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Chapter 23: Problem 27

For each of the following molecules or polyatomic ions, draw the Lewis structure and indicate if it can act as a monodentate ligand, a bidentate ligand, or is unlikely to act as a ligand at all: (a) ethylamine, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{NH}_{2}\), (b) trimethylphosphine, \(\mathrm{P}\left(\mathrm{CH}_{3}\right)_{3}\), (c) carbonate, \(\mathrm{CO}_{3}^{2-}\) (d) ethane, \(\mathrm{C}_{2} \mathrm{H}_{6}\).

Short Answer

Expert verified
(a) Ethylamine: Monodentate ligand; Lewis structure: H-C-C-N with one lone pair on N. (b) Trimethylphosphine: Monodentate ligand; Lewis structure: P surrounded by three CH3 groups with one lone pair on P. (c) Carbonate: Bidentate ligand; Lewis structure: O=C-O^--O^- with lone pairs on both negatively charged O atoms. (d) Ethane: Unlikely to act as a ligand; Lewis structure: H-C-C-H with no available lone pairs.

Step by step solution

01

(a) Ethylamine, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{NH}_{2}\): Lewis Structure

To draw the Lewis structure for ethylamine, first, we can build the skeleton structure as follows: a nitrogen (N) atom connected to a -CH2 connected to another -CH3 group. Then we can complete the octet by adding the electron pairs around the atoms. \( \mathrm{H} \\ \:| \\ \mathrm{H}\mathrm{C} - \mathrm{C-H} \\ \:| \\ \mathrm{H} - \mathrm{N} |\\ \:| \\ \mathrm{H}\)
02

(a) Ethylamine, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{NH}_{2}\): Ligand Type

In the Lewis structure of ethylamine, the nitrogen atom has one lone pair of electrons that can be donated to a central metal atom, making it a monodentate ligand.
03

(b) Trimethylphosphine, \(\mathrm{P}\left(\mathrm{CH}_{3}\right)_{3}\): Lewis Structure

To draw the Lewis structure for trimethylphosphine, place a phosphorus (P) atom in the center and connect it to three methyl groups (-CH3). Then, complete the octets by adding the corresponding electron pairs around the atoms. \( \\ \mathrm{CH}_{3} \\ | \\ \mathrm{P} - \mathrm{CH}_{3} \\ | \\ \mathrm{CH}_{3}\)
04

(b) Trimethylphosphine, \(\mathrm{P}\left(\mathrm{CH}_{3}\right)_{3}\): Ligand Type

In the Lewis structure of trimethylphosphine, the phosphorus atom has one lone pair of electrons that can be donated to a central metal atom. Therefore, it can act as a monodentate ligand.
05

(c) Carbonate, \(\mathrm{CO}_{3}^{2-}\): Lewis Structure

To draw the Lewis structure for carbonate, place a carbon (C) atom in the center and connect it to three oxygen (O) atoms with double bonds to one oxygen and single bonds to the other two oxygen atoms. Add electron pairs around the oxygen atoms to complete their octets. The 2- charge comes from the two extra electrons in the system. \[ \mathrm{O} = \mathrm{C} - \mathrm{O}^- - \mathrm{O}^- \]
06

(c) Carbonate, \(\mathrm{CO}_{3}^{2-}\): Ligand Type

Carbonate ion has two electron-rich oxygens, each with a lone pair that can be donated to a central metal atom. Therefore, it can act as a bidentate ligand.
07

(d) Ethane, \(\mathrm{C}_{2} \mathrm{H}_{6}\): Lewis Structure

To draw the Lewis structure for ethane, connect two carbon (C) atoms in the center and complete the octets by adding three hydrogen (H) atoms to each carbon atom. \( \mathrm{H} \\ \:| \\ \mathrm{H} - \mathrm{C} - \mathrm{C} - \mathrm{H} \\ \:| \\ \mathrm{H}\)
08

(d) Ethane, \(\mathrm{C}_{2} \mathrm{H}_{6}\): Ligand Type

In the Lewis structure of ethane, there are no lone pairs of electrons available for donation to a central metal atom. Thus, ethane is unlikely to act as a ligand.

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Most popular questions from this chapter

Identify each of the following coordination complexes as either diamagnetic or paramagnetic: (a) \(\left[\operatorname{CoBr}\left(\mathrm{NH}_{3}\right)_{5}\right]^{2+}\) (b) \(\left[\mathrm{W}(\mathrm{CN})_{6}\right]^{3-}\) (c) \(\left[\mathrm{VF}_{6}\right]^{3-}\) (d) \(\left[\mathrm{Rh}(\mathrm{o}-\mathrm{phen})_{3}\right]^{3+}\)

A four-coordinate complex \(\mathrm{MA}_{2} \mathrm{~B}_{2}\) is prepared and found to have two different isomers. Is it possible to determine from this information whether the complex is square planar or tetrahedral? If so, which is it?

Consider an octahedral complex, \(\mathrm{MA}_{2} \mathrm{~B}_{4}\). How many geometric isomers are expected for this compound? Will any of the isomers be optically active? If so, which ones?

(a) Using Werner's definition of valence, which property is the same as oxidation number, primary valence or secondary valence? (b) What term do we normally use for the other type of valence? (c) Why can \(\mathrm{NH}_{3}\) serve as a ligand but \(\mathrm{BH}_{3}\) cannot?

Explain why the transition metals in periods 5 and 6 have nearly identical radii in each group.
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