Consider the following energy levels of a hypothetical atom. E 4 _________ -1.0

Question

Consider the following energy levels of a hypothetical atom.

E4 _________ -1.0 ? 10?19 J
E3 _________ -5.0 ? 10?19 J
E2 _________ -10 ? 10?19 J
E1 _________ -15 ? 10?19 J

(a) What is the wavelength of the photon needed to excite an electron from E1 to E4? (in nm)

(b) What is the energy (in joules) a photon must have in order to excite an electron from. E2 to E3? (in J)

(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. (in nm)

Explanation / Answer

A) From E1 to E4

energy diffrence is (15-1)*10^-19 = 14*10^-19

but E = h*c/lamda = 14*10^-19

wavelength lamda = h*c/(14*10^-19) = (6.625*10^-34*3*10^8)/(14*10^-19) = 1.419 *10^-7 m = 141.9 nm

B) E = (10-5)*10^-19 = 5*10^-19 J

C) energy diffrence is (15-5)*10^-19 = 10*10^-19

but E = h*c/lamda = 10*10^-19lamda = h*c/(10*10^-19) = (6.625*10^-34*3*10^8)/(10*10^-19) = 1.987 *10^-7 m = 198.7 nm

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