Fictitious element X has the electron energy levels shown in the figure below, i
ID: 1638210 • Letter: F
Question
Fictitious element X has the electron energy levels shown in the figure below, in which E1 = -9.8 eV, E2 = -4.5 eV, and E3 = -3 eV. The dashed line is not an energy level, but rather just shows the location of zero energy.
(a) How much energy does it take to ionize, or remove, an electron that is in the ground state of this atom?
_______ eV
(b) Calculate the (i) shortest and (ii) next-shortest wavelengths observed in the absorption spectrum of element X. Think about how energy is related to wavelength when you decide which wavelength will be the shortest. (Enter these into the table below.)
(c) Specify whether each of your wavelengths in part b corresponds to ultraviolet, visible, or infrared light.
(i) shortest (ii) next shortest
(nm)
Explanation / Answer
(A) E1 = - 9.8 eV
to ionise from ground level,
minimum 9.8 eV energy is needed.
(B) (i) for shortest, energy will be maximum.
deltaE= 9.8 eV
wavelength = h c / E = 1240 eV-nm / 9.8eV
Shortest wavelength = 126.5 nm
(ii) next shortest.
delatE = - 4.5 - (-9.8) = 5.3 eV
wavelength = 1240/5.3 = 234 nm
(C) both are in ultraviolet region.
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