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    A particular hydrogen atom makes a transition from the energy level at −1.51 eV to the energy level at −0.85 eV

    What is the energy of the photon involved in this process?

    Do I add the energy or minus it to work it out? I know you minus it if a photon is emitted but I'm not sure if you add them when a photon is absorbed

    Thanks
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    (ooh the physics forum I feel like a traitor)

    fairly sure that it means the atom has lost energy toward the ground state
    therefor the photon is emmited so i would find the difference!
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    The energy change is the energy of the photon involved. So whether the hydrogen energy increases (photon absorbed) or decreases (photon emitted), its just the difference. The minus sign is just a convention.

    So in this case, the hydrogen has absorbed a photon of energy 1.51-0.85 = 0.66eV
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    (Original post by Geek1337)
    A particular hydrogen atom makes a transition from the energy level at −1.51 eV to the energy level at −0.85 eV

    What is the energy of the photon involved in this process?

    Do I add the energy or minus it to work it out? I know you minus it if a photon is emitted but I'm not sure if you add them when a photon is absorbed

    Thanks
    the hydrogen atom has moved from a lower energy to higher energy level so a photon must have been absorbed , -0.85+1.51= 0.66 ev . Now times this by 1 ev (1.6 * 10^{-19}) to get the energy which is in joules
 
 
 
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