metal oxide nanoparticles: synthesis and reactivity
TRANSCRIPT
Corinne Chanéac
UMR - CNRS 7574
Laboratoire Chimie de la Matière Condensée de Paris,
Site Collège de France
Groupe Nanomatériaux Inorganiques
Metal oxide nanoparticles:
Synthesis and Reactivity
Environmental Nanotechnologies, 7-8 July 2011, Aix en Provence, France
Stage 1: List of Endpoints
• Nanomaterial Information/Identification
• Physical-Chemical Properties and Material
Characterization
• Environmental Fate
• Environmental Toxicology
• Mammalian Toxicology
• Material Safety
About the Research into Safety of Manufactured Nanomaterials
List of Manufactured Nanomaterials (14)
• Fullerenes (C60)
• Single-walled carbon
nanotubes (SWCNTs)
• Multi-walled carbon nanotubes
(MWCNTs)
• Silver nanoparticles
• Iron nanoparticles
• Carbon black
• Titanium dioxide
• Aluminium oxide
• Cerium oxide
• Zinc oxide
• Silicon dioxide
• Polystyrene
• Dendrimers
• Nanoclays
Soft
Chemistry
About the Research into Safety of Manufactured Nanomaterials
Morphology and Nanoparticles
Gœthite Anatase
Rutile
Formation of natural crystals in geological conditions
Bottom-up Approach
M OH M OH2 H2O
Strong acidity :Catalysis of oxolation
Condensation : olation
[Ti(OH)4(OH2)2]0
hydrolysis
[Ti(OH2)6]3+
Anatase
Rutile
Weak acidity:
olation then oxolation
Aqeous Sol-Gel Process for nanoparticle synthesis
M O M OH HO
Gœthite Anatase
Rutile
20 nm
50 nm
800 nm
w 56 nm
Durupthy, O.; Bill, J.; Aldinger, F. Cryst. Growth Des. 2007, 7, 2696
JACS, 2007,129 (18),5904 Chem. Comm., 5, 2004, pp. 481-487
Morphology and Nanoparticles
Morphologie et Nanoparticules
Gœthite Anatase
Rutile
20 nm
50 nm
800 nm
w 56 nm
Durupthy, O.; Bill, J.; Aldinger, F. Cryst. Growth Des. 2007, 7, 2696
JACS, 2007,129 (18),5904 Chem. Comm., 5, 2004, pp. 481-487
How control the nanocrystal
growth?
OSurf/OT
2 10 20 40 nm D 5
0,6
0,4
0,2
Change in chemical and physical properties
Solid formation DGformation° = nDG°Bulk + DG°surface
Variation of surface energy with the particle size (Sodium Chloride):
Side Total Surface aera Surface Energy
(cm) (cm2) (J/g)
0,1 28 5,6. 10-4
0,01 280 5,6. 10-3
10-4 (1mm) 2,8. 104 0,56
10-7 (1nm) 2,8. 107 560
Huge surface energy for nano-solids - Thermodynamically unstable system
Calculation
for a cube of
Sodium Chloride
Surface Sci. 60, 445, 1976
Surface energy : origin
>0
How determine the surface energy?
Unstability of nanometric colloidal dispersion:
Surface : motive power of growth
E surface : stability DG° = nDG°Bulk + DG°surface
Surface energy : origin
Spontaneous evolution of nanoparticles to minimise the surface contribution
Sintering, Oswald ripening
Surface energy : origin
DG° = nDG°Bulk + DG°surface g = (dG/ dA)ni, T, P
g : surface energy
energy requiered to create an unit of aera
g = ½ Nb e ra
Number of broken bonds per atom
Bond strength
Surface atomic density
Rough estimation of surface energy:
- surface relaxation
- surface restructuring with formation of new chemical bond
- same value of e for all the atoms
- no entropic consideration/ pressure or volume Surface Sci. 60, 445, 1976
g = ½ Nb e ra
g{100} = ½ 2/a2.4.e
= 4 e/a2
g{110} = 5e/√2 a2
= 3,52 e/a2
g{111} = 2√3e/a2
= 3,46 e/a2
FCC Structure
Coordination number of 12
Lattice parameter a
Nb = 4 Nb = 5 Nb = 3
Surface energy depends of the index of facets :
low index facets = low surface energy
Origine de l’énergie de surface
Relation between surface energy and crystal shape
Shape of nanoparticle : total surface energy reaches minimum
Wulff construction
Morphologies for a 2D crystal for 10 and 11 faces
Bi doped with Cu
Equilibrium crystal
5 nm
Surface energy at the atomic scale
T. Hiemstra et al., J. Colloid Interface Sci. 184, 680 (1996)
Brønsted basic site
M M
Od-1
H
Od Od-1
H+ H
M M M M M
M
H+
M M
Od-2
H H
Site m3
Site m2
Kprotonation= f (structure, hydratation)
MnO (nv-2) + H+solv MnOH (nv-1) Kn,1
MnOH (nv-1) + H+solv MnOH2
nv Kn,2
Model of multisite complexation , MUSIC2
-Ln Kn,x = - A(SSj -2+m)
A = 19,8
SH = 0,8
OH m1 p+m = 2
OH m2 p+m = 1 ou 2
OH m3 p+m = 1
S Sj = Si SMe + p SH + m(1- SH)
Example : face 111Oh of magnetite, 2 sites m2 and m3
10,86 3,3
Fe2-OH2 +0,8 Fe2-OH -0,4
Fe3-OH +0,6 Fe3-O -1,8
pH
-1.5
-1
-0.5
0
0.5
1
1.5
2
2 4 6 8 10 12
111 Oh100Somme pondérée
pH
Ch
arg
e d
e s
urf
ace
(C
.m2)
PZC
Good valuation of surface charge and of point of zero charge
Surface energy at the atomic scale
Model of multisite complexation , MUSIC2
5 nm
Surface energy at the atomic scale
T. Hiemstra et al., J. Colloid Interface Sci. 184, 680 (1996)
Brønsted basic site
M M
Od-1
H
Od Od-1
H+ H
M M M M M
M
H+
M M
Od-2
H H
Site m3
Site m2
D g = g - g 0 = RT
F 0 . 22 I - 2 0 . 0136 I + s 2
- s max ) ln( 1 - s
s max )
Surface charge density
J.P. Jolivet et al., J. Mater. Chem., 2004, 14, 3281
DG°surface >0 gA
Gibbs’s Law : Dg = -Sk idmi
Surface Energy Effect
Two ways
Decrease of A : Oswald ripening
D g = g - g 0 = RT
F 0 . 22 I - 2 0 . 0136 I + s 2
- s max ) ln( 1 - s
s max )
Density of
Surface charge
Previously described
g decreases when the charge density, s, increases
For H>PCN
J.P. Jolivet et al., J. Mater. Chem., 2004, 14, 3281
> 0
Metastable Object
DG° = nDG°Bulk + DG°surface
Decrease of g
gA
Gibbs Law : Dg = -Sk idmi
(g ,surface energy)
(A, surface area)
0
-2
-4
-6
-8
-10
-12 0 2 4 6 8 10 12 14 pH
1,0
1,1
1,2
1,3
1,4
2,2 3,4
Log [Fex(OH)y]
solubility
PZC
Size, Shape =
f(Surface energy)
The surface energy is lesser
far from the PZC
Surface Energy Effect
As s = f(pH)
4 5 6 7 8 9 10 pH
s 2 +
pK1
s 1 +
s 1 -
s 2 -
Su
rfa
ce c
ha
rge
den
sity
s
s PZC (point of zero charge)
pK2
Site 1
Site 2
Isotropic Nanoparticles
Precipitation of FeCl2 / FeCl3 : Fe3O4 magnetite
IRM, Hyperthermia
Precipitation of TiCl4 : TiO2 anatase
Photocatalysis, Photovoltaic
2 3 4
J. of Colloid Interface Sci., 1998, 205, 205 & J. Mater. Chem., 2003, 13, 877
pH 10 11 12
2
4
6
8
10
12
14
8 9 10 11 12 13
D (nm)
pH
1week
Size = f(Surface Energy)
4
5
6
7
8
9
10
11
1 2 3 4 5 6 7 8
-0.2
-0.1
-0.3
0.1
0.2 D (nm)
pH
1 week
Pottier A. (1999), Thèse UPMC, Paris 6
Charged surface = stopped growth
Su
rface
ch
arg
e (C
/m2)c
S
urfa
ce
ch
arg
e (C
/m2)
Isotropic Nanoparticles
Precipitation of FeCl2 / FeCl3 : Fe3O4 magnetite
IRM, Hyperthermia
pH
Size = f(Surface Energy)
Stability of nanoparticle = f(solution acidity), reversible phenomena
50 nm
pH 10
9 nm
After 3 weeks aging at pH 13.5 at 25°C
Anisotropic Nanoparticles
Precipitation of Al(NO3)3 : g-AlO(OH) boehmite
Morphology
= f(Surface Energy of each face)
Handbook of Porous Materials, Ed. F. Schüth, Wiley-VCH, 2002, p. 1591 & J. Mater. Chem., 2004, 14, 1-9
(010)
(001) (101) (100)
Wulff construction :
Equilibrium crystal = faces of lesser energy
0,4
0,5
0,6
0,7
0,8
0,9
4 5 6 7 8 9 10 11 12
hkl g (J/m2)
pH
(010)
(001)
(100)
(101)
0,4
0,5
0,6
0,7
0,8
0,9
4 5 6 7 8 9 10 11 12
hkl g (J/m2)
pH
(010)
(001)
(100)
(101)
pH = 6.5
L= 8 ± 1 nm
e = 3.7 nm
50 nm
(101)
(010)
(001)
(100)
pseudo-hexagonal platelets
Precipitation of Al(NO3)3 : g-AlO(OH) boehmite
pH = 11.5
(101)
(010)
50 nm
104°
réf
L= 13 ± 4 nm
e = 4.9 nm
diamond shape platelets
pH = 4.5
(101)
(001)
(010)
5 nm 100 nm
L= 4,5 nm
e = 3.7 nm
small aggregated pseudo-isotropic particle
Handbook of Porous Materials, Ed. F. Schüth, Wiley-VCH, 2002, p. 1591 & J. Mater. Chem., 2004, 14, 1-9
Anisotropic Nanoparticles
(101)
(101)
(001)
(100)
(101) (001)
(100)
A
B
C
(010)
(010)
(010)
8,9
10,2
9,5
Precipitation of Al(NO3)3 : g-AlO(OH) boehmite
50 nm 50 nm 50 nm
A B C
Electric Properties = f(Morphology)
(001)
7,5
8
8,5
9
9,5
10
10,5
IEP
-20
-10
0
10
20
30
40
50
4 5 6 7 8 9 10 11 12
A B C
Zeta
po
ten
tial (m
V)
pH
Anisotropic Nanoparticles
23
Morphology is kept after the heat treatment
Euzen, P., et al., Handbook of Porous Solids, Wiley-VCH Verlag GmbH, 2002, Vol. 3, 1591-1676
Boehmite Gama Alumina : topotactic transformation
(110)al
(111)al (100)al
(110)al
(010)b
(101)b (100)b
(001)b calcination
450°C
Boehmite Alumine g
20 nm
104° 50 nm
104° 450°C
Anisotropic Nanoparticles
Surface complexation
Precipitation of Al(NO3)3 with polyols: g-AlO(OH) boehmite
[polyol]=0.007M
C2
C4
C3
HO
OH
HO OH
OH
HO
OH
OH
OH
OH
OH
OH
OH
HO
HO
OH
OH
OH
OH
OH
C5
C6
Polyols
Hydroxycarboxylates
O
O-O
-O
O
O-
O
-O
O
O-
O
-O
OHO
-O
O
O-
OH
OHO
-O
O
O-
C2
C4
C3
Dicarboxylates
Complexing molecules and growth of cristallites
pH = 11.5 50 nm
104°
réf
[Al]=0.07M
(101)
(010)
12.6 nm
6.0 nm
éthylène glycol
50 nm
C2
glycérol 50 nm C3
erythritol
50 nm C4
6.6 nm
4.2 nm
arabinitol 50 nm
C5
dulcitol
50 nm C6
6.0 nm
(101)
(010)
3.6 nm
HO
OH
HO OH
OH
HO
OH
OH
OH
HO
OH
OH
OH
OH
OH
(101)
(010) (101)
(010)
10.6 nm
5.2 nm
(101)
(010)
12.0 nm
6.5 nm
OH
OH
OH
OH
HO
The size of nanoparticles decreases with the length of polyols
Precipitation of Al(NO3)3 with polyols: g-AlO(OH) boehmite
[polyol]=0.007M
Surface complexation by polyols
[polyol] 10 % mol
Chiche D. (2007), Thesis UPMC- IFP, Paris 6
Heterogenous Catalysts, Elsevier, 2006, 393
Ribitol : 180 m2/g
Xylitol : 290 m2/g
150
200
250
300
350
400
0 1 2 3 4 5 6 7
threo
erythro
xylitol
ribitol
dulcitol
average
standard synthesis
Su
rface s
pécif
iqu
e (
m²/
g)
erythro
Nombre de fonction OH
threo
Stereochemistry
effect
Precipitation of Al(NO3)3 with polyols: g-AlO(OH) boehmite
Surface complexation by polyols
50 nm
C3
50 nm
C2
50 nm
C4
50 nm
C5
(101)
(010)
12.6 nm 6.0 nm
R = L/e
2.2
glycerol
(101)
(010)
12.0 nm
6.5 nm
1.8
ethylene glycol
(101)
(010)
10.6 nm
5.2 nm
erythritol
2
6.6 nm
4.2 nm
arabinitol
(101)
(010) 1.4
Specific adsorption of Polyols
on (101) face:
Selectivity of adsorbed species
Phys. Chem. Chem. Phys., 2009, 11, 11310 - 11323
Precipitation of Al(NO3)3 with polyols: g-AlO(OH) boehmite
Aspect ratio evolution :
Preferential adsorption upon
lateral surfaces
Surface complexation by polyols
46
48
50
52
54
56
58
60
0 1 2 3 4 5 6
threo
erythro
moyenne
synthèse standard
S 1
01 (
%)
Nombre de fonction OH
(101)
(010)
(101)
(010)
(101)
(010)
Stabilisation énergétique des faces (101)
DFT calculations
(010)
(101)
« Nest » effect
Eads(0K) = -118 kJ.mol-1
Eads(0K) = -87 kJ.mol-1
Phys. Chem. Chem. Phys., 2009, 11, 11310 - 11323
Preferential adsorption upon
lateral surfaces : concavitie and stabilisation
Surface complexation by polyols
50 nm
O
O-
O
-O
OHO
-O
O
O-
OH
OHO
-O
O
O-
50 nm
50 nm
poly(hydroxy)carboxylates 0.007M
malate
succinate
tartrate
R = l/e
1,6
1,1
(101)
(010)
(101)
(010)
(101)
(010)
Size variation is not homothetic :
Strong decrease of anisotropy
2,2
45
50
55
60
65
standardsuccinate malate tartrate
S1
01 (
%)
Carboxylate
Selective adsorption
on (101) face
Surface complexation by hydroxy carboxylate
Acidity of OH groups is strengthened by the
complexation
Al
O OO
Al
O OO
OO
O
O-O
X
Al
O OO
OO
O
O-O
X
Al
O OO
OO
O
-O O
-O
Hydroxy carboxylate chemisorption
Geffroy 1999, Haines 1974, Martell 1984
Lower reactivity of (010) face due to m2-OH sites.
Increase of (101) face stabilization with the distance between –COOH groups: more
available adsorption sites.
(010)
(101)
O
O--O
O
O- O-
OO
~ 2,7 Å ~ 2,9 Å
O
O-
O-
O
~ 2,8 à 5,3 Å
D(O-O) (Å)
μ1-OH / μ2-OH
μ1-OH / μ1-OH
μ2-OH / μ2-OH
2,7 - 4,0 - 4,7 - 6,3
2,5 - 4,7 - 5,5 - 6,3
2,5 - 2,8 - 3,8 - 4,9 - 5,3 - 5,7
(101)
Surface complexation by hydroxy carboxylate
Surface complexation and shape of anatase nanoparticles
Anatase nanoparticles
obtained without complexant
In presence of glutamic acid
In presence of oleic acid
20 nm
Only 101 faces
Durupthy, O.; Bill, J.; Aldinger, F. Cryst. Growth Des.
2007, 7, 2696
Matijevic, J. Colloid Interface Sci. 103 (1985)
(100) and (001) faces
30 nm
Ethylenediamine
(100) faces
Sugimoto, T.; Zhou, X. P.; Muramatsu, A. Journal of Colloid and Interface Science 2003, 259, 53
What are the relevant parameters to control the growth of
nanoparticles ?
0
-2
-4
-6
-8
-10
-12
0 2 4 6 8 10 12 14 pH
1,0
1,1
1,2
1,3
1,4
2,2 3,4
Log [Fex(OH)y]
solubility
PZC
Size, Shape =
f(Solubility)
Size, Shape =
f(Surface energy)
Titanium oxide Nanoparticles
Rutile
Cristalline structure depends on synthesis
conditions
Anatase
Mine Falls Park, Nashua, NH
(I41/amd) (P42/mnm)
Stony Point, Alexander County, NC
(Pcab)
Mina Maria,Caneca, Sonora, Mexico
Brookite
DH°f ( kJ.mol-1)
r (g/cm-3)
-939 -941 -944
3,84 4,17 4,26
3 polymorphs
Pigment : paints, papers, plastics, cosmetic
and pharmacy
Photocatalysis, photovoltaic …
Alcalinisation
2 ≤ pH ≤ 6
Ti(OH)4(OH2)20
Thermolysis in acidic medium
Ti(OH)2(OH2)4 2+
≈ 100°C
TiO2 anatase
brookite
rutile
Thermolysis with
chlorides
Ti(OH)2X2(OH2)20
Oxolation
Olation
[Ti(OH)4(OH2)2]0 TiO2
Titanium oxide Nanoparticles
[H+]sol
1 M 2 M 4M
R = 6 R = 10 R = 13,5
R = length
wide
solubility increase
20 30 40 50 60 70 2
(002)
(110)
Weak nucleation : slow precipitation
High solubility : favour the growth
20 30 40 50 60 70 2
(110)
(002)
Thermolysis of TiCl4 : TiO2 rutile
Titanium oxide Nanoparticles
A. Pottier, S. Cassaignon, C. Chaneac , F. Vilain, E. Tronc, J.P. Jolivet, J. Mater. Chem., 13, 877 (2003)
0
20
40
60
80
100
0 1 2 3 4 5 6[HCl] / mol dm-3
Re
lative
pro
po
rtio
n (
%)
10,6 17,3 24,0 30,6 37,3 44,0
Cl/Ti
Rutile
[Ti(OH)2Cl2(H2O)2]0
17 <Cl/Ti <35
TiCl4 0,15 M / HCl / 95°C 48 hours
Thermolysis of TiCl4 with chloride : TiO2 brookite
3M brookite
3 nm 48 h
111
Titanium oxide Nanoparticles
A. Pottier et al. J. Chem. Mater. 2001, 11, 1116
Thermolysis of TiCl4 with chloride : TiO2 brookite
Structure control by a complexing agent
Titanium oxide Nanoparticles
Hydrolysis of Ti(III)
0,5 1 3 4,5
pH Ti(OH2)6
3+
Oxidation
Precipitation
Ti3+ Ti3+
Oxidation
Precipitation
Tix(OH)a(OH2)bz+
Oxid. /Précip.
S. Cassaignon et al., J. Phys. Chem. Solids (2007), doi:10.1016
rutile brookite rutile anatase
New Morphologies for TiO2
Titanium oxide Nanoparticles
Growth control and Seeding
TiO2 Rutile : TiCl4 3 M / HNO3 15M / 120°C 24 hours
+ Growth solution :
C(Ti4+)=0,3M
50 nm 50 nm
50 nm
Volume fraction : f = 13,3%
Q. Huang, L. Gao, Chem. Letters, 2003, 32,7
Seed
L = 160 ± 40 nm
D = 15 ± 5 nm
R = L/l
12
JACS, 2007,129 (18),5904
seed-mediated
growth process
9
20 30 40 50 60 70 2q
Mesoparticles
Dessombz A.,Thesis UPMC-Orsay,Paris 11
Properties of long nanorods
0
0.2
0.4
0.6
0.8
1
0 2 4 6 8 10 12 14 16
Nem
atic P
ropo
rtio
n
Volume Fraction (%)
Isotr
opic
Bip
hasic
nematic droplets
100 µm
f = 10,6%
f = 8,2%
S=0,75 ± 0,05
d ~ 50 nm
JACS, 2007,129 (18),5904
Collaboration : Patrick Davidson, LPS Orsay, Pierre Panine, ESRF Grenoble
Dessombz A.,Thesis UPMC-Orsay, Paris 11
Nematic phase
First order transition
Rotated Film
1 cm
Methylene blue
0
0.05
0.1
0.15
0.2
0.25
0.3
620 630 640 650 660 670 680 690 700
(nm)
Inte
nsité
(u
a.)
De
gra
da
tio
n
JACS, 2007,129 (18),5904
Polarizer //
agitation
┴
UV lamp
365 nm, 1h
Oriented Film
Collaboration : Patrick Davidson, LPS Orsay, Pierre Panine, ESRF Grenoble
Dessombz A.,Thesis UPMC-Orsay,Paris 11
Methylene blue degradation (10-5 M)
Oriented aggregation: Increase of the photocatalytic activity
Film in rotation
Film oriented (┴)
Properties of long nanorods
Photocatalysis study
Film oriented (//)
Properties of long nanorods
Anisotropy of electric properties; Photoactivation of current
Conclusion
• Aqueous chemistry of metal cations: environmentally friendly, Low cost
• Versatile way to tune oxide nanoparticles
Size, shape and crystalline structure
• Identification of relevant synthesis parameters to tune size and shape:
pH and acidity,
used of polyfunctionnal complexant : Polyols, Polycarboxylates
Surface energy and solubility of nanoparticles are the
driving force of their evolution
Microscopy staff Gervaise Mosser, Patrick Le Griel (LCMC)
Patricia Beaunier (UPMC)
Dominique Jalabert, Fabienne Warmont (Univ. Orléans)
Sophie Cassaignon, MdC
Olivier Durupthy, MdC
David Portehault, CR
Jean-Pierre Jolivet, Prof.
Elisabeth Tronc, CR
Tamar Saison, Hanno Kamp, David Chiche, Nicolas Chemin, Arnaud Dessombz, (PhD)
Agnès Pottier, Cédric Froidefond, Micaëla Nazaraly
Yuheng Wang, Anne Carton, Roberta Brayner, Pierre Gibot (Post Doc), Christelle Roy
(Master)
IFP French institute of petrol , Lyon
Rhodia, Aubervilliers
Draka Comtech, Marcoussis
Saint – Gobain Research, Aubervilliers
Lhoist, Belgium
Funding
Acknowledgements
Thank you for your attention
University Pierre et Marie Curie, Paris, France
Mélanie Auffan ,
Jérôme Rose
CEREGE
Jean-Yves Bottero, Mark Wiesner