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Chapter 7: Problem 90

Write the ground-state electron configurations for the following elements: Ge, Fe, Zn, Ni, W, TI.

Short Answer

Expert verified
The ground-state electron configurations for the elements are Ge : [Ar] 3d10 4s2 4p2, Fe : [Ar] 3d6 4s2, Zn : [Ar] 3d10 4s2, Ni : [Ar] 3d8 4s2, W : [Xe] 4f14 5d4 6s2, TI : [Xe] 4f14 5d10 6s2 6p1

Step by step solution

01

Identifying the Element in the Periodic Table

The place of an atom in the periodic table determines the electron configuration. Ge (Germanium) is in group 14, period 4. Fe (Iron) is in group 8, period 4. Zn (Zinc) is in group 12, period 4. Ni (Nickel) is in group 10, period 4. W (Tungsten) is in group 6, period 6. TI (Thallium) is in group 13, period 6.
02

Writing Electron Configurations

Write the electron configurations using the positions in the periodic table. \n\n - Ge : [Ar] 3d10 4s2 4p2 \n - Fe : [Ar] 3d6 4s2 \n - Zn : [Ar] 3d10 4s2 \n - Ni : [Ar] 3d8 4s2 \n - W : [Xe] 4f14 5d4 6s2 \n - TI : [Xe] 4f14 5d10 6s2 6p1
03

Verification

Check if sum of superscripts equal each element's atomic number. For instance, Ge has atomic number 32, hence 18 (from [Ar])+10 (from 3d10)+ 2 (from 4s2)+ 2 (from 4p2) = 32.

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Most popular questions from this chapter

Use the Aufbau principle to obtain the ground-state electron configuration of selenium.

Discuss the similarities and differences between a \(1 s\) and a \(2 s\) orbital.

An electron in an excited state in a hydrogen atom can return to the ground state in two different ways: (a) via a direct transition in which a photon of wavelength \(\lambda_{1}\) is emitted and (b) via an intermediate excited state reached by the emission of a photon of wavelength \(\lambda_{2}\). This intermediate excited state then decays to the ground state by emitting another photon of wavelength \(\lambda_{3}\). Derive an equation that relates \(\lambda_{1}\) to \(\lambda_{2}\) and \(\lambda_{3}\)

$$ \begin{array}{lccccc} \lambda(\mathrm{nm}) & 405 & 435.8 & 480 & 520 & 577.7 \\ \hline \mathrm{KE}(\mathrm{J}) & 2.360 \times & 2.029 \times & 1.643 \times & 1.417 \times & 1.067 \times \\ & 10^{-19} & 10^{-19} & 10^{-19} & 10^{-19} & 10^{-19} \end{array} $$ (a) What is the lowest possible value of the principal quantum number \((n)\) when the angular momentum quantum number \((\ell)\) is \(1 ?\) (b) What are the possible values of the angular momentum quantum number ( \(\ell\) ) when the magnetic quantum number \(\left(m_{\ell}\right)\) is 0 , given than \(n \leq 4 ?\)

Indicate the total number of (a) \(p\) electrons in \(\mathrm{N}\) \((Z=7),(b) s\) electrons in \(\operatorname{Si}(Z=14),\) and (c) \(3 d\) electrons in \(\mathrm{S}(Z=16)\)
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