Calculate the number of joules of potential energy required to ... | Filo
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\begin{tabular} { | l | } \hline Calculate the energy in joule... | Filo
\begin{tabular} { | l | } \hline Calculate the energy in joule... | Filo
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SOLVED: Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 to the n = 4 principal energy level. Then calculate the wavelength of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen:En = -2.18 x 10^-18 J(1/n^2)My work:ni = 1nf = 4E = -2.18 x 10^-18 J [(1/1^2) - (1/4^2)] = -2.18 x 10^-18 J [0.9375] = -2.04 x 10^-18 JThe answer is
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