Why Is the Calculated Wavelength Incorrect in This Hydrogen Atom Problem?

AI Thread Summary
The discussion centers on calculating the energy of an electron in the first excited state of a hydrogen atom and the subsequent wavelength of emitted photons. The correct energy formula is E = -13.6 (z/n)^2, but confusion arises regarding the calculation of wavelength using E = hc/λ. It is clarified that the question likely pertains to the wavelength of the photon emitted when the electron transitions to the ground state, not the energy of the excited state itself. Additionally, the de Broglie wavelength formula is mentioned as inappropriate for this context. Accurate understanding of the problem's requirements is crucial for correct calculations.
Suyash Singh

Homework Statement


Calculate energy of electron in first excited state of hydrogen atom.

Homework Equations


n=2
when i use E=-13.6 (z/n)^2
and then use E=hc/lamda(wavelength)
then wavelength is coming wrong

The Attempt at a Solution


the correct answer is 6.68 armstrong.
 
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Ångström (not armstrong) is a unit of length, not a unit of energy. It is likely that you are not being asked what you have stated that you are being asked about here. The question is likely what the wavelength of the photon emitted when the electron in the first excited state of hydrogen transits to the ground state. This is not the same thing as the energy in the first excited state.
 
Suyash Singh said:
when i use E=-13.6 (z/n)^2
and then use E=hc/lamda(wavelength)
then wavelength is coming wrong
Are you trying to find the deBroglie wavelength of the electron when it is in the first excited state? If so, the formula E = hc/λ is not the correct formula.
 
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