Ch.21 - Transition Elements and Coordination Chemistry

McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook

McMurry 8th Edition

Ch.21 - Transition Elements and Coordination Chemistry

Problem 21.29

Chapter 21, Problem 21.29

The oxalate ion is a bidentate ligand as indicated in Figure 21.8. Would you expect the carbonate ion to be a monodentate or bidentate ligand? Explain your reasoning.

Verified step by step guidance

Step 1: Understand the terms. A ligand is a molecule or ion that binds to a central metal atom to form a coordination complex. Ligands can be monodentate (binds through one site) or bidentate (binds through two sites).

Step 2: Look at the structure of the carbonate ion (CO3^2-). It has three oxygen atoms, each with a lone pair of electrons. These lone pairs can potentially act as binding sites to a metal ion.

Step 3: However, due to the planar structure of the carbonate ion and the 120-degree angle between the oxygen atoms, it is not possible for more than one oxygen atom to simultaneously bind to a metal ion.

Step 4: Therefore, despite having three potential binding sites, the carbonate ion can only bind through one site at a time.

Step 5: Based on this reasoning, we would expect the carbonate ion to act as a monodentate ligand.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ligands

Ligands are ions or molecules that can donate a pair of electrons to a central metal atom to form a coordination complex. They can be classified based on the number of donor atoms they possess. Monodentate ligands have one donor atom, while bidentate ligands have two, allowing them to form multiple bonds with the metal center.

Bidentate vs. Monodentate Ligands

Bidentate ligands can attach to a metal ion at two separate sites, creating a more stable complex due to the chelation effect. In contrast, monodentate ligands bind through a single donor atom. The ability of a ligand to act as bidentate or monodentate depends on its structure and the presence of multiple donor atoms.

Structure of Carbonate Ion

The carbonate ion (CO3^2-) has a trigonal planar structure with three oxygen atoms surrounding a central carbon atom. Each oxygen atom can potentially act as a donor atom, but due to the geometry and bonding characteristics, carbonate typically acts as a monodentate ligand, binding through one oxygen atom at a time.

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Textbook Question

In excess of NH3(aq), Zn2+ forms a complex ion, [Zn(NH3)4]2+ which has a formation constant Kf = 7.8 x 10^8. Calculate the concentration of Zn2+ in a solution prepared by adding 1.00 x 10^-2 mol Zn(NO3)2 to 1.00 L of 0.250 M NH3. (a) 7.9 x 10^-4 M(b) 2.8 x 10^-6 M(c) 3.9 x 10^-9 M(d) 6.4 x 10^-11 M

Textbook Question

Draw a crystal field energy-level diagram for the 3d orbitals of titanium in [Ti(H₂O)₆]³⁺]. Indicate the crystal field splitting, and explain why is [Ti(H₂O)₆]³⁺] colored.

Textbook Question

Draw the three possible diastereoisomers of the triethylenetetramine complex [Co(trend)Cl₂]⁺. Abbreviate the flexible tetradentate trien ligand H₂NCH₂CH₂NHCH₂CH₂NHCH₂CH₂NH₂ as . Which of the isomers can exist as a pair of enantiomers?

Textbook Question

What is the oxidation state of the metal in each of the complexes?

a. AgCl₂^–

b. [Cr(H2O)₅Cl]²⁺

c. [Co(NCS)₄]^2–

d. [ZrF₈]^4–

e. [Fe(EDTA)(H₂O)]^–

Textbook Question

What is the electron configuration of Co²⁺ and how many unpaired electrons are in the free transition metal ion?

(a) [Ar]3d⁵4s²; 5 unpaired electrons

(b) [Ar]3d⁵4s²; 1 unpaired electron

(d) [Ar]3d⁷; 1 unpaired electron