- Ch.1 - Chemical Tools: Experimentation & Measurement167
- Ch.2 - Atoms, Molecules & Ions145
- Ch.3 - Mass Relationships in Chemical Reactions162
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms91
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory66
- Ch.7 - Covalent Bonding and Electron-Dot Structures59
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy114
- Ch.10 - Gases: Their Properties & Behavior121
- Ch.11 - Liquids & Phase Changes52
- Ch.12 - Solids and Solid-State Materials72
- Ch.13 - Solutions & Their Properties70
- Ch.14 - Chemical Kinetics84
- Ch.15 - Chemical Equilibrium70
- Ch.16 - Aqueous Equilibria: Acids & Bases86
- Ch.17 - Applications of Aqueous Equilibria101
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium77
- Ch.19 - Electrochemistry137
- Ch.20 - Nuclear Chemistry82
- Ch.21 - Transition Elements and Coordination Chemistry126
- Ch.22 - The Main Group Elements92
- Ch.23 - Organic and Biological Chemistry11
Chapter 21, Problem 21.127a
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)
Video transcript
Predict the crystal field energy-level diagram for a linear ML2 complex that has two ligands along the :
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.
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)
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]+
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>-
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>