chemistry and physics of low dimensional molecular conductors
|
|
- Phoebe Edwards
- 6 years ago
- Views:
Transcription
1 chemistry and physics of low dimensional molecular conductors Patrick Batail UMR CNR 6200 MOLTECH Angers Ecole du GDR MICO 5-11 juin 2010 AUOI d (EDT-TTF-CONMe 2 ) 2 AsF 6 cristaux et photo Cécile Mézière
2 TTF HO TMTTF TMTF
3 a typical molecular metal: (TMTF) 2 + PF 6
4 electrocrystallization an invaluable tool for the construction of electroactive molecular solids one single, day-to-weeks experiment achieves: carriers generation carriers stabilization by delocalization/localization within stacks / slabs (intermolecular conjugation) electrostatic self-assembly / auto-templating into bi-continuous O-I hybrid frameworks allows: halogen-bonded co-assembly into ternary systems upon engaging neutral functional p-conjugated spacers
5 I org I inorg halogen bonding interactions associate in CH 3 CN : EDT-TTF- I 2 with either : the corner-sharing, perovskite-layerlike 2D polymer (BuNH 3+ ) 2 (PbI 4 2 ) or the edge-sharing 2D polymer PbI 2 in the presence of NaI Best crystals typically under controlled rhythmic reversal of the current flow in the e-cell (0.7 s in oxidation coupled to 0.3 s in reduction), see Hünig et al. Eur. J. Inorg. Chem 1999, 899. Thomas Devic
6 e-crystallization upon controlled rythmic reversal of dc current flow poor crystal quality at constant current rythmic reversal 1 mm 1 mm T. DEVIC, M. ÉVAIN, Y. MOËLO, E. CANADELL, P. AUBAN-ENZIER, M. FOURMIGUÉ, P. BATAIL J. Am. Chem. oc. 125, 3295 (2003) early example, see Hünig et al., Eur. J. Inorg. Chem. 1999, 899
7 b-(i 2 -EDT-TTF) + 2[(Pb 5/6 1/6 I 2 ) 1/3 ] 3 ingle crystals!! a bi-continuous hybrid composite T. Devic pseudo-intercalation of b-slab into lacunar, edge-sharing (CdI 2 -type), [Pb (1-x) I 2 ] ( 2x) hexagonal single layers interfacial Halogen-bonding : C I I = 3.81 and 4.09 Å charge balance from lead site occupancy
8 electrocrystallization laboratory d-(edt-ttf-conme 2 ) 2 AsF 6 et d-(edt-ttf-conme 2 ) 2 Br b-(edt-ttf-i 2 ) 2 + [(Pb 5/6 1/6 I 2 ) 1/3 ] 3 b-(edt-ttf-i 2 ) 2 + [(Pb 2/3+x Ag 1/3 2xx I 2 ) 1/3 ] 3 x 0.05 b -(EDT-TTF-I 2 ) 2 PbI 3 H 2 O Kagome (EDT-TTF-CONH 2 ) 6 [Re 6 e 8 (CN) 6 ] single crystals by Cécile Mézière June 2006 b-(edt-ttf-i 2 ) 2 [HO 2 C CH=CH CO 2 ] 1-x [ O 2 C CH=CH CO 2 ] x [(rac), (R) et ()-(EDT-TTF-Me-Oxazoline)] 2 X (X = AsF 6, PF 6, Au(CN) 2 ) chemistry and physics of intermolecular interactions act in unisson
9 objectif cet après-midi : crystal engineering of p-conjugated systems: getting familiar with redox chemistry and intermolecular interactions how to reveal a hidden structural detail relevant to pertinent features of a complex electronic structure and lying behind a beautiful low dim physics
10 OUTLINE 1. electrocrystallization 2. redox chemistry 3. intermolecular interactions, and their redox activation, direct the structure 4. orbitals and bands (in one dimension) 5. decipher B of TTF-TCNQ, Bechgaard salts 6. modify / control electronic structure 6.1 tune stoichiometry 6.2 tune anion charge 6.3 ternary phases by halogen bonding 6.4 [H + ]/[hole] mixed valence 6.5 chemical pressure
11 November 2004 Volume 104 Number 11
12 OUTLINE 1. electrocrystallization 2. redox chemistry
13 iegfried Hünig s Reversible 2-teps Redox ystems of the Violene Type X X n -e +e X X n -e +e resonance / conjugation X X n Y Y n -e +e Y Y n -e +e Y Y n Hückel formalism: treat heteroatom/group as a perturbation Chem. Rev. 104, 5535 (2004)
14 X X n -e +e X X n -e +e X X n -e -e TTF TTF + TTF 2+ tetrathiafulvalene
15 iegfried Hünig s Reversible Two-teps Redox ystems of the Violene Type X X n -e +e X X n -e +e resonance / conjugation X X n Y Y n -e +e Y Y n -e +e Y Y n NC CN NC CN NC CN NC CN NC CN NC CN TCNQ 2 TCNQ TCNQ Chem. Rev. 104, 5535 (2004)
16 Hückel formalism: treat heteroatom/group as a perturbation propene k p k i p i j j j
17 propene
18 TTF HO TMTTF TMTF
19 characterization of redox properties: cyclic voltammetry experiments I V
20
21 Torrance Mol. Cryst. Liq. Cryst. 1985, 126, 5567 p-donor vs p-acceptors
22 OUTLINE 1. electrocrystallization 2. redox chemistry 3. intermolecular interactions, and their redox activation, direct the structure
23 intermolecular interactions p p -p p overlap, p-p, vdw, H- and Hal-bonding direct the structure weak Directing the tructures and Collective Electronic Properties of Organic Metals: the Interplay of Overlap Interactions and Hydrogen Bonds K. HEUZÉ, M. FOURMIGUÉ, P. BATAIL, E. CANADELL, P. AUBAN-ENZIER Chem. Eur. J. 5(9), (1999) Activation of Hydrogen and Halogen Bonding Interactions in Crystalline Molecular Conductors M. FOURMIGUE, P. BATAIL Chem. Rev. 104, (2004)
24 p-p interactions interactions between p-conjugated closed shell molecules quadrupoles quadrupoles interactions + + repulsion + + C. A. Hunter and J. K. M. anders, J. Am. Chem. oc. 1990, 112, 5525
25 C. A. Hunter and J. K. M. anders, J. Am. Chem. oc. 1990, 112, 5525
26 pentacene, a paradigm for p-p interactions / stacking herring-bone pattern of intermolecular interactions C. A. Hunter and J. K. M. anders, J. Am. Chem. oc. 1990, 112, 5525
27 hydrogen bonds 1) normal hydrogen bonds 2) weak hydrogen bonds: C sp3 H X and C sp2 H X D H d+ A d electrostatic, between an H-bond donor and an H-bond acceptor directional vanishes very slowly with distance Fourmigué, Batail Chem. Rev. 2004, 104, 5379
28 O H O et N H O: normal hydrogen bonds NH 4+ OH 2 19 kcal mole ev HO H Cl 13.5 kcal mole ev HO H OH 2 5 kcal mole ev CH X: weaker hydrogen bonds HC C H OH kcal mole ev H 2 C=C H OH 2 1 kcal mole ev 1 kcal mole 1 = ev Chem. Rev. 2004, 104, 5382
29 [C 6 H 5 NH 3+ ][Me 3 TTF PO 3 H ] e [Me 3 TTF + PO 3 H ] a neutral, zwitterionic radical A. Dolbecq et al. Chem. Eur. J., 2(10), (1996)
30 REDOX ACTIVATION TRONG H-bond acceptor character DENIED! O N Me H H izeable H-bond donor character Redox state (off/on) Intermolecular interactions Molecular recognition (binding strenght) - e + e Competition : charges and spins localization (magnetism) vs delocalization (transport). + Chem. Commun (2003) O H N H Me ENHANCED!
31 b -(EDT-TTF-CONHMe) 2 [Cl H 2 O] O N H d + Cl - d + H.+ not involved Chem. Mater. 2000, 12, b HOMO-HOMO interaction energies I ev II III IV V
32 b -(EDT-TTF-CONHMe) 2 [Cl H 2 O] Chem. Mater. 2000, 12,
33 OUTLINE 1. electrocrystallization 2. redox chemistry 3. intermolecular interactions, and their redox activation, direct the structure 4. orbitals and band (in one dimension)
34 low dimensional molecular solids intermolecular interactions (those which direct the structure: p p -p p overlap, vdw, H- and Hal-bonding) are weak understanding crystal and electronic structure correlation: easier (back of the envelop arguments) in materials with stronger, covalent and/or ionic interactions it is a much more delicate task to look for such correlations for systems with weak interactions because we lack the kind of feeling and control of the relative weight of the different interactions, all of which are weak
35 extended-hückel tight-binding band structure calculations Grant Whangbo Hoffmann Burdett Mori Canadell anisotropy of the system in the momentum space Purpose: how to reveal a hidden, apparently innocuous structural detail relevant to pertinent features of their electronic structures and lying behind a beautifull physics?
36 basic concepts: orbitals and bands in one-dimension working with small, simple things:
37
38
39 a n c 0 c 1 c 2 c 3 c 4 k = e ikna c n n Roald Hoffmann Angew. Chem. Int. Ed. 1987, 26,
40
41 Band Width that the bands extend unsymmetrically around their origin (energy of a free H atom at ev) is a consequence of the inclusion of overlap: for two levels, a dimer: E ± = H AA ± H AB 1 ± AB the bonding E + combination is les stabilized than the antibonding one E is destabilized
42 orbitals and bands in one dimension
43
44 see how they run: k = e ikna c n p x along x : x? the band of p orbitals runs down from zone center to zone edge
45 stack of square planar d 8 PtL 4 complexes try predict the approximate band structure of K 2 Pt(CN) 4 and K 2 Pt(CN) 4 Br 0.3 without calculation eclipsed staggered the Pt Pt distance has been shown to be inversely related to the degree of oxidation of the materials
46 topology of d block orbitals
47 types of overlap p d type : strong, axis of rotation type p: medium, lateral, co-planar type d: weak, face-to-face
48 inventory of all possible modes of overlap within pairs of orbitals s, p or d along z z overlap type only between orbitals s, p or d z 2 p p x, p y, d xz or d yz d d x 2 y 2 or d xy
49 try and see how they run (along z)? a p band out of N p orbitals: runs up, moderate yet sizeable dispersion a p band out of d xz s: runs down, moderate yet sizeable dispersion a band out of d z2 s: runs up, dispersion is large a d band out of d xy s: runs up, barely (not quite flat though)
50 Bloch functions at the zone center (k = 0) and the zone edge (k = p/a)
51 (2p z ) i orbitals of the 4 carbon atoms (i = 1, 2, 3, 4) of cyclobutadiene
52 z y x
53 d x 2 y 2 interacts strongly with 4 ( type) 4 y x d z d x 2 y 2 1
54 the d orbitals of square-planar ML 4 unit
55 d d p
56 predicted considerations of band width and orbital topology extended Huckel calculation at Pt Pt = 3.0 Å
57 Pt(II) d 8 where are the electrons? e F K 2 [Pt II (CN) 4 ] 3H 2 O K 2 [Pt II (CN) 4 ]Br 0.33 H 2 O
58
59 more than one unit per unit cell : chemists fold bands too!
60 More than one electronic unit in the unit cell. Folding bands.
61
62 butadiene A A
63 butadiene
64 butadiene A A
65 a
66
67 stays still there before going back down (equilibrium) V that goes in = V that goes out
68 goes through a mid-point in energy where the net number of bonding states equals that of antibonding states
69 folding bands
70 a = 3a a = 4a
71
72 band diagram of a dimerized system. Peierls. electron count. 2k F the chemist s intuitive feeling for what a model chain of hydrogen atoms would do:
73 H n, uniform chain H n, dimerized chain orbitals at the Fermi level for the chain (H 2 ) n
74 band diagram of the dimerized system (H2)n
75
76 electron count 2 molecules Pt(CN) 4 per unit cell a = 10 3 e F 2p a x = 2 x 5p 6a K 2 [Pt II (CN) 4 ]Br 0.33 H 2 O 3p/6a 4p/6a 5p/6a
77 K 2 [Pt II (CN) 4 ]Br 0.33 H 2 O electron # is: 2 x 5p 6a e F 3p/6a 4p/6a 2 k F = p 3a = a* 3 in the momentum space
78 2.4 polyacetylene
79 N
80 frontier p orbitals LUMO HOMO low lying states
81 N
82 N N
83 discrete, fully ionic dimers in [(TTF + ) 2 ][(I 3 ) 2 ] HO TTF + HO TTF + HO TTF + HO TTF + strong bonding: type p p p p overlap eclipsed and diamagnetic HO TTF + + HO TTF +
84 discrete, mixed valence dimer in (TTF) 2 + [Re 6 5 Cl 9 ] HO TTF + HO TTF + HO TTF HO TTF + HO TTF + + HO TTF + milder bonding: p type p p p p overlap slipped and paramagnetic
85 3.360 Å Å vdw p p recouvrements p p p p ( ) + p (TTF) 2 2+ (TTF) 2 +
86 OUTLINE 1. electrocrystallization 2. redox chemistry 3. intermolecular interactions, and their redox activation, direct the structure 4. orbitals and band (in one dimension) 5. decipher B of TTF-TCNQ, Bechgaard salts
87 TCNQ N N C C C C N N LUMO
88 TTF TCNQ
89 between C 2pz s
90 antibonding (k = 0)
91 bonding Y (k = p/b)
92 TTF TCNQ E(k) 0 k F p/b k
93 at = 0, the in-phase combination is bonding
94 TTF TCNQ = 0.59 E(k) 0 k F p/b k uncommensurate band filling
95 TTF TCNQ recent first principles B calculation by Pablo Ordejón and Enric Canadell Barcelona
96
97 TTF-TCNQ Jérome Chem. Rev. 2004, 104, 5565
98 TMTF-DMTCNQ = 0.5!! Peierls transition suppressed at 9 kbars!! Metallic down to liquid helium temperatures under 10 kbars instead of 0.59 in TTF-TCNQ Jérome Chem. Rev. 104, 5575 (2004)
99 Jérome Chem. Rev. 2004, 104 p. 5575
100 TMTF-DMTCNQ = 0.5!! Peierls transition suppressed at 9 kbars!! Metallic down to liquid helium temperatures under 10 kbars instead of 0.59 in TTF-TCNQ Jérome Chem. Rev. 104, 5575 (2004)
101 a typical molecular metal: (TMTF) 2 + PF 6
102 TTF HO TMTTF TMTF
103 the molecule is symmetric 3.66 Å 3.63 Å centers of symmetry allow for any amount of dimerization 2 to 1 e e e e 2 molecules per unit in chain along a Bechgaard and Fabre salts
104 a typical molecular metal: (TMTF) 2 PF = 3 e F 0 p/2a p/a 0 p/a a = 2a p/4a
105 dimerization slightly dispersed in transverse direction also E F (TMTF) 2 PF 6 2 bands 3 electrons half-filled band (a*/2, 0) (0,0) (0, b*/2) (a*/2, b*/2) ( a*/2, b*/2)
106 nesting vector
107 Jérome Chem. Rev. 2004, 104, p and p. 5577
108 Jérome Chem. Rev. 2004, 104 p. 5578
109
110 OUTLINE 1. electrocrystallization 2. redox chemistry 3. intermolecular interactions, and their redox activation, direct the structure 4. orbitals and band (in one dimension) 5. decipher B of TTF-TCNQ, Bechgaard salts 6. modify / control electronic structure
111 Roald Hoffmann How Chemistry and Physics Meet in the olid tate Angew. Chem. Int. Ed. Engl. 1987, 26, Jeremy K. Burdett Chemical Bonding in olids Oxford University Press, 1995 Christophe Iung, Enric Canadell Description orbitalaire de la structure électronique des solides 1. De la molécule aux composés 1D Ediscience international, Paris, 1997 Roger Rousseau, Marc Gener, Enric Canadell tep-by-step construction of the electronic structure of molecular conductors: Conceptuals aspects and applications Adv. Funct. Mater. 2004, 14, 201
112 Chem. Rev. 1991, 91,
113 1D / 2D Band tructures and Fermi urfaces
114 very pure samples the combination of very pure samples and admixtures of 1D/2D F makes for a rich low dimensional physics, especially under high B s see, Mark V. Kartsovnik Chem. Rev. 2004, 104, 5737
115 a series of 2D metals yet with two different types of charge carriers with different dimensionality a-(bedt-ttf) 2 [M + Hg 2+ (QCN ) 4 ] M = Tl, K, NH 4 ; Q =, e Mark V. Kartsovnik Chem. Rev. 2004, 104, 5737 all exhibit giant dh oscillations: 2D closed sections of F (16% of first Brillouin zone) rooom temperature crystal structures, B and F very similar some exhibit a density wave instability: nested 1D parts of F Rousseau, Figueras, Canadell J. Mol. truct. (Theochem) 1998, 424, 135 see also Organic uperconductors by Ishiguro, Yamaji, aito pringer-verlag 1998
116 modifying the electronic structure 0 p/a
117 OUTLINE 1. electrocrystallization 2. redox chemistry 3. intermolecular interactions, and their redox activation, direct the structure 4. orbitals and band (in one dimension) 5. decipher B of TTF-TCNQ, Bechgaard salts 6. modify / control electronic structure 6.1 tune anion charge
118 [Ti 2 F 8 (C 2 O 4 )] 2 [Ta 2 F 11 ] [(TMTF) ] 2( +) 3 [Ti 2 F 8 (C 2 O 4 )] [(TMTF)] + 3 [Ta 2 F 11 ] ynth. Met. 1988, 22, 201 ynth. Met. 1991, 41-43, 1939
119 predict band diagram and conductivity uniform chains metallic e F 6 2 i.e. 4 electrons in three bands: highest one is empty insulating 6 1 i.e. 5 electrons in three bands: highest one is half-filled 0 k p/b 0 k p/b b = 3b 3:1 2 p/6a 3:1
120 predict band diagram and conductivity trimerized chains metallic e F insulating 3:1 2 p/6a 3:1 b = 3b
121 [Ti 2 F 8 (C 2 O 4 )] 2 [Ta 2 F 11 ] Y [(TMTF) ] 2( +) 3 [Ti 2 F 8 (C 2 O 4 )] [(TMTF)] + 3 [Ta 2 F 11 ]
122
123 molecular engineering and band filling change the anion charge change electron count by tuning the stoichiometry Modulating the Framework Negative Charge Density in the ystem BDT-TTP + /[Re 6 5 Cl 9 1 ]/[Re 6 (/e) 6 Cl 8 2 ]/[Re 6 7 Cl 7 3 ]: Templating by Isosteric Cluster Anions of Identical ymmetry and hape, Variations of Incommensurate Band Filling, and Electronic tructure in 2D Metals. PERRUCHA, K. BOUBEKEUR, E. CANADELL, Y. MIAKI, P. AUBAN-ENZIER, C. PAQUIER, P. BATAIL J. Am. Chem. oc. 130(11), (2008)
124 OUTLINE 1. electrocrystallization 2. redox chemistry 3. intermolecular interactions, and their redox activation, direct the structure 4. orbitals and band (in one dimension) 5. decipher B of TTF-TCNQ, Bechgaard salts 6. modify / control electronic structure 6.1 tune anion charge 6.2 tune stoichiometry
125 Morita-Nakasuji s TTF-imidazole N N H N N H Angew. Chem. Int. Ed. 43, 6343 (2004)
126 Morita-Nakasuji s TTF-imidazole e Cl Cl O N N H N N H N N H O Cl Cl redox activated hydrogen bonding allows to control stoichiometry Angew. Chem. Int. Ed. 43, 6343 (2004)
127 e N N H N N H N N H O O O O redox activated hydrogen bonding allows control of stoichiometry
128 (TTF-Im) 2 (CHL) redox activated hydrogen bonding allows control of stoichiometry
129 (TTF-Im) 2 (CHL) P 1 uniform stacks
130 (TTF-Im) 2 (CHL) TTF Im + spin only Heisenberg chain of spins on uniform chloranil stacks
131 (TTF-Im) 2 (CHL)
132 OUTLINE 1. electrocrystallization 2. redox chemistry 3. intermolecular interactions, and their redox activation, direct the structure 4. orbitals and band (in one dimension) 5. decipher B of TTF-TCNQ, Bechgaard salts 6. modify / control electronic structure 6.1 tune anion charge 6.2 tune stoichiometry
133 EDT-TTF-CONH 2 vs Re 6 e 8 (CN) 6 ] 4 /3 Batail et al. Chem. Rev. 2001, 101, 2037 redox active, luminescent, hexanuclear, molecular chalcogenide cluster 0.3 V/CE asaki, Fedorov et al. Chem. Lett. 1999, 1121 how H-bonding express octahedral symmetry of inorganic cluster anion
134 6 EDT-TTF-CONH 2 + Re 6 e 8 (CN) 6 ] 4 /3 3
135 R3 a = (2) Å a = (2) V = Å 3 Kagome net = 1/2
136 (EDT-TTF-CONH 2 ) 6 (4- )+ [Re 6 e 8 (CN) 6 ] (4- ) b HOMO-HOMO intradimer ev interdimer ev Canadell
137 (EDT-TTF-CONH 2 ) 6 (4- )+ [Re 6 e 8 (CN) 6 ] (4- ) NO OVERLAP 2D Canadell
138 (EDT-TTF-CONH 2 ) 6 (4- )+ [Re 6 e 8 (CN) 6 ] (4- ) e F ( = 0) e F ( = 1) Canadell
139 single crystal esr H H Coulon, Clérac
140 ER conductivity d 0 / 2 1/ 2 = 8 cm -1
141 carriers at room temperature: (EDT-TTF-CONH 2 ) 6 (3.92)+ [Re 6 e 8 (CN) 6 (4) ] e cluster, diamagnetic [Re 6 e 8 CN) 6 3( ) ] e, Jahn-Teller active, paramagnetic = ½ cluster (EDT-TTF-CONH 2 ) 6 (4)+ [Re 6 e 8 (CN) 6 ] (4) (EDT-TTF-CONH 2 ) 2 (1)+ (EDT-TTF-CONH 2 ) 2 (1)+ (EDT-TTF-CONH 2 ) 2 (2)+ below transition charge disproportionation charge ordering
142 (TTF) 2 2+ (TTF) 2 +
143 triclinic 100 K charge localization coupled to molecular motion [EDT-TTF-CONH 2 + ] 2 téphane Baudron Lika Zorina [EDT-TTF-CONH 2 ] 2 +
144 Mott localization below 200 K T(K) mixed valence, slipped fully oxidized, more ecliped 2+ charges are ordered 2+ XRD vs P: andra Carlsson, Dave Allan, Paul Attfield - U of Edimburg
145 Conclusion: Mott localization M-I transition coupled to phase transition molecular motion (softness of interfacial H-bond interactions). A. BAUDRON, P. BATAIL, C. COULON, R. CLERAC, E. CANADELL, V. LAUKHIN, R. MELZI, P. WZIETEK, D. JEROME, P. AUBAN-ENZIER,. RAVY, J. Am. Chem. oc. 127(33), (2005)
146 try and control the property HOW? keeping with Kagome lattice change anion charge!
147 substitute one Re(III) for one Os(IV) [Re III 6e 8 (CN) 6 ] 4 [Re III 5Os IV e 8 (CN) 6 ] 3 Baudron, Batail + Tulski, Long France-Berkeley Program
148 (EDT-TTF-CONH 2 ) 4 (3)+ [Re 5 Ose 8 (CN) 6 ] (3) (EDT-TTF-CONH 2 ) 6 (4)+ [Re 6 e 8 (CN) 6 ] (4)
149 OUTLINE 1. electrocrystallization 2. redox chemistry 3. intermolecular interactions, and their redox activation, direct the structure 4. orbitals and band (in one dimension) 5. decipher B of TTF-TCNQ, Bechgaard salts 6. modify / control electronic structure 6.1 tune anion charge 6.2 tune stoichiometry 6.3 ternary phases by halogen bonding
150 O H O et N H O: normal hydrogen bonds NH 4+ OH 2 19 kcal mole ev HO H Cl 13.5 kcal mole ev HO H OH 2 5 kcal mole ev CH X: weaker hydrogen bonds HC C H OH kcal mole ev H 2 C=C H OH 2 1 kcal mole ev halogen bonds: comparable to normal hydrogen bonds C Cl N C 2.4 kcal mole ev CF 3 I NH 3 6 kcal mole ev 1 kcal mole 1 = ev Chem. Rev. 2004, 104, 5382
151 halogen bonding in the solid state: as strong and even more directional than hydrogen bonding d r max C X d +d r min direction of maximum attractive electrostatic interaction towards electron-rich (lone pairs) region of Lewis bases polar flattening O, C=O, C= sp 3 and sp 2 amines (pyridine) N C goups I>Br>Cl Fourmigué, Batail Chem. Rev., 104(11), (2004)
152 halogen bonding in the solid state: as strong and even more directional than hydrogen bonds C X 1 2 X C type I 1 = 2 X X C C type II 1 = 90, 2 = 180 Desiraju et al. JAC, 111, 8725 (1989) Fourmigué, Batail Chem. Rev. 104, (2004)
153 EDT TTF + [Re 6 e 8 (CN) 6 ] 4 also probing the extend of a covalent component to halogen bonding: * C I N C I I C I a current crystal engineering issue
154 (EDT-TTF) 8 (p-bib) [Re 6 e 8 (CN) 6 ] Anne-Lise Barrès 8:1:1 n:2:1 n:3:1
155 halogen-bonded co-polymer I I (EDT-TTF) 8 (p-bib) [Re 6 e 8 (CN) 6 ]
156 (EDT-TTF) 8 (p-bib) [Re 6 e 8 (CN) 6 ] A.-L. BARRÈ, A. EL-GHAYOURI, L. V. ZORINA, E. CANADELL, P. AUBAN-ENZIER, P. BATAIL Chem. Commun (2008)
157 OUTLINE 1. electrocrystallization 2. redox chemistry 3. intermolecular interactions, and their redox activation, direct the structure 4. orbitals and band (in one dimension) 5. decipher B of TTF-TCNQ, Bechgaard salts 6. modify / control electronic structure 6.1 tune stoichiometry 6.2 tune anion charge 6.3 ternary phases by halogen bonding 6.4 [H + ]/[hole] mixed valence 6.5 chemical pressure
158 d (EDT-TTF-CONMe 2 ) 2 X, X = AsF 6, Br genuine 3/4-filled band Mott insulators H H O NMe 2 H H C 1 symmetry H K. HEUZÉ, M. FOURMIGUÉ, P. BATAIL, C. COULON, R. CLÉRAC, E. CANADELL, P. AUBAN-ENZIER,. RAVY, D. JÉROME Adv. Mater. 15, (2003)
159 Me 2 N O H Me 2 N O H Me 2 N O H Me 2 N O H [±c/2] NMe 2 O H NMe 2 O H NMe 2 O H NMe 2 O H apply glide plane P2 1 /c
160 glide plane imposed by the C 1 Molecular ymmetry P K t t glide 1/4 and 3/4 along b glide plane imposes stack uniformity non dimerized, 2 molecules, 1 hole per unit along chain: band is ¼-filled with holes t = + 71 mev despite criss-cross overlap:
161 band structure and Fermi surface: a sizeable t Transfer integrals Br vs [AsF 6 ] Z along stack X total bandwidth is 0.31 ev for AsF 6 : very similar to (TMTTF) 2 Br which, however, has a small dimerization gap of ev Enric Canadell
162 Mott insulator!!: the underlying mechanism for fermions localization can only come from the quarter-filling umklapp AsF 6 - Mott gap mostly controlled by the on-site and nearest neighbor interactions Auban-enzier Jérome Adv. Mater. 15, (2003)
163 decrease Mott gap by applying chemical pressure: V (AsF 6 ) = V (Br ) + 76 Å 3 7 kbar
164 band structure and Fermi surface: a sizeable t Transfer integrals Br vs [AsF 6 ] Z along stack X total bandwidth is 0.31 ev for AsF 6 : very similar to (TMTTF) 2 Br which, however, has a small dimerization gap of ev Enric Canadell
165
166 (EDT-TTF-CONMe 2 ) 2 X Transport sous pression : c (P) à T ambiante X = AsF 6 (1bar) = 0.03 (.cm) -1 X = Br (1bar) = 1 (.cm) -1 Conductivité (.cm) X = Br (EDT-TTFCONMe 2 ) 2 X T = 295K X = AsF P. Auban-enzier C. Pasquier D. Jérome Pression (kbar) (TMTTF) 2 PF 6 ) (1bar) = 40 (.cm) -1 forte augmentation de (P) à basse pression (régime localisé) puis dépendance linéaire (idem (TM) 2 X) (régime métallique) à partir de X= AsF 6 : décalage de 7 kbar / X=Br et de 15 kbar / (TMTTF) 2 PF 6 Conductivité (.cm) AsF 6 X = Br X = AsF 6 (EDT-TTFCONMe 2 ) 2 X T = 295K Pression (kbar) Br = 7 kbar
167 Temperature (K) NON-DIMERIZED Q-1D ¼ filled systems (EDT-TTF-CONMe 2 ) 2 X, X=AsF 6, Br X = AsF 6 X = Br 1000 T CO ( P)) Conductor 1D T T* 100 Insulator CO P CO ( P)) T MI ( ) Conductor 2D T MI () 10 T AF ( 13 C T 1 ) Antiferromagnetic T AF ( 1 H T 1 ) T MI ( // ) Insulator CDW FL Pressure (kbar) D dim = 0 CO with AF ground state, no P, no DW, no C CO / AF CDW FL Phase diagram of quarter-filled band organic salts, [EDT-TTF-CONMe 2 ] 2 X, X =AsF 6 and Br P. AUBAN-ENZIER, C. R. PAQUIER, D. JEROME,. UH,. E. BROWN, C. MEZIERE, P. BATAIL Phys. Rev. Lett. 102, (2009)
168 INGLE CRYTAL 13 C NMR AsF 6 13 C NMR pectrum recorded at T = 200 K and applied field B = T. For arbitrary orientations, there are four non-equivalent sites (labelled A1, A2, B1, B2) teve uh, tuart E. Brown, UCLA
169 T 1-1 (s -1 ) AsF sites A1,A2 sites B1,B2 13 C T 1-1 (T) Charge rich site B 10 1 Charge depleted site A A B temperature(k) B / A = 9 / 1 T 1-1 (B) / T 1-1 (A) = ( B / A ) 2 large and T independent charge ratio r B / r A = 9 / 1 10 <T< 200K Charge ratio 3 / 1 in (DI-DCNQI) 2 Ag, K.Hiraki, K. Kanoda., PRL 80, 4737 (1998) (TMTTF) 2 AsF 6, F. Zamborszky et al., PRB 66, (R) (2002)
170 full refinement and analysis of symmetry of 3D CO structure based on single crystal synchrotron X-ray data identify an anti-phase, static modulation wave of Br - atoms, in synchronicity with on-site localization of holes Leokadiya Zorina, ergey imonov, Cécile Mézière, Enric Canadell, teve uh, tuart E. Brown, Pierre Fertey, Pascale Foury-Leylekian, Jean-Paul Pouget, Patrick Batail J. Mater. Chem. 19, (2009)
171 (DI-DCNQI) 2 Ag REFINED WIGNER TRUCTURE T. Kakiuchi, Y. Wakabayashi, H. awa, T. Itou, K. Kanoda, Phys. Rev. Lett., 2007, 98, a-(bedt-ttf) 2 I 3 T. Kakiuchi, Y. Wakabayashi, H. awa, T. Takahashi, T. Nakamura, J. Phys. oc. Jpn., 2007, 76, (EDO-TTF) 2 PF 6. Aoyagi, K. Kato, A. Ota, H. Yamochi, G. aito, H. uematsu, M. akata, M. Takata, Angew. Chem. Int. Ed., 2004, 43, (BEDT-TTF) 2 RbZn(CN) 4 M. Watanabe, Y. Noda, Y. Nogami, H. Mori, J. Phys. oc. Jpn., 2004, 73, 921.
172 PAUL ATTFIELD s WORK ON CO IN INORGANIC powder neutron diffraction studies on half-doped manganites (Pr 0.5 Ca 0.5 MnO 3, TbBaMn 2 O 6, YBaMn 2 O 6 ) and magnetite (Fe 3 O 4 ) J. P. Attfield, olid t. c., 2006, 8, R. J. Goff, J. P. Wright, J. P. Attfield, P. G. Radaelli, J. Phys. Cond. Mat., 2005, 17, R. J. Goff, J. P. Attfield, Phys. Rev. B, 2004, 70, J. P. Wright, J. P. Attfield, P. G. Radaelli, Phys. Rev. Lett., 2001, 87,
173 Br Pmna at 300 K for averaged structure one independent molecule in asymetric unit do NOT allow for charge ordering
174 twinned monoclinic structure below 190 K Pmna Lika Zorina P2 1 /a keeps with local two-fold axial symmetry about a
175 Br MONOCLINIC P2 1 /a ORTHORHOMBIC Pmna Change in the γ lattice angle across the structural phase transition. Blue rhombuses and red circles below the transition are data points for the two different twin domains in the monoclinic phase.
176 P2 1 /a 150 K
177 Bruker 4-circle CCD, Angers ynchrotron OLEIL Pmna, 2?, 4 collected independent R 1 [I>2 (I)] a large collection of systematic absences reflections to work with in orthorhombic symmetry
178 compatible with Pmnn, P2nn, P P2nn analysis of synchrotron data
179 two independent molecules in asymetric unit 2b in agreement with CO
180
181 activation of large collections of CH O hydrogen bonds in synchronicity with CO: activated charge disproportionation carriers crystallize mixed valence metallic de-activated concerted mechanism long range electrostatic modulation Wigner structure Mott insulator
182 synchrotron data collected at Br absorption hedge modulation of Br displacements
183 P2nn anti-phase modulation
184 3D charge ordered structure P2nn compatible with ferroelectricty
185 Br static modulation wave
186 Pmna P2nn despites the occurrence of CO, stacks appear to remain essentially uniform
187 Résumé chimie et physique des interactions intermoléculaires faibles à l unisson dans les conducteurs moléculaires en basse dimension
A Variety of Ground States in Salts of Unsymmetrical TTFs. Marc Fourmigué
A Variety of Ground States in Salts of Unsymmetrical TTFs Marc Fourmigué Sciences Chimiques de Rennes, UMR 6226 CNRS-UR1 Equipe Matière Condensée et Systèmes Electroactifs Campus de Beaulieu, 35042 RENNES,
More informationLes instabilités d ordre de charge dans les conducteurs organiques quasi-unidimensionnels
Les instabilités d ordre de charge dans les conducteurs organiques quasi-unidimensionnels J.P. POUGET Laboratoire de Physique des Solides CNRS- Université Paris Sud F-91405 Orsay outline Focus on organic
More informationExcitations and Interactions
Excitations and Interactions Magnon gases A7 A8 Spin physics A3 A5 A9 A10 A12 Quantum magnets A3 A8 B1 B2 B3 B4 B5 Synthesis B4 B6 B10 E Spectroscopy B11 Excitations and Interactions Charge-transfer induced
More informationELEMENTARY BAND THEORY
ELEMENTARY BAND THEORY PHYSICIST Solid state band Valence band, VB Conduction band, CB Fermi energy, E F Bloch orbital, delocalized n-doping p-doping Band gap, E g Direct band gap Indirect band gap Phonon
More informationOrganic Conductors and Superconductors: signatures of electronic correlations Martin Dressel 1. Physikalisches Institut der Universität Stuttgart
Organic Conductors and Superconductors: signatures of electronic correlations Martin Dressel 1. Physikalisches Institut der Universität Stuttgart Outline 1. Organic Conductors basics and development 2.
More informationElectronic structure Crystal-field theory Ligand-field theory. Electronic-spectra electronic spectra of atoms
Chapter 19 d-metal complexes: electronic structure and spectra Electronic structure 19.1 Crystal-field theory 19.2 Ligand-field theory Electronic-spectra 19.3 electronic spectra of atoms 19.4 electronic
More informationElectronic states of a strongly correlated two-dimensional system, Pd(dmit) 2 salts, controlled by uni-axial strain and counter cations
J. Phys. IV France 114 (2004) 411-417 EDP Sciences, Les Ulis DOI: 10.1051/jp4:2004114099 411 Electronic states of a strongly correlated two-dimensional system, Pd(dmit) 2 salts, controlled by uni-axial
More informationTransport and ordering of strongly correlated electrons in kagome system at partial filling
Transport and ordering of strongly correlated electrons in kagome system at partial filling Eduard TUTIŠ Institute of Physics, Zagreb, Croatia ECRYS 2017, Cargèse in collaboration with & inspired by EXPERIMENTAL
More informationRDCH 702 Lecture 4: Orbitals and energetics
RDCH 702 Lecture 4: Orbitals and energetics Molecular symmetry Bonding and structure Molecular orbital theory Crystal field theory Ligand field theory Provide fundamental understanding of chemistry dictating
More informationChemistry 3211 Coordination Chemistry Part 3 Ligand Field and Molecular Orbital Theory
Chemistry 3211 Coordination Chemistry Part 3 Ligand Field and Molecular Orbital Theory Electronic Structure of Six and Four-Coordinate Complexes Using Crystal Field Theory, we can generate energy level
More informationIf you put an electron into the t 2g, like that for Ti 3+, then you stabilize the barycenter of the d orbitals by 0.4 D o.
Crystal Field Stabilization Energy Week 2-1 Octahedral Symmetry (O h ) If you put an electron into the t 2g, like that for Ti 3+, then you stabilize the barycenter of the d orbitals by 0.4 D o. Each additional
More informationOrbitals and energetics
Orbitals and energetics Bonding and structure Molecular orbital theory Crystal field theory Ligand field theory Provide fundamental understanding of chemistry dictating radionuclide complexes Structure
More informationLINZ LECTURES. Lecture 1. The Development of Organic Conductors: Metals, Superconductors and Semiconductors
LINZ LECTURE Lecture 1. The Development of Organic Conductors: Metals, uperconductors and emiconductors Lecture 2A. Introduction and ynthesis of Important Conjugated Polymers Lecture 2B. olid tate Polymerization
More informationMolecular structure and bonding
Chemistry 481(01) Spring 2017 Instructor: Dr. Upali Siriwardane e-mail: upali@latech.edu Office: CTH 311 Phone 257-4941 Office Hours: M,W 8:00-9:00 & 11:00-12:00 am; Tu,Th, F 9:30-11:30 a.m. April 4, 2017:
More informationCoordination Chemistry: Bonding Theories. Crystal Field Theory. Chapter 20
Coordination Chemistry: Bonding Theories Crystal Field Theory Chapter 0 Review of the Previous Lecture 1. We discussed different types of isomerism in coordination chemistry Structural or constitutional
More informationName CHM 4610/5620 Fall 2017 December 14 FINAL EXAMINATION SOLUTIONS Part I, from the Literature Reports
Name CHM 4610/5620 Fall 2017 December 14 FINAL EXAMINATION SOLUTIONS Part I, from the Literature Reports I II III IV V VI VII VIII IX X Total This exam consists of several problems. Rough point values
More informationBEGIN: High symmetry LINEAR chain, sheet or a cubic close packed 3D lattice. vibrational deformation modes, asymmetric can couple and reduce symmetry
Bonds bands Molecules olids Jahn Teller Peierls BEGN: High symmetry LNEAR chain, sheet or a cubic close packed 3D lattice rbitals : highly symmetrical but ordered structure often does not correspond to
More informationOne Dimensional Metals
One Dimensional Metals Sascha Ehrhardt Introduction One dimensional metals are characterized by a high anisotropy concerning some of their physical properties. The most obvious physical property is the
More informationSolids. properties & structure
Solids properties & structure Determining Crystal Structure crystalline solids have a very regular geometric arrangement of their particles the arrangement of the particles and distances between them is
More informationOutline. Introduction: graphene. Adsorption on graphene: - Chemisorption - Physisorption. Summary
Outline Introduction: graphene Adsorption on graphene: - Chemisorption - Physisorption Summary 1 Electronic band structure: Electronic properties K Γ M v F = 10 6 ms -1 = c/300 massless Dirac particles!
More informationFor more info visit Chemical bond is the attractive force which holds various constituents together in a molecule.
Chemical bond:- Chemical bond is the attractive force which holds various constituents together in a molecule. There are three types of chemical bonds: Ionic Bond, Covalent Bond, Coordinate Bond. Octet
More informationChapter 10. Structure Determines Properties! Molecular Geometry. Chemical Bonding II
Chapter 10 Chemical Bonding II Structure Determines Properties! Properties of molecular substances depend on the structure of the molecule The structure includes many factors, including: the skeletal arrangement
More informationMolecular Geometry and Bonding Theories. Chapter 9
Molecular Geometry and Bonding Theories Chapter 9 Molecular Shapes CCl 4 Lewis structures give atomic connectivity; The shape of a molecule is determined by its bond angles VSEPR Model Valence Shell Electron
More informationCondensed Molecular Materials Laboratory, RIKEN, 2-1, Hirosawa, Wako-shi, Saitama, , Japan; (C.H.)
Crystals 2012, 2, 861-874; doi:10.3390/cryst2030861 Article OPEN ACCESS crystals ISSN 2073-4352 www.mdpi.com/journal/crystals Cation Dependence of Crystal Structure and Band Parameters in a Series of Molecular
More informationThe symmetry properties & relative energies of atomic orbitals determine how they react to form molecular orbitals. These molecular orbitals are then
1 The symmetry properties & relative energies of atomic orbitals determine how they react to form molecular orbitals. These molecular orbitals are then filled with the available electrons according to
More informationElectronic structure / bonding in d-block complexes
LN05-1 Electronic structure / bonding in d-block complexes Many, many properties of transition metal complexes (coordination number, structure, colour, magnetism, reactivity) are very sensitive to the
More informationNano-Science of Organic (Super)conductors
Nano-cience of rganic (uper)conductors Gunzi aito Grad. chool of cience, Kyoto Univ.Yamochi, A.tsuka, M.Maesato, Y.Yoshida, K.Nishimura,.Drozdova, D.V.Konarev, K.Balodis β'-(et) 2 ICl 2 T c (on set)=14.2k
More informationChapter 10 Chemical Bonding II
Chapter 10 Chemical Bonding II Valence Bond Theory Valence Bond Theory: A quantum mechanical model which shows how electron pairs are shared in a covalent bond. Bond forms between two atoms when the following
More informationCH1010 Exam #2 Study Guide For reference see Chemistry: An Atoms-focused Approach by Gilbert, Kirss, and Foster
CH1010 Exam #2 Study Guide For reference see Chemistry: An Atoms-focused Approach by Gilbert, Kirss, and Foster Chapter 3: Atomic Structure, Explaining the Properties of Elements Trends to know (and be
More informationReview Outline Chemistry 1B, Fall 2012
Review Outline Chemistry 1B, Fall 2012 -------------------------------------- Chapter 12 -------------------------------------- I. Experiments and findings related to origin of quantum mechanics A. Planck:
More informationSpin correlations in conducting and superconducting materials Collin Broholm Johns Hopkins University
Spin correlations in conducting and superconducting materials Collin Broholm Johns Hopkins University Supported by U.S. DoE Basic Energy Sciences, Materials Sciences & Engineering DE-FG02-08ER46544 Overview
More informationCh. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.
Ch. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. I. Review: Comparison of ionic and molecular compounds Molecular compounds Ionic
More informationCartoon courtesy of NearingZero.net. Chemical Bonding and Molecular Structure
Cartoon courtesy of NearingZero.net Chemical Bonding and Molecular Structure Chemical Bonds Forces that hold groups of atoms together and make them function as a unit. 3 Major Types: Ionic bonds transfer
More informationChapter 5. Molecular Orbitals
Chapter 5. Molecular Orbitals MO from s, p, d, orbitals: - Fig.5.1, 5.2, 5.3 Homonuclear diatomic molecules: - Fig. 5.7 - Para- vs. Diamagnetic Heteronuclear diatomic molecules: - Fig. 5.14 - ex. CO Hybrid
More informationLecture 2: Bonding in solids
Lecture 2: Bonding in solids Electronegativity Van Arkel-Ketalaar Triangles Atomic and ionic radii Band theory of solids Molecules vs. solids Band structures Analysis of chemical bonds in Reciprocal space
More informationMOLECULAR ORBITAL DIAGRAM KEY
365 MOLECULAR ORBITAL DIAGRAM KEY Draw molecular orbital diagrams for each of the following molecules or ions. Determine the bond order of each and use this to predict the stability of the bond. Determine
More informationNAME: SECOND EXAMINATION
1 Chemistry 64 Winter 1994 NAME: SECOND EXAMINATION THIS EXAMINATION IS WORTH 100 POINTS AND CONTAINS 4 (FOUR) QUESTIONS THEY ARE NOT EQUALLY WEIGHTED! YOU SHOULD ATTEMPT ALL QUESTIONS AND ALLOCATE YOUR
More informationPaper No. 1: ORGANIC CHEMISTRY- I (Nature of Bonding and Stereochemistry)
Subject Chemistry Paper No and Title Paper 1: ORGANIC - I (Nature of Bonding Module No and Title Module Tag CHE_P1_M10 TABLE OF CONTENTS 1. Learning Outcomes 2. Introduction 3. Non-Covalent Interactions
More information1. Which response contains all the molecules below that violate the octet rule, and no others? SF 4, SiCl 4, H 2Te, AsF 5, BeI 2
Chem 1100 Pre-Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which response contains all the molecules below that violate the octet rule, and no
More informationUltrashort Lifetime Expansion for Resonant Inelastic X-ray Scattering. Luuk Ament
Ultrashort Lifetime Expansion for Resonant Inelastic X-ray Scattering Luuk Ament In collaboration with Jeroen van den Brink and Fiona Forte What is RIXS? Resonant Inelastic X-ray Scattering Synchrotron
More informationQuiz 5 R = lit-atm/mol-k 1 (25) R = J/mol-K 2 (25) 3 (25) c = X 10 8 m/s 4 (25)
ADVANCED INORGANIC CHEMISTRY QUIZ 5 and FINAL December 18, 2012 INSTRUCTIONS: PRINT YOUR NAME > NAME. QUIZ 5 : Work 4 of 1-5 (The lowest problem will be dropped) FINAL: #6 (10 points ) Work 6 of 7 to 14
More informationChapter 7. Chemical Bonding I: Basic Concepts
Chapter 7. Chemical Bonding I: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely
More informationBonding/Lewis Dots Lecture Page 1 of 12 Date. Bonding. What is Coulomb's Law? Energy Profile: Covalent Bonds. Electronegativity and Linus Pauling
Bonding/Lewis Dots Lecture Page 1 of 12 Date Bonding What is Coulomb's Law? Energy Profile: Covalent Bonds Electronegativity and Linus Pauling 2.1 H 1.0 Li 0.9 Na 0.8 K 0.8 Rb 0.7 Cs 0.7 Fr 1.5 Be 1.2
More informationPAPER No. 7: Inorganic chemistry II MODULE No. 5: Molecular Orbital Theory
Subject Chemistry Paper No and Title Module No and Title Module Tag 7, Inorganic chemistry II 5, Molecular Orbital Theory CHE_P7_M5 TABLE OF CONTENTS 1. Learning Outcomes 2. Introduction to Ligand Field
More informationBonding. Honors Chemistry 412 Chapter 6
Bonding Honors Chemistry 412 Chapter 6 Chemical Bond Mutual attraction between the nuclei and valence electrons of different atoms that binds them together. Types of Bonds Ionic Bonds Force of attraction
More informationChapter 6 Chemistry Review
Chapter 6 Chemistry Review Multiple Choice Identify the choice that best completes the statement or answers the question. Put the LETTER of the correct answer in the blank. 1. The electrons involved in
More informationMolecular Orbital Theory (MOT)
Molecular Orbital Theory (MOT) In this section, There are another approach to the bonding in metal complexes: the use of molecular orbital theory (MOT). In contrast to crystal field theory, the molecular
More informationAnomalous quantum cri/cality linking an/ferromagne/sm and superconduc/vity in organic metals
Anomalous quantum cri/cality linking an/ferromagne/sm and superconduc/vity in organic metals C. Bourbonnais NQS2011, Kyoto, November 2011 Coll. A. Sedeki N. Doiron- Leyraud S. René De Cotret L. Taillefer
More informationHomework 08 - Bonding Theories & IMF
HW08 - Bonding Theories & IMF This is a preview of the published version of the quiz Started: Jun 4 at 11:4am Quiz Instructions Homework 08 - Bonding Theories & IMF Question 1 A sigma bond... stems from
More informationChapter 7. Ionic & Covalent Bonds
Chapter 7 Ionic & Covalent Bonds Ionic Compounds Covalent Compounds 7.1 EN difference and bond character >1.7 = ionic 0.4 1.7 = polar covalent 1.7 Electrons not shared at
More informationCarbon and Its Compounds
Chapter 1 Carbon and Its Compounds Copyright 2018 by Nelson Education Limited 1 1.2 Organic Molecules from the Inside Out I: The Modelling of Atoms Copyright 2018 by Nelson Education Limited 2 s orbitals:
More informationElectronic structure of correlated electron systems. G.A.Sawatzky UBC Lecture
Electronic structure of correlated electron systems G.A.Sawatzky UBC Lecture 6 011 Influence of polarizability on the crystal structure Ionic compounds are often cubic to maximize the Madelung energy i.e.
More informationDFT EXERCISES. FELIPE CERVANTES SODI January 2006
DFT EXERCISES FELIPE CERVANTES SODI January 2006 http://www.csanyi.net/wiki/space/dftexercises Dr. Gábor Csányi 1 Hydrogen atom Place a single H atom in the middle of a largish unit cell (start with a
More informationCHAPTER 3. Crystallography
CHAPTER 3 Crystallography Atomic Structure Atoms are made of Protons: mass 1.00728 amu, +1 positive charge Neutrons: mass of 1.00867 amu, neutral Electrons: mass of 0.00055 amu, -1 negative charge (1 amu
More informationMore Chemical Bonding
More Chemical Bonding Reading: Ch 10: section 1-8 Ch 9: section 4, 6, 10 Homework: Chapter 10:.31, 33, 35*, 39*, 43, 47, 49* Chapter 9: 43, 45, 55*, 57, 75*, 77, 79 * = important homework question Molecular
More informationCoordination Chemistry II: Bonding
d x2-y2 b 1g e g d x2-y2 b 1g D 1 t 2 d xy, d yz, d zx D t d d z2, d x2-y2 D o d z2 a 1g d xy D 2 d z2 b 2g a 1g e d z2, d x2-y2 d xy, d yz, d zx d xy b 2g D 3 t 2g e g d yz, d zx e g d yz, d zx 10 Coordination
More information5.04 Principles of Inorganic Chemistry II
MIT OpenCourseWare http://ocw.mit.edu 5.04 Principles of Inorganic Chemistry II Fall 008 For information about citing these materials or our Terms of Use, visit: http://ocw.mit.edu/terms. 5.04, Principles
More informationThree Most Important Topics (MIT) Today
Three Most Important Topics (MIT) Today Electrons in periodic potential Energy gap nearly free electron Bloch Theorem Energy gap tight binding Chapter 1 1 Electrons in Periodic Potential We now know the
More informationin Halogen-Bonded Complexes
9 Resonance Assistance and Cooperativity in Halogen-Bonded Complexes Previously appeared as Covalency in Resonance-Assisted Halogen Bonds Demonstrated with Cooperativity in N-Halo-Guanine Quartets L. P.
More informationPEIERLS INSTABILITY AND CHARGE-DENSITY-WAVE TRANSPORT IN FLUORANTHENE AND PERYLENE RADICAL CATION SALTS
Vol. 87 (1995) ACTA PHYSICA POLONICA A No. 4-5 Proceedings of the IV International Seminar on Organic Materials for Molecular Electronics, Zajączkowo 1994 PEIERLS INSTABILITY AND CHARGE-DENSITY-WAVE TRANSPORT
More informationCh 6 Chemical Bonding
Ch 6 Chemical Bonding What you should learn in this section (objectives): Define chemical bond Explain why most atoms form chemical bonds Describe ionic and covalent bonding Explain why most chemical bonding
More informationMolecular Geometry and intermolecular forces. Unit 4 Chapter 9 and 11.2
1 Molecular Geometry and intermolecular forces Unit 4 Chapter 9 and 11.2 2 Unit 4.1 Chapter 9.1-9.3 3 Review of bonding Ionic compound (metal/nonmetal) creates a lattice Formula doesn t tell the exact
More informationWhat Do Molecules Look Like?
What Do Molecules Look Like? The Lewis Dot Structure approach provides some insight into molecular structure in terms of bonding, but what about 3D geometry? Recall that we have two types of electron pairs:
More informationCrystal Properties. MS415 Lec. 2. High performance, high current. ZnO. GaN
Crystal Properties Crystal Lattices: Periodic arrangement of atoms Repeated unit cells (solid-state) Stuffing atoms into unit cells Determine mechanical & electrical properties High performance, high current
More informationQuantum chemical studies of the physics around the metal-insulator transition in (EDO- TTF)2PF6 Linker, Gerrit
University of Groningen Quantum chemical studies of the physics around the metal-insulator transition in (EDO- TTF)2PF6 Linker, Gerrit IMPORTANT NOTE: You are advised to consult the publisher's version
More informationCHEMISTRY XL-14A CHEMICAL BONDS
CHEMISTRY XL-14A CHEMICAL BONDS July 16, 2011 Robert Iafe Office Hours 2 July 18-July 22 Monday: 2:00pm in Room MS-B 3114 Tuesday-Thursday: 3:00pm in Room MS-B 3114 Chapter 2 Overview 3 Ionic Bonds Covalent
More informationChapter 11 Answers. Practice Examples
hapter Answers Practice Examples a. There are three half-filled p orbitals on, and one half-filled 5p orbital on I. Each halffilled p orbital from will overlap with one half-filled 5p orbital of an I.
More informationCHAPTER TEN MOLECULAR GEOMETRY MOLECULAR GEOMETRY V S E P R CHEMICAL BONDING II: MOLECULAR GEOMETRY AND HYBRIDIZATION OF ATOMIC ORBITALS
CHAPTER TEN CHEMICAL BONDING II: AND HYBRIDIZATION O ATOMIC ORBITALS V S E P R VSEPR Theory In VSEPR theory, multiple bonds behave like a single electron pair Valence shell electron pair repulsion (VSEPR)
More informationSUPPLEMENTARY INFORMATION
DOI: 1.138/NMAT3449 Topological crystalline insulator states in Pb 1 x Sn x Se Content S1 Crystal growth, structural and chemical characterization. S2 Angle-resolved photoemission measurements at various
More informationAtomic Structure and Bonding. Chapter 1 Organic Chemistry, 8 th Edition John McMurry
Atomic Structure and Bonding Chapter 1 Organic Chemistry, 8 th Edition John McMurry 1 Common Elements Groups First row Second row In most organic molecules carbon is combined with relatively few elements
More informationStudying Metal to Insulator Transitions in Solids using Synchrotron Radiation-based Spectroscopies.
PY482 Lecture. February 28 th, 2013 Studying Metal to Insulator Transitions in Solids using Synchrotron Radiation-based Spectroscopies. Kevin E. Smith Department of Physics Department of Chemistry Division
More informationOrganic Chemistry I Dr Alex Roche Organic chemistry is the chemistry of Carbon and its compounds. Organic molecules constitute the essence of life (fats, sugars, proteins, DNA), and also permeate our everyday
More information1051-3rd Chem Exam_ (A)
1051-3rd Chem Exam_1060111(A) MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The molecular-orbital model for Ge shows it to be A) a conductor,
More information1051-3rd Chem Exam_ (B)
1051-3rd Chem Exam_1060111(B) MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) In liquids, the attractive intermolecular forces are. A) strong enough
More information1051-3rd Chem Exam_ (C)
1051-3rd Chem Exam_1060111(C) MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The hybridizations of iodine in IF3 and IF5 are and, respectively.
More informationMarks for each question are as indicated in [] brackets.
Name Student Number CHEMISTRY 140 FINAL EXAM December 10, 2002 Numerical answers must be given with appropriate units and significant figures. Please place all answers in the space provided for the question.
More informationLuigi Paolasini
Luigi Paolasini paolasini@esrf.fr LECTURE 4: MAGNETIC INTERACTIONS - Dipole vs exchange magnetic interactions. - Direct and indirect exchange interactions. - Anisotropic exchange interactions. - Interplay
More informationMolecular Orbitals of Ethene
Molecular Orbitals of Ethene 1 Molecular Orbital Analysis of Ethene Dimerisation the reaction is said to be a "symmetry forbidden" interestingly, this reaction is rare and very slow! Molecular Orbitals
More informationCHAPTER 6 CHEMICAL BONDING SHORT QUESTION WITH ANSWERS Q.1 Dipole moments of chlorobenzene is 1.70 D and of chlorobenzene is 2.5 D while that of paradichlorbenzene is zero; why? Benzene has zero dipole
More informationLecture 1. OUTLINE Basic Semiconductor Physics. Reading: Chapter 2.1. Semiconductors Intrinsic (undoped) silicon Doping Carrier concentrations
Lecture 1 OUTLINE Basic Semiconductor Physics Semiconductors Intrinsic (undoped) silicon Doping Carrier concentrations Reading: Chapter 2.1 EE105 Fall 2007 Lecture 1, Slide 1 What is a Semiconductor? Low
More informationCHEMISTRY 362 Descriptive Inorganic Chemistry. M. Y. Darensbourg. Examination II March 29, Name:
CHEMISTRY 362 Descriptive Inorganic Chemistry M. Y. Darensbourg Examination II March 29, 2017 Name: An Aggie does not lie, cheat or steal or tolerate those who do. Signed: Point Group Assignment S = Σm
More information4. Interpenetrating simple cubic
2 1. The correct structure t of CsClCl crystal is 1. Simple cubic 2. Body centered cubic 3. Face centered cubic 4. Interpenetrating simple cubic If corner as well as the particle at the center are same
More informationSupplementary Figures
Supplementary Figures Supplementary Figure 1 Measured versus calculated optical transitions in the CPX. The UV/Vis/NIR spectrum obtained experimentally for the 1:1 blend of 4T and F4TCNQ (red curve) is
More informationCrystal Field Theory
Crystal Field Theory It is not a bonding theory Method of explaining some physical properties that occur in transition metal complexes. Involves a simple electrostatic argument which can yield reasonable
More informationCovalent Bonding. In nature, only the noble gas elements exist as uncombined atoms. All other elements need to lose or gain electrons
In nature, only the noble gas elements exist as uncombined atoms. They are monatomic - consist of single atoms. All other elements need to lose or gain electrons To form ionic compounds Some elements share
More informationChiral Electroactive Precursors and Materials
Chiral Electroactive Precursors and Materials arcis Avarvari MLTECH-Anjou, Université d Angers, C, FACE Conferinta Diaspora tiintifica, Bucuresti, 21-24 eptembrie 2010 Current research topics in the group
More informationChapter 20 d-metal complexes: electronic structures and properties
CHEM 511 Chapter 20 page 1 of 21 Chapter 20 d-metal complexes: electronic structures and properties Recall the shape of the d-orbitals... Electronic structure Crystal Field Theory: an electrostatic approach
More informationCHEM1901/ J-5 June 2013
CHEM1901/3 2013-J-5 June 2013 Oxygen exists in the troposphere as a diatomic molecule. 4 (a) Using arrows to indicate relative electron spin, fill the left-most valence orbital energy diagram for O 2,
More informationOrigin of the Metal-to-Insulator Transition in H 0.33 MoO 3
Inorg. Chem. 1997, 36, 4627-4632 4627 Origin of the Metal-to-Insulator Transition in H 0.33 MoO 3 Roger Rousseau, Enric Canadell,*, Pere Alemany,*, Donald H. Galván, and Roald Hoffmann*, Institut de Ciència
More informationTopics in the November 2009 Exam Paper for CHEM1101
November 2009 Topics in the November 2009 Exam Paper for CHEM1101 Click on the links for resources on each topic. 2009-N-2: 2009-N-3: 2009-N-4: 2009-N-5: 2009-N-6: 2009-N-7: 2009-N-8: 2009-N-9: 2009-N-10:
More informationValence bond theory accounts, at least qualitatively, for the stability of the covalent bond in terms of overlapping atomic orbitals.
Molecular Orbital Theory Valence bond theory accounts, at least qualitatively, for the stability of the covalent bond in terms of overlapping atomic orbitals. Using the concept of hybridization, valence
More informationThe wavefunction that describes a bonding pair of electrons:
4.2. Molecular Properties from VB Theory a) Bonding and Bond distances The wavefunction that describes a bonding pair of electrons: Ψ b = a(h 1 ) + b(h 2 ) where h 1 and h 2 are HAOs on adjacent atoms
More informationAP Chemistry Chapter 7: Bonding
AP Chemistry Chapter 7: Bonding Types of Bonding I. holds everything together! I All bonding occurs because of! Electronegativity difference and bond character A. A difference in electronegativity between
More informationCrystal Field Theory History
Crystal Field Theory History 1929 Hans Bethe - Crystal Field Theory (CFT) Developed to interpret color, spectra, magnetism in crystals 1932 J. H. Van Vleck - CFT of Transition Metal Complexes Champions
More informationBonding and Elastic Properties in Ti 2 AC (A = Ga or Tl)
Printed in the Republic of Korea http://dx.doi.org/10.5012/jkcs.2013.57.1.35 Bonding and Elastic Properties in Ti 2 AC (A = Ga or Tl) Dae-Bok Kang* Department of Chemistry, Kyungsung University, Busan
More informationCH676 Physical Chemistry: Principles and Applications. CH676 Physical Chemistry: Principles and Applications
CH676 Physical Chemistry: Principles and Applications Crystal Structure: XRD XRD: Diffraction Peak Positions Centering Allowed Peaks I-centered h+k+l is an even number F-centered hkl either all even or
More informationPAPER No.11: Inorganic Chemistry-III MODULE No.29: Metal- metal bonds and their evidences
1 Subject Chemistry Paper No and Title Module No and Title Module Tag 11: Inorganic Chemistry-III (Metal π-complexes and Metal Clusters) 29: Metal-metal bonds and their evidences CHE_P11_M29 2 TABLE OF
More informationBonding - Ch Types of Bonding
Types of Bonding I. holds everything together! II. All bonding occurs because of III. Electronegativity difference and bond character A. A between two atoms results in a when those two atoms form a bond.
More informationUnit Six --- Ionic and Covalent Bonds
Unit Six --- Ionic and Covalent Bonds Electron Configuration in Ionic Bonding Ionic Bonds Bonding in Metals Valence Electrons Electrons in the highest occupied energy level of an element s atoms Examples
More informationCoordination Chemistry: Bonding Theories. Molecular Orbital Theory. Chapter 20
Coordination Chemistry: Bonding Theories Molecular Orbital Theory Chapter 20 Review of the Previous Lecture 1. Discussed magnetism in coordination chemistry and the different classification of compounds
More information