4. 20_431
Sc Ti V Cr Mn Fe Co Ni Cu Zn
Y Zr Nb Mo Tc Ru Rh Pd Ag Cd
La Hf Ta W Re Os Ir Pt Au Hg
Ac Unq Unp Unh Uns Uno Une Uun Uuu
Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
5. 20_432
d-block transition elements
Sc Ti V Cr Mn Fe Co Ni Cu Zn
Y Zr Nb Mo Tc Ru Rh Pd Ag Cd
La* Hf Ta W Re Os Ir Pt Au Hg
Ac† Unq Unp Unh Uns Uno Une Uun Uuu
f-block transition elements
*Lanthanides Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
† Actinides Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr
6.
7.
8.
9.
10. 20_435
0.2
La
1st series (3d)
Y 2nd series (4d)
Hf 3rd series (5d)
Atomic radii (nm)
Zr
Sc Ta
Au
Nb W Ag
0.15 Re
Mo Os Pt
Ti Tc Ru Ir
V Rh Pd
Cr Fe Cu
Mn Co Ni
0.1
Atomic number
13. Color and Magnetism
e- in partially filled d sublevel absorbs visible light
moves to slightly higher energy d orbital
Magnetic properties due to unpaired electrons
16. Valence-State Electronegativity
Electronegativity, EN:
electron “pulling power”
Valence-state EN:
metal in higher oxidation state
is more positive
has stronger pull on electrons
is more electronegative
“Effective EN”
21. Coordination Compound
Consist of a complex ion and necessary counter ions
[Co(NH3)5Cl]Cl2
Complex ion: [Co(NH3)5Cl]2+
Co3+ + 5 NH3 + Cl-
= 1(3+) + 5 (0) + 1(1-)
= 2+
Counter ions: 2 Cl-
22. [Co(NH3)6]Cl3 [Pt(NH3)4]Br2
Complex ion remains intact upon dissolution in water
23. Complex Ion
Species where transition metal ion is surrounded
by a certain number of ligands.
Transition metal ion: Lewis acid
Ligands: Lewis bases
Co(NH3)63+
Pt(NH3)3Br+
24.
25. Ligands
Molecule or ion having a lone electron pair that
can be used to form a bond to a metal ion
(Lewis base).
coordinate covalent bond: metal-ligand bond
monodentate: one bond to metal ion
bidentate: two bond to metal ion
polydentate: more than two bonds to a metal
ion possible
26.
27.
28. Formulas of Coordination Compounds
1. Cation then anion
2. Total charges must balance to zero
3. Complex ion in brackets
K2[Co(NH3)2Cl4]
[Co(NH3)4Cl2]Cl
29. Names of Coordination Compounds
1. Cation then anion
2. Ligands
in alphabetical order before metal ion
neutral: molecule name*
anionic: -ide → -o
prefix indicates number of each
3. Oxidation state of metal ion in () only if more
than one possible
4. If complex ion = anion, metal ending → -ate
37. Structural Isomerism 2
Ligand isomerism:
Same complex ion structure but point of
attachment of at least one of the ligands differs.
[Co(NH3)4(NO2)Cl]Cl
and [Co(NH3)4(ONO)Cl]Cl
41. 20_444
Cl
Cl
H3N NH 3
H3N NH3
Co Co
H3N NH 3 H3N Cl
Cl NH 3
Cl Cl
Co Co
Cl
Cl
(a) (b)
42. Stereoisomerism 2
Optical isomerism:
20_446
Have opposite effects on plane-polarized light
(no superimposable mirror images)
Polarizing
filter
Tube
containing
Unpolarized
sample
light θ
Polarized
light
Rotated
polarized light
43. 20_448
Mirror image
of right hand
Left hand Right hand
44.
45. 20_449
N
N N
Mirror image
Co
N N of Isomer I
N
N N
N N N N
Co Co
N N N N
Isomer I Isomer II
N N
46. 20_450
Cl The trans isomer and Cl Isomer II cannot be
its mirror image are superimposed exactly
N N identical. They are not N N on isomer I. They are
Co isomers of each other. Co not identical structures.
N N N Cl
Cl Cl Cl
Cl N
N N N Cl N N
trans Co cis Co Co
N N N N N Cl
Cl Isomer I N Isomer II N
Isomer II has the same
structure as the mirror
(a) (b) image of isomer I.
47.
48.
49.
50. Crystal Field Theory
Focus: energies of the d orbitals
Assumptions
1. Ligands: negative point charges
2. Metal-ligand bonding: entirely ionic
strong-field (low-spin): large splitting of d orbitals
weak-field (high-spin): small splitting of d orbitals
51.
52.
53. 20_454
eg(d z2, d x 2 – y2)
∆
t2g (d xz, d yz, d xy)
E
∆ = crystal field splitting
Free metal ion
3d orbital
energies
64. 20_461
Square Planar & Linear Complexes
dx2 - y2
dz2
E
E dxy dxz dyz
dz2
dxy dx2 - y2
dxz dyz
Free metal ion Complex
Free metal ion Complex
x
M
M z
y
(a) (b)
Approach along x-and y-axes Approach along z-axis