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]+

검증된 단계별 안내

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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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.

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.

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.

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]+