1 title surface chemistry the molecular/atomic interactions ➔ chemisorbtion ➔ physisorbtion the...
TRANSCRIPT
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Title
Surface Chemistry
The Molecular/Atomic Interactions➔ Chemisorbtion➔ Physisorbtion
The Free Surface energy➔ Thermodynamics Considerations➔ Decreasing the surface energy
Description of a Surface T-L-K Model
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Molecular/Atomic Interactions
■ Chemisorption Formation of molecules Short Distance
■ Physisorption No molecules formation Long Distance
In most of the case: Physisorption before Chemisorption
U(r)
r
Hc
rec
Hp
rep
Eact
Chemisorption
Physisorption
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Types of interactions
Type of interactions Nature of interactionsCovalent Bonding Chemisorption Electrons ExchangeIonic Bonding Chemisorption Electrons ExchangeMetallic Bonding Chemisorption Electrons ExchangeCoulomb Forces Physisorption Charge interactionsVan der Waals Forces Physisorption Charge interactionsHydrogen Bonding Physisorption Charge interactions
■ Physisorption Exothermic lHp l < 20 kJ/mol > 1 layer adsorbed Not Specific Kinetic: Fast - since it is a non-activated process
■ Chemisorption Exothermic lHc l > 100 kJ/mol Only 1 layer adsorbed Specific Kinetic: Depends of the activation energy
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Covalent/Ionic
■ Directional■ Transfer of one or more
electron from one atom to the other
Covalent bonding
Ionic bonding
■ Directional■ Partial Exchange of
electrons■ Formation of Molecular
orbitals
Difference of Electronegativity (capacity to attract electrons) defines the type of liaison
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Metallic Bonding
■ In a solid, a huge number of atoms:
➔ Many molecular orbitals together lead to the formation of bands (conduction, valence,…)
■ Some electrons are delocalized and form a cloud
■ Is the origin of the properties of the solid: conductivity, optic, magnetic properties,...
Electrons cloud
Atom
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Van der Waals Forces
■ Interactions between dipoles
■ 3 parts: London (Dispersion) Forces
➔ Induced dipole/ Induced dipole
Debye Forces➔ Permanent dipole/ Induced
dipole Keesom Forces
➔ Permanent dipole/ Permanent dipole
■ Induced Dipole = polarizable molecules or atoms
chargedneutral
Induced dipolePermanent dipole
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Coulomb Forces and Hydrogen Bridges
■ Hydrogen bondings Directional Electrostatic interaction
between hydrogen and electronegative atoms (O, Cl, F,...)
24 r
QQF
o
ba
■ Columbic interaction Interaction between
permanent charged particles
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Surface Free Energy
Creation of a surfaceYou need energy to create a
surface!You break chemical bonds
Work to create a surface define the free surface energy γ
Thermodynamically, every system want to decrease its surface energy
Driving force for solids
dAdW
T=∞
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Surface Free Energy (2)
■ Minimizing the surface free energy:
1. By reducing the amount of surface area exposed
2. By predominantly exposing surface planes which have a low surface free energy
3. By altering the local surface atomic geometry in a way which reduces the surface free energy
Aggregation of the particles
Crystal Shapes
Relaxation/Reconstruction
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Crystal Surface
■ Example: fcc crystal Bulk
➔ In vacuum the most stable surfaces are :
fcc (111) > fcc (100) > fcc (110)
Surface
(100) face8 neighbors
(110) face7 neighbors
(111) face9 neighbors
Determination of crystals shapes
12 neighbors
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Relaxation/Reconstruction (1)
■ Relaxation adjustments in the surface
layers spacings perpendicular to the surface
■ Reconstruction change in the periodicity of
the surface structure and surface symmetry
Relaxed surface (d1-2 < dbulk
)
Unrelaxed surface
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More realistic case (Thin films)
Solid-solid interface (a) and (b) are abrupt interfaces
since there is no mixing that occurs
The non-abrupt interfaces mixing (or interdiffusion) reactive (forming new chemical
compounds, possibly multiple phases, the stability of which are dependent on thermodynamic parameters)
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T-L-K Model
■ Ex: move an atom from a terrace site to a kink site
➔ Difference: the energy of two bonds
■ Describes the structure of equilibrium surfaces
■ Assumption: all bonds are equal in the solid
■ T=Terrace■ L=Ledge■ K=Kink
terracekink WWG kTGNen
Number of atoms doing transitions