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Chapter 21: Problem 59

How many unpaired electrons are present in the tetrahedral ion \(\mathrm{FeCl}_{4}^{-} ?\)

Short Answer

Expert verified
The \(\mathrm{FeCl}_{4}^{-}\) ion contains 3 unpaired electrons.

Step by step solution

01

Find the atomic number for Fe.

The atomic number can be found on the periodic table. It is the number associated with the chemical symbol for iron, which is Fe. According to the periodic table, the atomic number for Fe is 26.
02

Determine the number of electrons in Fe.

Iron in its elemental state should have as many electrons as its atomic number, which is 26. Iron (Fe) atoms in their ground (unexcited) state have 26 electrons.
03

Write the electronic configuration of neutral Fe.

The electronic configuration for iron (Fe) in the ground state can be written as follows: \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{6}\).
04

Write the electronic configuration of \(\mathrm{FeCl}_{4}^{-}\).

When Fe forms the \(\mathrm{FeCl}_{4}^{-}\) ion, it loses 3 electrons from the \(4s\) and \(3d\) shells. This results in 23 electrons, and their configuration can be written as: \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{3}\).
05

Calculate the number of unpaired electrons.

To determine the number of unpaired electrons, count the number of electrons in the d orbitals that are not paired. From the computed electronic configuration, there are 3 unpaired electrons in the d orbitals. So, the \(\mathrm{FeCl}_{4}^{-}\) ion contains 3 unpaired electrons.

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Most popular questions from this chapter

A certain first-row transition metal ion forms many different colored solutions. When four coordination compounds of this metal, each having the same coordination number, are dissolved in wa ter, the colors of the solutions are red, yellow, green, and blue Further experiments reveal that two of the complex ions are para magnetic with four unpaired electrons and the other two are dia magnetic. What can be deduced from this information about th four coordination compounds?

Give formulas for the following. a. potassium tetrachlorocobaltate(II) b. aquatricarbonylplatinum(II) bromide c. sodium dicyanobis(oxalato)ferrate(III) d. triamminechloroethylenediaminechromium(III) iodide

When an aqueous solution of \(\mathrm{KCN}\) is added to a solution containing \(\mathrm{Ni}^{2+}\) ions, a precipitate forms, which redissolves on addition of more KCN solution. Write reactions describing what happens in this solution. [Hint: \(\mathrm{CN}^{-}\) is a Br贸nsted-Lowry base \(\left(K_{\mathrm{b}}=10^{-5}\right)\) and a Lewis base. \(]\)

a. Calculate the molar solubility of AgBr in pure water. \(K_{\text {sp }}\) for AgBr is \(5.0 \times 10^{-13}\) b. Calculate the molar solubility of AgBr in \(3.0 M \mathrm{NH}_{3}\). The overall formation constant for \(\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}\) is \(1.7 \times 10^{7}\), that is, \(\mathrm{Ag}^{+}(a q)+2 \mathrm{NH}_{3}(a q) \longrightarrow \mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}(a q) \quad K=1.7 \times 10^{7}\) c. Compare the calculated solubilities from parts a and b. Explain any differences. d. What mass of \(\mathrm{AgBr}\) will dissolve in \(250.0 \mathrm{~mL}\) of \(3.0 \mathrm{M} \mathrm{NH}_{3}\) ? e. What effect does adding \(\mathrm{HNO}_{3}\) have on the solubilities calculated in parts a and \(\mathrm{b}\) ?

Name the following coordination compounds. a. \(\mathrm{Na}_{4}\left[\mathrm{Ni}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}\right]\) b. \(\mathrm{K}_{2}\left[\mathrm{CoCl}_{4}\right]\) c. \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{SO}_{4}\) d. \(\left[\mathrm{Co}(\mathrm{en})_{2}(\mathrm{SCN}) \mathrm{Cl}\right] \mathrm{Cl}\)
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