MENA 3200 Energy Materials Materials for Electrochemical Energy Conversion Part 2 General principles of materials proper - PowerPoint PPT Presentation

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MENA 3200 Energy Materials Materials for Electrochemical Energy Conversion Part 2 General principles of materials proper

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  1. MENA 3200 Energy Materials Materials for Electrochemical Energy Conversion Part 2 General principles of materials properties and requirements Truls Norby

  2. Overview of this part of the course • What is electrochemistry? • Types of electrochemical energy conversion devices • Fuel cells, electrolysers, batteries • General principles of materials properties and requirements • Electrolyte, electrodes, interconnects • Conductivity • Catalytic activity • Stability • Microstructure • Examples of materials and their properties • SOFC, PEMFC, Li-ion batteries

  3. Main materials classesElectrolyteElectrodesInterconnects

  4. R Main materials classes + 4H+ 2O2 2H2O • Solid state electrochemical energy conversion devices contain three main functional materials classes • We will use Proton Ceramic Fuel Cells (PCFCs) and Solid Oxide Fuel Cells (SOFCs) as examples • Electrolyte • Conducts ions only • Electrodes • Conducts electrons • Anode • Cathode • Interconnect • Conducts electrons only 2H2 4e- Proton conducting fuel cell Why? Why?

  5. R Exercise - I + 4H+ O2 2H2O 2H2 4e- Concentrate on the upper half of the PCFC case • What reactants flow to the anode (fuel) and what exits in the exhaust from it? • What reactants flow to the cathode (air) compartment and what exits from it? • Does this type of cell have any advantages and disadvantages in terms of the above? Proton conducting fuel cell

  6. Exercise - II Now concentrate on the upper half of the SOFC case • What reactants flow to the anode (fuel) and what exits in the exhaust from it? • What reactants flow to the cathode (air) compartment and what exits from it? • Does this type of cell have any advantages or disadvantages as compared to the PCFC?

  7. Electrolyte • The job of the electrolyte is to conduct ions • PCFC • Proton H+ conductor • E.g. hydrated Y-substituted BaZrO3 (BZY) • SOFC • Oxide ion O2- conductor • E.g. Y-substituted ZrO2 (YSZ) • What is the effect if the electrolyte conducts also electrons?

  8. Electrodes • The main job of the electrode is to conduct electrons • PCFC • Anode: H2(g) = 2H+ + 2e- • Cathode: 4H+ + O2(g) + 4e- = 2H2O(g) • SOFC • Anode: H2(g) + O2- = H2O(g)+ 2e- • Cathode: O2(g) + 4e- = 2O2-

  9. Electrodes exercise • The main job of the electrode is to conduct electrons Concentrate on the upper halves of either of the cells • What is a secondary important job of the electrode material? Where the reactants and products of the electrochemical reactions meet are called triple-phase boundaries (3pb) • Point out the 3pb’s. What are the three phases? • What is the dimensionality of these 3pb’s?

  10. Electrodes with mixed transport Now concentrate on the lower halves of either of the cells The cathodes and the SOFC anode are shown with transport of the relevant ion in addition to electrons • The electrodes have mixed conduction • Example cathode: Sr-doped LaMO3 (M = Mn, Fe, Co) • Example anode: Ni + YSZ cermet • Where does the electrochemical reaction take place now? • What is the dimensionality of this location? The PCFC anode is shown with transport of atomic H • Example: Ni • What happens at the surface of the anode? • Where does charge transfer take place now?

  11. Just a distraction…DFT and TEM of Ni-LaNbO4 electrode interface

  12. Interconnects • Alternative name: Bipolar plates • The jobs of the interconnects are to • Conduct electrons from one cell to the next so as to connect the cells in series • Separate the fuel and oxidant gases • The interconnect must conduct only electrons • What is the effect if the interconnect also conducts ions?

  13. Dense or porous? Electrolyte? Electrodes? Interconnect?

  14. ConductivityFundamentals of electrical conductivityConductivity requirements

  15. Resistivity and resistance • Charged particles in an electric field E feel a force F • The force sets up a net flux density and current density i • The ratio ρ(rho) = E/i is termed resistivity and is an intensive materials property • Resistivity has units (V/m)/(A/m2) = (V/A)m = ohm*m = Ωm • For an object we may instead express a current I and voltage U • The ratio R = U/I (Ohm’s law) is termed resistance and is an extensive property for the object • Resistance has units V/A = ohm = Ω • The resistanceof a current-carryingobject is obtained from theresistivityρ, lengthl, and cross-sectional area a: R = ρ*l/a

  16. Conductivity and conductance • Conductivity σ (sigma) is the inverse ofresistivity: σ = 1/ρ • Conductance G is the inverse ofresistance: G = 1/R • The units for G and σare S (siemens) and S/m, respectively. • (Other/olderunits for conductancecompriseΩ-1, ohm-1, and mho) • G = σ*a/l

  17. Exercises • A rectangular solid sample has a length of 2 cm and a cross-section with sides 5 x 5 mm2. Electrodes for merasurements are painted on its far faces. • If its conductivity is 1000 S/cm, what is its conductance? • And its resistance? • A circular disk has thickness 2 mm and diameter 2 cm. We paint electrodes on its two faces and measure the resistance. • If the resistance is 10 Ω, what is theresistivity? • If the conductance is 10 S, what is the conductivity?

  18. Total conductivity, transport numbers • The conductivityof a substance has contributions from all species, mechanisms, and pathwaysofcharge carriers: • Electronic and ionic • Electronic: electrons and holes • Ionic: cations and anions • Or more detailed, for instance, protons, oxide ions, and metal cations • Mechanisms: vacancies and interstitials • Microstructuralpathways: bulk, grainboundaries, surfaces… • The total conductivity is a sum ofpartialconductivities over all species, mechanisms, and pathways: • The fractionofthe total conductivity (and ideallythefractionofanycurrentgoingthroughthesubstance) is termedthe transport number or transferencenumber for s:

  19. Exercise • Normally, only one or two charge carriers, defects, mechanisms, or pathways dominate to the extent that we need to take them into account. The others can be neglected. • What dominates the conductance in • Si? As-doped Si? • Pt? • NaCl(s)? NaCl(aq)? • H2O(l)? HCl(aq)? • Y-doped ZrO2? • La2NiO4+δ? • Alumina single crystal? Dense alumina ceramic? Porous alumina ceramic?

  20. Exercise • One can enhance or depress selected contributions for measurements or use • Discuss how you might affect the contributions below in the case of solid samples: • Electronic conductivity vs oxide ion conductivity • Proton conductivity • Bulk conductivity • Grain boundary conductivity • Outer surface conductivity • Inner surface (pore wall) conductivity

  21. Series resistance contributions • Till now, we have looked at parallel possibilities that add to conductance and give more current • There are also many sources to series problems that add to resistance and give less current (more voltage): • Bulk resistance • Traps • Grain boundary resistance • Electrode (contact) resistance • Note the difference between grain boundary conduction and grain boundary resistance • What is the source of each one? • How can they be affected?

  22. Conductivity; charge, concentration, and mobility • The conductivity of a species s is given by its charge zs, volume concentration cs, and charge mobility us. • The charge is an integer multiple zs of e or F, depending of whether the concentration is given in number of particles or moles of particles per unit volume: • The concentration cs may arise from different models comprising doping and thermodynamics for electrons and/or point defects. • Charge mobility us is the product of mechanical mobility Bs and charge zse:

  23. Charge mobility; itinerant carriers (metallic mobility) • In materials with metallic mobility (itinerant electrons or holes, broad bands) the mobility is determined by scattering, and the mobility is proportional to the mean free length between scattering events and inversely proportional to the electron or hole effective mass and the mean velocity at the mobile electrons’ energy level (Fermi level): • Scatterersaredefects (e.g. impurities) or phonons (latticevibrations) • Both contribute to resistance in series: • Typical temperature dependencies: • Typically, impurities dominate at low T and lattice vibrations at high T.

  24. Charge mobility; diffusing carriers • For ions that move by defects in materials and for non-itinerant (trapped) electrons in semiconductors, the mobility of the ionic defect or electronic species is determined by diffusion; thermally activated jumps from site to site: • Note that usT (and thus σsT) is an exponential function of 1/T, and therefore the activation enthalpy may be extracted from the slope of a plot of ln(usT) orlog(usT) versus 1/T (similar to an Arrhenius plot). • Such electronic charge carriers are called small polarons – the electron deeply trapped in the relaxation of the lattice around itself. Small polaronmobilities are orders of magnitude smaller than itinerant (metallic) mobilities. • Electronic charge carriers trapped in more shallow relaxations are called large polarons and have intermediate mobilities.

  25. Concentrations cS of charge carriers - overview • Metals: Concentration of electrons approx. equal to the concentration of valence electrons • Electronic semiconductors: Concentration of electrons n or holes p fixed by donor or acceptor dopants • Solid ionic conductors: Concentration of defects (e.g. oxygen vacancies or protons) fixed by acceptors or structural disorder • Liquid ionic conductors: Concentration of ions…

  26. Conductivity of components and defects • For foreign species, like protons in an oxide, the conductivity of the defect is simply e.g. • But for a component, like oxide ions in an oxide, conductivity can be expressed in terms of the component or the defect • Components need defects to move, and defects need components to move

  27. Exercise • Which is bigger? Cd or Cc? • Which is bigger: ud or uc? • Which is faster? The component atoms or the defects?

  28. In order to understand, analyse, and affect the conductivity in crystalline solids, we need to understand defect concentrations Introductory on defect chemistry

  29. Briefhistoryofdefects • Earlychemistryhadnoconceptof stoichiometry or structure. • The findingthat compounds generallycontained elements in ratiosofsmallintegernumberswas a greatbreakthrough! H2O CO2 NaCl CaCl2 NiO • Understandingthatexternalgeometryoftenreflectedatomicstructure. • Perfectnessruled. Variable composition (non-stoichiometry) wasout. • However, variable composition in some intermetallic compounds became indisputable and in the end forcedre-acceptanceofnon-stoichiometry. • But real understandingofdefectchemistryof compounds mainlycameabout from the 1930s and onwards, attributable to Frenkel, Schottky, Wagner, Kröger…, manyofthemphysicists, and almost all German! Frenkel Schottky Wagner

  30. Notice the distortions of the lattice around defects The size of the defect may be taken to be bigger than the point defect itself Defects in an elemental solid (e.g. Si or Ni metal) Adapted from A. Almar-Næss: Metalliske materialer, Tapir, Oslo, 1991.

  31. Defects in an ionic solid compound

  32. Bonding • Bonding: Decrease in energy when redistributing atoms’ valence electrons in new molecular orbitals. • Three extreme and simplified models: • Covalent bonds: Share electrons equally with neighbours! • Strong, directional pairwise bonds. Forms molecules. Bonding orbitals filled. • Soft solids if van derWaals forces bond molecules. • Hard solids if bonds extend in 3 dimensions into macromolecules. • Examples: C (diamond), SiO2 (quartz), SiC, Si3N4 • Metallic bonds: Electron deficiency: Share with everyone! • Atoms packed as spheres in sea of electrons. Soft. • Only partially filled valence orbital bands. Conductors. • Ionic bonds: Anions take electrons from the cations! • Small positive cations and large negative anions both happy with full outer shells. • Solid formed with electrostatic forces by packing + and – charges. Lattice energy.

  33. Formal oxidation number • Bonds in compounds are not ionic in the sense that all valence electrons are not entirely shifted to the anion. • But if the bonding is broken – as when something, like a defect, moves – the electrons have to stay or go. Electrons can’t split in half. • And mostly they go with the anion - the most electronegative atom. • That is why the ionic model is useful in defect chemistry and transport • And it is why it is very useful to know and apply the rules of formal oxidation number, the number of charges an ion gets when the valence electrons have to make the choice

  34. Bonding – some important things to note • Metallic bonding (share of electrons) and ionic bonding (packing of charged spheres) only have meaning in condensed phases. • In most solids, any one model is only an approximation: • Many covalent bonds are polar, and give some ionic character or hydrogen bonding. • Both metallic and especially ionic compounds have covalent contributions • In defect chemistry, we will still use the ionic model extensively, even for compounds with little degree of ionicity. • It works! • …and we may understand why.

  35. Formal oxidation number rules • Fluorine (F) has formal oxidation number -1 (fluoride) in all compounds. • Oxygen (O) has formal oxidation number -2 (oxide) , -1 (peroxide) or -1/2 (superoxide), except in a bond with F. • Hydrogen (H) has oxidation number +1 (proton) or -1 (hydride). • All other oxidation numbers follow based on magnitude of electronegativity (see chart) and preference for filling or emptying outer shell (given mostly by group of the periodic table).

  36. Point defects

  37. We will now start to consider defects as chemical entities We need a notation for defects. Many notations have been in use. In modern defect chemistry, we use Kröger-Vink notation (after Kröger and Vink). It describes any entity in a structure; defects and “perfects”. The notation tells us Whatthe entity is, as the main symbol (A) Chemical symbol or v (for vacancy) Wherethe entity is, as subscript (S) Chemical symbol of the normal occupant of the site or i for interstitial (normally empty) position Its charge, real or effective, as superscript (C) +, -, or 0 for real charges or ., /, or x for effective positive, negative, or no charge Note: The use of effective charge is preferred and one of the key points in defect chemistry. We will learn what it is in the following slides Kröger-Vink notation

  38. The effective charge is defined as the charge an entity in a site has relative to (i.e. minus) the charge the same site would have had in the ideal structure. Example: An oxide ion O2- in an interstitial site (i) Real charge of defect: -2 Real charge of interstitial (empty) site in ideal structure: 0 Effective charge: -2 – 0 = -2 Effective charge

  39. Example: An oxide ion vacancy Real charge of defect (vacancy = nothing): 0 Real charge of oxide ion O2- in ideal structure: -2 Effective charge: 0 – (-2) = +2 Example: A zirconium ion vacancy, e.g. in ZrO2 Real charge of defect: 0 Real charge of zirconium ion Zr4+ in ideal structure: +4 Effective charge: 0 – 4 = -4 Effective charge – more examples

  40. Dopants and impurities Y3+ substituting Zr4+ in ZrO2 Li+ substituting Ni2+ in NiO Li+ interstitials in e.g. NiO Electronic defects Defect electrons in conduction band Electron holes in valence band Kröger-Vink notation – more examples

  41. Cations, e.g. Mg2+ on normal Mg2+ sites in MgO Anions, e.g. O2- on normal site in any oxide Empty interstitial site Kröger-Vink notation – also for elements of the ideal structure (constituents)

  42. Silicon atom in silicon Boron atom (acceptor) in Si Boron in Si ionised to B- Phosphorous atom (donor) in Si Phosphorous in Si ionised to P+ Kröger-Vink notation of dopants in elemental semiconductors, e.g. Si

  43. Protonic defects • Hydrogen ions, protons H+ , are naked nuclei, so small that they can not escape entrapment inside the electron cloud of other atoms or ions • In oxidic environments, they will thus always be bonded to oxide ions –O-H • They can not substitute other cations • In oxides, they will be defects that are interstitial, but the interstitial position is not a normal one; it is inside an oxide ion. • With this understanding, the notation of interstitial proton and substitutional hydroxide ion are equivalent.

  44. A few tips: • Defects and charges are done seemingly a little different in elemental semiconductors and ionic solids • The donor and acceptor dopants are by tradition entered in doping reactions neutral in the former and effectively charged (ionised to their preferred valency) in the latter. Don’t let it confuse or disencourage you. • Physicists use + and – for effective and real charges alike, and actually don’t differentiate them much. Don’t let physicists confuse or disencourage you , and be kind with them . • Don’t mix real and effective charges in one reaction equation or electroneutrality consideration. • Use effective charges only in defect chemistry, which can only refer to one single phase. • Use real charges in all cases of exchange of charge between phases, like in electrochemistry. • I use v and i for vacancy and interstitial, while Kröger and Vink (and most of the rest still) use V and I.

  45. Electroneutrality

  46. Electroneutrality • One of the key points in defect chemistry is the ability to express electroneutrality in terms of the few defects and their effective charges and to skip the real charges of all the normal structural elements •  positive charges =  negative charges can be replaced by •  positive effective charges =  negative effective charges •  positive effective charges -  negative effective charges = 0

  47. The number of charges is counted over a volume element, and so we use the concentration of the defect species s multiplied with the number of charges z per defect Example, oxide MO with oxygen vacancies, acceptor dopants, and defect electrons: If electrons dominate over acceptors, we can simplify: Note: These are not chemical reactions, they are mathematical relations and must be read as that. For instance, in the above: Are there two vacancies for each electron or vice versa? Electroneutrality

  48. Examples of some important defect chemical reactions

  49. Stoichiometric compounds – intrinsic disorders Disorders that do not exchange mass with the surroundings, and thus do not affect the stoichiometry of the compound.

  50. Schottky disorder in MO M2+ new structural unit O2- or, equivalently: