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During an emission, electrons move from a higher energy orbital to a lower energy orbital. Which of the following are valid transitions that produce lines in the emission spectrum of Zn?
A) [Ar]4s23d10 → [Ar]4s13d11
B) [Ar]4s13d106s1 → [Ar]4s23d10
C) [Ar]4s23d10 → [Ar]4s23d104p2
D) [Ar]4s23d10 → [Ar]3d10
E) [Ar]3d10 → [Ar]4s23d10
F) [Ar]4s23d10 → [Ar]4s13d106s1
Scientists can analyze metals using the emission spectrum produced when the sample is introduced into the flame of an emission spectrometer. The flame provides the energy to excite the electrons of the metal atoms to higher energy states. When the electrons return to the ground state, lines of characteristic wavelengths are produced. The lines in the emission spectrum are characteristic of the metal because each atom's ground-state electron configuration is unique.
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Based on our data, we think this problem is relevant for Professor Davis & Chen's class at McMaster University.