orbit with a radius of 3.3856x10m to the ground state?
n atom emits a photon having a wavelength of 388.9049 nm and the electron relaxes down to the n-2 level. What was the initial higher energy level of the electron?
An excited hydrogen atom emits light with a wavelength of 397.2 nm to reach the energy level for which n = 2. In which principal quantum level did the electron begin? It would be very helpful if the last step could be over explained, thats where my answer is going wrong.