The figure above represents some of the lower energy levels of the hydrogen atom in simplified form.
If the transition of an electron from $E_{4}$ to $E_{2}$ were associated with the emission of blue light, which one of the following transitions could be associated with the emission of red light?

E_{4}

E_{1}

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E_{3}

E_{1}

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E_{3}

E_{2}

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E_{1}

E_{3}

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Solution

The correct option is C $E_{3}$ to $E_{2}$
Wavelength of blue is less than wavelength of red.
For transition into $n = 2$ (Balmer series), wavelength is inversely proportional to n
Hence, for wavelength to increase, $n$ should be less than $4$
Therefore, $n = 3$

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The figure above represents some of the lower energy levels of the hydrogen atom in simplified form.If the transition of an electron from E4 to E2 were associated with the emission of blue light, which one of the following transitions could be associated with the emission of red light?

The correct option is C E3 to E2Wavelength of blue is less than wavelength of red.For transition into n=2 (Balmer series), wavelength is inversely proportional to nHence, for wavelength to increase, n should be less than 4Therefore, n=3

The figure above represents some of the lower energy levels of the hydrogen atom in simplified form.
If the transition of an electron from $E_{4}$ to $E_{2}$ were associated with the emission of blue light, which one of the following transitions could be associated with the emission of red light?

The correct option is C $E_{3}$ to $E_{2}$
Wavelength of blue is less than wavelength of red.
For transition into $n = 2$ (Balmer series), wavelength is inversely proportional to n
Hence, for wavelength to increase, $n$ should be less than $4$
Therefore, $n = 3$