bonding in transition metals and coordination complexes
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Bonding in Transition Metals and Coordination Complexes. Bonding in Transition Metals and Coordination Complexes. Chemistry of the Transition metals. Properties. Atomic Radius : lanthanide contraction – unusual contraction of lanthanide ions. - PowerPoint PPT PresentationTRANSCRIPT
Bonding in Transition Metals and Coordination Complexes
Bonding in Transition Metals and Coordination Complexes
Chemistry of the Transition metals
Properties
Atomic Radius : lanthanide contraction – unusual contraction of lanthanide ions.
Binding energy: higher – more unpaired electrons i.e.) m.p. -- higher in the middle of the row : W ( 3410oC), Hg (-39oC)
Oxidation states: higher oxidation state– more covalent bond character lower oxidation state – more ionic bond character
Mn(OH)2, Mn(OH)3, H2MnO3, H2MnO4, HMnO4
basic acidic
Chemistry of the Transition metals
Coordination complex ; coordination chemistry 배위화학
CuSO4 : greenish white
Coordination complex : Cu(H2O)42+
CuSO4.4H2O : bluev.s.
Mn+ + mL M Lmn+
coordinationLigand
Lewis baseLewis acid
Ag+ + 2NH3 (Ag(NH3)2+
Au+ + 2CN- (Au(CN)2-
Coordination number : total number of metal-to-ligand bondUsually 2 ~ 6
Ligands
Br-
Cl-
N3-
CN-
OH-
NH3
H2O
CO
NO2-
O2-
Bromo
Chloro
Azido
Cyano
Hydroxo
Ammine
Aqua(o)
Carbonyl
Nitro
Oxo
H-
ONO-
SCN-
NCS-
NO+
CO32-
Hydrido
Nitrito
Thiocyanato
Isothiocyanato
Nitrosyl
Carbonato
OxalateO
-O
O
O-
H2N NH2Ethylenediamine (En)
bidentateligand
chelates
Nomenclature
NH4[Cr(NH3)2(NCS)4] Reinecke’s salt
Systematic naming
[Co(NH3)5Cl]Cl2 Purpureocobaltic chloride
[Co(NH3)5Cl]Cl2 Pentaamminechlorocobalt(III) chloride
K4[Fe(CN)6] Potassium Hexacyanoferrate(II)
Making coordination complex
charge of a complex = sum of charges of metals and ligandscharge of a complex + charges of counter ions = 0
coordination number = numbers of donor atoms
Rules of Nomenclature
1. Cation Anion b
2. In the complex : names of ligands come first and then name of metal among ligands : alphabetical order
3. Names of ligands : anion – change the last letter to o neutral – same as the original ones
4. Counting number of ligands : di, tri, tetra, penta, hexa, hepta….. if the ligand contains these names in it, use : bis, tris, tetrakis, pentakis……
5. If the compex is an anion : at the end of the name put ate
6. Oxidation number of metal : in parenthesis with roman letter - (IV)
Pentaamminechlorocobalt(III) chloride Potassium Hexacyanoferrate(II)
Influence of Coordination
1. Color
Pale yellow
[Fe(H2O)6]3+ + SCN- [Fe(H2O)5SCN]2+ + H2O
orange
2. Reduction potential
Ag+ + e- Ag Eo = +0.799V
[Ag(CN)2]+ + e- Ag Eo = -0.31V+ 2CN-
3. Chemical reactivity
Structure of coordination complexes
CoCl3.6NH3
CoCl3.5NH3
CoCl3.4NH3
CoCl3.3NH3
Chemical formular(19thC.) color
orange-yellow
pruple
green
green
[Co(NH3)6]3+Cl-3
Chemical formular (Werner)
[Co(NH3)5Cl]2+Cl-2
[Co(NH3)4Cl2]+Cl-
[Co(NH3)3Cl3]
structure
octahedral
[Co(NH3)6]3+Cl-3
[Co(NH3)5Cl]2+Cl-2
[Co(NH3)4Cl2]+Cl-
Cl +2
[Co(NH3)3Cl3]
[Co(En)2Cl2]+Cl-
cis transGeometrical isomers
Chiral structures
[Co(NH3)2(H2O)2Cl2]+
[Pt(En)3]4+
Structure of coordination complexes
Linear[Ag(NH3)2]+
[Zn(NH3)4]2+
Atomic orbitalof metal
coordinationnumber
2
structure
Tetrahedral4
[Pt(NH3)4]2+ Square Planar4
[Co(NH3)6]3+ Octahedral6
d10
d9
d8
d6
Super chelating ligand
EDTA ( ethylenediaminetetraacetate)
Strong affinity to certain metal ionsSolubilize metal ions
[Ni(H2O)6]2+ + 6NH3 [Ni(NH3)6]2+ + 6H2O
Kf = 4 x 108
[Ni(H2O)6]2+ + 3en [Ni(en)3]2+ + 6H2O
Kf = 2 x 1018
Entropy factor : bigger S
Transition Metals
Partially filled d orbitals
Octet rule in transition metal chemistry : 18 electron rule
Coordination complexStructural variety
Low-lying unoccupied orbitals color
Unpaired electrons Magnetic property
Many oxidation states Catalysts, new reactions
Ligands Donates electron pairs
coordination Changes color, reactivity, reduction potential
number of electrons in 4s + 3d + 2 x number of ligands = 18
18-electron rule for transition metal complexes
Octet rule : Lewis structure
consider a transition metal : Cr
Chromium: [Ar] (4s)2(3d)4 6 valence electrons
Chromium need 18 electrons in its most outer shell. 18-electron rule
Therefore the complex of Cr with CO will look like
i.e. CO provides 2 x 6 = 12 electrons Cr provides 6 electrons
Total 18 electrons
Using the 18-electron rule
Given that H2Fe(CO)x exists, what does x equal?
Iron: [Ar] (4s)2(3d)6 8 valence electrons 8
n = 4
Total : 10 + 2n = 18 electrons
hydrogen: 1s1 1 valence electrons x 2 = 2
CO: 2 valence electrons x n = 2n
H2Fe(CO)4
Understanding of metal-ligand binding mode
1. Color : only for partially filled d orbitals i.e. d0, d10 : colorless
facts
2. magnetism: paramagetic v.s. diamagnetic unpaired electrons
[Co(NH3)6]3+ diamagnetic – no unpaired electrons
[CoF6]3- paramagnetic – 4 unpaired electrons
[CrF6]3- [Cr(H2O)6]3+ [Cr(NH3)6]3+
[Cr(CN)6]3-
green violet yellow yellow
3. tetrahedral or square planar
[NiCl4]2- [Ni(CN)4]2-
tetrahedral square planar
Crystal Field Theory
Color, magnetic properties, and choice of tetrahedral, square planar & octahedralHow to explain
Crystal field theory : ionic description of the metal-ligand bonds
Consider only the energy changes of d orbitals of metal during coordination
Consider only electrostatic interaction with ligands : charge-charge, charge-dipole
Begin with octahedral geometry
Low spin complex : when o is large
High spin complex : when o is small
magnetism
d1 ~ d5 : always paramagnetic
d7 ~ d9 : always paramagnetic
d10 : always diamagnetic
d6 : depending on the ligands
Square planar & tetrahedral complexes
Tetrahedral Reversal of octahedral !
M
Square planar & tetrahedral complexes
Tetrahedral
Reversal of octahedral !
Square planar & tetrahedral complexes
Square planar Removal of axial ligands from octahedral
Square planar Removal of axial ligands from octahedral
I- < Br- < Cl- < F-, OH- < H2O < NCS- < NH3 < en < CO, CN-
Spectrochemical Series
Color of complexes and magnetic properties are determined by o
o can be determined by ligands
Weak field Ligands Strong field Ligands
small olarge o
High spin complex Low spin complex
[CoF6]3- [Co(CN)6]3-v.s.
Weak point of crystal field theory
1. Coordination is not fully ionic.
2. Spectrochemical series is all empirical. Ligand field theory
Ligand Field Theory
Consider ionic interaction onlyCrystal field theory :
Modification : addition of covalent aspect of coordination.
How? : construction of molecular orbitals.
Using 4s, 4p, 3d orbitals of metals & coordinating orbitals of ligands
Ligand field theory :
For an octahedral complex
1. Orbital overlap is 0 for dxy, dyz, dzx
become nonboinding orbitals
2. Varying overlapping ligand orbitals
for Cl- : p NH3 : sp3
3. MO’s can be formed from 6 ligand orbitals and 6 metal orbitals (4s, 4p, 3d)
For [CoF6]3-
I- < Br- < Cl- < F-, OH- < H2O < NCS- < NH3 < en < CO, CN-
Now, we can explain Spectrochemical Series
Weak field Ligands Strong field Ligands
small olarge o
Interaction between dxy of metal and py of halide :
ionic ---- increases energy level of t2g
Makes smaller o for I- and less smaller one for F-
back-bonding
bonding of ligand can overlap with dxy orbital
Lowers the energy level of t2g
Makes larger o for CO, CN-
For [CoF6]3-
Organometallic compounds and Catalysis
Catalytic converter : Pt catalyst
CO + O2 CO2
Pt ( cat.)
Haber process
N2 + 3H2 NH3
Fe ( cat.)
Olefin metathesis reaction
+Ru ( cat.)X
Y
Z
W
+
ZX
WY“Grubbs catalyst”
2005 Nobel Prize in Chemistry
Coordination complexes and Life
We need transition elements for life : V, Cr, Mn, Fe, Co, Ni, Cu, Zn, Mo…….
Porphine structure Important for oxygen transfer, detoxification,
photosynthesis, nitrogen fixation
숙제18 장 : 6, 12, 22, 26, 34, 42, 46
제출일 : 10 월 19 일