bonding and adsorption: theoretical …...1. c-o bond weakening • c-o bond becomes longer • c-o...
TRANSCRIPT
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BONDING AND ADSORPTION:
THEORETICAL ASPECTS
Peter Saalfrank
Universitat Potsdam
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1. A. Groß, “Theoretical Surface Science”, Springer Verlag
2. S. Holloway and J. Nørskov, “Bonding at Surfaces”, Liverpool University Press
3. R. Hoffmann, “Solids and Surfaces”, Wiley
• Literature
1. Introduction
2. Physisorption
2.1 Basic characteristics
2.2 Van der Waals interaction
2.3 Physisorption at metal surfaces
3. Chemisorption
3.1 Basic characteristics
3.2 Chemical bonding in molecules
3.3 Chemical bonding at surfaces
3.4 Chemisorption of CO as a case study
4. Adsorption from first principles
4.1 Models
4.2 Methods
4.3 A few examples
• Content
CONTENT, LITERATURE
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➊ Understanding why atoms / molecules bind to surfaces
➋ Understanding how they bind to surfaces, e.g.
➌ Understanding what makes a surface reactive, e.g.
Insight rather than quantitative computation
• Goals of this lecture
1. Introduction
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Adsorbent and adsorbate
Adsorption energy Eads and free energy ∆Gads
Eads = Eads. mol. − (Efree mol. + Efree sub.) ∼ ∆Uads ∼ ∆Hads
∆Gads = ∆Hads − T∆Sads
∆Sads = entropy change = Sads. mol. − Sfree < 0 mostly=⇒ ∆Gads is usually less negative than Eads = ∆Uads
Here: Adsorption on metal surfaces mostly
• A few definitions
1. Introduction (cont’d)
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Role of adsorbate Role of surface Role of site(He on jellium, DFT)
physisorption = “physical adsorption”
2.1 Basic characteristics
2. Physisorption
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2.2 Van der Waals interaction
attractive repulsive total
dispersion Pauli repulsion Van der Waals interaction
Eattr = − CR6 Erep =
AR12 E =
A
R12−C
R6
C = 32αAαB
IPAIPBIPA+IPB
or: E = 4ε
{
(σ
R
)12
−(σ
R
)6}
“12-6 potential”
2. Physisorption (cont’d)
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Eattr = e2[
−1
2Z−
1
2(Z − r)+ 2
1
2Z − r
]
= e2[
−2(Z − r)(2Z − r)− 2Z(2Z − r) + 8Z(Z − r)
4Z(Z − r)(2Z − r)
]
= −e2
2
[
r2
Z(Z − r)(2Z − r)
]
In the limit Z ≫ r (far from surface): limZ≫r
Eattr = −e2
4
r2
Z3
Oversimplified model calculation for the attractive part (H atom as an example)
By “infinite sum” over surface-atom interactions, one gets
E =A′
Z9−C ′
Z3
“9-3 potential”
2.3 Van der Waals interactions at metal surfaces
2. Physisorption (cont’d)
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Specifity*:
chemisorption = “chemical adsorption”
3.1 Basic characteristics
3. Chemisorption
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➊ ∆−/∆+ = (1 + S)/(1− S) > 1
➋ occupation n = 0: no effectoccupation n = 1, 2: stabilizingoccupation n = 4: destabilizing
• Solve electronic Schrodinger equation Helψel = Eelψel within LCAO-MO
• For 2 atoms, 1 orbital ϕ (AO) each (e.g. H(1s)), ansatz for wavefunction (MO)
ψel = CAϕA + CBϕB CA, CB = coefficients
• In the symmetric orbital case (e.g., H2), the SE has two solutions
with HAA = 〈ϕA|Hel|ϕA〉 = HBB, HAB = 〈ϕA|Hel|ϕB〉, S = 〈ϕA|ϕB〉 (overlap integral)
• Discussion:
(1) LCAO-MO theory: The symmetric 2-orbital problem
3.2 Chemical bonding in molecules
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➊ occupation n = 1, 2: stabilizingoccupation n = 4: destabilizing
➋ ψ1 is “B-like”, ψ2 is “A-like” (B=more electronegative)
➌ 2nd order PT: ∆(2)1 = |HAB|
2/(HAA −HBB)
• ∆1 (mixing) small, if |HAA −HBB| large
• ∆1 small, if HAB small or zero
note: HAB ∼ KS(HAA +HBB) (Wolfsberg-Helmholtz)
• For asymmetric orbital case (A 6= B, 1 orbital each, e.g. H-He):
• Discussion:
(2) LCAO-MO theory: The asymmetric 2-orbital problem
3.2 Chemical bonding in molecules (cont’d)
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• ➀ (LUMO A / HOMO B) > ➁ (LUMO B / HOMO A) ≫ ➂
(HLALA −HHBHB) < (HLBLB −HHAHA) < (HiBiB −HjAjA)
• Interactions between close-lying empty orbitals (n=0) or full or-bitals (n=4) have no effect or are non-bonding
• HOMO-LUMO interactions control interatomic interactions
frontier orbital perspective
• Discussion:
(3) LCAO-MO theory: The N-orbital, 2-atom problem
3.2 Chemical bonding in molecules (cont’d)
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• Energetic picture: Metal vs. semiconductor / insulator
• Density of states (DOS) for metals
• Surfaces: Energetic / spatial picture
(1) A simple model for a metal surface: Bands
3.3 Chemical bonding at surfaces
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type energetic effect other effects➂ 2e-2 “orbital” stabilizing A → surface CT; A-S bond formation➁ 2e-2 “orbital” stabilizing surface → A CT; A-S bond formation➀ 0e-2 “orbital” weakly stabilizing surface → A CT; A-S bond formation
➃ 4e-2 “orbital” slightly destabilizing A → surface CT; A-S bond formation
A-surface bonds tend to form easier than A-B bonds
Orbital interaction picture(2) Chemical adsorption:
3.3 Chemical bonding at surfaces (cont’d)
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Lang, Williams, PRB 18, 616 (1978)
Adsorption of Li, Si, Cl on “jellium”:
Case 1: Single-level atoms
Energetic / spatial picture
(2) Chemical adsorption:
3.3 Chemical bonding at surfaces (cont’d)
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τ =tunneling time(Lorentzian) resonance width: ∆E =
h
τ
Example: H+ on jellium (PRB 18, 616 (1978))
εa ∼ ε∞a − 1/4Z
∆E ∝ e−λZ
acceptor levels shift and broaden
Case 1: Single-level atoms, a distance-dependent, closer look
(2) Chemical adsorption: Energetic / spatial picture
3.3 Chemical bonding at surfaces (cont’d)
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• A slight refinement of the energetic / spatial picture
• weakening of H-H (A-B) bond
• strengthening of H-surface bond
LUMO (A) often dominates interaction
example: H2 / metal surface
Case 2: Molecules
(2) Chemical adsorption: Energetic / spatial picture
3.3 Chemical bonding at surfaces (cont’d)
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MOs of N2 and CO:
a useful analogy:
(1) General binding mechanism
3.4 Chemisorption of CO as a case study
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more complete picture:
dominant interactions:
(1) General binding mechanism: CO bonding in TM complexes
3.4 Chemisorption of CO as a case study
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1. C-O bond weakening
• C-O bond becomes longer• C-O stretch frequency ν becomes smaller
2. M-C bond formation
3. Approximate charge neutrality
4. Consequences
• linear upright orientation of CO• binding via C to M, not O to M
• Consequences of synergetic bonding mechanism
Blyholder model
dominant interactions:
(1) General binding mechanism: CO bonding to TM surfaces
3.4 Chemisorption of CO as a case study (cont’d)
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• c(2×2) CO-Ni(100): (Extended Huckel) Charges
(face centered cubic, fcc)
• Cuts through metal surfaces
(2) Example: CO on Ni(100)
3.4 Chemisorption of CO as a case study (cnt’d)
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• more metal atoms
• stronger back-donation,weaker C-O bond, smaller ν
• analogy metal carbonyls
• Other adsorption sites: CO/Ni(100)
• c(2×2)CO-Ni(100): Density of states (EHT calculation)
3.4 Chemisorption of CO as a case study (cont’d)
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(EHT results)Example: CO on various Ni faces
(or Fermi energy EF )Effect of workfunction Φ
• Effect of crystal face:
• Effect of adsorption site: Large coordination =⇒ weak C-O bond
(3) Trends in CO chemisorption
3.4 Chemisorption of CO as a case study (cont’d)
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Charges for TM/CO (EHT calculation)
early TM more reactive
Trends for transition metals (from Ti → Ni):
➊ Increasing Z =⇒more contracted d-orbitals
➋ Increasing Z =⇒higher ionization potential (lower EF , larger Φ)
• Effect of metal type:
(3) Trends in CO chemisorption
3.4 Chemisorption of CO as a case study (cont’d)
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approximate relation:∆Hads ∼ M → 2π∗ back-donation
Binding energies
• Breaking C-O bonds:
(3) Trends in CO chemisorption
3.4 Chemisorption of CO as a case study (cont’d)
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Baerends et al., Chem. Phys. 177, 399 (1993)
advantages disadvantages
• no lateral boundaries • low coverage
• faster convergence • impurities
• high coverage • excited states
• metals: D(EF ) • periodicity along z
slab models supercell models
(2) Periodic models
advantages disadvantages
• molecular • boundary effects
=⇒ quantum chemistry =⇒ embedding
• excited states • which cluster?
• good for insulators, • bad for metals
semiconductors
e.g. H2O/Al9
(1) Cluster models
4.1 Models
4. Adsorption from “first principles”
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electronicstructure
basedwavefunction density
based
semi−empirical
firstprinciples
DFTKohn−Sham
many−bodycorrections
ab initio
Hartree−Fock (HF)
post−HF
semi−empirical
HMO, EHT, CNDO,AM1, ....
GW
LDA, GGA,B3LYP, ....
CI, MPn, CC, CASSCF, ....
EAM, TBDFT
r = electronic, R = nuclear DOF, n = state, Eel= electronic energy, Vnuc,nuc = nuclear repulsion
Potential energy surfaces:
Vn(R) = Eel,n(R) + Vnuc,nuc(R)
Electronic Schrodinger equation:
HelΨel,n(r, R) = Eel,n(R) Ψel,n(r, R)
(1) Overview over methods
4.2 Electronic structure methods
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Example: Dissociation energies (meV) of 2 graphene layers
functional DFT DFT-D2 DFT-D3
BLYP -29 62 59
RPBE -31 65 55
PBE -1 47 41
exp. 52 ± 5JCP 132, 154104 (2010)
Example: Grimme D2 correction
ED2disp = −s6
NA∑
A
NA∑
B>A
CAB6
R6AB
fd(RAB)
Edisp = −C6/R6 − C8/R
8 − C10/R10 · · ·
EDFT-D = EDFT + Edisp
• The DFT+D method(s) for weak interactions
• Methods for non-bonded interactions
rank method (type) HB CT DI WI average
1 MPWB1K (m-h-GGA) 0.61 0.50 0.52 0.22 0.46
2 MP2 (WFT) 0.66 0.60 0.55 0.16 0.49
16 B3LYP (h-GGA) 0.77 0.80 0.78 0.60 0.74
31 PBE (GGA) 0.50 2.94 0.49 0.28 1.05
44 SVWN5 (LDA) 4.63 6.73 2.93 0.40 3.67
average 1.28 1.78 0.92 0.56 1.14HB=H-bonded; CT=charge transfer; DI=dipolar interactions; WI=weakinteractions; MAD (kcal/mol), 22 data sets; Truhlar JCTC 1, 415 (2005)
• Potential curve of Ar-Ar
3 4 5 6 R (Angstrom)
−0.01
0
0.01
V(R
) /e
V
4 5 6 7
RHF
MP4
MP2
(a) (b)
LJ
MP4
ε
σ
B3LYP
(2) Dispersion forces and other non-bonded interactions
4.2 Electronic structure methods (cont’d)
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for H/Pd(100)
Groß, “Theoretical Surface Science”
• Surface reconstruction
• Site, coverage, index dependence
(1) H atoms at Pd low-index surfaces
4.3 A few selected examples
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CO adsorptionO adsorption
Ann. Rev. Phys. Chem. 53, 319 (2002)
• First principles vs. model expression
Ed−hyb = −2(1− f )V 2
|εd − εa|+ αV 2
f = d-band filling V=coupling adsorbate level / d-bandεd,a = d-band centre, adsorbate level α = constant
• Chemisorption energy: d-band contribution (atoms)
(2) Trends: Hammer-Nørskov model for adsorption on transition metals
4.3 A few selected examples (cont’d)
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∆Eads(Pt(11,7,5), Pt(111))∼ 0.7 eV
defects / kinks are more reactive
can be explained by d-band model
• CO adsorption on stepped CO/Pt(11,7,5) kink sites
(755) surface(911) surface
• Stepped and structured surfaces
(3) Adsorption on structured surfaces
4.3 A few selected examples (cont’d)
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Ann. Rev. Phys. Chem. 53, 319 (2002)
• Further examples
(3) Adsorption on structured surfaces
4.3 A few selected examples (cont’d)
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Nørskov et al., Ann. Rev. Phys. Chem. 53, 319 (2002)
=⇒ reaction proceeds at steps
• Stationary points for (1): N2/Ru(0001)
=⇒ step (1) is rate-limiting
• Reaction:
N2 + 3 H2
surface, p, T⇋ 2 NH3
(4) Steps of ammonia synthesis
4.3 A few selected examples (cont’d)
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(if not too fast)
particles follow adiabatic potential
➊ chemisorption curve
➋ physisorption curve
➌ chemisorption minimum
➍ physisorption minimum
➎ barrier to dissociation
➏ dissociation energy in gas phase
diabatic picture adiabatic picture
(5) Activated, dissociative adsorption: Lennard-Jones picture
A few selected examples (cont’d)
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• Potential energy surfaces
• Reaction dynamics
• Reaction kinetics
• Heterogeneous catalysis
• Outlook
• Physisorption and chemisorption
• Chemisorption: Affinity level matters
• Chemisorption: (Metal) Fermi energy matters
•Molecules: Molecular & dissociative adsorption
• Summary
Summary and outlook