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School of Chemistry, University of Nottingham,UK 1
Why Does Star Formation Need Surface Why Does Star Formation Need Surface Science? Science?
Using Laboratory Surface Science to Understand the Using Laboratory Surface Science to Understand the Astronomical Gas-Grain InteractionAstronomical Gas-Grain Interaction
Martin McCoustra
School of Chemistry, University of Nottingham,UK 2
Gas, Dust and Grains– A Chemist’s Guide to Astronomy
Probing the Gas-Grain Interaction– Surface Science for Astronomers
Some Examples– Water Ice Film Growth and Desorption
– The Carbon Monoxide - Water Ice System
Where Do We Go From Here? Conclusions and Acknowledgements
Outline
School of Chemistry, University of Nottingham,UK 3
Gas, Dust and Grains
Eagle Nebula
Horsehead Nebula Triffid Nebula
30 Doradus Nebula
School of Chemistry, University of Nottingham,UK 4
Gas, Dust and Grains
Hot, Shiny Things– Stars etc.
• Elemental Foundaries
• Small molecules, e.g. H2O, C2, SiO, TiO, SiC2 …, in cooler parts of stellar atmospheres
• Nanoscale silicate and carbonaceous dusts
School of Chemistry, University of Nottingham,UK 5
Gas, Dust and Grains
Cold, Dark Stuff– Interstellar Medium (ISM)
• Generally cold and dilute, but there are some hot and some dense regions
Photoionisation regions Clouds
• Spectroscopic observations have found over 110 different types of chemical species
Atoms, Radicals and Ions, e.g. H, N, O, …, OH, CH, CN, …, H3
+, HCO+, ...
Simple Molecules, e.g. H2, CO, H2O, CH4, NH3, …
“Complex” Molecules, e.g. HCN, CH3CN, CH3OH, C2H5OH, CH3COOH, (CH3)2CO, amino acids(?), nucleic acids(?)
School of Chemistry, University of Nottingham,UK 6
Gas, Dust and Grains
Molecules are associated with star forming regions and are crucial for maintaining the current rate of star formation
Thermal motion will resist further gravitational collapse unless the cloud is radiatively cooled
Rovibrational transitions in complex molecules resulting in radio, microwave and infrared emission provide the means of doing so
Cold Cloud
Gravitational Collapse Hot Cloud
School of Chemistry, University of Nottingham,UK 7
Gas, Dust and Grains Complex molecules point to a surprisingly
complex chemistry– Low temperatures (<20 K) mean that reactions
can’t be thermally activated
– Low pressures (<<10-10 mbar) mean that three-body processes are unlikely
The chemistry must be efficient– Ion-Molecule Reactions
• e.g. C+ + H2 CH+ + H
– Neutral Exchange/Abstraction Reactions• e.g. N + OH NO + H; H2 + OH H2O
+ H
But ...
School of Chemistry, University of Nottingham,UK 8
Gas, Dust and Grains
Gas-dust interactions are invoked as a means of accounting for the discrepancy between gas-phase only chemical models and observations– “Catalytic” Surfaces
• e.g. H+H H2
– “Freeze Out” Surfaces
About 1% of the mass of the interstellar medium is in the form of ice-covered dust grains
Ground- and space-based IR astronomy tells us its scale and composition
School of Chemistry, University of Nottingham,UK 9
Gas, Dust and Grains Grains are typically no more
than a few 10’s of nm across Have a core and mantle
structure Mantle may have an onion-like
layering of materials if grown by accretion
The common core materials are believed to be amorphous and crystalline silicates, amorphous hydrogenated carbon materials and PAHs
School of Chemistry, University of Nottingham,UK 10
Gas, Dust and Grains
Composition of the mantle depends on the age of the cloud containing the grain.– Young Clouds (H atom rich,
[H]/[H2]>1)
• Polar Ices
• H2O, CH4, CH3OH ,…
– Old Clouds (H atom depleted, [H]/[H2]<1)
• Apolar Ices
• CO, CO2, N2, O2 ,...
School of Chemistry, University of Nottingham,UK 11
Gas, Dust and Grains
Grains have several crucial roles in the clouds– Act as catalysts for the formation of H2 from H atoms
– Reservoir of molecules used to radiatively cool collapsing clouds
– Chemical factories on and in which complex new chemical species are formed by reactions induced by photons and cosmic rays
Surface physics and chemistry play a key role in these processes, but the surface physics and chemistry of grains is poorly understood.
School of Chemistry, University of Nottingham,UK 12
NeutralsElectrons
Ions
Photons
Neutrals IonsElectrons
Photons
Looking at Grain Surfaces
Surface science attempts to paint an atomistic picture of the gas-solid interaction– Routinely achievable pressures in the UHV
– Clean, well-characterised and (perhaps) well-defined surfaces with which to work
– Tools that permit us to characterise surfaces either by being intrinsically surface specific or capable of operating in a surface sensitive manner
School of Chemistry, University of Nottingham,UK 13
Reflection-Absorption Infrared Spectroscopy (RAIRS)– Grazing incidence reflection from a metal substrate
yields a 50 to 60-fold increase in sensitivity over transmission spectroscopy
– Thin (< 50 nm) films minimise bulk absorption
– Identification of adsorbed species by their infrared spectra
– Use of a metal substrate potentially allows determination of adsorbate orientation
Looking at Grain Surfaces
School of Chemistry, University of Nottingham,UK 14
Temperature Programmed Desorption (TPD)– Mass spectrometric detection of desorbed neutrals as
film is heated
– Line-of-sight geometry employed to localise region of the surface from which desorption is detected
– Film composition and reaction products
– Mechanistic and kinetic information
Looking at Grain Surfaces
School of Chemistry, University of Nottingham,UK 15
Gold Film
Cool to Below 10 K
InfraredBeam
MassSpectrometer
Looking at Grain Surfaces
School of Chemistry, University of Nottingham,UK 16
Looking at Grain Surfaces
H. J. Fraser, M. P. Collings and M. R. S. McCoustraRev. Sci. Instrum., in print
School of Chemistry, University of Nottingham,UK 17
Direct molecular beam measurements of the condensation and evaporation of water ice films by Kay and co-workers (J. Phys. Chem., 1996, 100, 4988)
Water Ice Films
Cooled (80-250 K) Ruthenium single
crystal
H2OBeam
QMS
School of Chemistry, University of Nottingham,UK 18
Water Ice Films
King and Wells method used to investigate temperature variation of condensation coefficient, .
School of Chemistry, University of Nottingham,UK 19
Water Ice Films
Condensation coefficient reflects balance of adsorption and desorption processes occurring at the surface
Input Flux, JinReflected Flux, Jref
Adsorbed Flux, Jads
Desorbed Flux, Jdes
in
desin J
)T(k)T(S)J,T(
School of Chemistry, University of Nottingham,UK 20
Water Ice Films
School of Chemistry, University of Nottingham,UK 21
Water Ice Films
School of Chemistry, University of Nottingham,UK 22
Water Ice Films
Sticking coefficient, S, of H2O is unity and independent of temperature
Exponential increase in rate of desorption with temperature suggests that desorption kinetics of ice multilayers are zero order
Edes=48.25 ±0.80 kJ mol-1
School of Chemistry, University of Nottingham,UK 23
Water Ice Films
TPD measurements of ice deposited at ca. 10 K (McCoustra and co-workers, Mon. Not. Roy. Astron. Soc., 2001, 327, 1165-1172)
Confirms zero order desorption kinetics of multilayer ice films
School of Chemistry, University of Nottingham,UK 24
Water Ice Films
Kinetic analysis gives the rate coefficient for desorption of multilayer water ice films
1-2-RT/500000,48230)bulk(OH s cm moleculese10dt
dn2
School of Chemistry, University of Nottingham,UK 25
At temperatures around 10 K, ice grows from the vapour phase by ballistic deposition. The resulting films are highly porous (Kay and co-workers, J. Chem. Phys., 2001, 114, 5284-5294; ibid 5295-5303)
Thermal processing of the porous films results in pore collapse at temperatures above ca. 30 K
TEM studies show the IhdaIlda phase transition occurring between 30 and 80 K and the Ilda Ic crystallisation process at ca. 140 K in UHV (Jenniskens and Blake, Sci. Am., 2001, 285(2), 44-50)
Water Ice Films
School of Chemistry, University of Nottingham,UK 26
CO on Water Ice
20 L of CO exposed to the substrate at 7 K.– On gold we clearly have
multilayer and monolayer desorption.
– On water ice, TPD is much more complex with evidence for strong binding of the CO to the surface and trapping of CO in the ice matrix.
CO on Gold
CO on Water Ice
School of Chemistry, University of Nottingham,UK 27
CO on Water Ice
At low exposures, the CO monolayer peak occurs at much greater temperatures than on gold (50 K cf. 30 K).
CO is much more strongly bound to the ice surface than previously thought.
School of Chemistry, University of Nottingham,UK 28
CO on Water Ice
As the exposure increases, the monolayer peak moves to lower temperature.
This suggests that the CO is perhaps sampling more weakly bound sites.
School of Chemistry, University of Nottingham,UK 29
CO on Water Ice
High temperature volcano features associated with crystallisation (ca. 140 K) and ice film evaporation seem to saturate out.
School of Chemistry, University of Nottingham,UK 30
CO on Water Ice
At sub-monolayer exposures, CO RAIR spectrum shows two features that grow in at 2152 and 2140 cm-1, respectively
Two binding sites for CO on the water surface?
School of Chemistry, University of Nottingham,UK 31
At sub-monolayer exposures, CO RAIR spectrum shows two features that grow in at 2152 and 2140 cm-1, respectively
Two binding sites for CO on the water surface?
CO on Water Ice
Extended Compact
?2152 cm-1 2140 cm-1
School of Chemistry, University of Nottingham,UK 32
Two multilayer features grow on top of the monolayer features at 2142 and 2138 cm-1
Splitting of longitudinal (LO - 2138 cm-1) and transverse optical (TO - 2142 cm-1) modes of the solid CO - LST Splitting
CO on Water Ice
School of Chemistry, University of Nottingham,UK 33
Between 8 and 15 K, redistribution of IR intensity without significant loss to the gas phase suggests CO diffusion into porous ice structure.
At least two CO binding sites characterised by 2152 cm-1 and 2138 cm-1 features.
CO on Water Ice
School of Chemistry, University of Nottingham,UK 34
High frequency feature lost as pores collapse between 30 and 80 K.
A single CO site is preferred above 80 K until volcano desorption occurs.
Single feature, 2138 cm-1, is all we observe if we adsorb on to non-porous ice grown at 80 K.
CO on Water Ice
School of Chemistry, University of Nottingham,UK 35
< 10 K
Tem
pera
ture
10 - 20 K
30 - 70 K
135 - 140 K
160 K
CO on Water Ice
M. P. Collings, H. J. Fraser, J. W. Dever, M. R. S. McCoustra and D. A. WilliamsAp. J. Lett., submitted
School of Chemistry, University of Nottingham,UK 36
We have constructed a kinetic model that reproduces our TPD observations– CO is deposited as a
monolayer (i) and multilayers (s) at the water ice interface
CO on Water Ice
)g(CO)i(CO
)g(CO)s(CO
School of Chemistry, University of Nottingham,UK 37
We have constructed a kinetic model that reproduces our TPD observations– Warming results in
diffusion from the multilayer material to monolayer sites in pores (i-p)
CO on Water Ice
)g(CO)i(CO
)g(CO)s(CO
)pi(CO)s(CO
School of Chemistry, University of Nottingham,UK 38
We have constructed a kinetic model that reproduces our TPD observations– Monolayer CO desorption
is the same from the open surface and from pore surfaces
CO on Water Ice
)g(CO)i(CO
)g(CO)s(CO
)pi(CO)s(CO
)pg(CO)pi(CO
School of Chemistry, University of Nottingham,UK 39
We have constructed a kinetic model that reproduces our TPD observations– There is a bottleneck
restricting escape of gas phase molecules from pores allowing re-adsorption to compete
CO on Water Ice
)g(CO)i(CO
)g(CO)s(CO
)pi(CO)s(CO
)pg(CO)pi(CO
)pi(CO)pg(CO
)g(CO)pg(CO
School of Chemistry, University of Nottingham,UK 40
We have constructed a kinetic model that reproduces our TPD observations– Pore collapse, trapping
CO in the ice matrix, is assumed to be autocatalytic
CO on Water Ice
)g(CO)i(CO
)g(CO)s(CO
)pi(CO)s(CO
)pg(CO)pi(CO
)pi(CO)pg(CO
)g(CO)pg(CO
)pt(CO)pi(CO)pt(CO
)pt(CO)pi(CO
School of Chemistry, University of Nottingham,UK 41
We have constructed a kinetic model that reproduces our TPD observations– Trapped CO desorbs with
the same kinetics as bulk water ice
CO on Water Ice
)g(CO)i(CO
)g(CO)s(CO
)pi(CO)s(CO
)pg(CO)pi(CO
)pi(CO)pg(CO
)g(CO)pg(CO
)pt(CO)pi(CO)pt(CO
)pt(CO)pi(CO
)g(CO)pt(CO
School of Chemistry, University of Nottingham,UK 42
Using reasonable values for the various kinetic parameters, this model qualitatively reproduces our observations
CO on Water Ice
School of Chemistry, University of Nottingham,UK 43
Just like opening Pandora’s Box In terms of work at Nottingham
– Short Term• Tie up the loose ends on the Water-Carbon Monoxide System
Kinetics Spectroscopy
• TPD survey of other molecules in dilute mixtures with water
– Medium Term• Water-Carbon Dioxide, Water-Methane and Water-Ammonia
Systems
• Others ?
– Longer Term• Atoms, Radicals, Ions and Photons
Where Do We Go From Here?
School of Chemistry, University of Nottingham,UK 44
Growing number of European groups working in the area– Chalmers University
• Photon-induced processes on ice
– Leiden• Studies on the O+CO reaction
– UCL• Theory and Experiment of state-resolved studies on H+HH2
• Studies on the H+CO etc.
– Université de Provence• IR studies of small molecules in/on ice
• Theoretical modelling of ice surfaces
– …
Where Do We Go From Here?
School of Chemistry, University of Nottingham,UK 45
Surface Science techniques (both experimental and theoretical) can help us understand heterogeneous chemistry in the astrophysical environment
Much more work is needed and it requires a close collaboration between laboratory surface scientists, chemical modellers and observers
Traditional astronomy funding agencies have to appreciate the differences between observational/theoretical work and laboratory work
Framework 6?
Conclusions
School of Chemistry, University of Nottingham,UK 46
Acknowledgements
Professor David Williams (UCL)Dr. Helen Fraser (University of Leiden)
John Dever and Dr. Mark Collings (University of Nottingham)
££ PPARC, EPSRC and the University of Nottingham ££
School of Chemistry, University of Nottingham,UK 47
School of Chemistry, University of Nottingham,UK 48
Why UHV?
Number densities in UHV approach those of dense clouds
Atmospheric Pressure
UHV
HV
XHV
DenseCloudsDiffuse
Clouds
GeneralISM
School of Chemistry, University of Nottingham,UK 49
Why UHV?
UHV helps us to keep a surface clean.
Assuming each molecule striking a surface sticks, the time it takes to fill the surface can be estimated from the equation below.
Tmk2
PZ
Bw
School of Chemistry, University of Nottingham,UK 50
School of Chemistry, University of Nottingham,UK 51
Surface Probes
Over 50 different experimental probes available to the surface scientist– Surface Atomic and Molecular Structure/Composition
• AES, EELS, LITD, UPS, RAIRS, SFG, SIMS, TPD, VEELS, XPS, …
– Surface Structure and Geometry• HAD, LEED, SRXD, XAFS, XSW, …
– Gas-Solid Interactions and Reactions• Atomic/Molecular Beam Scattering, State-resolved
Techniques, Time-resolved Techniques