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AP Physics 2
15.3 Emission and Absorption Spectra
15.2 The Bohr Model of Atomic Structure
BeginnerMCQMathematicalConceptual18.3k
An energy level diagram with a vertical axis on the left labeled Energy, E (eV). Four horizontal lines represent the energy levels: n=1 at -12 eV, n=2 at -6 eV, n=3 at -3 eV, and n=4 at -1 eV. Three downward vertical arrows represent transitions: Arrow I goes down from level n=4 to n=3, arrow II goes down from level n=3 to n=2, and arrow III goes down from level n=2 to n=1. No other labels, lines, text, or axes appear.
Energy level diagram showing electron transitions I, II, and III.
An atom has four energy levels labeled \(n = 1, 2, 3, 4\) with energy values \(E_1 = -12\text{ eV}\), \(E_2 = -6\text{ eV}\), \(E_3 = -3\text{ eV}\), and \(E_4 = -1\text{ eV}\), as shown in the diagram. Three downward electron transitions, labeled I, II, and III, result in the emission of photons with wavelengths \(\lambda_I\), \(\lambda_{II}\), and \(\lambda_{III}\), respectively. Which of the following correctly ranks the wavelengths of the emitted photons?

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