Self-assembled Transition Metal Coordination Frameworks of ...

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J K” ‘ | | | | | | | 263 2&3 3]] Q0 34) 36] $3 Bo [mu C0pper(II) complexes Fig. 4.33. Experimental (black) and simulated best fit (blue) of the EPR spectrum of complex 18 in DMF at 77 K m.__...,_.._=.//l T” | | | | | | | 263 23] 330 Q0 340 36] 333 B. [mu Fig. 4.34. Experimental (black) and simulated best fit (blue) of the EPR spectrum of complex 19 in DMF at 77 K. l65
Chapter 4 The shifting of g values from 2.0023 in transition metal complexes are due to the mixing, via spin-orbit coupling of the metal orbitals involved in molecular orbitals containing the unpaired electrons, with the empty or filled ligand orbitals. Since the g values here suffer a positive shift, it indicates mixing with the filled ligand orbitals. The magnitude of shift is a measure of the degree of covalency of the complex. The g“ values of some of the species in these compounds are too high than expected, may be attributed to weak coordination to metal centers [35]. The electron donating capacity of a ligand to Cu(H) will determine the magnitude of g". The presence of electron poor water ligation can also be behind the high g" values, for example. The very low A" values also support this. These high g" values expect a positive net charge for the complex part. So the possibility of ionic copper at NNN centers and its weakening may be behind this and is in accordance with thiolato/enolato coordination assigned to second Cu(H) for ll, 12, 18 and 19. For complexes having the same atoms of ligation, a decrease in charge of the metal-ligand complex decreases g" and increases A" [35]. Conversely, the smaller g values for some other species indicate increased delocalization of the unpaired spin density away from the copper nucleus, and has been often interpreted in terms of increased covalency in the metal-ligand bond [43,44]. In all the complexes having different Cu(H) species g"> g i> 2.0023 and G values within the range 1.68-5.14 are consistent with a d_‘_2_ _, ground state in a square planar or square pyramidal geometry, as would be expected, and rules out the possibility of a trigonal bipyramidal structure which would be expected to have g i > g". Octahedral geometry is rarely sustained in Cu(H) complexes as they are most prone to Jalm Teller distortion giving 166
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7,2/H5 Self-assembled Transition Me
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, Phone orr. 0484-2575804 ; Phone R
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‘ilC7(,'NO’WLQ'I(D QEMEWT In tl
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PREFACE In its method, chemistry is
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CONTENTS CHAPTER 1 Introduction to
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4.3.5. Magnetochemistry 4.3.6. Char
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Chapter I__ _ _ irreducible, is a n
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Chapter I W 7 _ W _ 7 pg _ jg to pr
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Chapter I H_ g g 7 g 7 7 __ harvest
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Chapter I _ _ ______g__H _ g involv
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Chapter I _ g plays a pivotal role
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Chapter I g g _ exhibit considerabl
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Chapter I _, assemblies to generate
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Chapter I _ ,_ of mono or dinuclear
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Chapter I M W 7 7 _ __ 1.3.1.1. Ant
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Chapter I _ _ _ _ \_ 4- Jm _. _.
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Chapter In g_ g _ E __ _ E __( > es
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Chapter I W__‘ _ 1.6.6. MALDI MS
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Chapter I ,,_ g electron spin (the
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Chapter I W _ _ Traditional magnets
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Chapter I L.K. Thompson, O. Waldman
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Chapter I i __ _ Org. Chem. 31 (200
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Chapter In _g , g H g 85. S. Padhye
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Chapter 2 1 g anticipation of Cu(H)
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Chapter 2 _. M_ _ up 1. Quinoline-2
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Chapter 2 chloroform solution and d
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Chapter2 V _ _ _ _, 7 _ with aceton
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Chapter 2 _ 7 f __ i 2.3. Results a
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100s0- I > J 20
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— — 1 Ligands 1
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Ligands The ‘H and "C NMR spectra
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Ligands The ‘H NMR spectrum of HZ
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M1 1‘ 11 IL; Fig. 2.11. 'H NMR sp
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' | Ligands uo no 1&0 150 no no no
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Ligands Table 2. 3. Crystal data an
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Ligands The C-S bond distances of 1
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ligands between the planes of Cg(2)
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" F Ligands A indicates a typical d
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' ' Q 0' ¢ ¢" .~ 0~ I Q Q Q \ ' Q
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2.4.2. M TT Cell Proliferation Assa
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Table 2.9. Cell proliferation effec
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7 y _ i _ W Ligands B. Moubaraki, K
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CHAPTER Ni(II) complexes of carbohy
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_ _ __ g_ g W g H__ Ni(ll) complexe
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_ g A __ Ni(lI) complexes The reddi
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3.3. Results and discussion g_g _ N
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3.3.1. MALDI MS spectral studies of
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Ni(Il) complexes In the case of com
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100 U-
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3.3.2. IR and electronic spectral s
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Chapter 3 The electronic spectra of
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t§hqphw*3 v(Ni—S), further suppo
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Chapter 3 charge transfer bands. Fo
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Chapter 3 were refined anisotropica
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Chapter 3 3.3.3.1. Crystal structur
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Chapter 3 Table 3.7. Selected bond
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Chapter 3 N(l3)—C(35), N(2l)-C(58
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3.3.3.2. Crystal structures 0f[Ni(H
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Table 3.10. Selected bond lengths (
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Ni(lI) complexes significant 1t---1
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3.3.4. Magnetochemistry of the mole
Page 126 and 127: Ni(Il) complexes The allowed values
Page 128 and 129: in xn In
Page 130 and 131: g 7 Ni(Il) complexes 3.4. Concludin
Page 132 and 133: 11 12 13 14 15 16 17 18 19 20 21 22
Page 134 and 135: 41 42 43 44 45 46 47 48 49 50 51 52
Page 136 and 137: _ g “FOUR CHAPTER Cu(II) complexe
Page 138 and 139: _g C0pper(II) complexes complex of
Page 140 and 141: _ _ , p f 7, Copper-(II) complexes
Page 142 and 143: pp g _g _4_,_ C0pper(II) complexes
Page 144 and 145: g _,_,_ g g Copperfll) complexes in
Page 146 and 147: i ____ 3+ i --—- C 0pper(H) 2+ co
Page 148 and 149: C0pper(Il) complexes 499 100i ~04 7
Page 150 and 151: .04Copper(II) complexes 385 50.1I 1
Page 152 and 153: 100-I 4 -1 U ” Q 7°-J 59-: "1
Page 154: C0pper(lI) complexes confirm the po
Page 158 and 159: C0pper(ll) complexes 100 80" I
Page 160 and 161: C0pper(1l) complexes state, similar
Page 162 and 163: 2 5 2.5MW 20 Q 1.51 2oo'aoo'45o's
Page 164: Copper(lI) complexes F1 = g",3B:S:
Page 167 and 168: Chapter 4 for both species consider
Page 169 and 170: Chapter 4 The spectrum of compound
Page 171 and 172: Chapter 4 stability alone could not
Page 173 and 174: Chapter 4 zénzénzénzénénaloeé
Page 175: Chapter 4 164 | | | 252 272 2Q 31 B
Page 179 and 180: Chapter 4 _|“. / "| 1' '| |' | 1'
Page 181 and 182: Chapter 4 The solid state and some
Page 183 and 184: Chapter 4 U 1 .I - O i I . I II I
Page 185 and 186: _ I Chapter 4 — I I I — I '
Page 187 and 188: . , Chapter 4 2.5 I I ' I ' I ' I '
Page 189 and 190: Chapter 4 The field dependence of m
Page 191 and 192: Chapter 4 Where ,1’ M is the magn
Page 193 and 194: Chapter 4 g e The powder and frozen
Page 195: Chapter 4 various aspects like bond
Page 198 and 199: C0pper(ll) complexes Table 4.6. Sel
Page 200 and 201: ,____ p _p C0pper(H) complexes from
Page 202 and 203: Ed. Engl. 31 (1992) 733. 7___7 7 7
Page 204 and 205: __ ,_ f W C 0pper(l1) complexes Che
Page 206 and 207: -_ FIVE CHAPTER Spectral and magnet
Page 208 and 209: __ g_ _g g H g __ Manganese(II) com
Page 210 and 211: q H _ Manganesefll) complexes [Mn2(
Page 212 and 213: Manganese(Il) complexes lcmzmoll in
Page 214 and 215: 1W3 "l U 70 60 40 30 10 490 740 979
Page 216 and 217: Manganese(II) complexes MALDI MS sp
Page 218 and 219: 5.3.2. EPR spectral studies Mangane
Page 220 and 221: Manganese(II) complexes D and E , e
Page 222 and 223: the pattern is uncertain and it is
Page 224 and 225: __ I . l r Manganese(II) complexes
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" |\ Man ganese(II) complexes 80" 6
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Chapter 5 thiocarbohydrazone comple
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Chapter 5 To fit and interpret the
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Chapter 5 #1 IT 0.00 1 — ‘ I '
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Chapter 5 The temperature dependenc
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Chapter 5 ___ M _ 357 (2004) 2694.
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Chapter5 p _ _ S. Sivakumar, Struct
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Chapter 6 _ _ __ 7 the latter have
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Chapter6A, 0 0 _, 0 0 _* 4, W 0 0 0
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Chapter 6 g _ _ [Cd(HL2) ].,(1v0_.)
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Chapter 6 / ‘~ ' if‘ . l \ N N/
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1 | Chapter 6 100m__ ‘ 76$ mi, 16
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3 - i El Q I Chapter 6 - '3“ 1999
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Chapter 6 The compound 27 exhibits
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(T71aq7tew'¢5 centered at 1711.9 c
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1 . 1 Chapter 6 1244 100--1-; 1245
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Chapter 6 6.3.2. Electronic and IR
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Chapter 6 band at 19160 and 23920 c
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Zinc(II) & Cadmium(II) complexes Th
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.- 60- I ‘J TZinc(Il) & Cadmium(l
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Zinc(Il) & Cadmium(Il) complexes re
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Zinc(II) & C admium(ll) complexes T
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Fig. 6.25. The molecular structure
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Zinc(lI) & Cadmium(ll) complexes Al
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Zi!lC(II) & Cadmlum(II) C0mlexes Ta
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V _ i Zinc(1I) & Cadmium(lI) comple
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_ g _ g g V Zinc(lI) & Cadmiumfll)
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_, _ g pg L Summary and conclusion
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W g _ g mm Summary and conclusion a
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__ ,_ _ W A _ _ Summary and conclus
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Curriculum Vitae PERSONAL PROFILE N
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2-Hydroxyacetophenone 4-phenylthios
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