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Review Questions -- Chapter 23 1. For each of the following metal complexes, give the oxidation state of the metal and the complete, systematic name of the compound or ion. (a) Na[Fe(CN)3(NH3)3] (b) [Cr(en)2Br2]2SO4 (c) [Rh(NH3)5CN]Cl2. 2. Draw clear, 3-dimensional structures of all of the isomers, geometric and/or optical, of the following complex. Points will be deducted if the same structure is drawn more than once. Co(en)2(CN)Br 3. For each of the following complexes, A and B, sketch a properly-labeled d-orbital splitting diagram. Then answer the questions below in a manner consistent with your diagrams. A: [Mn(H2O)6]2+ B: [Mn(NO2)6]4- (a) How many unpaired electrons does complex A have? (b) Which complex, A or B, will absorb light of longer wavelength? 4. a. An octahedral manganese (III) complex has a spin of 2 (i.e., 4 × ½). Sketch the energy level diagram for the d orbitals in this complex. b. Which of the following ligands is most likely to be attached to the Mn ion in this complex. Explain briefly. Cl- CN- . 5. For the complex [Pt(NH2Me)(NH3)2Cl]+, draw the structures for all the possible isomers of the cation. [Note: Me represents a methyl or CH3 group.] 6. Draw the structure for the geometric isomers of Co(en)NH3Cl3. en = H2NCH2CH2NH2 7. Give the structural formula for each of the following. . a. tetrakis(trimethylamine)palladium (II) nitrate page 2 b. potassium hexacyanoferrate (II) 8. Predict the spin state (high or low) and the number of unpaired electrons in the following complexes. Show how you arrived at your answers. [CoF6]-3 [Fe(CN)6]-3 [Ir(NH3)6]+3 page 3 Answers 1. For each of the following metal complexes, give the oxidation state of the metal and the complete, systematic name of the compound or ion. (a) Na[Fe(CN)3(NH3)3] Name: (b) Charge on Fe is 2+ sodium triamminetricyanoferrate(II) [Cr(en)2Br2]2SO4 Name: Charge on Cr is 3+ dibromobis(ethylenediamine)chromium(III) sulfate (c) [Rh(NH3)5CN]Cl2. Name: pentamminecyanorhodium(III) chloride 2. Draw clear, 3-dimensional structures of all of the isomers, geometric and/or optical, of the following complex. Points will be deducted if the same structure is drawn more than once. Co(en)2(CN)Br Br N N Co N N N N CN N N Co N Br N N CN CN trans Co Br N enantiomers of the cis isomer 3. For each of the following complexes, A and B, sketch a properly-labeled d-orbital splitting diagram. Then answer the questions below in a manner consistent with your diagrams. A: [Mn(H2O)6]2+ B: [Mn(NO2)6]4- See lecture notes and/or textbook for the d-orbital splitting diagrams. complexes are Mn2+ which is a d5 configuration. Both Complex B will have a larger splitting energy (∆) than A because CN- is a strong field ligand whereas H2O is a weak field ligand. page 4 Consequently, A will have 5 unpaired electrons and B will have 1. Complex A, which has the smaller ∆ value, will absorb light of lower energy, lower frequency, and hence longer wavelength. 4. a. An octahedral manganese (III) complex has a spin of 2 (i.e., 4 × ½). Sketch the energy level diagram for the d orbitals in this complex. eg dz2 dx2-y2 ∆ t2g dxy b. dxz dyz Which of the following ligands is most likely to be attached to the Mn ion in this complex. Explain briefly. ClCN- Chloride (Cl-) is most likely to be the ligand because it is the weakest field ligand according to the spectrochemical series so ∆ will be the smallest resulting in more unpaired electrons 5. For the complex [Pt(NH2Me)(NH3)2Cl]+, draw the structures for all the possible isomers of the cation. [Note: Me represents a methyl or CH3 group.] NH3 Cl Pt NH2Me + NH3 NH3 Cl trans Pt NH3 NH2Me cis 6. Draw the structure of the geometric isomers of Co(en)NH3Cl3. en = H2NCH2CH2NH2 Cl Cl N N Co NH3 Cl N N Co Cl 7. Give the structural formula for each of the following. . a. tetrakis(trimethylamine)palladium (II) nitrate NH3 Cl Cl + page 5 {Pd[N(CH3]3)4}(NO3)2 b. potassium hexacyanoferrate (II) K4[Fe(CN)6] 8. Predict the spin state (high or low) and the number of unpaired electrons in the following complexes. Show how you arrived at your answers. [CoF6]-3 [Fe(CN)6]-3 eg dz2 dz2 dx2-y2 dz2 dx2-y2 dyz high spin (∆ is small) 4 unpaired electrons dx2-y2 ∆ t2g dxz eg eg ∆ dxy [Ir(NH3)6]+3 ∆ t2g t2g dxy dxz dyz low spin (∆ is large) 1 unpaired electron dxy dxz dyz low spin (∆ is large) 0 unpaired electrons