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Chapter 7: Problem 92

Identify the following elements. a. An excited state of this element has the electron configuration \(1 s^{2} 2 s^{2} 2 p^{5} 3 s^{1}\). b. The ground-state electron configuration is [Ne] \(3 s^{2} 3 p^{4}\). c. An excited state of this element has the electron configuration \([\mathrm{Kr}] 5 s^{2} 4 d^{6} 5 p^{2} 6 s^{1}\) d. The ground-state electron configuration contains three unpaired \(6 p\) electrons.

Short Answer

Expert verified
(a) Neon (in an excited state) (b) Sulfur (in its ground state) (c) Silver (in an excited state) (d) Praseodymium (with three unpaired 6p electrons in its ground state)

Step by step solution

01

Count the electrons

Count the total number of electrons in the excited state electron configuration: \(1s^2: 2 \ electrons \\ 2s^2: 2 \ electrons \\ 2p^5: 5 \ electrons \\ 3s^1: 1 \ electron \) Now add the electrons: \\ \(2 + 2 + 5 + 1 = 10\) \\ There are 10 electrons in the excited state.
02

Identify the element

Using the periodic table, find the element with an atomic number (number of electrons) equal to 10. The element with an atomic number of 10 is Neon (Ne). Answer (a): Neon (in an excited state) #b. Ground state: [Ne] \(3s^2 \ 3p^4\)#
03

Count the electrons

Count the total number of electrons in the ground state electron configuration: \([Ne] : 10 \ electrons \\ 3s^2: 2 \ electrons \\ 3p^4: 4 \ electrons \) Now add the electrons: \\ \(10 + 2 + 4 = 16\) \\ There are 16 electrons in the ground state.
04

Identify the element

Using the periodic table, find the element with an atomic number (number of electrons) equal to 16. The element with an atomic number of 16 is Sulfur (S). Answer (b): Sulfur (in its ground state) #c. Excited state: \([\mathrm{Kr}] \ 5s^2 \ 4d^6 \ 5p^2 \ 6s^1\)#
05

Count the electrons

Count the total number of electrons in the excited state electron configuration: \([\mathrm{Kr}]:36 \ electrons \\ 5s^2: 2 \ electrons \\ 4d^6: 6 \ electrons \\ 5p^2: 2 \ electrons \\ 6s^1: 1 \ electron \) Now add the electrons: \\ \(36 + 2 + 6 + 2 + 1 = 47\) \\ There are 47 electrons in the excited state.
06

Identify the element

Using the periodic table, find the element with an atomic number (number of electrons) equal to 47. The element with an atomic number of 47 is Silver (Ag). Answer (c): Silver (in an excited state) #d. Ground state: three unpaired 6p electrons#
07

Count the electrons

With three unpaired 6p electrons, the ground state electron configuration is [Xe] \(6s^2 \ 6p^3\), where Xe is the noble gas Xenon with 54 electrons. Now count the total number of electrons in the ground state electron configuration: \([Xe]: 54 \ electrons \\ 6s^2: 2 \ electrons \\ 6p^3: 3 \ electrons \) Now add the electrons: \\ \(54 + 2 + 3 = 59\) \\ There are 59 electrons in the ground state.
08

Identify the element

Using the periodic table, find the element with an atomic number (number of electrons) equal to 59. The element with an atomic number of 59 is Praseodymium (Pr). Answer (d): Praseodymium (with three unpaired 6p electrons in its ground state)

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