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AP Physics 2
15.3 Emission and Absorption Spectra
15.2 The Bohr Model of Atomic Structure
IntermediateMCQMathematicalProportional Analysis19.1k
An energy-level diagram for a hydrogen atom showing three horizontal dashed lines stacked vertically, labeled n = 1 at the bottom, n = 2 in the middle, and n = 3 at the top. Two downward vertical arrows represent electronic transitions: one long arrow extends from n = 3 down to n = 1 and is labeled E_1; a second shorter arrow extends from n = 3 down to n = 2 and is labeled E_2. No other labels, lines, text, or axes appear.
Energy level transitions for a hydrogen atom.
An electron in a hydrogen atom transitions from the \(n = 3\) energy level to the \(n = 1\) ground state, emitting a photon with energy \(E_1\). In a separate process, an electron in a hydrogen atom transitions from the \(n = 3\) level to the \(n = 2\) level, emitting a photon with energy \(E_2\). What is the ratio \(\dfrac{E_1}{E_2}\)?

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