(c) this atom's electron can only transition from the n=4 level to the n=5 level by absorbing light with a wavelength of 872 nm and no other wavelengths.
Reason : According to Bohr atomic model, energuy levels are quantised meaning only specific energy can excite electrons to higher staes. In this case it is a ohoton with wavelength 872 nm
4. An atom emits a photon with a wavelength of 872 nm when its electron moves from the n = 5 energy level to the n...
1. A hydrogen atom with its electron in the n = 5 energy level emits a photon of IR light. (i)[3 marks] Calculate the change in energy of the atom and (ii) [2 marks] Calculate the wavelength (in nm) of the photon.
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?
"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?"
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?
An isolated atom of a certain element emits light of wavelength 512 nm when the atom falls from its fifth excited state into its second excited state. The atom emits a photon of wavelength 411 nm when it drops from its sixth excited state into its second excited state. Find the wavelength of the light radiated when the atom makes a transition from its sixth to its fifth excited state. An isolated atom of a certain element emits light of...
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)
1. (5 points) An electron in a hydrogen atom is initially at n=2 energy level. When the atom is exposed to 434.2 nm light, the electron becomes excited. Determine the final energy level to which the electron is promoted during the excitation.
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.
How many different energies of light are emitted from an H atom with the electron in the n=4 energy shell? Group of answer choices a. 3 b. 4 c. 5 d. 6 2.. Would a photon of visible light (photons with wavelengths = 400 - 700 nm) have sufficient energy to excite an electron in a hydrogen atom from n = 1 to n = 5? NOTE: You'll need to calculate how much energy is required for the transition from...
Chapter 4, Question 79 A hydrogen atom emits a photon as its electron changes from n = 5 ton = 1. What is the wavelength of the photon? In what region of the electromagnetic spectrum is this photon found? nm These photons fall in the region. the tolerance is +/-29 Click if you would like to Show Work for this question: Open Show Work