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Quantitative aspects of IR spectroscopy as applied to adsorbed
species
Edoardo Garrone
Dipartimento di Scienze dei Materiali ed Ingegneria Chimica, Politecnico di Torino, Corso Duca degli
Abruzzi 24, 10129 Torino Italy
IR spectroscopy: mainly a qualitative technique, useful for recognising species
Group frequencies:
- carbonylic groups C=O at 1700-1750 cm-1,
- Si-H groups around 2200 cm-1, etc.
[e.g. G. Socrates, Infrared and Raman characteristic group frequencies: tables and charts. (2001) Wiley, Chichester, United Kingdom]
Examples of qualitative use of IR Spectroscopy concerning adsorbed species
- carbon dioxide on basic oxides: carbonate species may be formed, and/or species molecularly adsorbed onto cations
(G. Ramis, G. Busca, V. Lorenzelli, Mater. Chem. Phys. 29 (1991) 425)
- pyridine (or ammonia) adsorption: Brønsted or
Lewis sites revealed by the formation of pyridinium (ammonium) species, or molecularly bound species
(H. Knözinger, Adv. Catal. 25 (1976) 184)
A puzzling case concerning ethylene dissociative adsorption with extended metal surfaces:
ethylidene species C-CH3
(C. E. Anson, N. Sheppard, D. B. Powell, J. R. Norton, W. Fischer, R. L. Keiter, B.F.G.Johnson, J.Lewis, A.K. Bhattacharrya, S. A. R.
Knox, M. L. Turner, J. Am. Chem. Soc. 116 (1994) 3058)
IR Spectroscopy also yields information on the local symmetry and the types of bonds
- carbonate species (unidentate, bidentate, etc)
- carbonylic species (CO on metals): “on- top”, bidentate, tridentate CO species, with different C-O bond order and frequencies, all below 2143 cm-1 (isolated molecule)
- adsorption of CO on cations: C-O stretch with a frequency usually > 2143 cm-1
Much less developed the quantitative use of IR
spectroscopy of surface species!
Modalities of measurement
Most common measurement type in the case of adsorbed species is transmission.
Also available:
• Diffuse Reflectance (DRIFT) techniques
• Attenuated Total Reflection (ATR) or Grazing Angle
• with metal ideal surfaces, the appropriate version of vibrational spectroscopy is the Electron Energy Loss Spectroscopy (EELS)
In the present survey, only transmission measurements are
considered!
Types of transmission cells: a few categories, according to the working temperature (T), and the its control.
• Those working at room T. The actual temperature of the sample is slightly higher than the ambient (heating effect of the IR beam), and not precisely known. If pressure p changes, the temperature of the sample is also not strictly constant.
• Those working at fixed low T (coolant bath, usually liquid nitrogen at the NBP). The temperature is nominally 77 K: the actual temperature is higher (typically ca. 100 K), and not strictly constant with pressure
To vacuum line
thermal treatments
KBr windows
Cell with small optical path, working at RT
Sample holder (Cu)
KBr windows
Thermal treatments
Liquid N2
To vacuum line
IR cell working at low temperature ca. 100 K
• A few cells work at variable T
A) A.A. Tsyganenko: allows accurate measurement of T and p, but not their control. It works in a T range below ambient. Changes in T and p are slow enough so that equilibrium phenomena can be followed
B) A. Zecchina and co-workers: equipped with a cryostat: strict control over T. It works below ambient T and may operate down to 4 K.
C) A commercial cell (AABSPEC) working at controlled T and p also in a range above room T. Limited dead volume (few cubic centimetres)
Tsiganenko cell: T variable, but not controlled
(C.Otero Areán, O.V. Manoilova, A.A. Tsyganenko, G. Turnes Palomino, M. Peñarroya Mentruit, G. Geobaldo, E. Garrone, Eur. J. Inorg. Chem. (2001) 1739)
Zecchina cell: cryostat down to liquid He
(G. Spoto, E. N. Gribov, G. Ricchiardi, A. Damin, D. Scarano, S. Bordiga, C. Lamberti, A. Zecchina, Prog. Surf. Sci. 76 (2004) 71)
For simplicity, from now on an adsorbate showing only one
band will be considered
Measurable quantities for an IR band:
i) frequency (peak position)
ii) intensity (either at the peak or integrated intensity)
iii) half-width
iv) other parameters entering the analytical representation of the band: e.g., fraction of Lorentzian and Gaussian functions
Frequency
(peak position)
most readily measured quantity
Information on the adsorbing centre comes from the perturbation of a significant IR mode (e.g., stretching mode of CO) from a reference value (unperturbed molecule) Usually, the stronger the interaction, the larger the perturbation.
In simple cases, when considering a set of similar systems, the extent of perturbation has a quantitative meaning.
Correlations of the frequency (more commonly, the shift) with:
- the adsorption enthalpy, measured independently
- another frequency of the same system
- the frequency of another (similar) system
- another feature of the same IR band (e.g. halfwidth)
- the adsorption enthalpy, measured independently
- another frequency of the same system
- the frequency of another (similar) system
- another feature of the same IR band (e.g. halfwidth)
Two examples:
- CO adsorbed on cations
- H-bonding
CO adsorbed on cations
either non d, d0 or d10, (non classical carbonyls, with stretching frequencies higher than the isolated molecule)
Linear dependence between calorimetrically measured heats of adsorption and the hypsochromic shift:
Correlation between CO shift and heat of adsorption for non-d carbonyls
Shift is positive with respect to 2143 cm-1
Non d cations
Cu carbonyls
V. Bolis, A. Barbaglia, S. Bordiga, C. Lamberti, A. Zecchina, J. Phys. Chem. B 108 (2004) 9970.
Only electrostatics involved, no proper chemical bond
If double interactions take place with both ends of the CO molecule as in Al-rich zeolites, the linear relationship does not hold lower frequency and larger interaction enthalpy
(C. Otero Areán, M. Rodriguez Delgado, C. Lopez Bauçà, L. Vrbka, P. Nachtigall, Phys. Chem. Chem. Phys. 9 (2007) 457)
H-bonding: the shift of the O-H stretch Δν(O-H) measures the strength of H-bond
A few formulas proposed: electrostatics basically involved!
Classical work by N. Sheppard and G.C. Pimentel.
(N. Sheppard, in Hydrogen Bonding, ed. D. Hadzi, Pergamon Press, London, 1959, p. 85.
G. C. Pimentel and A. L. McClellan, in The Hydrogen Bond, W. H. Freeman and Co., San Francisco, 1960).
- the adsorption enthalpy, measured independently
- another frequency of the same system
- the frequency of another (similar) system
- another feature of the same IR band (e.g. halfwidth)
Correlation between two different modes of the same type of adduct.
CO H-bonded to different acidic hydroxyls: the C-O frequency linearly correlated to Δν (O-H)
(O. Cairon, T. Chevreau, J.C. Lavalley, J. Chem. Soc. Faraday Trans. 94 (1998)
3039)
- the adsorption enthalpy, measured independently
- another frequency of the same system
- the frequency of another (similar) system
- another feature of the same IR band (e.g. halfwidth)
Example:
the silanol in phenylene Periodic Mesoporous Organosilica (PMO) H-bonded to molecules with increasingly basic character
C
H
O
Si
b
a
C
H
O
Si
b
a
Figure 1
Inagaki, S.; Guan, S.; Ohsuna, T.; Terasaki, O. Nature 2002, 416, 304.
1,4diphenylene PMO
Onida, B.; Borello, L.; Busco, C.; Ugliengo, P.; Goto, Y.; Inagaki, S.; Garrone, E. J.Phys. Chem. B, 109 (2005) 11961
Computer models
periodic
cluster
3800 3600 3400 3200 3000 2800
0.5 A.u.
Ab
sorb
an
ce
wavenumbers (cm-1)
N2
CO
C6H6
Propene
Ammonia
Acetone
Cyclohexene
Mesitylene
Increasing basicity
Bellamy-Hallam-William plot
Comparison of the shifts suffered by the O-H stretch of silanols in:
- phenylene PMO
- amorphous silica
Proportionality constant: a measure of the relative acidity of the two O-H species
Proportionality constant ca. 0.96 Silanol in PMO slightly less acidic than in silica
For bridged OH species in zeolites proportionality constant ca. 3 (much more acidic!)
Deviations may occur!
0 30 60 90 120 150 1800
100
200
300
400
500
1,3,5-TMB
C3H
6
C6H
6
C2H
4
CO
N2
S
i(O
H)A
l SA
PO
-40 c
m-1
SiOHAerosil
(cm)
SAPO-40
Benzene and mesytilene show deviations with respect to the BHW plot
0 20 40 60 80 100 120 140 1600
100
200
300
400
500
600
C3H
6
C7H
8
C6H
6
C2H
4
CO
N2
S
i(O
H)A
l ZS
M-5 (
cm-1)
SiOHAerosil
(cm-1)
H-ZSM-5
Benzene and toluene show deviations
C3H6
C6H6 (CH3)2CO
C2H4
Hindrance of the interaction by the surroundings
freehindered
- the adsorption enthalpy, measured independently
- another frequency of the same system
- the frequency of another (similar) system
- another feature of the same IR band (e.g. halfwidth, intensity)
In H-bonding, the larger the shift, the wider and the more intense the band of the stretching mode of the O-H species engaged
Quantitative relationships are known
3800 3600 3400 3200 3000 2800
0.5 A.u.
Ab
sorb
an
ce
wavenumbers (cm-1)
N2
CO
C6H6
Propene
Ammonia
Acetone
Cyclohexene
Mesitylene
Intensity
More troublesome quantity
IR transmission experiment concerning solutions: measurement of the population of absorbing centres through the classical
Lambert-Beer law (LBL)
A = absorbance; k = absorption coefficient; c = concentration of absorbing centres; d = thickness of the sample; ε = molar extinction coefficient,
LBL: A = k d = ε c d
IRS measurements concerning a pellet:
A = ε N/ S
S = geometrical surface of the pellet N = number of moles of adsorbing centres in the whole sampleε = molar extinction coefficient
Absorbance measures the number of moles in the sample! quantitative aspects!
Two reasons could impede the applicability of LBL:
i) the presence of scattering because of the
powder structure of the samples;
ii) a change in the environment of the absorbing centres due to a change in pressure, in reversible adsorptions (not really important)
Treatment of scattering: Schuster-Kubelka-Munk model (the same for Diffuse Reflectance)
A forward flux I and a backward flux J:
-dI/dx = (k + s) I – s J
+ dJ/dx = -s I + (k + s) J
s = scattering coefficient, k = absorption coefficient
(G. Kortum, Reflectance spectroscopy : principles, methods, applications. (1969), Sprinter-Verlag, New York)
T = [1 - R2] exp [- b s d] / 1 - R
2 exp [- 2 b s d]
b = [(1 + k/s)2 - 1]1/2; d = sample thickness, R = reflectance of the sample at infinite thickness
R = 1 + k/s - [(k/s)2 + 2 k/s] 1/2
In case of moderate scattering (s < 10% k),
-ln T = Aapp sd + kd + (s/k) 2 [1 – kd]
k depends on the concentration c, s does not.
k = k0 + ε N/S s = s0
(k0 = absorption of the solid alone): k is growing with coverage
Result: in case of moderate scattering (s < 10% k), LBL holds (small offset, the term sd). For larger values of s/k, deviations may occur.
Note: scatter of radiation is more often due to voids in the sample than to the actual particles. Silica samples, white when powdered, tend to become transparent when pelleted. The condition s << k is more readily fulfilled for pelleted samples than for loose powders
Example showing that the intensity of a band has to be considered with care:
Porous silicon
Also shows a peculiar way of making a quantitative use of IR spectroscopy!
Teflon CellTeflon Cell
PREPARATIONPREPARATION
Silicon piece (1.1x1.1cm)Silicon piece (1.1x1.1cm)
The The electrochemical electrochemical cell, in figure, is cell, in figure, is made of Teflon, made of Teflon, resisting to HF. The resisting to HF. The cathode is a cathode is a platinum rod, platinum rod, whereas the anode whereas the anode is the silicon itself.is the silicon itself.The electrolyte is The electrolyte is an ethanoic HF an ethanoic HF solution.solution.
Etching parameters (HF concentration,
current density and etching time) define
PS morphology, porosity, and specific
surface area
MICRO-, MESO-, MACRO-POROUS
SILICON
TEM Image of p+ Porous Silicon
by CNR LAMEL (Bologna)
STRUCTURESTRUCTURE
SEM Image of p+ Porous Silicon
by IUT-Lannion (France)
1. etching process does not remove
the doping atoms
2. the surface is passivated by
hydrogen (SixHy species)
CHEMICAL COMPOSITIONCHEMICAL COMPOSITION
Morphology of Porous Silicon p+
1. Loss of conductivity due to etching process nearly
insulating material
2. IR TRANSPARENT
3. Electrical reactivation in presence of
NONO2 2 TRACESTRACES
Characteristic vibrations of Si-HCharacteristic vibrations of Si-Hx x bondsbonds
Curve a: PSi as such
Curve b: in contact with .25 mbar NO2
Two effects:
- marked increase in the background
- decrease in the intensity of Si-H bands (not their location)
Cause: injection of charge carriersAffects intensity, not frequency!
(F. Geobaldo, P. Rivolo, S. Borini, L. Boarino, G. Amato, M. Chiesa and E. Garrone J. Phys. Chem. B 108 (2004) 18306)
Same phenomenon observed with reducible oxides (ZnO, SnO2)
Reduction converts an insulator oxide into a semiconductor!
In conclusion, is LBL valid?
LBL validated a posteriori (several examples in this talk)
• LBL probably holds in the vast majority of cases.
• The problem with LBL, though, is that determination of ε is difficult, because very seldom A and N are simultaneously determined.
• More often, A and N are measured in separate experiments, one spectroscopic, one volumetric: identity of temperature not assured.
Example of the uncertainties on molar extinction coefficients: non classical carbonyls on cationic centres.
Generally believed that ε increases with the frequency, though moderately, e.g.
ε = 0.7 + b (ν -2143)
when ε is given in 106 cm/mol, b = 0.050.
A.A. Tsyganenko has recently proposed a decreasing behaviour of ε with frequency for a set of carbonyls in zeolitic cationic centres
E.V. Kondriateva, O.V. Manoilova and A.A. Tsyganenko, Kinetics
and Catalysis 49 (2008) 451.
Entirely different measurement of ε through the vibrational polarizability αv
(CO) = 4 3 v2
Data concerning the vibrational polarizability αν of CO adsorbed at regular faces of microcrystalline oxides or halides
αν proportional to ε
αν measured through the shifts with coverages (Hammaker equation)
(D. Scarano et al. Adv. Catal. Vol 64)
Non-classical carbonyls
π*-d backdonation
Concerning ε, CO adsorbed on zeolitic isolated cationic centres is different from CO adsorbed at regular faces of oxides?
In the following: cases of quantitative use of IR spectra,
relying on LBL, not requiring the knowledge of ε.
Simple case of one species characterised by one band of intensity A. If the maximum intensity AM is known, the value of θ results:
θ = A/AM
The equation of state for the adsorbed species is:
F (A, T, p) = 0 or F (θ, T, p) = 0
By keeping constant one observable at a time, one obtains:
- the isostere p = p(T) at constant A
- the isotherm A = A(p) at constant T
- the isobar A = A(T) at constant p
Also possible:
- the isochore at constant overall V volume
- the isostere p = p(T) at constant A
- the isotherm A = A(p) at constant T
- the isobar A = A(T) at constant p
- the isochore at constant V
The isosteric heat is related to the change in the pressure yielding a certain value of A with temperature, through a Clausius-Clapeyron-like relationship:
[ ln p/ T]A = -qiso/RT2 or
[ ln p/ (1/T)]A = qiso/R
This procedure does not require the assumption of any model, and the procedure may be repeated at different coverages (intensities).
E. A. Paukshtis, R. I. Soltanov, E. N. Yurchenko, React. Kin. Catal. Lett. 23 (1983) 339
In principle:
in the presence of several species, isosteric heat may be calculated for each species: advantage over direct calorimetry!
Same for isotherm, etc…
Separation into several contributions!
- the isostere p = p (T) at constant A
- the isotherm A = A (p) at constant T
- the isobar A = A (T) at constant p
- the isochore at constant V
Two cases:
- Ideal adsorption (Langmuir model)
- non-ideal (UNILAN, Temkin model)
Ideal (Langmuir) model: sites all alike and non-interacting
Langmuir equation:
A / AM = θ = K(T) p/[1 + K(T) p]
K(T) = exp [ΔS°/R] exp [-ΔH°/RT]
(van’t Hoff equation)
IRS provides a priori indications on the ideal nature of the adsorption
Related IR band is expected: - to be narrow - to have a Lorentzian shape- not to shift with coverage.
Definite evidence comes from a constant heat of adsorption, as measured independently.
Identity among sites is provided by the structure in some cases.
Requirements for non-interaction among sites:
- the solid constitutes an insulator matrix
- a low density of sites
Examples of ideal adsorbing systems:
- Boron atoms at the surface of PSi
- isolated silanols on amorphous silica (Aerosil, MCM- 41, etc.)
- carboxylic groups on functionalized silica
- cationic sites on zeolites
- Boron atoms at the surface of PSi
- isolated silanols on amorphous silica (Aerosil, MCM- 41, etc.)
- carboxylic groups on functionalized silica - cationic sites on zeolites
Mechanism of interaction of NO2 with PSi(hole injection)
Each adsorbed molecule injects a carrier (hole)
the background of IR spectrum rises increase in volume concentration of
carriers (Drude formula) adsorbed amount isotherm
Spectra at increasing equilibrium pressures of NO2
0 100 200 300 400
1/p
- p
0 (n
um
be
r o
f ca
rrie
rs/c
m3 )
1/PNO
2
(mbar)
2
2
1
max
NO
NOadsads KP
KPNN
2
/1/1/1/1 maxmaxNOadsadsads PKNNN
DATA FOLLOW THE LANGMUIR MODELDATA FOLLOW THE LANGMUIR MODEL
2. 2. Carriers increase describable by a REVERSIBLEREVERSIBLE
CHEMISORPTION PROCESSCHEMISORPTION PROCESS
3. ADSORPTION ISOTHERM 3. ADSORPTION ISOTHERM applicable
1. REGENERATED CARRIERS1. REGENERATED CARRIERS ≈≈ [[B]B] (3X1019
atoms/cm3) almost all carriers have been
reactivated
Sites for NO2 adsorption (surface B atoms):
• isolated
• non interacting
because of the low concentration of B atoms in the pristine sample
Langmuir conditions
- Boron atoms at the surface of PSi
- isolated silanols on amorphous silica (Aerosil, MCM- 41, etc.)
- carboxylic groups on functionalized silica - cationic sites on zeolites
O-H band at 3750 cm-1:
- very thin, all sites equivalent
- low density (ca. 1 OH/100 Å2)
The coverage θ is calculated from the ratio between the actual intensity and the maximum intensity
Methylcyclohexene on Silica (B. Onida, M. Allian, E. Borello, P. Ugliengo, E. Garrone Langmuir 13 (1997) 5107)
Langmuir isotherm
Check of the isotherm and evaluation of K
Absence of solvation
ammonia
Deviation from ideality because of solvation
Check of the isotherm and evaluation of K
Benzene, methylcyclohexene, acetone, etc.
- Boron atoms at the surface of PSi
- isolated silanols on amorphous silica (Aerosil, MCM- 41, etc.)
- carboxylic groups on functionalized silica - cationic sites on zeolites
SBA-15-COOH deg 200°C: adsorption of NH3
2000 1800 1600 1400-0.2
-0.1
0.0
0.1
0.2
0.3
0.4
0.5
A
wavenumber (cm -1)
deg 200 6.2 11.6 20.7 32.1 44.2 72.0 87.7 105.7 124.4 145.8
2000 1900 1800 1700 1600 1500 1400 1300-0.4
-0.3
-0.2
-0.1
0.0
0.1
0.2
0.3
0.4
0.5
0.6
SBA-15-COOH spettri differenza invio NH3
A
wavenumber (cm -1)
Reversible formation of ammonium species:
R-COOH + NH3(g) R-COO- + NH4+
Carbonyl, ammonium and carboxylate modes all present in the IR spectrum!
Equilibrium constant:
K = θ/ [ (1 – θ) p]
as in Langmuir adsorption
0 20 40 60 80 100 120 140 160
0
2
4
6
8
10
12Parameter Value Error------------------------------------------------------------A -0.09641 0.02328B 0.04011 6.08931E-4------------------------------------------------------------
pNH3
Deviations because of solvation of ammonium species by molecular ammonia
Check of the isotherm: equilibrium constant evaluated!
- Boron atoms at the surface of PSi
- isolated silanols on amorphous silica (Aerosil, MCM- 41, etc.)
- carboxylic groups on functionalized silica - cationic sites on zeolites
CO/Na-ZSM-5 blue: Na; green: C; red: O
RT adsorption of CO on Na-ZSM-5
C-bonded adduct
O-bonded adduct
Three types of isotherms:
- volumetric
- calorimetric
- optical (sum of the intensities of C-down and O-down bands)
Optical isotherm as good as the others!
Non-ideal case: the Temkin (UNILAN) model
Temkin isotherm: Na = K1 ln[1 + K2p]
a variant of the UNILAN model: rectangular distribution of energies between two values E1 and E2, with E2 –E1 = 2 s.
Kh = equilibrium constant for E = (E1 + E2) / 2.
The Temkin isotherm generally assumed for structural heterogeneity: valid also for induced heterogeneity in a regular array of adsorption sites, all structurally equal.
Example: CO adsorption on TiO2 and ZrO2.
One to three CO species present. ZrO2 outgassed at 500°C: only one band is present.
Frequency not constant: proportionality between the shift and the overall intensity of the band.
The differential heat of adsorption, calorimetrically determined, has a nearly linear decrease
(V. Bolis, B. Fubini, E. Garrone, C. Morterra, J. Chem. Soc.,
Faraday Trans. 85 (1989) 1383)
- the isostere p = p(T) at constant A
- the isotherm A = A(p) at constant T
- the isobar A = A(T) at constant p
- the isochore at constant V
Rather rare in the literature on oxides. Example:adsorption of CO at the (100) face of MgO followed
at temperatures below 60 K
(G. Spoto, E. Gribov, A. Damin, G. Ricchiardi, A. Zecchina, Surf. Sci. Lett. 540 (2003) 605.).
As the adsorption has ideal features, the elaboration is straightforward: the equation (see below)
Ln [θ / p (1 – θ)] = ln [A / p (AM – A)] = ΔS° / R – ΔH° / RT
is used dropping the constant term in pressure. Information on ΔS° is lost!
Spectroscopic determination of thermodynamic features of CO adsorption on metal particles (substantial electronic effects): Bianchi and associates
Constancy of pressure is obtained by flowing the adsorbate gas in a dynamic system at a constant pressure.
Temkin model adopted
(A. Bourane, O. Dulaurent, D. Bianchi J. Catal. 196 (2000) 115)
Three peaks, coverage dependent:
• “on-top” • bridged• “hidden” species.
Each species follows a Temkin equation.
Analysis of the behaviour of the intensities with temperature through the Temkin equation allows the determination of E1
and E2.
- the isostere p = p(T) at constant A
- the isotherm A = A(p) at constant T
- the isobar A = A(T) at constant p
- the isochore at constant V
Constancy of volume: obtained by closing the cell after gas admission, then varying T and, consequently, p.
Desorption counterbalanced by the increase in pressure
Design of the cell: A.A. Tsiganenko
Methods: E. Garrone, C.O. Arean
(E. Garrone and C. Otero Areán, Chem. Soc. Rev. 34 (2005) 1)
Acronym: VTIR
Three types of process followed so far:
i) Langmuir-type adsorption on a cationic site (or hydroxyl species);
ii) isomerism between two forms of adsorbate (e.g. carbonyl/isocarbonyl);
iii) formation of dicarbonyls from monocarbonyls.
Langmuir-type adsorption on a cationic site (or hydroxyl species)
isomerism between two forms of adsorbate (e.g. carbonyl/isocarbonyl);
formation of dicarbonyls from monocarbonyls.
Suppose only one band is present, of absorbance A.
The three quantities A, T and p are related by a mass balance equation, e.g. of the type:
Nt = p Vg/RT + A/(ε S)
if the gas phase has an ideal behaviour (Nt = total number of moles and Vg = volume of the cell).
It is, however, convenient to treat T and p as independent variables, and to study the function
A = A(T, p).
Van’t Hoff equation, under the assumption of entropy and enthalpy of adsorption constant with temperature:
θ = A/AM = exp [S°/R] exp[-H°/RT] p / {1 + exp [S°/R]exp[-H°/RT] p}
AM = a parameter to be determined
More conveniently: ln [θ / p (1 – θ)] = ln [A / p (AM – A)] = ΔS° / R – ΔH° / RT
At very low coverages it results:
Ln [A / T)] = const – ΔH° / RT
does not require AM !
Two examples:
CO on protonic zeolites
H2 on cationic zeolites
Two examples:
CO on protonic zeolites
H2 on cationic zeolites
Coverage measured directly from the ratio of intensities
HY zeolite, interaction with CO
Results: ΔH° = -25.6 kJ/mol and ΔS° = -161 J mol-1K-1
Excellent agreement with the calorimetric value for H-ZSM-5 of - 27 kJ/mol (more acidic!)
(S. Savitz, A.L. Myers and J.R. Gorte J. Phys. Chem. B 103 (1999) 3687)
Two examples:
CO on protonic zeolites
H2 on cationic zeolites
VTIR spectra around 100 K of dihydrogen on Na-FER
Increasing T
H0 = - 6.0 kJ/mol
S0 = -78 J/(mol K)
Result not readily obtained in other ways! Low T calorimetry is difficult, volumetric isosteric methods as alternative
The study of H2 adsorption on several zeolitic systems has shown that ΔS0 values are correlated to the corresponding ΔH0 values.
Compensation effect.
Result relevant in storage problem
-10 0 10 20 30 40 50 60 70 80 90 100
0
5
10
15
20
25
Carbons
?
Ca-Y
(Mg,Na)-Y
K-FER
Na-MFIMg-X
Li-MFILi-FER
-H
0 (kJ
mol
-1)
-S0 (J mol-1 K-1)
Vertical segment represents carbons.
Vertical dotted line corresponds to the free gaseous molecule (loss of all degrees of freedom).
ΔS° vs ΔH° for H2 on several cation-exchanged zeolites.
Limiting value for ΔS°, corresponding to loss of translational modes
(E. Garrone, B. Bonelli and C. Otero Areán Chem. Phys. Letters 456 (2008) 68)
Langmuir-type adsorption on a cationic site (or hydroxyl species);
isomerism between two forms of adsorbate (e.g. carbonyl/isocarbonyl);
formation of dicarbonyls from monocarbonyls.
RT adsorption of CO on Na-ZSM-5
C-bonded adduct
O-bonded adduct
At relatively high T, both species are favoured, regardless their energy!
VTIR spectra of CO on Na-ZSM-5
HF band: C-bonded species
LF: O-bonded species
At low T, the more stable C-bonded species is favoured
Low-lying bands: CO species interacting with the cation through the O end
equilibrium between the two species, O-bonded and C-bonded:
M-CO M-OC
to which corresponds the equilibrium constant:
θ(CO)/θ(OC) = Kiso(T) A(CO)/A(OC)
and the van’t Hoff eqn.:
K(T) = exp [ΔS°/R] exp [-ΔH°/RT]
ΔH°iso is 3.8 kJ/mol, i.e. 14% of the enthalpy of formation of the C-bonded adduct.
Langmuir-type adsorption on a cationic site (or hydroxyl species);
isomerism between two forms of adsorbate (e.g. carbonyl/isocarbonyl);
formation of dicarbonyls from monocarbonyls.
Several cations in zeolites may coordinate more than one CO molecule.
Example: CO adsorbed on Ca(Na)Y
Up to tri-carbonyls formed with increasing coverage at 77 K
(K.I. Hadjiivanov, H. Knozinger Chem. Phys. Lett. 303 (1999) 513)
219
0
219
8
221
2
0,0
0,2
0,4
0,6
0,8
1,0
1,2
Abs
orba
nce
2100 2200 Wavenumbers (cm-1)
2149 20
95
2137
0.4
x15x15
21 C
-70 C
-196 C
-120 C
13C O-C
CO/CaNaY VTIR spectra. Low dose: monocarbonyl at 2198, dicarbonyl with two unresolved modes at 2190 cm-1
IR spectra at variable temperature concerning the adsorption of CO at variable temperature on SrY
One major band shifting with decreasing temperature (i.e. increasing coverage) from 2191 cm-1 to 2187 cm-1.
- monocarbonyl Sr(CO) 2191 cm-1
- dicarbonyl Sr(CO)2, two unresolved modes at 2187 cm-1
One minor band shifting from 2098 to 2095 cm-1
(O-bonded complexes)
(E. Garrone, B. Bonelli, A.A. Tsiganenko, M. Rodriguez Delgado, G. Turnes Palomino, O.V. Manoilova, C. Otero Areán J. Phys. Chem. B 107 (2003) 2537)
Behaviour of peak position with peak intensity
monocarbonyl
dicarbonyl
Opposite ends of the diagram: regions where the monocarbonyl or the dicarbonyl predominate. This allows, through the use of
θ = A/AM = exp [ΔS°/R] exp[-ΔH°/RT] p/{1 + exp [ΔS°/R] exp[-ΔH°/RT] p},
to measure the enthalpy changes of:
- monocarbonyl formation (adsorption on the naked cation)- dicarbonyl formation (coordination of a second CO molecule).
Use of:
θ(CO)/θ(OC) = Kiso(T) A(CO)/A(OC)
K(T) = exp [ΔS°/R] exp [-ΔH°/RT]
allows the evaluation of the enthalpy changes related to the isomerisms
Sr(CO)++ Sr(OC)++
Sr(CO)++2 Sr(CO,OC)++
Enthalpies of formation of the various CO adducts formed with SrY zeolite
Fairly complete energetic characterisation of the possible adducts!
Conclusions
Frequency readily measured: quantitative correlations possible with either, other IR features or quantities independently measured
Intensity troublesome: i) validity of LBL not always assured; ii) ε known with poor accuracy (band intensity and adsorbed amounts not measured simultaneously!)
Information may come from measurements relying on LBL but not actually using any ε.
All types of variable temperature IR measurements (including VTIR) yield thermodynamic data on:
i) ideal adsorption; ii) Temkin-like adsorption; iii) isomerism between species; iv) formation of multi-ligand complexes.
Advantage over direct calorimetry: possible separation of concurrent phenomena!
Thanks for your attention