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Chapter 24: Problem 10

Draw plausible structures corresponding to each of the following names. (a) pentamminenitrito- \(N\) -cobalt(III) ion (b) ethylenediaminedithiocyanato-S-copper(II) (c) hexaaquanickel(II) ion

Short Answer

Expert verified
The following structures correspond to the given names: (a) [Co(NH3)5(NO2)]^3+, (b) [Cu(C2H4(NH2)2)(SCN)2]^2+, (c) [Ni(H2O)6]^2+

Step by step solution

01

Naming coordination compounds: Step 1 - pentamminenitrito-N-cobalt(III) ion

The compound's name states that it contains cobalt with a 3+ charge as the central atom. There are five ammine (\(NH_3\)) ligands and one nitrite group bonded through nitrogen (\(NO_2^-\)). Therefore, the structure shows cobalt at the center, surrounded by five \(NH_3\) groups and one \(NO_2^-\) group.
02

Naming coordination compounds: Step 2 - ethylenediaminedithiocyanato-S-copper(II)

The compound's name specifies that it has a central copper atom with a 2+ charge. Its ligands include an ethylenediamine (\(C_2H_4(NH_2)_2\)) group and two thiocyanate groups (\(SCN^-\)). One of the thiocyanate groups is attached to the copper atom through sulfur. Therefore, the structure has copper in the center, surrounded by the ethylenediamine group and two \(SCN^-\) groups, with one \(SCN^-\) bound by sulfur.
03

Naming coordination compounds: Step 3 - hexaaquanickel(II) ion

The name of this compound indicates that it has a central nickel atom with a 2+ charge accompanied by six water molecules. So, the structure will have the nickel ion at the center surrounded by six water molecules.

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Most popular questions from this chapter

Explain the important distinction between each of the following pairs: (a) coordination number and oxidation number; (b) monodentate and polydentate ligands; (c) cis and trans isomers; (d) dextrorotatory and levorotatory compounds; (e) low-spin and highspin complexes.

Of the following, the one that is a Bronsted-Lowry acid is (a) \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+} ;\) (b) \(\left[\mathrm{FeCl}_{4}\right]^{-} ;\) (c) \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) (d) \(\left[\mathrm{Zn}(\mathrm{OH})_{4}\right]^{-}\).

Acetyl acetone undergoes an isomerization to form a type of alcohol called an enol. The enol, abbreviated acacH, can act as a bidentate ligand as the anion acac^-. Which of the following compounds are optically active: \(\operatorname{Co}(\mathrm{acac})_{3} ;\) trans\(\left[\mathrm{Co}(\mathrm{acac})_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right] \mathrm{Cl}_{2} ; \operatorname{cis}-\left[\mathrm{Co}(\mathrm{acac})_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right] \mathrm{Cl}_{2} ?\)

Which of these general structures for a complex ion would you expect to exhibit cis and trans isomerism? Explain. (a) tetrahedral (b) square-planar (c) linear

We have seen that complex formation can stabilize oxidation states. An important illustration of this fact is the oxidation of water in acidic solutions by \(\mathrm{Co}^{3+}(\) aq) but not by \(\left[\mathrm{Co}(\mathrm{en})_{3}\right]^{3+} .\) Use the following data. \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}+\mathrm{e}^{-} \longrightarrow\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) $$ E^{\circ}=1.82 \mathrm{V} $$ \(\left[\operatorname{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}+3 \mathrm{en} \longrightarrow\left[\mathrm{Co}(\mathrm{en})_{3}\right]^{2+}+6 \mathrm{H}_{2} \mathrm{O}(1)\) $$ \log \beta_{3}=12.18 $$ \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}+3 \mathrm{en} \longrightarrow\left[\mathrm{Co}(\mathrm{en})_{3}\right]^{3+}+6 \mathrm{H}_{2} \mathrm{O}(1)\) $$ \log \beta_{3}=47.30 $$ Calculate \(E^{\circ}\) for the reaction $$ \left[\mathrm{Co}(\mathrm{en})_{3}\right]^{3+}+\mathrm{e}^{-} \longrightarrow\left[\mathrm{Co}(\mathrm{en})_{3}\right]^{2+} $$ Show that \(\left[\mathrm{Co}(\mathrm{en})_{3}\right]^{3+}\) is stable in water but \(\mathrm{Co}^{3+}(\mathrm{aq})\) is not.
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