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Chapter 7: Problem 132

The first-row transition metals from chromium through zinc all have some biologic function in the human body. How many unpaired electrons are present in each of these first-row transition metals in the ground state?

Short Answer

Expert verified
The number of unpaired electrons in the ground state for the first-row transition metals from chromium to zinc are: Cr (5), Mn (5), Fe (4), Co (3), Ni (2), Cu (1), and Zn (0).

Step by step solution

01

Identify the atomic number of the elements

The elements are chromium (Cr), manganese (Mn), iron (Fe), cobalt (Co), nickel (Ni), copper (Cu), and zinc (Zn). Their atomic numbers are: Cr (24), Mn (25), Fe (26), Co (27), Ni (28), Cu (29), Zn (30).
02

Write the electronic configuration

Electronic configurations of these elements in the ground state are: - Cr (\(Z = 24\)): \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^5 4s^1\) - Mn (\(Z = 25\)): \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^5 4s^2\) - Fe (\(Z = 26\)): \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^6 4s^2\) - Co (\(Z = 27\)): \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^7 4s^2\) - Ni (\(Z = 28\)): \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^8 4s^2\) - Cu (\(Z = 29\)): \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^1\) - Zn (\(Z = 30\)): \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^2\)
03

Determine the number of unpaired electrons

To find the number of unpaired electrons, we need to count the number of electrons in the partially filled orbitals: - Cr: 3d orbital has 5 unpaired electrons. - Mn: 3d orbital has 5 unpaired electrons. - Fe: 3d orbital has 4 unpaired electrons. - Co: 3d orbital has 3 unpaired electrons. - Ni: 3d orbital has 2 unpaired electrons. - Cu: 3d orbital is fully filled and only the 4s orbital has 1 unpaired electron. - Zn: All orbitals are fully filled, so there are no unpaired electrons. So, the number of unpaired electrons in the ground state for the first-row transition metals from chromium to zinc are 5, 5, 4, 3, 2, 1, and 0, respectively.

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Most popular questions from this chapter

Consider the following approximate visible light spectrum: Barium emits light in the visible region of the spectrum. If each photon of light emitted from barium has an energy of \(3.59 \times\) \(10^{-19} \mathrm{~J}\), what color of visible light is emitted?

For each of the following pairs of elements \((\mathrm{C}\) and \(\mathrm{N}) \quad(\mathrm{Ar}\) and \(\mathrm{Br})\) pick the atom with a. more favorable (exothermic) electron affinity. b. higher ionization energy. c. larger size.

Write the expected electron configurations for each of the following atoms: \(\mathrm{Cl}, \mathrm{Sb}, \mathrm{Sr}, \mathrm{W}, \mathrm{Pb}, \mathrm{Cf}\).

Write the expected ground-state electron configuration for the following. a. the element with one unpaired \(5 p\) electron that forms a covalent with compound fluorine b. the (as yet undiscovered) alkaline earth metal after radium c. the noble gas with electrons occupying \(4 f\) orbitals d. the first-row transition metal with the most unpaired electrons

Cesium was discovered in natural mineral waters in 1860 by R. W. Bunsen and G. R. Kirchhoff using the spectroscope they invented in \(1859 .\) The name came from the Latin caesius ("sky blue") because of the prominent blue line observed for this element at \(455.5 \mathrm{~nm} .\) Calculate the frequency and energy of a photon of this light.
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