Transition Metals and Coordination Chemistry. 1. In the transition metals section chemical similarities are found within a and across a.
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1 Transition Metals and Coordination Chemistry 1. In the transition metals section chemical similarities are found within a and across a. 2. What are 2 transition metals that have unique electron configurations? What are the configurations? Possible explanation for configuration anomaly 3. In neutral transition metals the 3d has a energy compared to 4s. In transition metal ions the 3d has a energy compared to 4s. Why? 4. Write the electron configurations for each of the following Ti 2+ - Re 2+ - c. Re 3+ - d. Cu Ionization energies tend to increase going from to in the d-block. 6. What is a coordination compound composed of? c. 7. What is a complex ion? 8. What is a counter ion? 9. What is a ligand? What is a Lewis Base?
2 10. Two characteristics of many coordination compounds. 11. What is a primary valence? What does it correspond to? 12. What is a secondary valence? What does it correspond to? 13. Define Monodentate Bidentate c. Polydentate d. Chelate 14. Method for naming a coordination compound c. d. e. f. g. 15. Fill in these naming charts
3 16. Name the following [Co(NH 3 ) 6 ]Cl 2 K 2 [PtCl 4 ] c. [Co(H 2 O) 6 ]I 3 d. [Co(NH 3 ) 3 (NO 2 ) 3 ] e. Mn(NH 2 CH 2 CH 2 NH 2 ) 3 2+ f. [Pt(NH 3 ) 4 I 2 ][PtI 4 ] 17. Give the formulas for the following Sodium dicyanobis(oxalato)ferrate (III) Tetracarbonyldihydroxochromium(III) ion c. Triamminechloro(ethylenediammine)chromium (III) iodide d. Amminetrichloroplatinate (II) ion 18. A coordination compound of cobalt(iii) contains four ammonia molecules, one sulfate ion, and one chloride ion. Addition of aqueous BaCl 2 solution to an aqueous solution of the compound gives no precipitate. Addition of aqueous AgNO 3 to an aqueous solution of the compound produces white precipitate. Propose a structure for this coordination compound. 19. How many bonds could each of the following chelates form with a metal ion?
4 20. Predicting the shape of a complex ion depends on the 21. When the coordination number is c. d. i i 22. What is an isomer? 23. Complete Isomer Flow Chart 24. Define and give an example of each of the following Coordinate Isomerism Linkage Isomerism c. Geometric (cis-trans) Isomerism d. Optical Isomerism 25. Draw geometrical isomers of each of the following complex ions.
5 [Co(C 2 O 4 ) 2 (H 2 O) 2 ] - [Pt(NH 3 ) 4 I 2 ] Which of the following ligands are capable of linkage isomerism? SCN -, N 3 -, NO 2 -, NH 2 CH 2 CH 2 NH 2, OCN -, I Draw all the geometric isomers of Pt(CN) 2 Br 2 (H 2 O) 2. Which of these isomers has an optical isomer? Draw the various optical isomers. 28. How do you know if a complex ion, with tetrahedral geometry, is optically active? 29. In order for a molecule to be optically active it must be 30. In order to be chiral a molecule must have a. 31. Chiral isomers are called. 32. An isomer that rotates plane polarized light to the left is called. An isomer that rotates plane polarized light to the right is called. 33. What is a racemic mixture? 34. What is the crystal field model? 35. Show the interaction between the d-orbital and the negative point charge ligands 36. Based on the diagrams above, would all of the d orbitals have the same energy? If not which would be higher energy? 37. The phenomena of d orbital splitting can happen two ways 38. What affects the type of splitting that will happen? General Ligand Ordering 39. The the charge on the metal the stronger the splitting.
6 40. The Crystal Field Method can be used to explain the 41. How does this model explain color? 42. How can we determine the color we will see? 43. What is the d-orbital splitting for Tetrahedral Geometry Square Planar c. Linear 44. The Molecular Orbital Model gives the most complete and complicated understanding of bonding in coordination compounds. Draw the MO diagram for an octahedral compound with 6 ligands. 45. How does the electronegativity of a ligand affect the d orbital splitting? 46. Compounds of copper(ii) are generally colored, but compounds of copper(i) are not. Explain. Would you expect Cd(NH 3 ) 4 Cl 2 to be colored? 47. Consider the complex ions Co(NH 3 ) 6 3+, Co(CN) 6 3-, and CoF 6 3- / The wavelengths of absorbed electromagnetic radiation for these compounds are (in no specific order) 770 nm, 440 nm, and 290 nm. Match the complex ion to the wavelength of absorbed electromagnetic radiation. 48. How many unpaired electrons are in the following complex ions? Ru(NH 3 ) 6 2+ (low spin case) Ni(H 2 O) 6 2+ c. V(en) Draw the d-orbital splitting for the octahedral complex ions in each of the following. Fe 2+ (high and low spin) Ni 2+ c. Zn 2+
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