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AP Physics 2
15.3 Emission and Absorption Spectra
15.2 The Bohr Model of Atomic Structure
IntermediateMCQMathematicalConceptual14.6k
An energy-level diagram with four horizontal line segments representing atomic energy levels, stacked vertically from lowest to highest energy. The vertical axis is labeled 'Energy (eV)'. The lowest line is labeled 'n = 1' with energy value '-10.0 eV'. The second line is labeled 'n = 2' with energy value '-5.0 eV'. The third line is labeled 'n = 3' with energy value '-2.0 eV'. The top line is labeled 'n = 4' with energy value '-1.0 eV'. No other lines, arrows, or text appear.
Energy levels of the hypothetical atom.
An energy-level diagram for a hypothetical atom is shown, with energy values labeled in electron-volts (\(\text{eV}\)). A sample of gas containing these atoms is excited and emits light as the electrons transition between energy levels. One prominent line in the emission spectrum corresponds to a photon with a wavelength of \(\lambda = 413 \text{ nm}\). Which transition between energy levels accounts for the emission of this photon?

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