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Chapter 9: Problem 2

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.

Short Answer

Expert verified
The other peak should be at a much higher energy level than the first peak of 2.08 MJ/mole, given the principles of ionization energy and electron configuration of neon.

Step by step solution

01

Understand Ionization Energy

Ionization energy is the energy required to remove an electron from an atom or molecule. The first ionization energy refers to the energy needed to remove the first, outermost electron. Because of the stable configuration of noble gases, the first ionization energy of Neon is high, at 2.08 MJ/mole.
02

Evaluate Scenarios

As we move towards the core of an atom, the electrons are more tightly held by the nucleus. Therefore, removing the next electron would likely require more energy. So, the other peak representing the second ionization energy should be at a higher energy level.
03

Conclude

Considering the basic principles of ionization energy and the electron configuration of neon, the other peak should represent a much higher energy level than the first peak of 2.08 MJ/mole.

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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.)

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.)
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