Calculate the wavelength of light emitted from a mol of photons as they transition from in the hydrogen atom.

The question is incomplete, here is the complete question:

How do you calculate the wavelength of the light emitted from a mole of photons as they transition from the n = 4 to the n = 1 principal energy level in the hydrogen atom. Recall that for hydrogen

The wavelength of 1 mole of photons for the given transition is

Explanation:

To calculate the change in energy, we use the equation:

Or,

where,

= initial energy level = 4

= final energy level = 1

Putting values in above equation, we get:

To calculate the wavelength of light for 1 mole of photons, we use the equation:

where,

= Avogadro's number =

h = Planck's constant =

c = speed of light =

= wavelength of light = ?

E = energy emitted =  

Putting values in above equation, we get:

Hence, the wavelength of 1 mole of photons for the given transition is

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sulfur belongs to group 16 because it can be found in nature whether it is in a free or combined state.

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