Download Document

Inorganic Chemistry Homework I
2013, 06 . 11
(Due 2013. 06. 17)
1. Give plausible explanations for the following observations.
(a) The X-ray structure of CuCl53- complex shows that equatorial bond distances are longer
than the axial bond distances.
(b) The Ni(II) complexes in square-planar geometry have shorter Ni-L bond distances than
those in octahedral arrangement.
(c) [ReF8]2- has a square antiprismatic structure. Why is this more stable than cubic
coordination for rhenium(VI)?
(d) Chromium(II) fluoride and manganese(II) fluoride both have a central metal ion
surrounding with six fluoride ligands. The Mn-F bond lengths are equidistant, but four
of the Cr-F distances are long and two are short. Provide an explanation.
2. Draw the expected ionic radii for the low spin M3+ ions.
Sc Ti
V Cr Mn Fe
Co Ni Cu Zn Ga
3. Urea (NH2CONH2) ligand usually bond through the oxygen atom, although there are two
potential nitrogen donor atoms available as well. If you did not have the X-ray crystal
structure, what other experimental evidence might you use to differentiate between Obonding and N-bonding.
4. Sketch the d-orbital energy level diagrams for the following types of complexes.
a) 8-coordinate, square-antiprism b) 5-coordinate, square pyramidal
b) 6-coodinate, trigonal prismatic
5.
List the following ligands in the increasing order of Dq values.
Cl-, OH-, H2O, CN-, NH3, F-
6.
The following compounds have the indicated effective magnetic moments. Describe
the electronic configuration (eg. t2gxegy
eff values.
A.[Co(NH3)6](ClO4)2, 4.0 BM
B. Ni(PEt3)2Cl2; 0.0 BM
C. Ni(Ph3AsO)2Cl2; 3.95 BM
7.
List the possible isomers and geometry possible for a compound of the formula
NiCl2(PPh3P)2. How would you distinguish among the possible isomers?