1. LECTURE 5. СOMPLEX COMPOUNDS.REACTIONS OF COMPLEX FORMING. BIOLOGIC ACTIVE СOMPLEX COMPOUNDS. LECTURER: Professor A.D.DZHURAEV Department of Bioorganic and Biological Chemistry. Bioinorganic chemistry. I COURSE

2. THE LECTURE PURPOSE: Complex compounds are extremely common in organic and inorganic nature, important compounds like chlorophyll, hemoglobin, many enzymes, vitamins and drugs are complex compounds. Provide insight into the complex compounds, their structure, properties, proper construction of the name, consider the reaction complex- tion, to classify complexes in charge and the nature of the ligands, to consider the range of complex compounds constant instability and stability, introduce metallo- enzymes and chelation.

3. THE LECTURE PURPOSE: Give the notion about complex compounds, as they exceedingly broadly wide-spread in alive and not alive nature. Such are an important compounds as chlorophyll, hemoglobin, many ferments, vitamins and medicinal matters are a complex compounds. Solely great role of the complex compounds in process of the breathing, photosynthesis, biological oxidation, in ferment catalysis. Therefore future physician must have a belief about complex compounds, their structure, properties, correct building of the name of complex compounds, and etc. Of no small importance role play complex compounds when making medicinal preparation. For instance, anticancer preparations are created on base of complexes of platinum; the complexes of gold render the action against tuberculosis and leprosy.

4. D EALT of questions 1. Components of the complex compounds 2. The spatial structure of complex compounds 3. Classification of compounds, exogenous and endogenous complexes 4. Constant stability and instability of complex compounds 5. The value of the complex compounds in medicine 7. The nature of the chemical bonds in complexes

5. Complex copmounds The main points of the coordination theory: 1. Many elements of a valence of 2 of the main (main) (--------) and side (-------) 2. Each element in the compound seek satisfy their main and secondary valence 3. Auxiliary valence elements in space has a specific and purposeful nature. Hg II I I K+K+ K+K+

6. The structure of the complex compound: 1.Complexing - positive ion metal. 2.Ligands - ions of opposite sign or neutral molecules 3. Chelating ligands and form inner sphere or complex ion complex compound. integrated charge ion is equal to the algebraic sum of the charge chelating ligands and charge 4. Outer sphere - ions, which were not included in inner sphere К+К+ К+К+ К+К+ CN - Fe +3

7. Coordination numbers of some of complexing agents: 1. Cu +, Ag +, Au + = 2 2. Cu 2+, Hg 2+, Au 3+, Cd 2+, Pb 2+, Pt 2+, Pd 2+ = 4 3. Fe 2+, Fe 3+, Cr 3+, Cо 3+, Ni 2+, Al 3+, Pt 4+ = 6 4. Ca 2+, Sr 2+, Bа 2+ = 8

8. Classification of compounds cationic complexes  Pt (NH 3 ) 4 ]Cl 2 - aminokomplexes  Cu (NH 3 ) 4  SO 4 - aminokomplexes  Al (H 2 O) 6  Cl 3 - aquacomplexes neutral complexes  Pt(NH 3 ) 4 Cl 2  - aminokomplexes  Pt(NH 3 ) 4 Br 2  - aminokomplexes anionic complexes Na 3  Al(OH) 6  - hydroxo complexes K 3 [Fe(CN) 6 ] - acido complexes Na 3  Co(NO 2 ) 6  - acido complexes

9. Name of complex compounds K [PtCl 3 (C 2 O 4 )] – Seitz salt [Pt(NH 3 ) 5 Cl] Cl 3 – Chugaevs salt K 3 [Fe(CN) 6 ] – red blood salt K 4 [Fe(CN) 6 ] – yellow blood salt [Pt(NH 3 ) 2 NO 2 Cl] SO 4 – mononitromono- hlorodiaminplatina (IV) sulfate

10. Chelates NH 2 -CH 2 -COOH + Cu Cl 2 O = C - O NH 2 - C H 2 Сu + 2HCl CH 2 - NH 2 O - C = 0 CH 2 COOH N CH 2 COOH – complexon -I CH 2 COOH

11. Chelates CH 2 COOH O O Me N N C O H 2 C C O CH 2 H 2 C - CH 2 HOOCH 2 C CH 2 COOH CH 2 COOH(Na) (Na)HOOCH 2 C HOOCH 2 C N-CH 2 -CH 2 -N complexon III (Trilon B)

12. Stability of complex compounds  Ag(NH 3 ) 2  Cl   Ag(NH 3 ) 2  + + Cl -  Ag(NH 3 ) 2  +   AgNH 3  + + NH 3  AgNH 3  +  Ag + + NH 3 or  Ag(NH 3 ) 2  +  Ag + +2NH 3  Ag  +  NH 3  2  Ag(NH 3 ) 2  +  K B = ------------------ K Q = ------------------  Ag(NH 3 ) 2  +   Ag  +  NH 3  2

13. ISOMERISM COMPLEX CONNECTIONS geometric hydrated ionization optical

14. Geometric (cis - trans) isomers tetrahloroplatiny diamine- [Pt(NH 3 ) 2 Cl 4 ] Cis isomers Trans isomers

15. Hydrate isomerism [ Gr(H 2 O) 6 ]Cl 3 hexa aqua chrome chloride (III) purple [Gr Cl 2 (H 2 O) 4 ]Cl *2H 2 O tetra aqua chrome chloride (III) dark green

16. Ionization isomerism [CoBr(NH 3 ) 5 ]SO 4 [Co SO 4 (NH 3 ) 5 ] Br Sulphate penta ammin - bromo - cobalt (III) red- purple bromide penta amine - cobalt sulfate (III) red

17. Diamidehlorplatina [Pt(NH 3 )Cl 2 ] is in the form? 2 isomers: Cis isomer is anti-cancer activity, and trans isomer - inactive. Feramid [Fe(АНК) 2 ]SO 4 used in gynecology