Question

6) Consider just four of the energy levels in a certain atom, as shown in the diagram below. How many spectral lines will result from all possible transitions among these levels? Which transition corresponds to the highest-frequency light emitted? To the lowest frequency light emitted? n = 4 n = 3 n = 2 7) The atom from the previous example emits a photon with a wavelength of 354.24 nanometers when its electron transitions from the n = 2 to n = 1 state. It emits a photon with a wavelength of 1239.84 nanometers when its electron transitions from the n = 3 state to the n = 2 state. n = 1 a) What are the corresponding frequencies of the photons emitted when an electron transitions from n = 2 to n = 1 and n = 3 to n = 2? b) How much energy does the atom lose when it emits photons during each of these transitions? c) How much energy does the atom lose if its electron transitions directly from the n = 3 to n = 1 state? What is the corresponding frequency of the emitted photon? d) What is the wavelength of light this atom emits when its electron transitions from n = 3 to n = 1?

          6) Consider just four of the energy levels in a certain atom, as shown in the diagram below. How many spectral lines will result from all possible transitions among these levels? Which transition corresponds to the highest-frequency light emitted? To the lowest frequency light emitted?
n = 4
n = 3
n = 2
7) The atom from the previous example emits a photon with a wavelength of 354.24 nanometers when its electron transitions from the n = 2 to n = 1 state. It emits a photon with a wavelength of 1239.84 nanometers when its electron transitions from the n = 3 state to the n = 2 state.
n = 1
a) What are the corresponding frequencies of the photons emitted when an electron transitions from n = 2 to n = 1 and n = 3 to n = 2?
b) How much energy does the atom lose when it emits photons during each of these transitions?
c) How much energy does the atom lose if its electron transitions directly from the n = 3 to n = 1 state? What is the corresponding frequency of the emitted photon?
d) What is the wavelength of light this atom emits when its electron transitions from n = 3 to n = 1?

6) Consider just four of the energy levels in a certain atom, as shown in the diagram below. How many spectral lines will result from all possible transitions among these levels? Which transition corresponds to the highest-frequency light emitted? To the lowest frequency light emitted?
n = 4
n = 3
n = 2
7) The atom from the previous example emits a photon with a wavelength of 354.24 nanometers when its electron transitions from the n = 2 to n = 1 state. It emits a photon with a wavelength of 1239.84 nanometers when its electron transitions from the n = 3 state to the n = 2 state.
n = 1
a) What are the corresponding frequencies of the photons emitted when an electron transitions from n = 2 to n = 1 and n = 3 to n = 2?
b) How much energy does the atom lose when it emits photons during each of these transitions?
c) How much energy does the atom lose if its electron transitions directly from the n = 3 to n = 1 state? What is the corresponding frequency of the emitted photon?
d) What is the wavelength of light this atom emits when its electron transitions from n = 3 to n = 1?

Added by Dennis Y.

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