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Chapter 9: Problem 5

Based on the spectrum in Model 2, estimate the number of electrons at each of the three energy levels in Ne. Explain your reasoning clearly. (Hint: Recall that the total number of electrons should equal the number of electrons in a Ne atom.)

Short Answer

Expert verified
Based on the standard electron configuration of Neon (Ne) and without an actual spectrum provided: The first energy level has 2 electrons, the second has 2 electrons, and the third level has 6 electrons.

Step by step solution

01

Revisiting the Electron Configuration

Neon (Ne), element number 10 on the periodic table, has a total of 10 electrons which need to be distributed in energy levels. The electron configuration of Neon is \[1s^2, 2s^2, 2p^6\].
02

Examining the Spectrum

Based on the spectrum in Model 2, there should be three energy levels to distribute the electrons. However, a detailed spectrum is not provided here. Normally, this would involve looking at the intensity of the spectral lines which should correspond to the number of electrons transitioning from, or to, each energy level.
03

Distributing the Electrons

Electrons will fill the lowest energy levels first. So, according to standard electron configuration, the first energy level will have 2 electrons (from the 1s orbital), the second energy level would include 2 more electrons (from the 2s orbital), and the third energy level would have 6 electrons (from the 2p orbital).
04

Recap and explanation

This solution assumes the standard distribution of electrons among atomic energy levels. The specific details could be slightly altered based on the characteristics of the spectrum in model 2. The intensity and presence of spectral lines influence the actual electron transitions between energy levels, which in turn might affect the measurable electron distribution.

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Most popular questions from this chapter

Given the shell model and the stated assumptions in Model 1: a) how many peaks should there be in the photoelectron spectrum of Ne? b) predict the relative size of the peaks in the photoelectron spectrum. (Note that \(2 / 10\) of the electrons are in \(n=1\) shell and \(8 / 10\) of the electrons are in \(n=2\) shell.)

The first ionization energy of Ne is \(2.08 \mathrm{MJ} / \mathrm{mole}\). Thus one of the peaks in the photoelectron spectrum of Ne will be at \(2.08 \mathrm{MJ} / \mathrm{mole}\). At this point we do not have a good way of determining a very accurate estimate of what the energy of the other peak is, but we know that it will be very different than \(2.08 \mathrm{MJ} / \mathrm{mole}\). Will the other peak be at a much higher or much lower energy than \(2.08\) MJ/mole? Explain your reasoning.
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