1. CHEM 232 Inorganic Chemistry II (Spring 2006)
Instructor: Wa-Hung Leung (ext. 7360,
Office: Rm 4528 (Lift 25/26), Lab: Rm 7141
TAs: (1) Zhang Li
(2) Yi Xiaoyi
(3) Wong Wang Yee
(4) Au Yeung Siu Fung
Class schedule:
Lecture: Mon/Wed/Fri, 13:00-13:50 (Rm 2464)
Tutorial/example class (4) : To be confirmed

2. Course Contents Coordination Chemistry Crystal field theory
Spectral, magnetic, thermochemcial properties
Coordination equilibria, chelate effect
2. Organometallic chemistry
18 e rule,
Carbonyl, olefin, cycloolefin compounds,
Organometallic reactions, homogeneous catalysis
3. Main group chemistry
Hydride and alkyl compounds
Element-element multiple bonds
Inorganic rings and cages
Silicates and aluminosilicates

3. Assessment scheme Attendance of lectures and Quizzes (4) 8%
Assignments (2) 2x4%
Mid-term exam (~ week 8/9) 38%
Final exam 40%
Tutorials (4) and others 6%
Check out a PRS handset!

4. Textbooks and references books
“Inorganic Chemistry” by C. E. Housecroft and A. G. Sharpe, Prentice Hall (1st ed., 2001; 2nd ed., 2005)
Other suggested readings:
Inorganic Chemistry, 3rd ed., by D. F. Shriver et al., OUP (1999).
Basic Inorganic Chemistry, 3rd ed., by F. A. Cotton et al., Wiley (1995)
Concepts and Models of Inorganic Chemistry, 3rd ed., by B. Douglas et al., Wiley (1994)
Inorganic Chemistry, 3rd ed., by G.L. Miessler and D.A. Tarr, Prentice Hall (2004)

5. Websites Course homepage: http://webct.ust.hk Useful links
Department of Chemistry:
Textbook website:
Periodic table: For example,
Conduct in classroom:

6. Coordination Chemistry
Ref.: Housecroft (Chap. 20), Shriver (Chap. 7)
Introduction: the metals and ligands
Crystal field theory: octahedral, tetrahedral, and square planar geometry
Spectrochemical series (strong/weak field ligands)
Electron configurations: LFSE, LS and HS config.
Spectral, magnetic and thermochemical properties
Coordination equilibria, chelate effect
M.O. diagram of ML6

7. Coordination compounds (metal complexes)
Common geometry

8. The metals Transition elements (http://www.rsc.org/is/viselements.htm)
Elements with incomplete d shell
(A) Position
First/ second/ third row TMs
Size decreases down a group
Lanthanide contraction (filling of f orbitals)
Sizes of 2nd row and 3rd row TMs are similar
Ion Cr3+ Mo3+ Ru3+ Ir3+
Size/Å (CN = 6)

10. (B) Early/late TMs
Early: on the LHS of the periodic table (e.g. Ti)
Late: on the RHS of the periodic table (e.g. Pt)
Usually, for metal complexes
Early TM : high metal oxidation state, e.g. Ti(IV), V(V) (high valent); hard metal ions (binds to hard ligands)
Late TM : low metal oxidation state, e.g. Pt(II), Au(I) (low valent); soft metal ions (binds to soft ligands)
Why?

11. Atomic radius Ti Cu
Atomic number

12. IE Ti Cu
Atomic number

14. Ligands (A) Charge (formal charge) Neutral (e.g. :CO, :PR3, :NH3)
Anionic (e.g. Cl-, O2-, CH3-)
Cationic (rare!) (e.g. NO+, C7H7+)
(B) Hard/Soft properties
Hard : period 1 donor (NH3, OH2)
Soft : carbon (CO, CH3-, CH2=CH2) & period 2 donors (PR3, SR2)

15. (C) No. of donor atom
Metal complexes with polydentate (chelating) ligands
are more stable than those with unidentate analogues.
Chelate effect

18. (ii) p acceptors (p acids)

19. Exercises
Classify the following ligands as p donor, p acceptor, or s ligands
NMe3 I-
NO+
CN-
OH- H-
CH3-

20. Nomenclature (1) Ligands in alphabetical order
(3) Indicate O.N. of metal (in Roman no.: I, II, 0)
(4) Indicate the no. of L and M (di, tri, tetra etc.).
Also bis, tris, tetrakis
(5) Anionic ligand  o;
e.g. Cl- (chloro), H- (hydrido), CN- (cyano)
(6) Anionic complexes => ate
e.g. Mn (manganate), Fe (ferrate), Cr (chromate) etc

21. (7) Add structural prefixes, e.g. cis/ trans, fac/ mer etc.
Examples:
K3[Mn(CN)6]
Tripotassium hexacyanomanganate(III)
Na2[Fe(CO)4]
Disodium tetracarbonylferrate(-II)

22. Exercises Name the following compounds (1) [Mn2(CO)10], [Co2(CO)8]
(2) [Ru(PPh3)4Cl2]
(3) K2[Pt(CN)4]
(4) [Cr(NH3)3(H2O)(OH)Cl][NO3]