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Chapter 7: Problem 91

The elements Si, Ga, As, Ge, Al, Cd, S, and Se are all used in the manufacture of various semiconductor devices. Write the expected electron configuration for these atoms.

Short Answer

Expert verified
The electron configurations for the given elements are as follows: 1. Silicon (Si) - \(1s^1 2s^2 2p^6 3s^2 3p^2\) 2. Gallium (Ga) - \(1s^1 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^1\) 3. Arsenic (As) - \(1s^1 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^3\) 4. Germanium (Ge) - \(1s^1 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^2\) 5. Aluminum (Al) - \(1s^1 2s^2 2p^6 3s^2 3p^1\) 6. Cadmium (Cd) - \(1s^1 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10}\) 7. Sulfur (S) - \(1s^1 2s^2 2p^6 3s^2 3p^4\) 8. Selenium (Se) - \(1s^1 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^4\)

Step by step solution

01

Identify Element's Position in the Periodic Table

Look for the position of the given elements in the periodic table. Knowing their positions will help us to determine the electron configurations.
02

Determine Electrons and Atom's Levels

Calculate the total number of electrons in each atom and determine the filling order of their electron orbitals according to the periodic table. The filling order of electron orbitals is as follows: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, and so on.
03

Write Electron Configurations

Using the filling order of electron orbitals, write down the electron configurations for each element. 1. Silicon (Si) (Atomic Number: 14) - 1s¹ 2s² 2p⁶ 3s² 3p² 2. Gallium (Ga) (Atomic Number: 31) - 1s¹ 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p¹ 3. Arsenic (As) (Atomic Number: 33) - 1s¹ 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p³ 4. Germanium (Ge) (Atomic Number: 32) - 1s¹ 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p² 5. Aluminum (Al) (Atomic Number: 13) - 1s¹ 2s² 2p⁶ 3s² 3p¹ 6. Cadmium (Cd) (Atomic Number: 48) - 1s¹ 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 7. Sulfur (S) (Atomic Number: 16) - 1s¹ 2s² 2p⁶ 3s² 3p⁴ 8. Selenium (Se) (Atomic Number: 34) - 1s¹ 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁴ The electron configurations for Si, Ga, As, Ge, Al, Cd, S, and Se are now complete.

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Most popular questions from this chapter

Which of the following sets of quantum numbers are not allowed? For each incorrect set, state why it is incorrect. a. \(n=3, \ell=3, m_{\ell}=0, m_{s}=-\frac{1}{2}\) b. \(n=4, \ell=3, m_{\ell}=2, m_{s}=-\frac{1}{2}\) c. \(n=4, \ell=1, m_{\ell}=1, m_{s}=+\frac{1}{2}\) d. \(n=2, \ell=1, m_{\ell}=-1, m_{s}=-1\) e. \(n=5, \ell=-4, m_{\ell}=2, m_{s}=+\frac{1}{2}\) f. \(n=3, \ell=1, m_{\ell}=2, m_{s}=-\frac{1}{2}\)

The wave function for the 2\(p_{z}\) orbital in the hydrogen atom is $$\psi_{2 p_{z}}=\frac{1}{4 \sqrt{2 \pi}}\left(\frac{Z}{a_{0}}\right)^{3 / 2} \sigma \mathrm{e}^{-\sigma / 2} \cos \theta$$ where \(a_{0}\) is the value for the radius of the first Bohr orbit in meters \(\left(5.29 \times 10^{-11}\right), \sigma\) is \(Z\left(r / a_{0}\right), r\) is the value for the distance from the nucleus in meters, and \(\theta\) is an angle. Calculate the value of \(\psi_{2 p_{z}}^{2}\) at \(r=a_{0}\) for \(\theta=0^{\circ}\left(z \text { axis ) and for } \theta=90^{\circ}\right.\) (xy plane).

Using the Heisenberg uncertainty principle, calculate \(\Delta x\) for each of the following. a. an electron with \(\Delta v=0.100 \mathrm{m} / \mathrm{s}\) b. a baseball (mass \(=145 \mathrm{g} )\) with $\Delta v=0.100 \mathrm{m} / \mathrm{s}$ c. How does the answer in part a compare with the size of a hydrogen atom? d. How does the answer in part b correspond to the size of a baseball?

The electron affinities of the elements from aluminum to chlorine are \(-44,-120,-74,-200.4,\) and \(-384.7 \mathrm{kJ} / \mathrm{mol}\) respectively. Rationalize the trend in these values.

Arrange the following groups of atoms in order of increasing size. a. Te, S, Se b. K, Br, Ni c. Ba, Si, F
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