Unless otherwise stated, all images in this file have been reproduced from:
Blackman, Bottle, Schmid, Mocerino and Wille, Chemistry, 2007 (John Wiley)
ISBN: 9 78047081 0866
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e CHEM1002 [Part 2]
A/Prof Adam Bridgeman (Series 1)Dr Feike Dijkstra (Series 2)
Weeks 8 – 13
Office Hours: Monday 2-3, Friday 1-2Room: 543ae-mail: [email protected]: [email protected]
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Complexes I
• Solutions of metal ions are acidic because coordinated water loses H+ and this increases with the charge of the metal ion
• Ligands use lone pairs to bond to transition metal ions• Coordination compounds are made up of a complex ion,
containing a metal ion and ligands, and counter ions to balance the charge
• The common geometries of complex ions are tetrahedral and square planar (both 4 coordinate) and octahedral (6 coordinate)
Summary of Last Lecture
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Lecture 13• Isomerism• Stability• Blackman Chapter 13, Sections 13.1-13.4
Lecture 14• Transition Metals• Electron Configuration• Oxidation States• Colours• Magnetism• Blackman Chapter 13, Sections 13.4 and 13.7
Complexes II
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e Isomerism in Metal Complexes (1)
• Structural Isomerism: different atom connectivities If the counter ions are also potential ligands, they can
swap places to produce coordination sphere isomers:
[Cr(OH2)4Br2]Cl [Cr(OH2)4BrCl]Br
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H3NPt
Cl
Cl
H3N
ClPt
Cl
NH3
H3N
cis trans
Isomerism in Metal Complexes (2)
• Stereoisomerism: same atom connectivities but different arrangement of atoms in space geometric isomerism
cis trans
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mirror imagessuperposable(i.e. the same!)
mirror imagesnon-superposable
mirror imageOPTICALLY
ACTIVE
NiN N
NNOH2
OH2
2+
NiN N
NNOH2
OH2
2+
2+
NiH2O N
NH2ON
N
NiN OH2
OH2NN
N
2+
Isomerism in Metal Complexes
transisomer
cisisomer
• Stereoisomerism: same atom connectivities but different arrangement of atoms in space optical isomerism
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e Isomerism in Metal Complexes• Stereoisomerism: same atom connectivities but different
arrangement of atoms in space optical isomerism
[Ni(en)3]3+
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e Equilibria Involving Complexes
• Unlike the covalently bonded polyatomic ions such as NO3-,
SO42-, etc., which do not dissociate into their components,
metal complexes in solution are in an equilibrium:
[M(OH2)6]2+ + 6NH3 [M(NH3)6]2+ + 6H2O
[M(NH3)6]2+ + 3en [M(en)3]2+ + 6NH3
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e [Ni(H2O)6]2+ + 3en [Ni(en)3]2+ + 6H2O
Kstab =
Kstab = K1 K2 K3 = 1018.28
[Ni(en)2(H2O)2]2+ + en [Ni(en)3]2+ + 2H2Opurple
[Ni(en)(H2O)4]2+ + en [Ni(en)2(H2O)2]2+ + 2H2Olight blue
[Ni(H2O)6]2+ + en [Ni(en)(H2O)4]2+ + 2H2Ogreen blue-green
Stepwise Formation Constants
[[Ni(H2O)6]]2+][en]3
[[Ni(en)3]2+] = 1018.28
K2
K1
K3
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• Metal complex formation can greatly influence the apparent solubility of a compound.
AgCl(s) + 2NH3(aq) [Ag(NH3)2]+(aq) + Cl-(aq)
• This is actually a two stage process:
AgCl(s) Ag+(aq) + Cl-(aq) (1)
Ag+(aq) + 2NH3(aq) [Ag(NH3)2]+(aq) (2)
• Complex formation (reaction 2), removes free Ag+ from solution and so drives the dissolution of AgCl (reaction 1) forward.
Metal Complex Formation and Solubility
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i The One Pot Reaction
Ag+(aq) + OH-(aq) AgOH(s) brown AgOH(s) + H2PO4
-(aq) AgH2PO4(s) yellowAgH2PO4(s) + HNO3(aq) Ag+(aq) + H3PO4(aq)Ag+(aq) + Cl-(aq) AgCl(s) white Ksp = 1.8 x 10-10 M2
AgCl(s) + 2 NH3(aq) [Ag(NH3)2]+(aq) + Cl-(aq) Kstab = 1.7 x 107 M-2
[Ag(NH3)2]+(aq) + Br-(aq) AgBr(s) (green/white), Ksp = 5 x 10-13 M2
AgBr(s) + 2 S2O32-(aq) [Ag(S2O3)2]3-(aq)+Br-(aq) Kstab = 2.5 x 1013 M-2
[Ag(S2O3)2]3-(aq) + I-(aq) AgI(s) (yellow) Ksp = 8.3 x 10-17 M2
AgI(s) + 2 CN-(aq) [Ag(CN)2]-(aq) + I-(aq) Kstab = 6.3 x 1019 M-
2 [Ag(CN)2]-(aq) + S2-(aq) Ag2S(s) (black) Ksp = 8 x 10-51 M3
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e Summary: Complexes IILearning Outcomes - you should now be able to:
• Complete the worksheet• Identify isomers of complexes correctly• Answer review problems 13.59-13.62 in Blackman
Next lecture:
• Colour
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x Practice Examples1. What are the possible geometries of a metal complex with a
coordination number of 4?
A.square planar or tetrahedral or octahedralB.square planar or tetrahedralC.octahedral onlyD.tetrahedral onlyE.square planar only
2. Which one of the following is a coordination isomer of the complex salt,
trans- [Cr(H2O)4Cl2]Br?
A.cis- [Cr(H2O)4Cl2]BrB.trans- [Cr(H2O)4BrCl]ClC.trans- [Cr(H2O)4Br2]ClD.trans- [CrBr2(H2O)4]ClE.trans- [CrCl2(H2O)4]Br
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x Practice Examples3. Which of the following species exist as isomers?
[Co(NH3)6]3+, [PtCl2(NH3)2], [Co(OH2)6]Cl3, [Co(OH2)6]2+, [CdI4]2–
A.[PtCl2(NH3)2] and [Co(OH2)6]Cl3B.[PtCl2(NH3)2] onlyC.[CdI4]2– onlyD.[Co(NH3)6]3+ and [Co(OH2)6]2+
E.[Co(OH2)6]Cl3 and [Co(OH2)6]2+
4. How many geometrical isomers are possible for the complex [CrCl3(NH3)3]?
A.1B.2C.3D.4E.6