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AP Chemistry
1.7 Periodic Trends
1.6 Photoelectron Spectroscopy
1.5 Atomic Structure and Electron Configuration
AdvancedMCQGraphicalConceptual17.9k
A grayscale figure containing two vertically stacked photoelectron spectra sharing identical axes. The horizontal axis is labeled 'Binding Energy (MJ/mol)' and decreases from left to right with scale markings at 100, 10, and 1. The vertical axis is labeled 'Relative Number of Electrons' with unit tick marks at 2, 4, and 6. The top panel is labeled 'Spectrum X' and displays three distinct solid vertical peak lines: the first peak is at 84.0 MJ/mol with a height of 2 units; the second peak is at 4.68 MJ/mol with a height of 2 units; the third peak is at 2.08 MJ/mol with a height of 6 units. The bottom panel is labeled 'Spectrum Y' and displays three distinct solid vertical peak lines: the first peak is at 104 MJ/mol with a height of 2 units; the second peak is at 6.84 MJ/mol with a height of 2 units; the third peak is at 3.67 MJ/mol with a height of 6 units. No other lines, labels, gridlines, or annotations appear.
Photoelectron spectra of two isoelectronic species showing relative electron counts versus binding energy.
The complete photoelectron spectra of two isoelectronic chemical species, gas-phase \(\text{Ne}\) and gas-phase \(\text{Na}^+\), are shown in the figure. Which of the following correctly identifies the spectrum that corresponds to \(\text{Na}^+\) and provides the best explanation for the difference in peak positions between the two spectra?

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