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Ch.21 - Transition Elements and Coordination Chemistry
All textbooksMcMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblem 21.127b
Chapter 21, Problem 21.127b

For each of the following complexes, describe the bonding using valence bond theory. Include orbital diagrams for the free metal ion and the metal ion in the complex. Indicate which hybrid orbitals the metal ion uses for bonding, and specify the number of unpaired electrons. 
(b) [Ag(NH3)2]+

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1
Identify the central metal ion in the complex. In this case, it is Ag^+.
Determine the electron configuration of the free metal ion, Ag^+. Silver (Ag) has an atomic number of 47, so its electron configuration is [Kr] 4d^10 5s^1. As Ag^+ loses one electron, the configuration becomes [Kr] 4d^10.
Draw the orbital diagram for the free metal ion, Ag^+. Since Ag^+ has a filled 4d subshell, all 4d orbitals are paired, and there are no unpaired electrons.
Consider the ligands and their effect on the metal ion. NH3 is a neutral ligand and acts as a Lewis base, donating a pair of electrons to the metal ion. In [Ag(NH3)2]^+, the Ag^+ ion forms two coordinate covalent bonds with NH3 ligands.
Determine the hybridization of the metal ion in the complex. For [Ag(NH3)2]^+, the Ag^+ ion uses sp hybrid orbitals to accommodate the two pairs of electrons from the NH3 ligands, resulting in a linear geometry around the metal ion.

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Key Concepts

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

Valence Bond Theory

Valence Bond Theory (VBT) explains how atoms bond by overlapping their atomic orbitals to form covalent bonds. It emphasizes the role of hybridization, where atomic orbitals mix to create new hybrid orbitals that can accommodate electron pairs. This theory helps in understanding the geometry and bonding characteristics of complexes, such as how the shape of [Ag(NH3)2]+ is determined by the hybridization of the silver ion.
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Valence Shell Electron Pair Repulsion Theory

Hybridization

Hybridization is the process of combining atomic orbitals to form new hybrid orbitals that are suitable for the pairing of electrons to form chemical bonds. In the case of [Ag(NH3)2]+, the silver ion undergoes hybridization to form dsp2 hybrid orbitals, which allows it to bond with two ammonia ligands. Understanding hybridization is crucial for predicting the geometry and bond angles in coordination complexes.
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Hybridization

Unpaired Electrons

Unpaired electrons are electrons that are alone in an orbital and are crucial for determining the magnetic properties of a complex. In [Ag(NH3)2]+, the silver ion has a specific electron configuration that can lead to the presence of unpaired electrons, affecting its reactivity and interaction with ligands. Identifying the number of unpaired electrons is essential for understanding the electronic structure and bonding behavior of the metal ion in the complex.
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Related Practice
Textbook Question

Predict the crystal field energy-level diagram for a square pyramidal ML5 complex that has two ligands along the axes but only one ligand along the z axis. Your diagram should be intermediate between those for an octahedral ML6 complex and a square planar ML4 complex.

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Textbook Question

Give a valence bond description of the bonding in each of the following complexes. Include orbital diagrams for the free metal ion and the metal ion in the complex. Indicate which hybrid orbitals the metal ion uses for bonding, and specify the number of unpaired electrons. 

(b) [NiBr4]2- (tetrahedral) 

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Textbook Question

For each of the following complexes, describe the bonding using valence bond theory. Include orbital diagrams for the free metal ion and the metal ion in the complex. Indicate which hybrid orbitals the metal ion uses for bonding, and specify the number of unpaired electrons. 

(a) [AuCl4]2 (square planar)

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Textbook Question

There are two possible [M(OH)4]- complexes of first-series transition metals that have three unpaired electrons.

(a) What are the oxidation state and the identity of M in these complexes?

(b) Using orbital diagrams, give a valence bond description of the bonding in each complex.

(c) Based on common oxidation states of first-series transition metals (Figure 21.6), which [M(OH)4]- complex is more likely to exist? 

<QUESTION REFERENCES FIGURE 21.6>-

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Textbook Question

Two first-series transition metals have three unpaired electrons in complex ions of the type [MCl4]2-.

(a) What are the oxidation state and the identity of M in these complexes?

(b) Draw valence bond orbital diagrams for the two possible ions.

(c) Based on common oxidation states of first-series transition metals (Figure 21.6), which ion is more likely to exist?

<QUESTION REFERENCES FIGURE 21.6>

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Textbook Question

Nickel(II) complexes with the formula NiX2L2, where X− is Cl− or N-bonded NCS− and L is the monodentate triphenylphosphine ligand P(C6H5)3, can be square planar or tetrahedral.

(a) Draw crystal field energy-level diagrams for a square planar and a tetrahedral nickel(II) complex, and show the population of the orbitals.

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