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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
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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Michele_Laino
 one year ago
Best ResponseYou've already chosen the best response.1here we have to compute four energies, namely we have to apply this formula: \[E = \frac{{hc}}{\lambda }\]

Michele_Laino
 one year ago
Best ResponseYou've already chosen the best response.1so case red photon: \[E = \frac{{hc}}{\lambda } = \frac{{6.62 \times {{10}^{  34}}3 \times {{10}^8}}}{{770 \times {{10}^{  9}}}} = ...joules\]

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0i am confused... what does this mean? 10^34 3 ?

Michele_Laino
 one year ago
Best ResponseYou've already chosen the best response.1oops.. sorry: \[E = \frac{{hc}}{\lambda } = \frac{{6.62 \times {{10}^{  34}} \times 3 \times {{10}^8}}}{{770 \times {{10}^{  9}}}} = ...joules\]

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0oh! okie! so we get 2.579E19

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0does that mean choice A is our soluition?

Michele_Laino
 one year ago
Best ResponseYou've already chosen the best response.1no, we have to to the same computation for other wavelength. case green photon: \[E = \frac{{hc}}{\lambda } = \frac{{6.62 \times {{10}^{  34}} \times 3 \times {{10}^8}}}{{550 \times {{10}^{  9}}}} = ...joules\]

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0ok! so we get 3.61E19

Michele_Laino
 one year ago
Best ResponseYou've already chosen the best response.1case yellow photon: \[E = \frac{{hc}}{\lambda } = \frac{{6.62 \times {{10}^{  34}} \times 3 \times {{10}^8}}}{{590 \times {{10}^{  9}}}} = ...joules\]

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0and we get 3.366E19!

Michele_Laino
 one year ago
Best ResponseYou've already chosen the best response.1finally, case blue photon: \[E = \frac{{hc}}{\lambda } = \frac{{6.62 \times {{10}^{  34}} \times 3 \times {{10}^8}}}{{450 \times {{10}^{  9}}}} = ...joules\]

Michele_Laino
 one year ago
Best ResponseYou've already chosen the best response.1reassuming, we have these subsequent energies: 2.579E19 J, 3.61E19 J, 3.366E19 J, 4.42E19 J. which is the greatest one?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0the last! so our solution is choice D?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0oh wait oops sorry it is the first, right? so chocie A is our solution?

Michele_Laino
 one year ago
Best ResponseYou've already chosen the best response.1I think that 4.42 is greater than 2.579

Michele_Laino
 one year ago
Best ResponseYou've already chosen the best response.1that is an exponential, all our energies have 10^(19) as exponential

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0oh so our solution is still choice D?

Michele_Laino
 one year ago
Best ResponseYou've already chosen the best response.1yes! that's right!
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