Imagine that an electron in an excited state in a nitrogen molecule decays to iss ground state, emitting a photon with a frequency of $8.88 \times 1 0^{14} Hz$ . What is the change in energy. $? E$ , that the electron undergoes to decay to its ground state? Express your answer in electron volts to three significant figures. $? E = [[[eV$ Part B Considering that the highest intensity in the nitrogen spectrum is, in fact, recorded for radiation with a frequency of about $8.88 \times 1 0^{14} Hz$ , will your eyes be able to detect this radiation?

Question

Imagine that an electron in an excited state in a nitrogen molecule decays to iss ground state, emitting a photon with a frequency of

8.88 \times 1 0^{14} Hz

. What is the change in energy.

? E

, that the electron undergoes to decay to its ground state? Express your answer in electron volts to three significant figures.

? E = [[[eV

Part B Considering that the highest intensity in the nitrogen spectrum is, in fact, recorded for radiation with a frequency of about

8.88 \times 1 0^{14} Hz

, will your eyes be able to detect this radiation?

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