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hbk69

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## Homework Statement

Question 1)

For absorption transitions:

At n=1 the energy is 0.0eV (electron volts), at n=2 the energy is 3eV, at n=3=5eV

Question 2)

For emission transisions:

At n=1 the energy is 0.0eV, n=2 energy is 3eV and at n=3 energy is 5eV

Question 3)

The atom has energy levels n=1(0eV),n=2(2eV) and n=3(5eV). A photon has energy E=3eV which corresponds to spectral line with λ=414nm. Where would this spectral line be observed? absorption spectrum, emission spectrum, both or neither?

## Homework Equations

ΔE between the energy levels for an absorption transition ΔE= E1 - E2 etc..

ΔE between the energy levels for an emission transition ΔE=E3 - E2 etc..

λ=c*h/ΔE

## The Attempt at a Solution

Question 1)

So to find the difference in energy ΔE between the energy levels for an absorption transition at ΔE=E1 - E2, then ΔE= 0.0eV - 3eV = -3eV but in my notes this answer is positive 3eV what am i doing wrong?

Question 2)

To find emission transition at ΔE=E3 - E2 , then ΔE= 5eV-3eV= 2eV but in my lecture notes the answer given is negative -2eV i do not see how this is possible and where i went wrong?

Question 3)

Since E=3eV, I would assume it would be an emission spectrum because ΔE=E3 - E2=3eV but shouldn't the 3eV be negative because for an emission transion ΔE=E3 - E2 in question 2 the answer given was negative.