Be sure to answer all parts. Consider the following energy levels of a hypotheti

Question

Be sure to answer all parts. Consider the following energy levels of a hypothetical atom: E4 -1.81 x 10^-19J E3 -7.51 x10^-19J E2-1.25x10^-18J E1 -1.85 x 10^-18J (a) What is the wavelength of the photon needed to excite an electron from E1 to E4? x10 m (b) What is the energy (in joules) a photon must have in order to excite an electron from E2 to E3? x10 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. x 10 m

Explanation / Answer

a) energy required = E4-E1 = -1.81*10^-19 - (-1.85*10^-18 )

                   = 16.69 *10^-19 J

hc/lamda = E

6.626*10^-34*3*10^8 / lamda = 16.69 *10^-19

lamda = 1.19101258e-7 m = 119 nm

b) energy of the photon =E3-E2

              = -7.51*10^-19 - (-1.25*10^-18)

              = 4.99*10^-19J

c) del E =hc/lamda

E3-E1 = 6.626*10^-34*3*10^8 / lamda

-7.51*10^-19 - (- 1.85*10^-18 ) = 6.626*10^-34*3*10^8 / lamda

lamda = 1.80873521e-7 m = 180nm

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