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Transition Metals:

Inorganic Chemistry: Transition Metals

QuestionAnswer
1. where are most transition metals? d block - metals contain an incomplete d sub shell
2. when does a coordinate bond form? electrons pair form bond comes from one atom
3. why is Zn not a transition metal? only 1 oxidation state (+2) and is white transition metals form different colours at different oxidation states
4. coloured ions? because they lose variable number of ions at different oxidation states
5. form complexes? ligands form co-ordinate bonds to metal ions
6. oxidation states? exhibit variable oxidation states
7. another property? catalyst
8. describe their metallic nature? hard dense good conductors of heat + electricity high MP + BP (due to partially filled D block)
9. what is a ligand? ion/molecule which forms coordinate bonds with a transition metal atom / ion by donating a pair of electrons
10. what is a complex? central metal atom / ion with ligands co-ordinately bonded to it
11. what is the coordination number? number of coordinate bonds from ligands to metal ions
12. what is a lewis base for ligands? lone pair donor of ligands
13. what is a lewis acid for ligands? lone pair acceptor of ligands
14. FeEDTA? coordination number = 6 (multidentate)
15. what are unidentate/ monodentate ligands? form 1 coordinate bond to metal atom / ion
16. examples of unidentate / monodentate ligands? H2O OH- NH3 CN- Cl-
17. what are bidentate ligands? form 2 coordinate bonds to metal atom / ions
18. examples of bidentate ligands? 1,2-diaminoethane (en) -> eg Cr(NH2CH2CH2NH2)
19. what are multidentate ligands? form several coordinate bonds to metal atom / ions
20. examples of multidentate ligands? EDTA4-
21. describe EDTA4- coordination number =6 very stable put in rivers to remove poisonous heavy metal ions in shampoo to remove Ca ions
22. what is the chelate effect? substitution of monodentate by bi/multidentate to form more stable coordinate bonds increase of molecules positive entropy negative G and enthalpy close to 0
23. what is ligand substitution? ligand co-ordinately bonded to a metal atom/ ion in a complex ion is replaced by another ligand
24. if ligand substitution is similar size? coordination number no change
25. if ligand substitution is different size (bigger)? coordination number change
26. what determines shape and bond angle of complexes? charges on ligands which repel each other and coordination number
27. how can Cl- be substituted? from conc HCl or saturated NaCl
28. what is incomplete ligand substitution? when only some of the original ligands are substituted
29. LOST? linear octahedral square planar tetrahedral
30. octahedral shape? small ligands bond angle = 90 degrees eg [Co(NH3)6]2+ and [Cu(H2O)6]2+
31. tetrahedral shape? larger ligands bond angle = 109.5 degrees eg [CoCl4]2- and [FeCl4]- and [CuCl4]2-
32. square planar shape? usually Pt (platinum) usually no overall charge bond angle = 90 degrees eg [Pt(NH3)2Cl2]
33. linear shape? bond angle = 180 degrees eg [Ag(NH3)2]+ (used as Tollens's reagent)
34. stereoisomerism in octahedral shapes? monodentate ligands = cis/trans isomerism bidentate ligands = optical isomerism
35. stereoisomerism in square planar shapes? cis/ trans isomerism
36. degrees for cis? within 90 degrees of each other
37. degrees for trans? within 180 degrees of each other
Created by: chachink
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