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Chapter 24: Problem 6

Draw Lewis structures for the following ligands: (a) hydroxo; (b) sulfato; (c) oxalato; (d) thiocyanato- \(N\) -.

Short Answer

Expert verified
Lewis structures for the given ligands are drawn by understanding the composition of the molecule, its valence electrons and the rules of bonding. For hydroxo, it's a single bond between Hydrogen and Oxygen, with Oxygen carrying 2 lone pairs and an extra electron; for sulfato, there are 4 double bonds between Sulfur and Oxygen atoms, Oxygen carries the 2 extra electrons; for oxalato, there are 4 double bonds between them, with Carbon atoms sharing 4 electrons; for thiocyanato-\(N\), there's a single bond between Carbon and Sulphur, a double bond between Carbon and Nitrogen,with Sulphur carrying 2 lone pairs and the molecule carrying an extra electron due to the \(-\) charge.

Step by step solution

01

Drawing Lewis Structure for Hydroxo

First, write down the composition of Hydroxo. It consists of one Oxygen atom and one Hydrogen atom so it's \(\text{OH}^-\). Hydrogen carries 1 valence electron, Oxygen carries 6. They share 1 electron to form a bond and remaining layer of Oxygen is filled with electrons. The molecule carries 1 extra electron, hence the \(-\) sign.
02

Drawing Lewis Structure for Sulfato

Sulfato is an ion with the composition \(\text{SO}_4^{2-}\). Sulfur is at the center of the molecule. It carries 6 valence electrons. Oxygen, each carrying 6 valence electrons surround Sulfur and each shares 2 electrons to form double bonds. So, there are 4 double bonds in total. The ion is charged -2, so 2 extra electrons are added to the Oxygens.
03

Drawing Lewis Structure for Oxalato

Oxalato is a complex ion with the composition \(\text{C}_2\text{O}_4^{2-}\). The molecule consists of 2 Carbon atoms each double bonded to 2 Oxygen atoms. Calculation of valence electrons results in 4 remaining electrons. These electrons are shared between two Carbon atoms forming another double bond.
04

Drawing Lewis Structure for Thiocyanato-\(N\)

Thiocyanato-\(N\) is an anion with the composition \(\text{SCN}^-\) with Sulphur at one end, Nitrogen on the other and Carbon in between. Carbon double bonds with Nitrogen and single bonds with Sulphur. Remaining 4 electrons of Sulphur form 2 lone pairs. The molecule carries an extra electron due to the \(-\) charge.

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Most popular questions from this chapter

Explain the following observations in terms of complex-ion formation. (a) \(\mathrm{CoCl}_{3}\) is unstable in aqueous solution, being reduced to \(\mathrm{CoCl}_{2}\) and liberating \(\mathrm{O}_{2}(\mathrm{g}) .\) Yet, \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{3}\) can be easily maintained in aqueous solution. (b) AgI is insoluble in water and in dilute \(\mathrm{NH}_{3}(\mathrm{aq})\) but AgI will dissolve in an aqueous solution of sodium thiosulfate.

A structure that Werner examined as a possible alternative to the octahedron is the trigonal prism. (a) Does this structure predict the correct number of isomers for the complex ion \(\left[\mathrm{CoCl}_{2}\left(\mathrm{NH}_{3}\right)_{4}\right]^{+} ?\) If not, why not? (b) Does this structure account for optical isomerism in \(\left[\mathrm{Co}(\mathrm{en})_{3}\right]^{3+} ?\) Explain.

Supply acceptable names for the following. (a) \(\left[\mathrm{Co}(\mathrm{OH})\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}\left(\mathrm{NH}_{3}\right)\right]^{2+}\) (b) \(\left[\mathrm{Co}(\mathrm{ONO})_{3}\left(\mathrm{NH}_{3}\right)_{3}\right]\) (c) \(\left[\operatorname{Pt}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}\right]\left[\mathrm{PtCl}_{6}\right]\) (d) \(\left[\mathrm{Fe}(\mathrm{ox})_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right]^{-}\) (e) \(\mathrm{Ag}_{2}\left[\mathrm{HgI}_{4}\right]\)

The coordination number of \(\mathrm{Pt}\) in the complex ion \(\left[\mathrm{PtCl}_{2}(\mathrm{en})_{2}\right]^{2+}\) is \((\mathrm{a}) 2 ;(\mathrm{b}) 3 ;(\mathrm{c}) 4 ;(\mathrm{d}) 5 ;(\mathrm{e}) 6\).

Draw structures to represent these four complex ions: (a) \(\left[\mathrm{PtCl}_{4}\right]^{2-} ;\) (b) \(\left[\mathrm{FeCl}_{4}(\mathrm{en})\right]^{-} ;\) (c) \(\operatorname{cis}-\left[\mathrm{FeCl}_{2}(\mathrm{ox})(\mathrm{en})\right]^{-}\) (d) trans- \(\left[\mathrm{CrCl}(\mathrm{OH})\left(\mathrm{NH}_{3}\right)_{4}\right]^{+}\).
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