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Chapter 24: Problem 74

The number of unpaired electrons in the complex ion \(\left[\operatorname{Cr}\left(\mathrm{NH}_{3}\right)_{6}\right]^{2+}\) is (a) \(5 ;(\mathrm{b}) 4 ;(\mathrm{c}) 3 ;(\mathrm{d}) 2 ;(\mathrm{e}) 1\).

Short Answer

Expert verified
The correct answer is (b) 4. The metal atom Chromium (Cr) in the complex ion \(\left[\operatorname{Cr}\left(\mathrm{NH}_{3}\right)_{6}\right]^{2+}\) has 4 unpaired electrons.

Step by step solution

01

Identify the Metal

The complex ion in this problem is \(\left[\operatorname{Cr}\left(\mathrm{NH}_{3}\right)_{6}\right]^{2+}\). The metal atom in this complex ion, upon which its properties depend, is Chromium (Cr).
02

Determine the Electron Configuration

To solve this problem, knowledge of the electron configuration of Chromium is necessary. The electron configuration of Cr is \([Ar] 3d^5 4s^1\) in its ground state. However, when it loses 2 electrons to form \(\operatorname{Cr}^{2+}\), it loses 1 electron from the 4s orbital and one from the 3d orbital, making the configuration \([Ar] 3d^4\). Therefore, Chromium (Cr) in this complex ion has 4 unpaired electrons.
03

Match Answer Choice

According to the options provided, the number of unpaired electrons in the complex ion is either a) 5, b) 4, c) 3, d) 2, or e) 1. Thus, after determining that the number of unpaired electrons in Chromium in the complex ion is 4, we can see that the correct answer is (b) 4.

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Most popular questions from this chapter

Verify the statement on page 1101 that neither \(\mathrm{Ca}^{2+}\) nor \(\mathrm{Mg}^{2+}\) found in natural waters is likely to precipitate from the water on the addition of other reagents if the ions are complexed with EDTA. Assume reasonable values for the total metal ion concentration and that of free EDTA, such as \(0.10 \mathrm{M}\) each.

Draw a structure for cis-dichlorobis(ethylenediamine)cobalt(III) ion. Is this ion chiral? Is the trans isomer chiral? Explain.

Draw plausible structures corresponding to each of the following names. (a) pentamminesulfatochromium(III) ion (b) trioxalatocobaltate(III) ion (c) triamminedichloronitrito-O-cobalt(III)

Of the following complex ions, the one that is optically active is (a) \(\operatorname{cis}-\left[\operatorname{CoCl}_{2}(\text { en })_{2}\right]^{+} ;\) (b) \(\left[\operatorname{CoCl}_{2}\left(\mathrm{NH}_{3}\right)_{4}\right]^{+}\) (c) \(\left[\mathrm{CoCl}_{4}\left(\mathrm{NH}_{3}\right)_{2}\right]^{-} ;(\mathrm{d})\left[\mathrm{CuCl}_{4}\right]^{-}\).

Write equations to represent the following observations. (a) A mixture of \(\hat{M g}(O H)_{2}(s)\) and \(Z n(O H)_{2}(s)\) is treated with \(\mathrm{NH}_{3}(\mathrm{aq}) .\) The \(\mathrm{Zn}(\mathrm{OH})_{2}\) dissolves, but the \(\mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{s})\) is left behind. (b) When \(\mathrm{NaOH}(\mathrm{aq})\) is added to \(\mathrm{CuSO}_{4}(\mathrm{aq}),\) a pale blue precipitate forms. If \(\mathrm{NH}_{3}(\) aq) is added, the precipitate redissolves, producing a solution with an intense deep blue color. If this deep blue solution is made acidic with \(\mathrm{HNO}_{3}(\mathrm{aq}),\) the color is converted back to pale blue.
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