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anonymous

  • one year ago

Consider the following energy levels of a hypothetical atom: E4 -1.41 x 10^-19 J E3 -4.81 x 10-19 J E2 -1.15 x 10-18 J E1 -1.65 x 10 -18 J (a) What is the wavelength of the photon needed to excite an electron from E1 to E4?

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  1. aaronq
    • one year ago
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    First find the difference in energy between the levels, next use \(E=\dfrac{hc}{\lambda}\)

  2. anonymous
    • one year ago
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    (b) What is the energy (in joules) a photon must have in order to excite an electron from E2 to E3? (c) When an electron drops from the E3 level to the E1 level, the atom is said to undergo emission. Calculate the wavelength of the photon emitted in this process.

  3. aaronq
    • one year ago
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    It's pretty much all the same concept, find the energy difference between the energy levels and use Planck's equation.

  4. anonymous
    • one year ago
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    \[\frac{ 6.626 x 10^{-34} J/s x 3.0X10^{8}m/s }{ (-1.65 x10^{-18})-(-1.41 x 10^{-19}J) }\]

  5. aaronq
    • one year ago
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    the energy difference should be positive (just add absolute value bars), but yeah that's good for the first one

  6. anonymous
    • one year ago
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    0.000000132

  7. anonymous
    • one year ago
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    1.32 x 10^-7

  8. aaronq
    • one year ago
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    idk, sorry i can't check your answers, just put sometime into learning how to use your calc, the set up is correct.

  9. anonymous
    • one year ago
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    I think that's the right answer. I'm confused how to set up b since it's asking for energy instead of wavelength.

  10. aaronq
    • one year ago
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    it's just asking for the difference in energy

  11. aaronq
    • one year ago
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    no need to use Planck's equation here

  12. anonymous
    • one year ago
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    But you would use it for c right?

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