Coordination Compounds. Compounds containing Transition Metals
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1 Coordination Compounds Compounds containing Transition Metals
2 Coordination Compounds Transition Metals Sc 6 Cu 1st row Y 6 Ag 2nd row La 6 Au 3rd row
3 Properties of metals Not as reactive as group 1 or 2 1s or 2s valence electrons Highly colored compounds High mp, bp, density Hard, strong, conductors Form complex ions Many oxidation states Catalytic activity
4 Trends Down group: Same outer electron configuration Decrease in reactivity Across period Increase in atomic no. Increase in atomic mass Increase in nuclear charge, I.E. Slight decrease in radii
5 Reaction with acid Many react: Fe, Ni, Co 6 hydrogen Some inert: Cr, Au, Pt
6 Electron configuration 20Ca: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 = [Ar]4s 2 = 4s 2 21Sc 6 Cu e - added to 3d subshell 29 21Sc: 4s 2 3d 1 22Ti: 4s 2 3d 2 Exception: 24Cr: 4s 1 3d 5
7 Ions When metals lose elections to form (+) ions, electrons come from 4s before 3d Co: 4s 2 3d 7 6 Co 3+ : 3d 6
8 Oxidation states Variable in compounds Mostly +2 or +3 Reaches max at center of series High: VF Mn O CrO
9
10 Transition Metals
11 Naming Compounds Compounds may be: Cation Neutral Anion [Co(NH 3 ) 4 Cl 2 ]Br [Ni(CO) 4 ] K 3 [Fe(CN) 6 ] Learn steps for naming
12 Naming Compounds 1. Name cation, then anion (unless neutral) 2. Name ligands first (alphabetical) name metal give metal oxidation state
13 Naming Compounds Ligand Names: (table 20.3) Br - bromo CN - cyano H O aquo 2 NH ammine 3 CO carbonyl C O 2- oxalato 2 4
14 Naming Compounds Indicate number of ligands by prefix: di tri tetra penta hexa prefix not included in alphabetical order If ligand name has prefix use: bis tris tetrakis bis(ethylenediamine)
15 Naming Compounds 3. Metal oxidation state: iron(iii) 4. Anionic complex: table 20.4 add -ate ending to metal cobaltate chromate titanate ferrate cuprate aurate 5. Neutral complex: one word
16 Naming Compounds [Ag(NH ) ]Cl 3 2 [Ag(NH ) ] + Cl [Ag + (NH ) 0 2] + Cl - 3 diamminesilver(i) chloride
17 Naming Compounds K [Fe(CN) ] 4 6 K 4+ [Fe(CN) ] K 4+ [Fe 2+ (CN) 6-6] 4-4 potassium hexacyanoferrate(ii)
18 Naming Compounds [Co(NH 3 ) 4 (H 2 O)Cl]Cl 2 [Co(NH 3 ) 4 (H 2 O)Cl] 2+ Cl 2 2- [Co 3+ (NH 3 ) 0 4(H 2 O) 0 Cl - ] 2+ Cl 2 2- [cobalt(iii) tetraammine aquo chloro] chloride aquochlorocobalt(iii) chloride
19 Naming Compounds [Co(NH 3 ) 3 Cl 3 ] triamminetrichlorocobalt(iii)
20 Writing Formulas diamminedibromoplatinum(iv) chloride [Pt 4+ (NH 3 ) 2 Br 2 ] Cl
21 Writing Formulas potassium hexacyanoaurate(iii) K + [Au (CN) ] 3 6 K 3 [Au(CN) 6 ]
22 Isomers
23 Isomers
24 Isomers
25 Bonding Bonding theory must explain Color Magnetism Isomerism Bond Strength
26 Bonding Crystal Field Theory (CFT) Color Magnetism What bonds ligand to metal?
27 Crystal Field Theory 1. (+) metal : (-) ligand Y attraction 2. metal d e - : ligand lone pairs Y repulsion Know shapes of d-orbitals Fig 20.11
28 Crystal Field Theory Fig 20.11
29 Crystal Field Theory Lobes point along axes
30 Crystal Field Theory Lobes point between axes
31 Crystal Field Theory <Ligands approach along axes <Repels d-electrons <All orbitals go up in energy <Orbitals along axes go up more in energy
32 Crystal Field Theory CF splitting ) is energy difference
33 Crystal Field Theory What determines if ) is large or small? Metals Ligands Structure Size of ) determines color and magnetism
34 Crystal Field Theory
35 Fig 20.18Fig Fig 20.19
36 Crystal Field Theory For a given metal and ligand: ) o > ) t ) increases with increasing oxidation number
37 Crystal Field Theory For a given metal & oxidation state: Ligands ordered in spectrochemical series Ligands determine magnetic properties & )
38 Lots of unpaired e - Few unpaired e -
39 Counting d-electrons 21Sc 6 29 Cu Electrons added to 3d subshell 21Sc 6 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 1 21Sc 6 [Ar]4s 2 3d 1 22Ti 6 [Ar]4s 2 3d 2 Exceptions 24Cr 6 [Ar]4s 1 3d 5
40 Counting d-electrons When metals lose electrons to form ions, electrons come from 4s first 22Ti 6 [Ar]4s 2 3d 2 22Ti 2+ 6 [Ar]3d 2 Ti 2+ : d 2
41 Counting d-electrons When metals lose electrons to form ions, electrons come from 4s first 27Co 6 [Ar]4s 2 3d 7 27Co 3+ 6 [Ar]3d 6 Co 3+ : d 6
42 Magnetic Properties Odd number of d e - : paramagnetic Even number of d e - : diamagnetic
43
44 Color Wheel
45 Calculating ) [Ti(H 2 O) 6 ] 3+ Ti 3+ 6 [Ar]3d 1 Absorbed light 6 electron to jump 6 )
46 Calculating ) [Ti(H 2 O) 6 ] 3+ is a violet compound Absorbs yellow light: 8 = 550 nm = hν = hc λ
47 Calculating ) [Ti(H 2 O) 6 ] 3+ is a violet compound Absorbs yellow light: 8 = 550 nm = ( Js) ( 3 10 m / s) m 8
48 Calculating ) [Ti(H 2 O) 6 ] 3+ is a violet compound Absorbs yellow light: 8 = 550 nm = ( Js) ( 3 10 m / s) m 8 = J
49 White compounds When ) very large (>800 nm) or very small (<200 nm) falls outside of visible region When have no d electrons Mn 7+ or too many Zn 2+
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