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Chapter 7: Problem 110

How many unpaired electrons are present in each of the following in the ground state: \(\mathrm{O}, \mathrm{O}^{+}, \mathrm{O}^{-}, \mathrm{Os}, \mathrm{Zr}, \mathrm{S}, \mathrm{F}, \mathrm{Ar}\) ?

Short Answer

Expert verified
The number of unpaired electrons for each element in their ground state is as follows: \(\mathrm{O}\): 2 unpaired electrons, \(\mathrm{O}^{+}\): 1 unpaired electron, \(\mathrm{O}^{-}\): 3 unpaired electrons, \(\mathrm{Os}\): 2 unpaired electrons, \(\mathrm{Zr}\): 2 unpaired electrons, \(\mathrm{S}\): 2 unpaired electrons, \(\mathrm{F}\): 1 unpaired electron, and \(\mathrm{Ar}\): 0 unpaired electrons.

Step by step solution

01

Oxygen atom (O)

The electron configuration of Oxygen (\(\mathrm{O}\)) is \(1s^{2} 2s^{2} 2p^{4}\). There are two unpaired electrons in the 2p orbital.
02

Oxygen cation (O+)

The electron configuration of Oxygen cation (\(\mathrm{O}^{+}\)) is \(1s^{2} 2s^{2} 2p^{3}\). There is one unpaired electron in the 2p orbital.
03

Oxygen anion (O-)

The electron configuration of the Oxygen anion (\(\mathrm{O}^{-}\)) is \(1s^{2} 2s^{2} 2p^{5}\). There are three unpaired electrons in the 2p orbital.
04

Osmium atom (Os)

The electron configuration of Osmium (\(\mathrm{Os}\)) is \([Xe]6s^2 4f^{14} 5d^{6}\). There are two unpaired electrons in the 5d orbital.
05

Zirconium atom (Zr)

The electron configuration of Zirconium (\(\mathrm{Zr}\)) is \([Kr]5s^2 4d^{2}\). There are two unpaired electrons in the 4d orbital.
06

Sulfur atom (S)

The electron configuration of Sulfur (\(\mathrm{S}\)) is \(1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{4}\). There are two unpaired electrons in the 3p orbital.
07

Fluorine atom (F)

The electron configuration of Fluorine (\(\mathrm{F}\)) is \(1s^{2} 2s^{2} 2p^{5}\). There is one unpaired electron in the 2p orbital.
08

Argon atom (Ar)

The electron configuration of Argon (\(\mathrm{Ar}\)) is \(1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6}\). There are no unpaired electrons, as all orbitals are completely filled. Now, we have the number of unpaired electrons for each element: \(\mathrm{O}\): 2 unpaired electrons \(\mathrm{O}^{+}\): 1 unpaired electron \(\mathrm{O}^{-}\): 3 unpaired electrons \(\mathrm{Os}\): 2 unpaired electrons \(\mathrm{Zr}\): 2 unpaired electrons \(\mathrm{S}\): 2 unpaired electrons \(\mathrm{F}\): 1 unpaired electron \(\mathrm{Ar}\): 0 unpaired electrons

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Most popular questions from this chapter

X rays have wavelengths on the order of \(1 \times 10^{-10} \mathrm{m} .\) Calcu- late the energy of \(1.0 \times 10^{-10} \mathrm{m} \mathrm{X}\) rays in units of kilojoules per mole of \(\mathrm{X}\) rays. AM radio waves have wavelengths on the order of \(1 \times 10^{4} \mathrm{m}\) . Calculate the energy of \(1.0 \times 10^{4} \mathrm{m}\) radio waves in units of kilojoules per mole of radio waves. Consider that the bond energy of a carbon-carbon single bond found in organic compounds is 347 \(\mathrm{kJ} / \mathrm{mol}\) . Would \(\mathrm{x}\) rays and/or radio waves be able to disrupt organic compounds by breaking carbon-carbon single bonds?

Calculate the wavelength of light emitted when each of the following transitions occur in the hydrogen atom. What type of electromagnetic radiation is emitted in each transition? a. \(n=4 \rightarrow n=3\) b. \(n=5 \rightarrow n=4\) c. \(n=5 \rightarrow n=3\)

One of the visible lines in the hydrogen emission spectrum corresponds to the \(n=6\) to \(n=2\) electronic transition. What color light is this transition? See Exercise 150 .

Are the following statements true for the hydrogen atom only, true for all atoms, or not true for any atoms? a. The principal quantum number completely determines the energy of a given electron. b. The angular momentum quantum number, \(\ell,\) determines the shapes of the atomic orbitals. c. The magnetic quantum number, \(m_{\ell},\) determines the direction that the atomic orbitals point in space.

One bit of evidence that the quantum mechanical model is 鈥渃orrect鈥� lies in the magnetic properties of matter. Atoms with unpaired electrons are attracted by magnetic fields and thus are said to exhibit paramagnetism. The degree to which this effect is observed is directly related to the number of unpaired electrons present in the atom. Consider the ground-state electron configurations for Li, N, Ni, Te, Ba, and Hg. Which of these atoms would be expected to be paramagnetic, and how many unpaired electrons are present in each paramagnetic atom?
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