Công nghệ hóa học - Complexes

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1. Complexes • A central metal atom bonded to a group of molecules or ions is a metal complex. • If it’s charged, it’s a complex ion. Chemistry of • Compounds containing complexes are coordinationCoordination compounds. Compounds
2. Complexes • The molecules or ions coordinating to the metal are the ligands. • They are usually anions or polar molecules. • The must have lone pairs to interact with metal Chemistry of Coordination Compounds
3. A chemical mystery: Same metal, same ligands, different number of ions when dissolved • Many coordination compounds are brightly colored, but again, same metal, same ligands, different colors. Chemistry of Coordination Compounds
4. Werner’s Theory Co(III) oxidation state Coordination # is 6 • suggested in 1893 that metal ions have primary and secondary valences.  Primary valence equal the metal’s oxidation number Chemistry of  Secondary valence is the number of atoms directlyCoordination Compounds bonded to the metal (coordination number)
5. Werner’s Theory • The central metal and the ligands directly bonded to it make up the coordination sphere of the complex. • In CoCl3 ∙ 6 NH3, all six of the ligands are NH3 and the 3 chloride ions are outside the coordination sphere. Chemistry of Coordination Compounds
6. Werner’s Theory In CoCl3 ∙ 5 NH3 the five NH3 groups and one chlorine are bonded to the cobalt, and the other two chloride ions are outside the sphere. Chemistry of Coordination Compounds
7. Werner’s Theory Werner proposed putting all molecules and ions within the sphere in brackets and those “free” anions (that dissociate from the complex ion when dissolved in water) outside the brackets. Chemistry of Coordination Compounds
8. Werner’s Theory • This approach correctly predicts there would be two forms of CoCl3 ∙ 4 NH3.  The formula would be written [Co(NH3)4Cl2]Cl.  One of the two forms has the two chlorines next to each other.  The other has the chlorines opposite each other. Chemistry of Coordination Compounds
9. What is Coordination? • When an orbital from a ligand with lone pairs in it overlaps with an empty orbital from a metal Sometimes called a coordinate covalent M L bond So ligands must have lone pairs of electrons. Chemistry of Coordination Compounds
10. Metal-Ligand Bond • This bond is formed between a Lewis acid and a Lewis base.  The ligands (Lewis bases) have nonbonding electrons.  The metal (Lewis acid) has empty orbitals. Chemistry of Coordination Compounds
11. Metal-Ligand Bond The metal’s coordination ligands and geometry can greatly alter its properties, such as color, or ease of oxidation. Chemistry of Coordination Compounds
12. Oxidation Numbers Knowing the charge on a complex ion and the charge on each ligand, one can determine the oxidation number for the metal. Chemistry of Coordination Compounds
13. Oxidation Numbers Or, knowing the oxidation number on the metal and the charges on the ligands, one can calculate the charge on the complex ion. Example: Cr(III)(H2O)4Cl2 Chemistry of Coordination Compounds
14. Coordination Number • The atom that supplies the lone pairs of electrons for the metal-ligand bond is the donor atom. • The number of these atoms is the coordination number. Chemistry of Coordination Compounds
15. Coordination Number • Some metals, such as chromium(III) and cobalt(III), consistently have the same coordination number (6 in the case of these two metals). • The most commonly encountered numbers are 4 and 6. Chemistry of Coordination Compounds
16. Geometries • There are two common geometries for metals with a coordination number of four:  Tetrahedral Tetrahedral Square planar  Square planar Why square planar? We’ll get to that Chemistry of Coordination Compounds
17. Geometries By far the most- encountered geometry, when the coordination number is six, is octahedral. Chemistry of Coordination Compounds
18. Polydentate Ligands • Some ligands have two or more donor atoms. • These are called polydentate ligands or chelating agents. • In ethylenediamine, NH2CH2CH2NH2, represented here as en, each N is a donor atom. • Therefore, en is bidentate. Chemistry of Coordination Compounds
19. Polydentate Ligands Ethylenediaminetetraacetate, mercifully abbreviated EDTA, has six donor atoms. Wraps around the central atom like an Chemistry of Coordination octopus Compounds
20. Polydentate Ligands Chemistry of Chelating agents generally form more stable Coordination Compounds complexes than do monodentate ligands.
21. Chelating Agents 5- - - : : : : : : : : - - - • Bind to metal ions removing them from solution. • Phosphates are used to tie up Ca2+ and Mg2+ in hard water to prevent them from interfering with detergents. Chemistry of Coordination Compounds
22. Chelating Agents • Porphyrins are complexes containing a form of the porphine molecule shown at right. • Important biomolecules like heme and chlorophyll are porphyrins. Chemistry of Coordination Compounds
23. Chelating Agents Porphines (like chlorophyll a) are tetradentate ligands. Chemistry of Coordination Compounds
24. Nomenclature of Coordination Compounds • The basic protocol in coordination nomenclature is to name the ligands attached to the metal as prefixes before the metal name. • Some common ligands and their names are Chemistry of Coordination listed above. Compounds
25. Nomenclature of Coordination Compounds • As always the name of the cation appears first; the anion is named last. • Ligands are listed alphabetically before the metal. Prefixes denoting the number of a particular ligand are ignored when alphabetizing. Chemistry of Coordination Compounds
26. Nomenclature of Coordination Compounds • The names of anionic ligands end in “o”; the endings of the names of neutral ligands are not changed. • Prefixes tell the number of a type of ligand in the complex. If the name of the ligand itself has such a prefix, alternatives like bis-, tris-, etc., are used. Chemistry of Coordination Compounds
27. Nomenclature of Coordination Compounds • If the complex is an anion, its ending is changed to -ate. • The oxidation number of the metal is listed as a Roman numeral in parentheses immediately after the name of the metal. Chemistry of Coordination Compounds
28. Isomers Isomers have the same molecular formula, but their atoms are arranged either in a different order (structural isomers) or spatial arrangement Chemistry of Coordination (stereoisomers). Compounds
29. Structural Isomers If a ligand (like the NO2 group at the bottom of the complex) can bind to the metal with one or another atom as the donor atom, linkage isomers are formed. Chemistry of Coordination Compounds
30. Structural Isomers • Some isomers differ in what ligands are bonded to the metal and what is outside the coordination sphere; these are coordination-sphere isomers. • Three isomers of CrCl3(H2O)6 are The violet [Cr(H2O)6]Cl3, The green [Cr(H2O)5Cl]Cl2 ∙ H2O, and The (also) green [Cr(H2O)4Cl2]Cl ∙ 2 H2O. Chemistry of Coordination Compounds
31. Geometric isomers • With these geometric isomers, two chlorines and two NH3 groups are bonded to the platinum metal, but are clearly different. cis-Isomers have like groups on the same side. trans-Isomers have like groups on opposite sides. # of each atom the same Chemistry of Bonding the same Coordination Arrangement in space different Compounds
32. Stereoisomers • Other stereoisomers, called optical isomers or enantiomers, are mirror images of each other. • Just as a right hand will not fit into a left glove, two enantiomers cannot be superimposed on Chemistry of each other. Coordination Compounds
33. Enantiomers A molecule or ion that exists as a pair of enantiomers is said to be chiral. Chemistry of Coordination Compounds
34. Enantiomers • Most of the physical properties of chiral molecules are the same, boiling point, freezing point, density, etc. • One exception is the interaction of a chiral molecule with plane-polarized light. Chemistry of Coordination Compounds
35. Enantiomers • If one enantiomer of a chiral compound is placed in a polarimeter and polarized light is shone through it, the plane of polarization of the light will rotate. • If one enantiomer rotates the light 32° to the right, the other will rotate it 32° to the left. Chemistry of Coordination Compounds
36. Chemistry of Coordination Compounds
37. Chemistry of Coordination Compounds
38. Chemistry of Coordination Compounds
39. Explaining the properties of transition metal coordination complexes 1. Magnetism 2. color Chemistry of Coordination Compounds
40. Metal complexes and color The ligands of a metal complex effect its color Chemistry of Coordination Addition of NH3 ligand to Cu(H2O)4 changes its colorCompounds
41. Why does anything have color? Light of different frequencies give different colors We learned that elements can emit light of different frequency or color. But these coordination complexes are not emitting light Chemistry of They absorb light. Coordination Compounds How does that give color?
42. Light can bounce off an object or get absorbed by object No light absorbed, all reflected get white color All light absorbed, none reflected get Black color What if only one color is absorbed? Chemistry of Coordination Compounds
43. Complimentary color wheel If one color absorbed, the color opposite is perceived. Absorb Orange See Blue Absorb Red See Green Chemistry of Coordination Compounds
44. 3+ [Ti(H2O)6] Absorbs in green yellow. Looks purple. Chemistry of Coordination Compounds
45. A precise measurement of the absorption spectrum of Compounds is critical Chemistry of Coordination Compounds
46. Metal complexes and color But why do different ligands on same metal give Different colors? Why do different ligands change absorption? Chemistry of Coordination Addition of NH3 ligand to Cu(H2O)4 changes its colorCompounds
47. Model of ligand/metal bonding. Electron pair comes from ligand Bond very polarized. Assumption: interaction pure electrostatic. Chemistry of Coordination Compounds
48. Now, think of point charges being attracted to metal nucleus Positive charge. What about electrons in d orbitals? Ligand negative charge Is repelled by d electrons, d orbital energy goes up Chemistry of Coordination Compounds
49. Ligands will interact with some d orbitals more than others Depends on relative orientation of orbital and ligand Ligands point right at lobes Chemistry of Coordination Compounds
50. In these orbitals, the ligands are between the lobes Interact less strongly Chemistry of Coordination Compounds
51. Splitting due to ligand/orbirtal orientation. Chemistry of Coordination Compounds
52. Chemistry of = 495 nm Coordination Compounds
53. Different ligands interact more or less, change E spacing Of D orbitals. Chemistry of Coordination Compounds
54. Spectrochemical series (strength of ligand interaction) Increasing - - - - Cl < F < H2O < NH3 < en < NO2 < CN Increasing Chemistry of Coordination Compounds
55. Electron configurations of some octahedral complexes Chemistry of Coordination Compounds
56. As Energy difference increases, electron configuration changes “Low spin” “High spin” Co(III) is d6 Chemistry of Coordination Compounds
57. Chemistry of Coordination Compounds
58. Tetrahedral Complexes In tetrahedral complexes, orbitals are inverted. Again because of orientation of orbitals and ligands is always small, always low spin (less ligands) Chemistry of Coordination Compounds
59. Square planar complexes are different still Chemistry of Coordination Compounds
60. Chemistry of Coordination Compounds
61. Chemistry of Coordination Compounds
62. Intense color can come from “charge transfer” Ligand electrons jump to metal orbitals KMnO4 KCrO4 KClO4 No d orbitals in Cl, orbitals higher In energy Chemistry of Coordination Compounds
63. Chemistry of Coordination Compounds
64. Exam 4, MO theory and coordination compounds Chapter 9, end and Chapter 24. MO theory: Rules: • 1. The number of MO’s equals the # of Atomic orbitals • 2. The overlap of two atomic orbitals gives two molecular orbitals, 1 bonding, one antibonding • 3. Atomic orbitals combine with other atomic orbitals of similar energy. • 4. Degree of overlap matters. More overlap means bonding orbital goes lower in E, antibonding orbital goes higher in E. • 5. Each MO gets two electrons • 6. Orbitals of the same energy get filled 1 electron at a time until they are filled. Chemistry of Coordination Compounds
65. Difference between pi and sigma orbitals End on Side to side. Chemistry of Coordination Compounds
66. A typical MO diagram, like the one below. For 2p and 2s atomic orbital mixing. Chemistry of Coordination Compounds
67. Oxygen O2 is Paramagnetic, why? Chemistry of Coordination Compounds
68. Show me why. Chemistry of Coordination Compounds
69. Exam 4 Chapter 24. Concentrate on the homeworks and the quiz! Terms: 1. Coordination sphere 2. Ligand 3. Coordination compound 4. Metal complex 5. Complex ion 6. Coordination 7. Coordination number Same ligands different properties? Figuring oxidation number on metal Chemistry of Coordination Compounds
70. Polydentate ligands (what are they)? Isomers. structural isomers (formula same, bonds differ) geometric isomers (formula AND bonds same, structure differs) Stereoisomers: Chirality, handedness, Chemistry of Coordination Compounds
71. Chemistry of Coordination Compounds
72. Stereoisomers Chemistry of Coordination Compounds
73. Explaining the properties of metal complexes Magnetism and color How does seeing color work? Absorb Orange See Blue Absorb Red See Green Chemistry of Coordination Compounds
74. Different ligands on same metal give different colors Addition of NH3 ligand to Cu(H2O)4 changes its color Chemistry of Coordination Compounds
75. Splitting of d orbitals in an oxtahedral ligand field 2 2 2 dz dx -y dxy dyz dxz Chemistry of Coordination Compounds
76. Spectrochemical series (strength of ligand interaction) Increasing - - - - Cl < F < H2O < NH3 < en < NO2 < CN Increasing Chemistry of Coordination Know low spin versus high spin Compounds
77. There is also splitting from tetrahedral And square planar. Know they are different, don’t remember exactly what they are like. Chemistry of Coordination Compounds