The figure below depicts the first four energy levels in a hydrogen atom. (Enter an unrounded answer.) n = 4 n = 3 n = 2 n = 1 Three transitions shown as arrows, n = 2 → n=1, n= 3 → n= 1, and n = 4 → n = 1, emit ultraviolet light and occur at wavelengths of 121.566 nm, 102.583 nm, and 97.524 nm , respectively. Find the frequency of light (in Hz) that would be emitted in a transition from the st labeled as n = 4 to the state labeled as n = 3.
The figure below depicts the first four energy levels in a hydrogen atom. (Enter an unrounded answer.) n = 4 n = 3 n = 2 n = 1 Three transitions shown as arrows, n = 2 → n=1, n= 3 → n= 1, and n = 4 → n = 1, emit ultraviolet light and occur at wavelengths of 121.566 nm, 102.583 nm, and 97.524 nm , respectively. Find the frequency of light (in Hz) that would be emitted in a transition from the st labeled as n = 4 to the state labeled as n = 3.
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answer the given picture. thank you.
Transcribed Image Text:The figure below depicts the first four energy levels in a hydrogen atom. (Enter an unrounded answer.)
n = 4
n = 3
n = 2
n = 1
Three transitions shown as arrows, n = 2→ n = 1, n = 3 → n = 1, and n = 4 → n= 1, emit ultraviolet light and occur at wavelengths of
121.566 nm, 102.583 nm, and 97.524 nm , respectively. Find the frequency of light (in Hz) that would be emitted in a transition from the state
labeled as n = 4 to the state labeled as n = 3.
Hz
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