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Zeolites
Summer School in Energy and Environmental Catalysis
University of Limerick, July 2005
Tetrahedra made up of EITHER
SiO4
OR
AlO4- units
Every unit of AlO4- will have an associated cation in order to
maintain charge balance, H+, Li+, Na+, K+. NH4+ etc.
Si
O
O OO
Zeolite Chemistry
General formula for the composition of a zeolite is Mx/n[(AlO2)x(SiO2)y] . mH2Owhere cations M of valence n neutralize the negativelycharged zeolite framework.
SiO2 tetrahedra are electrically neutral (e.g., quartz)Substitution of Si(IV) by Al(III) creates an electrical imballanceand neutrality is provided by an exchangeable cation
Al
Si
Na+ Na+
imbalance
SBU of ZSM-5 zeolite
Combination of ZSM-5 SBUs shown along the a axis and
as a parallel projection along the b axis
Sinusoidal channels (0.54-0.56 nm wide
Straight channels (elliptical openings - 0.52-0.58 nm)
Channel Intersections 0.9 nm
Influence of Si/Al Ratio
Zeolites with a low [Al] are hydrophobic (and vice versa)
Lowensteins' rule, Al-O-Al linkages forbidden (Si/Al must be > or = 1)
If the counter ion is a proton then this is hydrogen bonded to the lone pairs of the neighbouring Oxygen bridging atom generating Bronstead Acidity
High temperature treatment can de-hydroxylate the zeolite and generate a Lewis acid site (i.e. lone pair acceptor) on Al atoms
High concentrations of protons (from a low Si/Al) give a high acidity but lower concentrations of protons yield STRONG acid sites
Acid Sites
Zeolite as synthesized
Bronsted acid form
Lewis acid form
Na+ Na+
H+ H+
+H2O -H2O (500 C)
+
USES OF ZEOLITES
(1) Adsorbents and desiccants- drying agents(2) Separation processes - in gas purification,(3) Animal feed supplements, (4) Soil improvements. (5) Detergent formulations (6) Wastewater treatment, (7) Nuclear effluent treatment,
(8) Catalysis
Properties that increase catalytic activity of ZEOLITES.
•molecular sieving (for shape selective catalysis)•well defined active sites•cationic exchange capacity, •high surface area,•variable acidity and controllable electrostatic fields (M2+ and M3+),•relatively good chemical and thermal stability.•sites for occluded species – generate “internal” metal particles
Examples of zeolites acting as selective catalysts in ACID CATALYSED reactions
Shape Selective Catalysis(1) Reactant selectivity,
(2) Product selectivity, and (3) Restricted transition-state selectivity
All these are examples of zeolites acting as selective catalysts in ACID CATALYSED reactions
Reactant Selectivity - reactant molecules too large to enter cavities.
e.g. Ca / A and Ca / X as catalysts for R-OH H2O + alkene
1° and 2° alcohols dehydrate on Ca/X
only 1° alcohols dehydrate of Ca/A (2° alcohols too large to get into the pores of zeolite A to the active Ca sites)
Active Sites
OH
OH
OH
OH+ H2O
Ca / X
OH
OH
OH
OH
+ H2O
Ca / A
Product Shape Selectivity;
benzene + methanol = xylene
Only para xylene can diffuse out of the ZSM-5 channel pores
Para-xylene is far more valuable than ortho or meta xylene - used in polyester manufacture
Transition State Shape Selectivity, some transition-state intermediates are too large to be accommodated within the pores/cavities of the zeolites, even thoughdiffusion of neither the reactants nor the products are restricted.
transalkylation of dialkylbenzenes
meta-xylene, 1,3,5- and 1,2,4-trialkylbenzene.
ZSM-5 Methanol gasoline catalyst
ACTIVE Sites are zeolitic protons ACID catalysis
Two intersecting sets of channels.
Methanol diffuses in through one set of channels and gasoline diffuses out the second set, thereby avoiding “counter-diffusional” limitations in the reaction rate.
What about the “surface” of the zeolitic particle, i.e. the external surface ?
Also has active sites - but no “space” constraints.
DURENE (unwanted C10 aromatic) formed on these external sites during MTG. This has been combated by
making larger zeolite particles (proportionately less external acid sites) or
Selectively poisoning external acid sites with bases too large to enter pores, e.g. tri-methyl phosphine
Bifunctional catalysis on zeolites
Ion-Exchanging a H-form zeolite with a metal removes Bronstead acidity, forming sites which may be active for other reactions –
Cu2+ in Cu ZSM-5 are active 2NO N2 + O2
(REDOX SITES)
If the system is then reduced with H2 the exchanged metal ions form small metal particles within the zeolite and the Bronstead acidity is restored.
2 effects – (a) very small (and active ??) metal
particles within pores –shape selectivity in metal catalysed reactions and
(b) Metal and acid sites in zeolite in very close proximity. Metals very good at promoting hydrogenation / dehydrogenation – Acids very good at promoting isomerisation / cracking. (ALSO More resistant to coking)
Methylcyclopentane cyclohexane 50 times faster on Pd H-Y compared to Pd
Na-Y + H-Y close proximity required!
ZSM-5 (Zeolite Synthesised by Mobil Corp (1974)
Baku Mosque – Azerbaijan (1086)
Some Characterisation Techniques
Temperature Programmed Desorption / Decomposition.
Infra Red Spectroscopy of Adsorbed Probe Molecules.
X-Ray Techniques
Temperature Programmed TechniquesTemperature Programmed Desorption (TPD)
Adsorption of molecular species onto the sample surface at low Temperature
Heating the sample with a linear temperature ramp monitoring desorption of species from surface back into gas phase.
TPD of CO from Pd
•area under peak amount originally adsorbed
•peak temperature is related to the enthalpy of adsorption, i.e. to the strength of binding to the surface..
TPD of (basic) NH3 also gives information about the concentration and strength and of surface acid sites.
NH3-TPD
Mordenite
ZSM-5
SAPO-11
ALPO-11
Weak Strong acidic sites
Amine-TPD, e.g. isopropyl amine – discriminate between Bronsted and Lewis Acid sites
Isopropyl amine adsorbs on B and Lacid sites
– During the TPD the desorption of propene and ammonia results from the decomposition of the amine occurring ONLY at Brønsted type acid sites, while desorption of isopropyl amine indicate the presence of Lewis type acid sites.
CO ( gas phase ) 2143 cm-1
Terminal CO 2100 - 1920 cm-1
Bridging ( 2f site ) 1920 - 1800 cm-1
Bridging ( 3f / 4f site ) < 1800 cm-1
CO on Pt
Very Useful as a “probe” detailing the surface
VIBRATIONAL SPECTROSCOPY
CO (g) has a stretching frequency of 2143 cm-1, CO as a ligand stretching 1700 cm-1 to 2200 cm-1
CO ligand bonds metal by (a) donating electron density (from its nonbonding lone pair) into a metal d-orbital
HOMO - orbital lone pair (weakly antibonding)
LUMO - * orbital (antibonding)
Stronger CO bond, higher energy stretch
Weaker CO bond, lower energy stretch
And (b) accepting electron density from a filled metal d-orbital of pi symmetry into it's pi* antibonding orbital. (BACKBONDING
a ba ba ba b
FTIR of Adsorbed NH3 (or pyridine) on a zeolite gives information about the types and concentrations of acid sites on the surface
i.e. adsorbing NH3 onto a Bronstead site NH4+
ads or R-NH3+
which has particular infra red stretching frequencies
adsorbing NH3 onto a Lewis acid site NH3ads or RNH2ads which has different stretching frequencies