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Chapter 6: Problem 80

The following electron configurations represent excited states. Identify the element and write its ground-state condensed electron configuration. (a) \(1 s^{2} 2 s^{2} 2 p^{4} 3 s^{1}\) (b) \([\mathrm{Ne}] 3 s^{1} 3 p^{4} 4 p^{1}\) (c) \([\mathrm{Ar}] 4 s^{2} 3 d^{6} 4 p^{1}\)

Short Answer

Expert verified
The short answer based on the provided solution is: (a) Fluorine (F): \(1 s^2 2 s^2 2 p^6 3 s^1\) (b) Sulfur (S): \([\mathrm{Ne}]3 s^2 3 p^6\) (c) Cobalt (Co): \([\mathrm{Ar}] 4 s^2 3 d^{10} 4 p^1\)

Step by step solution

01

(a) Find the total number of electrons

For the given excited state configuration, \(1 s^2 2 s^2 2 p^4 3 s^1\), let's find the total number of electrons. \(1 s^2\) = 2 electrons \(2 s^2\) = 2 electrons \(2 p^4\) = 4 electrons \(3 s^1\) = 1 electron Total number of electrons = 2 + 2 + 4 + 1 = 9 electrons
02

(a) Write the ground-state electron configuration

For 9 electrons, the ground-state electron configuration is: \(1 s^2 2 s^2 2 p^6 3 s^1\)
03

(a) Identify the element

The element with an atomic number (number of protons and electrons) of 9 is fluorine (F).
04

(b) Find the total number of electrons

For the given excited state configuration, \([\mathrm{Ne}] 3 s^1 3 p^4 4 p^1\), let's find the total number of electrons. Neon (Ne) has 10 electrons, so we start there and add the electrons from the configuration. \(3 s^1\) = 1 electron \(3 p^4\) = 4 electrons \(4 p^1\) = 1 electron Total number of electrons = 10 (Ne) + 1 + 4 + 1 = 16 electrons
05

(b) Write the ground-state electron configuration

For 16 electrons, the ground-state electron configuration is: \([\mathrm{Ne}]3 s^2 3 p^6\)
06

(b) Identify the element

The element with an atomic number of 16 is sulfur (S).
07

(c) Find the total number of electrons

For the given excited state configuration, \([\mathrm{Ar}] 4 s^2 3 d^6 4 p^1\), let's find the total number of electrons. Argon (Ar) has 18 electrons, so we start there and add the electrons from the configuration. \(4 s^2\) = 2 electrons \(3 d^6\) = 6 electrons \(4 p^1\) = 1 electron Total number of electrons = 18 (Ar) + 2 + 6 + 1 = 27 electrons
08

(c) Write the ground-state electron configuration

For 27 electrons, the ground-state electron configuration is: \([\mathrm{Ar}] 4 s^2 3 d^{10} 4 p^1\)
09

(c) Identify the element

The element with an atomic number of 27 is cobalt (Co). To summarize, the ground-state condensed electron configurations for the given excited state configurations are: (a) Fluorine (F): \(1 s^2 2 s^2 2 p^6 3 s^1\) (b) Sulfur (S): \([\mathrm{Ne}]3 s^2 3 p^6\) (c) Cobalt (Co): \([\mathrm{Ar}] 4 s^2 3 d^{10} 4 p^1\)

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Most popular questions from this chapter

The first 25 years of the twentieth century were momentous for the rapid pace of change in scientists' understanding of the nature of matter. (a) How did Rutherford's experiments on the scattering of \(\alpha\) particles by a gold foil set the stage for Bohr's theory of the hydrogen atom? (b) In what ways is de Broglie's hypothesis, as it applies to electrons, consistent with J. J. Thomson's conclusion that the electron has mass? In what sense is it consistent with proposals preceding Thomson's work that the cathode rays are a wave phenomenon?

Arrange the following kinds of electromagnetic radiation in order of increasing wavelength: infrared, green light, red light, radio waves, X rays, ultraviolet light.

Using the periodic table as a guide, write the condensed electron configuration and determine the number of unpaired electrons for the ground state of (a) $\mathrm{Cl},(\mathbf{b}) \mathrm{Al},(\mathbf{c}) \mathrm{Zr},(\mathbf{d})\( As, (e) \)\mathrm{Sb},(\mathbf{f}) \mathrm{W}$

For orbitals that are symmetric but not spherical, the contour representations (as in Figures 6.23 and 6.24 ) suggest where nodal planes exist (that is, where the electron density is zero). For example, the \(p_{x}\) orbital has a node wherever \(x=0\). This equation is satisfied by all points on the \(y z\) plane, so this plane is called a nodal plane of the \(p_{x}\) orbital. (a) Determine the nodal plane of the \(p_{z}\) orbital. (b) What are the two nodal planes of the \(d_{x y}\) orbital? (c) What are the two nodal planes of the \(d_{x^{2}-y^{2}}\) orbital?

The series of emission lines of the hydrogen atom for which \(n_{f}=4\) is called the Brackett series. (a) Determine the region of the electromagnetic spectrum in which the lines of the Brackett series are observed. (b) Calculate the wavelengths of the first three lines in the Brackett series - those for which \(n_{i}=5,6,\) and 7.
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