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Chapter 6: Problem 95

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) \(\mathrm{Si},\) (b) \(\mathrm{Zn}\), (c) \(\mathrm{Zr},(\mathrm{d}) \mathrm{Sn}\) (e) \(\mathrm{Ba},(\mathrm{f}) \mathrm{Tl}\)

Short Answer

Expert verified
(a) Si: electron configuration \(1s^2 2s^2 2p^6 3s^2 3p^2\), 2 unpaired electrons; (b) Zn: electron configuration \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10}\), 0 unpaired electrons; (c) Zr: electron configuration \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^2\), 2 unpaired electrons; (d) Sn: electron configuration \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^2\), 2 unpaired electrons; (e) Ba: electron configuration \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 6s^2\), 2 unpaired electrons; (f) Tl: electron configuration \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^{10} 6p^1\), 1 unpaired electron.

Step by step solution

01

(a) Silicon (Si) Electron Configuration and Unpaired Electrons

Silicon's atomic number is 14. The electron configuration follows the order: 1s, 2s, 2p, 3s, 3p. Therefore, Silicon's electron configuration is: 1s虏 2s虏 2p鈦� 3s虏 3p虏. To determine the unpaired electrons, we look at the highest energy level subshell (3p). There are two unpaired electrons in the 3p subshell.
02

(b) Zinc (Zn) Electron Configuration and Unpaired Electrons

Zinc's atomic number is 30. The electron configuration follows the order: 1s, 2s, 2p, 3s, 3p, 4s, 3d. Therefore, Zinc's electron configuration is: 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鹿鈦�. Zinc has no unpaired electrons (all subshells are filled).
03

(c) Zirconium (Zr) Electron Configuration and Unpaired Electrons

Zirconium's atomic number is 40. The electron configuration follows the order: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d. Therefore, Zirconium's electron configuration is: 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鹿鈦� 4p鈦� 5s虏 4d虏. To determine the unpaired electrons, we look at the highest energy level subshell (4d). There are two unpaired electrons in the 4d subshell.
04

(d) Tin (Sn) Electron Configuration and Unpaired Electrons

Tin's atomic number is 50. The electron configuration follows the order: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p. Therefore, Tin's electron configuration is: 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鹿鈦� 4p鈦� 5s虏 4d鹿鈦� 5p虏. To determine the unpaired electrons, we look at the highest energy level subshell (5p). There are two unpaired electrons in the 5p subshell.
05

(e) Barium (Ba) Electron Configuration and Unpaired Electrons

Barium's atomic number is 56. The electron configuration follows the order: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s. Therefore, Barium's electron configuration is: 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鹿鈦� 4p鈦� 5s虏 4d鹿鈦� 5p鈦� 6s虏. To determine the unpaired electrons, we look at the highest energy level subshell (6s). There are two unpaired electrons in the 6s subshell.
06

(f) Thallium (Tl) Electron Configuration and Unpaired Electrons

Thallium's atomic number is 81. The electron configuration follows the order: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p. Therefore, Thallium's electron configuration is: 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鹿鈦� 4p鈦� 5s虏 4d鹿鈦� 5p鈦� 6s虏 4f鹿鈦� 5d鹿鈦� 6p鹿. To determine the unpaired electrons, we look at the highest energy level subshell (6p). There is one unpaired electron in the 6p subshell.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Periodic Table
The periodic table is a powerful tool for understanding the properties and behaviors of elements. It arranges all known elements in an order that highlights periodic trends, which are patterns in the properties of elements. Each element is placed according to its atomic number, which increases from left to right across a period. Also, elements are sorted into groups or columns that share similar chemical properties.
  • The periodic table helps predict the electronic configuration of an element, as elements in the same group often have similar outer shell electron arrangements.
  • For example, using the periodic table, you can easily find that Silicon (Si) is in Group 14, and like other elements in its group, it has four electrons in its outermost shell.
Thus, the periodic table not only provides valuable information about individual elements but also about overall chemical trends.
Unpaired Electrons
In the study of electron configuration, identifying unpaired electrons is crucial because they largely determine the magnetic properties and chemical reactivity of an element. Unpaired electrons are the electrons that exist alone in an orbital and are not paired with another electron with an opposite spin.
  • To determine the number of unpaired electrons, look at the highest energy orbitals in an element's configuration. If there are orbitals that are only partially filled, there may be unpaired electrons present.
  • For instance, in the element Silicon (Si), with the electron configuration \(1s^2 2s^2 2p^6 3s^2 3p^2\), the 3p subshell contains two electrons in different orbitals, thus resulting in two unpaired electrons.
The presence of unpaired electrons can make an element paramagnetic, meaning they are attracted to magnetic fields.
Atomic Number
The atomic number of an element is perhaps its most foundational property. It is simply the number of protons found in the nucleus of an atom of the element. This number also determines the element's identity and its placement on the periodic table.
  • The atomic number is denoted by \(Z\) and it tells us how many electrons are in a neutral atom, as it must balance the number of protons.
  • For example, Silicon has an atomic number of 14, which means it has 14 protons and, in a neutral state, 14 electrons.
The atomic number increases as we move across a period or down a group, leading to an increase in the atomic mass and the complexity of electron arrangements.

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Most popular questions from this chapter

Among the elementary subatomic particles of physics is the muon, which decays within a few nanoseconds after formation. The muon has a rest mass 206.8 times that of an electron. Calculate the de Broglie wavelength associated with a muon traveling at a velocity of \(8.85 \times 10^{5} \mathrm{~cm} / \mathrm{s}\)

(a) What is the relationship between the wavelength and the frequency of radiant energy? (b) Ozone in the upper atmosphere absorbs energy in the \(210-230-\mathrm{nm}\) range of the spectrum. In what region of the electromagnetic spectrum does this radiation occur?

Explain how the existence of line spectra is consistent with Bohr's theory of quantized energies for the electron in the hydrogen atom.

Certain elements emit light of a specific wavelength when they are burned. Historically, chemists used such emission wavelengths to determine whether specific elements were present in a sample. Characteristic wavelengths for some of the elements are given in the following table: \(\begin{array}{llll}\mathrm{Ag} & 328.1 \mathrm{nm} & \mathrm{Fe} & 372.0 \mathrm{nm} \\ \mathrm{Au} & 267.6 \mathrm{nm} & \mathrm{K} & 404.7 \mathrm{nm} \\ \mathrm{Ba} & 455.4 \mathrm{nm} & \mathrm{Mg} & 285.2 \mathrm{nm} \\ \mathrm{Ca} & 422.7 \mathrm{nm} & \mathrm{Na} & 589.6 \mathrm{nm} \\ \mathrm{Cu} & 324.8 \mathrm{nm} & \mathrm{Ni} & 341.5 \mathrm{nm}\end{array}\) (a) Determine which elements emit radiation in the visible part of the spectrum. (b) Which element emits photons of highest energy? Of lowest energy? (c) When burned, a sample of an unknown substance is found to emit light of frequency \(6.59 \times 10^{14} \mathrm{~s}^{-1} .\) Which of these elements is probably in the sample?

The rays of the Sun that cause tanning and burning are in the ultraviolet portion of the electromagnetic spectrum. These rays are categorized by wavelength. So-called UV-A radiation has wavelengths in the range of \(320-380 \mathrm{nm},\) whereas \(\mathrm{UV}-\mathrm{B}\) radiation has wavelengths in the range of \(290-320 \mathrm{nm}\). (a) Calculate the frequency of light that has a wavelength of \(320 \mathrm{nm}\). (b) Calculate the energy of a mole of 320 -nm photons. (c) Which are more energetic, photons of UV-A radiation or photons of UV-B radiation? (d) The UV-B radiation from the Sun is considered a greater cause of sunburn in humans than is UV-A radiation. Is this observation consistent with your answer to part \((c)\) ?
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