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Ap Chem

This document provides problems related to electron configurations and photoelectron spectroscopy (PES). It asks students to: 1) Write the electron configuration, number of valence electrons, number of unpaired electrons, paramagnetic/diamagnetic nature, likely ions, and ion electron configurations for several elements. 2) Sketch the PES spectrum for aluminum using the spectrum for magnesium as a reference. 3) Sketch the PES spectrum for boron above the given spectra for hydrogen, helium, lithium, and beryllium. 4) Label the electron configurations of elements based on their PES spectra. 5) Explain why the 2s peak for beryllium is at

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Ethan Nguyen
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609 views2 pages

Ap Chem

This document provides problems related to electron configurations and photoelectron spectroscopy (PES). It asks students to: 1) Write the electron configuration, number of valence electrons, number of unpaired electrons, paramagnetic/diamagnetic nature, likely ions, and ion electron configurations for several elements. 2) Sketch the PES spectrum for aluminum using the spectrum for magnesium as a reference. 3) Sketch the PES spectrum for boron above the given spectra for hydrogen, helium, lithium, and beryllium. 4) Label the electron configurations of elements based on their PES spectra. 5) Explain why the 2s peak for beryllium is at

Uploaded by

Ethan Nguyen
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
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Download as DOC, PDF, TXT or read online on Scribd
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South Pasadena • AP Chemistry Name

8 ▪ Atomic Theory Period Date

8.2 PROBLEMS – ELECTRON CONFIGURATION


1. For each of the following elements, write: (i) its short form ground state electron configuration, (ii) the
number of valence electrons, (iii) the number of unpaired electrons, (iv) whether it’s paramagnetic or
diamagnetic, (v) its most likely ion(s), and (vi) the short form electron configuration of its most likely ion.
Element Electron Configuration # Valence e− #Unpaired e− Para | Dia Likely Ion(s) Electron Configuration

Se [Ar] 4s2 3d10 4p4 6 2 Para Se2− [Ar] 4s2 3d10 4p6

In+ [Kr] 5s2 4d10


In [Kr] 5s2 4d10 5p1 3 1 Para
In3+ [Kr] 4d10

Ba [Xe] 6s2 2 0 Dia Ba2+ [Xe]

W [Xe] 6s2 4f14 5d4 2 4 Para W6+ [Xe] 4f14


Ag
exception [Kr] 5s1 4d10 1 1 Para Ag+ [Kr] 4d10

Cd [Kr] 5s2 4d10 2 0 Dia Cd2+ [Kr] 4d10

Sn2+ [Kr] 5s2 4d10


Sn [Kr] 5s2 4d10 5p2 4 2 Para
Sn4+ [Kr] 4d10

Xe [Kr] 5s2 4d10 5p6 8 0 Dia Xe6+ [Kr] 5s2 4d10

2. The PES spectrum for Mg is


shown. Sketch in the spectrum
for Al on the same axes.

3. The PES spectra of H,


He, Li, and Be are given.
Sketch in the spectrum
for B above the other
spectra.

4. Label each of the 25 20 15 10 5 0


following spectra using Binding Energy (MJ/mol)
electron configuration notation
(1s2, 2s2, etc.) and determine the identity of each element.

2p

1s 2s
Ne

2p
1s 2s
F

1s 2s2p
O
1s 2p
2s
N
1s 2s 2p
C
1s 2s 2p
B

90 80 70 60 50 40 30 20 5 0
Binding
Energy (MJ/mol)

5. Which of the following best explains the relative positioning and intensity of the 2s peaks in the following
spectra?

(A) Be has a
greater nuclear charge than Li and more electrons in the 2s orbital
(B) Be electrons experience greater electron-electron repulsions than Li electrons
(C) Li has a greater pull from the nucleus on the 2s electrons, so they are harder to remove
(D) Li has greater electron shielding by the 1s orbital, so the 2s electrons are easier to remove

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