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anonymous

  • one year ago

Which of the following represents the greatest energy transition from a higher energy level to a lower one? A. emission of a red photon of 770 nm B. emission of a green photon of 550 nm C. emission of a yellow photon of 590 nm D. emission of a blue photon of 450 nm

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  1. Michele_Laino
    • one year ago
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    here we have to compute four energies, namely we have to apply this formula: \[E = \frac{{hc}}{\lambda }\]

  2. anonymous
    • one year ago
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    ok!

  3. Michele_Laino
    • one year ago
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    so case red photon: \[E = \frac{{hc}}{\lambda } = \frac{{6.62 \times {{10}^{ - 34}}3 \times {{10}^8}}}{{770 \times {{10}^{ - 9}}}} = ...joules\]

  4. anonymous
    • one year ago
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    i am confused... what does this mean? 10^-34 3 ?

  5. Michele_Laino
    • one year ago
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    oops.. sorry: \[E = \frac{{hc}}{\lambda } = \frac{{6.62 \times {{10}^{ - 34}} \times 3 \times {{10}^8}}}{{770 \times {{10}^{ - 9}}}} = ...joules\]

  6. anonymous
    • one year ago
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    oh! okie! so we get 2.579E-19

  7. Michele_Laino
    • one year ago
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    that's right!

  8. anonymous
    • one year ago
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    does that mean choice A is our soluition?

  9. Michele_Laino
    • one year ago
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    no, we have to to the same computation for other wavelength. case green photon: \[E = \frac{{hc}}{\lambda } = \frac{{6.62 \times {{10}^{ - 34}} \times 3 \times {{10}^8}}}{{550 \times {{10}^{ - 9}}}} = ...joules\]

  10. anonymous
    • one year ago
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    ok! so we get 3.61E-19

  11. Michele_Laino
    • one year ago
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    that's right!

  12. Michele_Laino
    • one year ago
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    case yellow photon: \[E = \frac{{hc}}{\lambda } = \frac{{6.62 \times {{10}^{ - 34}} \times 3 \times {{10}^8}}}{{590 \times {{10}^{ - 9}}}} = ...joules\]

  13. anonymous
    • one year ago
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    and we get 3.366E-19!

  14. Michele_Laino
    • one year ago
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    that's right!

  15. Michele_Laino
    • one year ago
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    finally, case blue photon: \[E = \frac{{hc}}{\lambda } = \frac{{6.62 \times {{10}^{ - 34}} \times 3 \times {{10}^8}}}{{450 \times {{10}^{ - 9}}}} = ...joules\]

  16. anonymous
    • one year ago
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    4.42E-19!

  17. Michele_Laino
    • one year ago
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    that's right!

  18. Michele_Laino
    • one year ago
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    reassuming, we have these subsequent energies: 2.579E-19 J, 3.61E-19 J, 3.366E-19 J, 4.42E-19 J. which is the greatest one?

  19. anonymous
    • one year ago
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    the last! so our solution is choice D?

  20. anonymous
    • one year ago
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    oh wait oops sorry it is the first, right? so chocie A is our solution?

  21. Michele_Laino
    • one year ago
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    I think that 4.42 is greater than 2.579

  22. anonymous
    • one year ago
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    but it is negative?

  23. anonymous
    • one year ago
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    E-19? :/

  24. Michele_Laino
    • one year ago
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    that is an exponential, all our energies have 10^(-19) as exponential

  25. anonymous
    • one year ago
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    oh so our solution is still choice D?

  26. Michele_Laino
    • one year ago
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    yes! that's right!

  27. anonymous
    • one year ago
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    yay! thanks:)

  28. Michele_Laino
    • one year ago
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    :)

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