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Natural Sciences Tripos Part IA MATERIALS SCIENCE Course F: Materials Under Extreme Conditions Dr Jess Gwynne Easter Term 2013-14 IA Name............................. College.......................... FH1 Course F: Materials under Extreme Conditions FH1 INTRODUCTION So far this year, you have had lecture courses about the atomic structure and microstructure of materials, device materials, mechanical properties, and biomaterials. In this course, we will explore a number of aspects of materials and their performance under extreme conditions. We will begin by considering the effect of high pressure on the structures of materials. We will then investigate materials at high temperatures, including melting and creep resistance (which is the resistance of a material to shape change under the combined effect of stress and temperature) and we will cover the superalloys used in the hottest part of jet engines. We will then look at the effect of radiation (in particular neutron radiation) on the structure and properties of materials and we will finish the course with a short section about life under extreme conditions. The aims of this course are to introduce you to new concepts and materials, but also to revise and build on material covered in the previous courses. Additional Resources Since this course builds on the earlier courses, and explicitly incorporates elements of revision, the books and web resources for earlier courses remain relevant. Some resources of particular relevance for this course are as follows: Web resources – DoITPoMS TLPs: Creep Deformation of Metals: http://www.doitpoms.ac.uk/tlplib/creep/links.php Materials for Nuclear Power Generation: http://www.doitpoms.ac.uk/tlplib/nuclear_materials/index.php Useful books: M.F. Ashby & D.R.H. Jones: “Engineering Materials Parts 1 and 2” D.A. Porter, K.E. Easterling & M.Y. Sherif, “Phase Transformations in Metals and Alloys” K.F. Kelton & A.L. Greer, “Nucleation in Condensed Matter” R.C. Reed, “The Superalloys: Fundamentals and Applications” K.L. Murty & I. Charit, “An Introduction to Nuclear Materials” FH2 Course F: Materials under Extreme Conditions FH2 Contents 1. Pressure 3 1.1 Definition; scale and units 3 1.2 Free energy (some revision from course C) 4 1.3 Pressure as a thermodynamic variable 5 1.4 Pressure-temperature phase boundaries: the Clausius-Clapeyron equation 6 1.5 Experimental determination of P-T phase diagrams 8 1.6 Calculation of P-T phase diagrams 10 1.7 What can we expect at high pressure? 11 1.8 Reconstructive phase transitions 12 2. Temperature 16 2.1 Melting 16 2.2 Mechanical performance at high temperature: Creep 21 2.3 Superalloys for jet engines 26 2.4 Thermal barrier coatings 34 2.5 Ice 37 3. Radiation damage 41 3.1 Introduction 41 3.2 The displacement cascade 42 3.3 Damage rates 43 3.4 Principal types of damage 44 4. Life under extreme conditions 47 4.1 Extremophiles 47 4.2 Tardigrades 48 4.3 Applications of extremophiles 49 Glossary 52 Abbreviations 55 Symbols, quantities and units 56 FH3 Course F: Materials under Extreme Conditions FH3 1. Pressure The role of temperature in phase transformations and the development of microstructure was covered in course C. Temperature affects the kinetics of a transformation (typically occurring faster at higher temperatures) and is also a thermodynamic variable. Likewise, pressure affects both the kinetics (typically slower at higher pressures) and the thermodynamics of a transformation, the latter being our focus in this section. Pressure-induced transformations can be exploited for materials synthesis and are of interest in a wide range of other contexts, notably geology. 1.1 Definition; scale and units The pressure of a gas is defined in terms of the force acting per unit area. In a solid, it is possible to have different forces acting on different surfaces, giving complicated stress states. Any such state, however, can be decomposed into components, one of which is the hydrostatic pressure: this is isotropic, with the same force per unit area acting normal to any surface. At zero temperature, the pressure P can be defined as the change in internal energy dU due to a change in volume dV: d d U P V Note that the negative sign arises because application of a positive pressure reduces the volume. The SI unit of pressure is the pascal (1 Pa 1 N m -2 ). Standard atmospheric pressure (1 atm) is 101325 Pa ( 1.01325 bar), i.e. approximately 10 5 Pa. Some other values: under a stiletto heel ~ 7 106 Pa 7 MPa in the deepest ocean trench ~ 10 8 Pa 100 MPa at the centre of the Earth ~ 3.8 1011 Pa 380 GPa maximum steady pressure in experiment ~ 5.6 1011 Pa 560 GPa at the centre of Saturn ~ 10 12 Pa 1 TPa in pulsed-laser experiments ~ 10 16 Pa 10 PPa at the centre of the Sun ~2.5 1016 Pa 25 PPa Note that we can also have negative pressures (as in tensile stress, but isotropic). FH4 Course F: Materials under Extreme Conditions FH4 1.2 Free energy (some revision from course C) The Gibbs free energy G plays a central role in the interpretation of phase transformations: G H TS where H is the enthalpy, T is the temperature and S is the entropy. Usually the extensive variables (G, H, S) are expressed per mole of formula units. The stable phase at any pressure or temperature is that with the lowest free energy. It is often useful to formulate the thermodynamic functions in terms of differentials: TSSTPVqTSSTHG dddδdddd where q is the heat supplied to the system, V is the volume and P is the pressure. From the second law of thermodynamics (CH16), for reversible changes: STq dδ which gives the standard differential form of the Gibbs free energy: TSPVG ddd 1.2.1 Phase transformations at constant pressure Phase changes as a result of changing temperature (at constant pressure) were considered in detail in Course C. From the differential form of G, it follows that at constant pressure (dP = 0): S T G P At low temperatures the entropy tends to zero, so the slope of the free energy curve must be zero at zero temperature. The slope is negative otherwise (i.e. positive entropy), and is increasingly negative at higher temperature, giving the characteristic form of the G curves. In the example below, the α phase has a lower enthalpy at zero temperature and hence is the stable phase at low temperatures. The β phase has a higher entropy at all temperatures (hence the slope of G is greater), and at a certain temperature the two curves cross. This defines the temperature of the phase transition. The phase of higher entropy is favoured by higher temperature. FH5 Course F: Materials under Extreme Conditions FH5 1.3 Pressure as a thermodynamic variable We can now extend the treatment in course C by consideringthe effects of changing the pressure as the temperature is held constant (dT = 0). From the differential form of G: V P G T In the example below, at low pressures the β phase has the lower free energy and is the stable phase. On increasing the pressure, the free energy of the phase with the higher volume increases faster. If the volume of the β phase is higher than that of the α phase, increasing the pressure eventually causes the free energy of the β phase to rise above that of the α phase, and above this pressure the α phase is the stable phase. The phase of lower volume is favoured by higher pressure. F re e en er g y Temperature Transition temperature α β F re e en er g y Pressure Transition pressure α β FH6 Course F: Materials under Extreme Conditions FH6 1.3.1 Pressure-temperature phase diagrams For a given phase, the variation of G with T and P is represented in a 3D plot by a curved plane. The G planes for two phases intersect on a line. The projection of that line onto the P−T plane gives the phase boundary between the phases on the pressure-temperature phase diagram. Such boundaries are approximately straight, as discussed in section 1.4. 1.4 Pressure-temperature phase boundaries: the Clausius-Clapeyron equation Consider the phase boundary between the and phases of a material: At all points along the phase-boundary line, the two phases are in equilibrium, and they therefore have the same free energy: Gα = Gβ. We can use the differential form of the free energy (giving the infinitesimal changes in G that arise from infinitesimal changes in T or P): d d d G V P S T P re ss ur e, P Temperature, T α β P re ss ur e, P Temperature, T α β Gα=Gβ dP dT FH7 Course F: Materials under Extreme Conditions FH7 For a small step along the phase boundary, given by dT and dP in the figure above, we have: TSPVG ddd ααα TSPVG ddd βββ TSPVG ddd The fact that dGα = dGβ along the phase boundary implies that 0d G , giving the final result: d Δ d Δ P S T V This is known as the Clausius–Clapeyron equation (sometimes shortened to the Clapeyron equation). It relates the slope of the phase boundary simply to the differences in entropy and volume of the two phases. Since the crystalline solids in a given system have similar specific heat capacities and compressibilities, S and V are to reasonable approximation independent of temperature and pressure. In that case, the phase boundary is a straight line, which is the case for many phase transformations. To predict the equation of a phase boundary we need to know one point on the phase boundary and values for ΔS and ΔV. In analytical treatments, we assume throughout that ΔS and ΔV are independent of T and P. FH8 Course F: Materials under Extreme Conditions FH8 1.5 Experimental determination of P-T phase diagrams The usual method of determining a phase diagram is to identify the stability fields of different phases in samples at a variety of temperatures and pressures. There are two ways of doing this: One is to hold a sample under a given temperature and pressure until it has equilibrated, and then to identify the phase in situ. The other way is to equilibrate the sample at a given temperature and pressure, quench it to room temperature, let the pressure down to ambient level, and then identify the phase at ambient temperature and pressure. Since reconstructive transformations (see section 1.8) are often slow, the quench preserves the structure obtained under the P−T conditions of the anneal. This approach cannot be applied for kinetically fast transformations, e.g. for displacive transitions and many order-disorder transitions. Even for reconstructive transitions, the degree to which they can be prevented by a quench can be open to doubt. High pressures and temperatures can be obtained by a variety of methods that vary widely in the conditions that can be attained, the sample size that can be processed, and the ease with which crucial property and structure measurements can be made in situ. 1.5.1 Piston-and-cylinder devices The first high-pressure devices used simple piston arrangements. The piston is pushed into the cylinder by an external press. The materials of which the press is constructed determine how much of the applied force can be translated into pressure on the sample. Heating of the sample is straightforward. 1.5.2 Opposed-anvil devices Anvils can be used to concentrate the force onto a small area, effectively magnifying the pressure. The gasket applies external constraint, avoiding extrusion of the sample from the sides. A good gasket material should be able to flow without fracture. A belt ring supports the gasket. Applied force Sample Sample Gasket Supporting belt FH9 Course F: Materials under Extreme Conditions FH9 This type of device can be used with diffraction equipment at a neutron or synchrotron X-ray source, and heating can be achieved by insertion of a heating element such as graphite. This type of device was used in the first synthesis of diamond (see section 1.8.3). 1.5.3 Multi-anvil devices In a multi-anvil press, the sample is squeezed within an arrangement of several truncated tungsten carbide or sintered diamond anvils, and then pressed in a large loading frame with a resistance heater incorporated in the sample assembly. Relatively large sample sizes can be used (up to 100 mg, depending on pressure) and good control of temperature and pressure can be achieved. However, it is difficult to observe samples in situ. Modern devices typically use 4, 6 or 8 anvils. 1.5.4 Diamond-anvil cell In a diamond-anvil cell, the sample is squeezed between opposed diamonds and heated with an infra-red laser focused on the sample for high temperatures, or an external heater for moderate temperatures. Sample sizes are limited by the size of the diamonds and are typically less than 50 mg. It is difficult to calibrate exact temperatures, but these can be very high. It is possible to perform in situ measurements such as X-ray diffraction and spectroscopy. 1.5.5 Pulsed-laser implosion Facilities such as the National Ignition Facility (USA, with 192 laser beams) or Orion (UK, 12 laser beams) are capable, with pulsed beams for very short times, of creating temperatures and pressures (> 1 PPa) similar to those in the cores of stars and giant planets. Achieving nuclear fusion in the laboratory is at the heart of the studies using such facilities. Tungsten carbide anvil Gasket Sample assembly 32 mm Gasket FH10 Course F: Materials under Extreme Conditions FH10 1.6 Calculation of P-T phase diagrams In many cases it may not be possible to determine phase diagrams by direct experiment. For example, it may not be possible to reach the necessary pressures and/or temperatures. In such cases it may be necessary to extrapolate from thermodynamic measurements made under not- so-extreme conditions. The Clapeyron equation is then very useful for calculating the equilibrium boundary between two phases. ΔV can be measured for the two phases at room temperature using X-ray diffraction. The experimentaldetermination of ΔS is not so straightforward, but it can be achieved by two methods: One approach is to determine S directly from calorimetric measurements of the enthalpy change (latent heat) for the transition at its equilibrium temperature eqT , using: eqT H S Alternatively, the absolute entropy of each phase can be determined by measuring the heat capacity from 0 K up to the required temperature 1T , and then integrating. Since T S TC d d P we have: i i T T H T T C TS d 1 0 P 1 , taking account of the latent heats iH of any transitions. (According to the third law of thermodynamics, K 0TS is zero.) Experimental measurements and thermodynamic analysis are usually supported with computer modelling. With modern computational methods, it is now possible to calculate phase properties sufficiently well to permit prediction of P-T phase diagrams. FH11 Course F: Materials under Extreme Conditions FH11 1.7 What can we expect at high pressure? At high pressure, lower volumes can be achieved by higher packing density, whether of atoms/ions, or of coordination polyhedra. Pressure may also force changes in local bonding configuration, or in the nature of the bonding (e.g. graphite-diamond). On pushing molecules together, the point must be reached where the distances between ‘non- bonded’ atoms are very similar to the distances between atoms within the molecules themselves; this provokes a loss of molecular identity as intermolecular electrons are delocalised between molecules, either locally (forming polymers, e.g. polymeric CO and CO2 under high pressure), or completely (forming metals). There is particular interest in forming metallic states. For example, the crystal structure of solid iodine at ambient pressure has the I2 molecules packed in a herringbone pattern. However, under pressure, the molecules dissociate and the new phase is metallic. Metallisation has even been achieved for hydrogen, at pressures exceeding 250 GPa (it has the hcp structure). Setting aside such extreme examples, the application of more modest pressures has proved to be exceptionally useful in generating a wide variety of novel structures with potentially exploitable properties (mechanical and electronic). These include: artificial diamond, cubic BN, and other super-hard materials new superconductors (clathrates, nitrides etc) new organometallic compounds nitride semiconductors thermoelectrics. FH12 Course F: Materials under Extreme Conditions FH12 1.8 Reconstructive phase transitions Many phase transitions that occur under pressure are between two structures that are not closely related. Such transitions are reconstructive and are in contrast to the displacive phase transitions met in Course B (BH29). Because the structures of the two phases involved are dissimilar, the transition involves breaking and re-forming of bonds. The phase transition is discontinuous and there is a sharp boundary between the phases during the transition. Reconstructive transitions are thermally activated, and it is possible for one phase to remain as a metastable state even under P−T conditions where the other phase should be stable. The metastable state of diamond at ambient pressure and temperature, where graphite is the thermodynamically stable phase, provides a good example. Reconstructive transitions require nucleation and growth of the new phase; many of the concepts used to describe precipitation (Course C) apply in this case also (coherence, TTT diagrams, supercooling for nucleation, preferential sites for nucleation such as grain boundaries and triple lines, diffusion for growth). The kinetics of reconstructive phase transitions are important in analysing many pressure- induced effects. 1.8.1 NaCl-MgO at high pressures At ambient pressure both NaCl and MgO adopt the rocksalt f.c.c. structure (for which NaCl of course is the classic example). In this structure, each ion has 6 nearest neighbours of the opposite type. However, at higher pressures, both materials adopt the cubic P CsCl structure, in which there is a denser packing with each ion having 8 nearest neighbours of the opposite type. FH13 Course F: Materials under Extreme Conditions FH13 1.8.2 The reconstructive transformation in Mg2SiO4 At ambient pressure, rocks are brittle, which is consistent with occurrence of earthquakes. However, some earthquakes originate deep in the Earth’s mantle where the high temperature and pressure mean that the rock flows plastically rather than failing in a brittle manner. Therefore, these deep-focus earthquakes cannot be caused by brittle fracture of the rocks, and are instead likely to be caused by a pressure-induced phase transition. The Earth is composed of distinct layers of different materials and densities. The inner core consists of an iron-rich solid phase, the outer core consists of an iron-rich liquid phase, and the mantle layers consist of various silicates, mainly (Mg0.9Fe0.1)2SiO4. In the uppermost layer, at lowest pressures, olivine is the stable phase. However, it undergoes a reconstructive phase transformation to the spinel phase as the pressure is raised (at about 400 km depth in the Earth). Each of these phases (or polymorphs) has a structure composed of SiO4 tetrahedra and MgO6 octahedra. In both structures, the Si cations are in tetrahedral sites, and the Mg cations are in octahedral sites. In olivine (below left, viewed down [100]), the oxygen atoms are in an approximately hcp arrangement, and the crystal structure is orthorhombic. In spinel (below right, viewed down [001]), the oxygen atoms are in an approximately ccp arrangement and the crystal lattice is cubic F. Note that Mg atoms are shown as circles and SiO4 tetrahedra are shaded. The large kinetic barrier to the transformation from olivine to spinel means that olivine exists metastably far beyond its equilibrium range, finally transforming to spinel at depths greater than 600 km, rather than in the range 300-400 km. A significant implosion shock results from the volume contraction of 8%, which causes the deep-focus earthquakes. P re ss u re ( G P a ) at 1000 C FH14 Course F: Materials under Extreme Conditions FH14 1.8.3 The graphite-diamond transformation Diamond is thermodynamically metastable under ambient conditions, but there is no risk of it transforming to the stable polymorph graphite (“diamonds are forever”). Transformation from diamond to graphite is extremely sluggish because a complete reconstruction of the bonding is required (sp 3 in diamond, sp 2 in graphite) and the activation energy is therefore very high. This sluggishness applies equally, of course, to the more desirable transformation from graphite to diamond. In the upper mantle, the temperature-pressure profile (the geothermal gradient) is such that diamond becomes thermodynamically stable at sufficient depth and natural diamonds form over millions of years at a depth of ~300 km. They are found in the necks of extinct volcanoes where they have been brought nearer to the surface (and also at meteorite impact sites). The most famous site is the Kimberley “big hole” in South Africa, which has yielded around 14.5 million carats of diamonds. At this site,deep-Earth materials were thrust upwards sufficiently quickly that the diamonds did not revert to graphite. On the P−T phase diagram for carbon, the equilibrium boundary between graphite and diamond is extremely difficult to determine directly, because the transformation (in either direction) is so sluggish. However, the boundary can be readily calculated from measured quantities such as heats of combustion or of solution. There has long been an interest in the production of artificial diamonds. This first achieved commercial success in 1954-5 with the “high-pressure high-temperature” (HPHT) process. This uses a liquid metallic solvent (Ni, Co, Fe) at ~ 5 GPa, ~ 1500°C into which graphite dissolves, and from which diamond precipitates (possibly on natural diamonds used as seeds). geothermal gradient FH15 Course F: Materials under Extreme Conditions FH15 Mostly small (dis)coloured stones are produced, suitable for most uses except gemstones. Nitrogen impurity, for example, accelerates diamond growth, but gives a yellow/brown discolouration. However, since the 1970s, it has been possible to synthesise gem-quality stones. Similar methods can be used to synthesise other superhard materials. A good example is cubic boron nitride, the second hardest substance known. At ambient temperature and pressure, the stable form of BN is hexagonal and has a similar structure to graphite (below left), but the cubic phase has the sphalerite structure (below right), which is analogous to diamond. Cubic boron nitride is widely used as an abrasive and has the advantage over diamond that it is much more chemically inert. For example, it is insoluble in metals such as steels, whereas diamond is soluble and forms carbides (which can cause embrittlement). FH16 Course F: Materials under Extreme Conditions FH16 2. Temperature We have seen that crystal structures, particularly when not closely packed, can be rather susceptible to change under pressure. We will now explore the behaviour of solids as the kinetic energy of their atoms is changed. As the temperature is lowered from ambient values, there can be interesting and important effects on physical properties, for example the onset of superconductivity and the appearance of exotic types of magnetic ordering, but the structural effects on solids are limited. As the temperature is raised, there can be phase transitions to other crystal structures, but our initial focus will be the stability of the crystalline state itself. Some temperature values: lowest temperature achieved in a laboratory 0.1 nK cosmic microwave background (temperature in space) 2.7 K boiling temperature of nitrogen N2 (at atmospheric pressure) 77 K standard room temperature (25°C) 298.15 K blue Bunsen flame 1870 K calculated melting point of diamond at atmospheric pressure 3823 K surface of the sun 5800 K core of the sun 13.6 MK plasma in a Tokamak fusion reactor 0.5 GK 2.1 Melting 2.1.1 Asymmetry between freezing and melting In course C, we saw that when a liquid is cooled, there is a distinct barrier to nucleation of the crystal (CH49). As a result, the liquid may be significantly supercooled below its equilibrium freezing temperature before solidification occurs. Significant changes in behaviour can be achieved by initiating freezing by using heterogeneous nucleants (e.g. CH52−CH53 and EH51‒EH52). In marked contrast, common experience suggests that there is no similar nucleation barrier to melting. This clear asymmetry is of interest to analyse. FH17 Course F: Materials under Extreme Conditions FH17 2.1.2 Theories of melting Lindemann theory: The first attempt to predict the bulk melting point of crystalline materials was made in 1910 by Frederick Lindemann. He suggested that melting occurs when the average amplitude of the atomic vibrations reaches a critical fraction of the interatomic spacing – at this point, the atoms start to collide with their neighbours, making the structure mechanically unstable and initiating the melting process. Experimentally, that fraction seems to be 0.15 to 0.30. Lindemann’s simple model works reasonably well, but cannot explain why the structure of a solid breaks down within such a narrow temperature range. Born theory: Another theory of bulk melting was formulated by Max Born in 1939. He suggested that melting occurs when one of the elastic shear moduli of the crystal goes to zero. This would constitute a rigidity catastrophe or mechanical melting in which the entire crystal lattice collapses, making a continuous transition into the liquid state. Actual melting, however, is not uniform throughout the solid, but typically begins at the solid surface and progresses inward. At the melting/freezing temperature, the solid and the liquid coexist with a well-defined interface between them. Importantly, although shear moduli do decrease with increasing temperature, at the melting temperature the solid is still rigid with non-zero moduli. 2.1.3 Surface melting For most crystals, some form of surface melting can be found at temperatures significantly below the bulk melting temperature. This can be simply interpreted in terms of interfacial energies. It is usually the case that the solid-vapour interfacial energy exceeds the sum of the liquid-solid and liquid-vapour interfacial energies: sv ls lvγ γ γ (Here ls is the quantity simply labelled on CH49‒50.) In that case, the crystal is wetted by its own melt (i.e. the contact angle of the liquid on the solid surface is zero, CH52) and a thin layer of liquid should coat the solid even below Tm. This of course explains why there is no nucleation barrier for melting. Below Tm, the liquid layer must remain very thin because the bulk liquid is not thermodynamically stable, but its thickness diverges as Tm is approached on heating. FH18 Course F: Materials under Extreme Conditions FH18 2.1.4 Melting of small particles If the inequality above is satisfied, then any particle of a crystal would be coated by a thin layer of liquid if close enough to the macroscopic melting temperature. If we take a spherical particle of radius r, then the crystal-liquid interface between the particle and its surface liquid is analogous to the surface of a critical nucleus (CH49). The critical radius for stability of that nucleus r* is given by (CH50): ls ls V V 2 2 * Δ Δ Δ γ γ r G S T where VS is the entropy of freezing per unit volume (a negative quantity) and T is the supercooling (a positive quantity, mΔT T T ). Well below Tm, the crystal is of course stable. The critical radius r* below which the crystal hypothetically would melt is much less than the actual particle radius (the crystal is “postcritical” and would naturally grow if it could). As the temperature is raised, however, the supercooling T decreases, the driving free energy for crystallisation VG decreases, and correspondingly r* increases. When r* equals and then exceeds the actual radius of the particle, it is suddenly preferable for any liquid coating to grow into the particle: i.e. the particle melts. We predict that this melting occurs below the bulk equilibrium melting temperature at a supercooling T given (from rearranging the above equation) by: * 2 V ls rS T The supercoolingis therefore inversely proportional to the particle radius. Such depressions of the melting temperature are measurable and very significant for nanoparticles, as shown in the data below for particles of gold. It is evident that common phenomena such as melting can be radically altered in the nanoscale regime. Note that for bulk gold, Tm = 1338 K. FH19 Course F: Materials under Extreme Conditions FH19 2.1.5 Suppression of surface melting and attainment of superheating If surface melting could be suppressed, then it would be possible to test how much the bulk crystal could be superheated above its own melting temperature. This can be achieved by arranging that the interior of the crystal is hotter than its surface, for example by focusing radiation inside a sample. Internal melting was first observed and analysed by Tyndall (1858) who noted the appearance of “flower-shaped figures” in Alpine ice exposed to sunlight. These dendrites of water show the six-fold symmetry of the ice within which they form, and can take up essentially identical faceted shapes as ice crystals. Just as dendritic crystals can only form in a liquid with sufficient supercooling, the dendritic melting can occur only with sufficient superheating (in the example of ice shown this is 0.15 K). Surface melting can also be suppressed by coating the crystal with a material of higher melting point, i.e. by embedding in a solid matrix. Recent experiments have used extreme confinement within fullerene shells. The limit to the stability of the crystal appears to be the point at which the liquid manages to nucleate within the crystal, either homogeneously, or heterogeneously on crystal defects such as dislocations. As nucleation is a kinetic process, its onset can be delayed by faster heating (using methods such as shock-wave loading, intense laser irradiation and electrical pulse heating) at rates up to 10 12 K s -1 . Using these methods, large superheatings can be attained. These show that crystal lattices under normal melting conditions are in fact internally very stable — it’s just that they have a higher free energy than a neighbouring liquid. Simple theory FH20 Course F: Materials under Extreme Conditions FH20 The table below shows the maximum temperatures reached by crystalline solids in a range of experiments and the corresponding superheats and relative superheats: Material Melting temp. Tm (K) Maximum temp. Tmax (K) Superheat ΔT =Tmax−Tm (K) Relative superheat ΔT/Tm Bulk single crystals SiO2 (quartz) 1698 > 2148 > 450 > 0.27 Embedded nanoparticles and layers Ag (coated with Au) 1234 1259 25 0.02 Sn (in fullerene) 505 > 770 > 265 > 0.52 Sn (in Sn/Si multilayer) 505 > 720 > 215 > 0.43 Pb (in Al matrix) 601 673 72 0.12 Ultra-fast heating (~10 12 K s −1 ): laser irradiation H2O (ice) 273 330 57 0.21 Al 933 1300 367 0.39 GaAs 1511 2061 550 0.36 FH21 Course F: Materials under Extreme Conditions FH21 2.2 Mechanical performance at high temperature: Creep In many engineering applications, components need to maintain their strength and their shape over long times at high temperature. To preserve shape, it might be thought sufficient to ensure that the applied stress stays below the (temperature-dependent) yield stress of the component material, but it is found that materials do show permanent shape changes at stresses well below their yield stress. This is creep, more evident at higher temperatures and longer times. 2.2.1 Creep: basic characteristics Creep is defined as time-dependent permanent deformation (i.e. plastic, not elastic) of a material under the action of a stress applied, the magnitude of which is less than the macroscopic yield stress y . The creep rate depends on: the material the applied stress the temperature: standard creep behaviour is seen at elevated temperatures: T > 0.3 mT for pure metals T > 0.4 mT for alloys and ceramics For macroscopic samples, creep shows three regimes: The primary and tertiary stages of creep are often quite short. We focus on secondary or steady-state creep, in which the strain rate is approximately constant and is given by an equation of the form: nA t d d where is the strain rate, σ is the stress, A is a constant, and n is the stress exponent, which reveals two regimes: FH22 Course F: Materials under Extreme Conditions FH22 Dislocation (power-law) creep is seen at high stress, n ≈ 3−10, and is analysed in terms of dislocation motion. Diffusion (linear, viscous) creep is seen at low stress, n ≈ 1, and is analysed in terms of atomic diffusion. 2.2.2 Dislocation (power-law) creep So far we have met dislocation motion in the form of glide on slip planes, which occurs on application of an applied stress. Obstacles (precipitate particles, tangles of other dislocations, etc.) on the slip plane may block dislocation glide and contribute to the observed yield strength. If dislocations could migrate onto a different slip plane they could move past obstacles and in this way creep could occur below the yield stress. The key event is this “climb”, but the sample’s deformation is due entirely to the subsequent glide. The process of migration to a different slip plane is climb, a process distinct from glide. Unlike glide, climb occurs entirely by the diffusive transport of atoms. The process is most readily visualised for edge dislocations, for which the dislocation line is effectively the end of an extra half-plane of atoms (although note that screw and mixed dislocations do also show climb). Removal of atoms from, or their addition to, the dislocation line itself clearly moves the line to a different slip plane. The dislocation line marks the location of the dislocation core, which is acting as a source or sink for atoms (which of course diffuse by exchanging with vacancies): FH23 Course F: Materials under Extreme Conditions FH23 Either positive or negative climb may assist a dislocation in avoiding obstacles. The climb is driven by local forces as the dislocations meet obstacles; these forces on the dislocations have components acting perpendicular to the slip plane. The climb can be such as to move a limited segment of dislocation line to a different slip plane. The climbed segment remains linked to the original dislocation by so-called jogs. The dominant path for diffusion of atoms to or from the dislocation core is dependent on temperature: Bulk diffusion dominates at higher temperatures, when there is enough mobility in the bulk lattice around the dislocations for the atoms to join or leave the dislocation core via the surrounding lattice. Core diffusion dominates at lower temperatures, when the only significant diffusion is along the dislocation cores themselves. That atomic diffusion might be involved in creep is revealed by the close link between the activation energies (and therefore the temperature dependences) of creep and diffusion. In this example, data for bulk lattice diffusion are compared with data for dislocation creep at high temperature. FH24 Course F: Materials under Extreme Conditions FH24 Taking the temperature dependence of the creeprate to derive entirely from that of the relevant diffusivity D, we can express the strain rate as: exp n n n Qε Aσ A σ D A σ RT where A, A and A are constants, Q is the activation energy for diffusion and R and T have their usual meanings. 2.2.3 Diffusion (linear, viscous) creep The diffusion of atoms, when biased in direction by an applied stress, enables grains to change shape, for example to elongate in response to tension. Again, there are two regimes, dependent on temperature: Nabarro-Herring creep is that seen at higher temperatures when diffusion within the bulk lattice is dominant. Coble creep is that seen at lower temperatures when diffusion is predominantly along grain boundaries. The creep strain rate in diffusion creep (for either of the above cases) must depend on the average grain diameter d of the polycrystalline material. We can express it as: 2 2 exp Dσ B σ Q ε B d d RT where B and B are constants, D is the relevant diffusivity, and Q is its activation energy. FH25 Course F: Materials under Extreme Conditions FH25 2.2.4 Summary of creep behaviour: Deformation-mechanism map As developed by Ashby, diagrams of stress (normalised by the shear modulus G) versus homologous temperature ( mTT ) are useful in permitting the display of regimes in which different deformation mechanisms dominate. This is a simplified map that shows the creep mechanisms discussed in this course. 2.2.5 Designing creep-resistant alloys To minimise creep rates, it would be desirable to have: a high-melting point system (since atomic diffusion relates to homologous temperature T/Tm) minimal dislocation motion at elevated temperatures stable precipitates (no coarsening) controlled grain size and grain orientations: - grain size: desirable to have large grains - grain boundaries (if present): should control orientation & pin them to prevent sliding. FH26 Course F: Materials under Extreme Conditions FH26 2.3 Superalloys for jet engines 2.3.1 Efficiency of an engine: the need for high temperatures The performance of a heat engine can be measured in terms of a thermodynamic cycle of its operating gas. The best known is the idealised Carnot cycle. This consists of two isothermal (constant temperature) stages and two adiabatic stages (in which the entropy is constant, as no heat is exchanged with the surroundings). There are two heat reservoirs, hot (T = TH) from which heat is extracted, and cold (T = TC) into which waste heat is lost. Stage 1: isothermal expansion of the gas at TH, with heat flowing in from the hot reservoir Stage 2: adiabatic expansion of the gas, during which it cools to TC Stage 3: isothermal compression at TC, with heat flowing out to the cold reservoir Stage 4: adiabatic compression of the gas, during which it heats back to TH. This is a cycle in pressure and volume of the gas, but it is most readily analysed on the T−S diagram. Bearing in mind that STq dδ , the total heat absorbed in stage 1 must be ABH SST , while the heat lost in stage 3 is ABC SST . The difference between these two quantities would appear to increase the internal energy of the system with every clockwise cycle, but the system in fact returns to the same internal energy because of the work done, which is therefore ABCH SSTT . The efficiency is H C ABH ABCH 1 inputheat total donework T T SST SSTT FH27 Course F: Materials under Extreme Conditions FH27 The cycle for a gas turbine looks a little different, but ideally, there are still four stages: Stage 1: Adiabatic compression of fresh air on entering the engine (S = constant) Stage 2: Heating in the combustion chambers (P = constant) Stage 3: Adiabatic expansion, with the turbine extracting work (S = constant) Stage 4: Dissipation of hot gases (P = constant). 2.3.2 The materials challenge A schematic diagram of a jet engine is shown below. (from Wikimedia commons) The blades at the hot end of an aeroengine operate under very challenging conditions, requiring strength, creep resistance, toughness and oxidation resistance. The temperature of the blade material may exceed 75% of its melting temperature. At 10,000 revolutions per minute, the blade tip velocity is 330 m s-1 (1200 km/h). The stresses are largely centrifugal and are nearly 200 MPa at the root of the blade. A typical lifetime is 3 years of use, equating to 5 million miles (200 Earth circumferences). FH28 Course F: Materials under Extreme Conditions FH28 The complete disc of ~100 blades extracts energy from the hot gas at a rate (power) of about 50 MW, i.e. each blade extracts ~500 kW, enough for >1000 homes at the average rate of household consumption (400 W). The graph below shows that the turbine entry temperature (TET) has risen dramatically over the years, by more than 700 K, using Rolls-Royce civil aeroengines as examples. Since the introduction of superalloys in the 1940s, the temperature at which turbine blade materials can operate (i.e. when they have adequate creep resistance) has risen by more than 300 K, but there has been a strong incentive to push operating temperatures even higher. In modern engines the TET exceeds (by > 400 K) the temperature at which the superalloy would have adequate creep resistance. The blades are kept cooler than the surrounding gas by passing cold air through them from the inside. This requires the casting of blades with complex internal channels, as shown on the right. Additionally, the blades are coated with a thin layer of a ceramic with a low thermal conductivity (a thermal barrier coating – see section 2.4). Obviously, these measures increase manufacturing costs. The need for materials with dramatically better temperature capabilities is very clear, but the search for such materials has proved very difficult. FH29 Course F: Materials under Extreme Conditions FH29 2.3.3 Possible materials Blades in an aeroengine need to be tough. With present technologies, ceramics are not sufficiently tough throughout the temperature range from start-up to operation, so for high- temperature blades, metallic alloys are the only option. We have already seen that all types of creep are related to atomic diffusion, and in general terms, the rates of diffusion and creep at a given temperature are lowered by choosing a material of higher melting temperature Tm. The present materials of choice for high- temperature aeroengine blades are alloys based on nickel (Tm = 1728 K). However, there are metals with much higher melting points, so why are they not used? Potential problems include: (i) Polymorphism: Blades cycle through wide temperature ranges and repeated changes of phase (e.g. bcc ↔ ccp in iron) would not be acceptable. (ii) Intrinsic diffusivity: Typical atomic diffusivities at a given homologous temperature vary with crystal structure. Of the simple metallic structures, the diffusivity at Tm is in the sequence ccp < hcp < bcc. Thus ccp metals are favoured. (iii) Brittleness: Some metals are intrinsically too brittle. (iv) High density: It is never desirable to increase the weightof aeroengine components, but it is especially bad to use a high-density material in rotating parts as centrifugal forces are thereby increased, making creep more difficult to resist. (v) Poor oxidation resistance is a problem for several metals. (vi) Cost: Even for a high-technology product such as a turbine blade, the cost of the main constituent metal may be an issue. Two metals that, because of high Tm values, might be considered attractive for high- temperature use are tungsten (Tm = 3660 K) and tantalum (Tm = 3253 K). They do not show polymorphism, but their structure is bcc, giving relatively high diffusion rates (at a given homologous temperature), and that they also suffer from every other problem in the above list. Nickel is ccp and this phase is very stable in the presence of alloying additions. It has no serious problem with any of the items in the above list, and is the base metal of choice. FH30 Course F: Materials under Extreme Conditions FH30 2.3.4 Nickel-based superalloys 2.3.4.1 Composition and microstructure With many decades of development, rather complex compositions have evolved, designed to improve strength, creep resistance, oxidation resistance, etc. As an example, one of the first generation of alloys designed for use in single-crystal blades (see section 2.3.4.2) was PWA1480, which consists of nickel as the base metal, plus the following alloying additions (in weight %): 10.0 Cr 5.0 Co 4.0 W 5.0 Al 1.5 Ti 12.0 Ta Nickel-based superalloys essentially consist of a dense dispersion of precipitates (often faceted) in a matrix, the so-called γ-γ (gamma/gamma prime) microstructure, as shown on the right. Gamma: the nickel-based ccp solid solution. Gamma prime: is a closely related phase based on an ordering of solute-atom sites. The archetype is Ni3Al. The AlNi3 structure has the Al atoms not randomly occupying Ni-atom sites (as would be true in a ccp solid solution), but instead located only at the corners of the unit cell: The unit cell: The γ unit cell: cubic F lattice, ccp structure 1 atom per lattice point On average, each lattice site has the overall alloy composition. Cubic P lattice 4 atoms (3 Ni + 1 Al) per lattice point The structure is fully ordered. There are no Al-Al nearest neighbours. 2 m FH31 Course F: Materials under Extreme Conditions FH31 In real superalloys, the Al sites are occupied also by Ti and Ta atoms, so γ can be represented as Ta Ti, Al,Ni3 . The solute atoms partition between the and γ phases, mildly affecting the lattice parameter of each. It is possible for the lattice parameters of the and γ phases to match very closely, in which case the γ-γ interface can be fully coherent (CH55). This is highly desirable, as fully coherent interfaces have very low interfacial energy, and therefore provide very low driving force for the detrimental coarsening of precipitates. 2.3.4.2 Single-crystal blades Analysis of creep (FH21−FH25) shows that grain boundaries can contribute to atomic diffusion, and their presence also degrades creep resistance in other ways. The detrimental influence of grain boundaries on creep life is minimised when they are parallel to the main tensile stress (i.e. parallel to the length of the blade). Directional solidification can give blades with grain boundaries aligned in this way. It is then a short step to control the solidification a little more and to make single-crystal blades: In this picture, solidification starts from the bottom, where many grains are formed, and proceeds through the liquid- filled mould towards the top. Growth of the solid through the helical path (pig-tail grain selector) leads to just one grain growing into the main blade cavity. This grain is oriented with the 100 preferred growth direction parallel to the blade length. The single-crystal nature of the blades is checked on the production line by back-reflection X-ray photography. FH32 Course F: Materials under Extreme Conditions FH32 2.3.4.3 Order hardening As noted above in section 2.3.4.1, superalloy compositions are selected so that the γ-γ interface is fully coherent. While this is desirable (in inhibiting coarsening), it means that the interfaces themselves offer no extra resistance to the passage of dislocations. However, the γ precipitates do have a strong hardening effect, so the hardening effect in superalloys is of particular interest to analyse. The Burgers vector of a dislocation must be a lattice vector, and is generally the shortest possible. In the ccp phase the slip systems are of the type 2 a 111011 . However, in the γ AlNi3 structure vectors of the type 2 a 011 are no longer lattice vectors. If a dislocation with such a Burgers vector were to glide through the γ phase, it would move Al atoms to Ni- atom sites and some Ni atoms to Al-atom sites, and create some Al-Al nearest neighbours (which are forbidden in the ordered γ structure). The slip plane would be a boundary between two γ structures that are out of step with each other. This is an anti-phase boundary (APB), shown schematically here. In Ni3Al, APBs have rather high energies of ~ 0.1 J m -2 . In γ , the shortest lattice vectors are 100a , but the phase in fact deforms as compatibly as possible with the deformation of , according to the slip systems 111011a . In this way, the same dislocations mediate the deformation of both phases. phase: γ phase: b = 2 a 011 b = 011a FH33 Course F: Materials under Extreme Conditions FH33 A dislocation with a b = 2 a 011 entering a γ precipitate must create an APB. In consequence, it feels a strong resistance (drag). The passage of a second dislocation with the same Burgers vector restores the undefected γ structure (i.e. removes the APB). Accordingly the dislocations move in pairs, the first meeting great resistance, and the second not, giving rather characteristic shapes of the dislocation lines as shown here. The pair of dislocations has an effective Burgers vector 011a and constitutes a perfect dislocation for γ . This is called a superdislocation; each individual dislocation is a superpartial. As the pair of dislocations moves through γ , the APB exists only on the ribbon of slip plane between them. The energy dissipation and associated dislocation drag from creating APBs gives order hardening, and this is by far the dominant contribution to hardening in superalloys. FH34 Course F: Materials under Extreme Conditions FH34 2.4 Thermal barrier coatings Despite the increased hardness and creep-resistance of nickel-based superalloys, turbine blades require additional protection from the high temperatures, because (as mentioned in section 2.3.2), the temperatures inside jet engines exceed the temperature at which the superalloy would have sufficient creep resistance, by several hundred Kelvin. Cold air is passed through internal channels within the blade, and they are additionally protected from the high temperatures by thermal barrier coatings. The main requirements for a thermal barrier coating are: a low thermal conductivity a high melting point and maximum service temperature adequate strength The main component in a thermal barrier coating is a layer of the ceramic zirconia, ZrO2 (in the form of yttria-stabilised zirconia). As seen in the materials selection maps below, the technical ceramics are the materials with the best combination of strength and maximum service temperature, and of these, the material with by far the lowest thermal conductivity is zirconia. Selection map showing yield strength against maximum service temperature. Technical ceramics are in the top right corner. ZrO2 FH35 Course F: Materials under Extreme Conditions FH35 Selection map showing thermal conductivity against thermal diffusivity. Most technical ceramics are in the top right corner, but zirconia is significantly lower. However, in order to make a good thermal barrier coating, the ceramic needs to adhere well to the turbine blade. The blade surface must therefore first be coated with a thin bond coat, which is an alloy of Ni-Cr-Al-Y and essentially acts as a glue between the blade and ceramic coating. One potential problem is that oxygen diffuses readily through YSZ (see BH48), which would make the superalloy liable to undergo oxidation. To overcome this problem, a thin dense layer of alumina (which has a low oxygen mobility) is added between the bond coat and the zirconia. Another potential problem is that zirconia has a lower coefficient of thermal expansion than the nickel-based superalloy from which the blades are manufactured, which would induce thermal stresses and cause cracking of the zirconia on heating and cooling. To overcome this, the ceramic layer is grown such that it has a columnar structure perpendicular to the surface of the blade. When the blade heats and expands, the columns are able to separate very slightly, but not enough for a significant amount of hot gas to penetrate to the surface of the blade. ZrO2 FH36 Course F: Materials under Extreme Conditions FH36 (From http://www.bren.ucsb.edu/facilities/MEIAF/images.html) Thermal barrier coatings therefore have a relatively complex 4-layer structure, as illustrated schematically below. (adapted from J. Mater. Chem., 2011, 21, 1447-1456) YSZ layer (250–500 μm) Dense alumina layer (3–10 μm) Bond coat (75–150 μm) Nickel-based superalloy FH37 Course F: Materials under Extreme Conditions FH37 2.5 Ice Ice covers a significant fraction of the Earth’s surface and plays a role in regulating climate. Very unusually for materials under normal conditions, ice is always at a temperature close to its melting point. Ice also has the unique feature that it remains profoundly brittle right up to its melting temperature, a property that can be explained in terms of its structure. Other materials that we think of as brittle, such as ceramics, are all a long way from their melting point: when these materials approach their melting point, they become ductile, but this is not the case for ice. 2.5.1 Structure, bonding and proton disorder The H2O molecule has a bond angle close to the tetrahedral angle of 109.47°. Hydrogen bonding to other water molecules is in a tetrahedral format, with each oxygen covalently bonded to two hydrogens in the same molecule and hydrogen-bonded to two further hydrogens in neighbouring molecules. The most common crystal structure of ice is Ih, which is stable under ambient conditions. This is a tetrahedrally linked framework of hexagonal symmetry, the arrangement of oxygens being equivalent to that of the Zn and S atoms in wurtzite (BH28). The water molecules remain intact, but at a given tetrahedral centre (i.e. O) there are up to six possible orientations of the molecule: The neighbouring orientations are related because the ice rules must be obeyed: there must be two hydrogens adjacent to each oxygen there is only one hydrogen per bond. hydrogen bonds FH38 Course F: Materials under Extreme Conditions FH38 Even with these constraints, the positions of the hydrogens are not determined throughout the structure. The limited degree of disorder (proton disorder) has a profound effect on the properties of ice Ih. Ice exhibits a number of phases, as illustrated in the pressure-temperature phase diagram below. All phases have a network of tetrahedrally coordinated oxygen atoms, sometimes with and sometimes without proton disorder. In high-pressure phases, the H atom may become equidistant from both O neighbours, blurring the distinction between water molecules. Tetrahedral coordination gives low packing densities. The highest pressure phases increase their density while keeping the 4-fold coordination by means of two interpenetrating networks. 2.5.2 Mechanical properties As previously mentioned, ice is brittle all the way up to its melting point (at normal strain rates). This behaviour arises because of the proton disorder described above. This diagram shows a layer of the ice Ih structure projected on to the (100) plane. The proton disorder disrupts the translational symmetry and greatly impedes dislocation motion. [001] [010] FH39 Course F: Materials under Extreme Conditions FH39 However, because temperatures are typically so close to the melting point, it is possible for ice to undergo creep (usually power-law creep). Large ice masses deform under their own weight, resulting in phenomena such as glacier flow, which has significantly shaped the Earth’s land surface. 2.5.3 Surface melting As noted earlier (in section 2.1.3), crystals can show some degree of surface melting even below the macroscopic melting temperature. We nearly always encounter ice in the extreme condition close to its melting point there is significant melting of the surface layers. Computer simulations have shown that this starts at about −33°C: the liquid-like layer is 12 nm thick at −24°C and 70 nm at −0.7°C. This surface melting can account for: the low coefficient of friction of ice (exploited, for example in skating) the high adhesion of ice surfaces the ease of compaction of ice (compared to a normal powder). When two ice surfaces touch (for example two ice cubes), the liquid-like layer between them solidifies. 2.5.4 Regelation The ice Ih to liquid phase boundary (unusually) has a negative slope, which can be explained using the Clausius-Clapeyron equation: d Δ d Δ P S T V Since ice is less dense than water, ΔV is negative for melting, whereas ΔS is positive (as usual). Therefore, as pressure increases, the melting point of the ice decreases. FH40 Course F: Materials under Extreme Conditions FH40 This effect is exploited in the phenomenon of regelation, in which a material melts under pressure but refreezes when the pressure is reduced. It can only occur in materials whose densities decrease when they melt (if the density increases, the slope of the phase boundary is positive, meaning that the melting point increases as pressure increases). Regelation can be clearly demonstrated in an experiment in which weights are hung from a thin wire looped over a cylinder of ice. The pressure exerted by the wire lowers the melting point of the ice, causing it to melt and the wire to pass through the ice. The ice abovethe wire then refreezes once the pressure is removed and eventually, the wire will have passed the whole way through the ice cylinder, leaving it intact. (Note that it is actually slightly more complicated than this because the wire will absorb heat from the room and conduct it through the wire, which also contributes to the melting of the ice) Apart from creep, regelation is another factor that contributes to the movement of glaciers. They can undergo basal sliding, in which the movement of a glacier is lubricated by the presence of liquid water created by the high pressure exerted by the weight of the glacier above it. FH41 Course F: Materials under Extreme Conditions FH41 3. Radiation Damage 3.1 Introduction Radiation damage refers to microscopic defects produced in materials due to irradiation, and results in changes to their physical, chemical and mechanical properties. Of course, many types of radiation are possible (using ion accelerators, for example), but here we will focus on neutrons. Nuclear fission produces fast neutrons with energies of approximately 1 MeV. In fusion, neutrons with energies as high as 14 MeV are produced. The main components of a fission reactor are: The fuel (usually uranium or uranium dioxide), which absorbs neutrons and undergoes fission, in which the nucleus splits into two smaller nuclei but also releases neutrons to keep the chain reaction going. The cladding (usually austenitic stainless steel, or a zirconium alloy), which surrounds the fuel, protecting it from corrosion and giving it structural integrity. Control rods, which absorb neutrons and can be raised or lowered to control the chain reaction (or lowered completely in an emergency to stop the reaction). The coolant, which removes heat generated during fission and is used to produce steam to drive turbines for electricity generation. There are many types of nuclear fission reactor, but the most common type is the Pressurised Water Reactor (PWR). Schematic of a Pressurised water reactor (from Wikimedia Commons) FH42 Course F: Materials under Extreme Conditions FH42 3.2 The displacement cascade Radiation damage in crystals has been widely studied because of its importance in structural components in and near the cores of nuclear reactors. The damage follows the sequence: 1. An energetic incident particle (such as a fast neutron) strikes an atom in the crystal 2. The transfer of kinetic energy to the atom is large enough to displace it from its position in the lattice and it becomes a primary knock-on atom, or PKA, leaving behind a vacant site 3. The PKA moves through the lattice, creating further knock-on atoms in a displacement cascade; the mean free path between displacement collisions depends on the energy of the knock-on atoms, but is typically in the range 1 nm to 1 m 4. The PKA and other knock-on atoms eventually come to rest as interstitial atoms Each knock-on event produces a pair of defects: a vacancy and an interstitial (a Frenkel pair). The above sequence of events occurs extremely quickly: in about 10 -11 s. In the following 10 -9 s, things settle down, with some recombination of vacancies and interstitials occurring, but the extent of this (energetically desirable) recombination is limited because the vacancies and interstitials diffuse away from each other. The initial mean free path between collisions is of the order of 1 cm for fast neutrons but decreases as energy is dissipated in successive collisions; the result is that displacement cascades are concentrated in volumes 1 to 10 nm in diameter. A displacement cascade is illustrated schematically in this image. There is a high density of vacancies in the core, with the surrounding material rich in interstitials. FH43 Course F: Materials under Extreme Conditions FH43 This atomistic simulation of copper illustrates the effect of an incident neutron of very high energy (e.g. from a fusion reactor). The displacement cascade is spread out and can be interpreted as a branching series of subcascades. grey: vacant lattice sites black: displaced atoms 3.3 Damage rates The displacement energy, Ed, is the minimum energy that must be transferred to a lattice atom in order for it to be displaced from its lattice site (typically about 25 eV). If the energy transferred by a knock-on atom to the struck lattice atom is less than the displacement energy, the lattice atom will not be dislodged from its lattice site. It will instead vibrate around an equilibrium position and the energy will be dissipated as heat. We begin with an example calculation to estimate how many atoms are involved in a displacement cascade. On collision, the maximum energy transferable from a neutron of energy En to a nucleus of atomic mass number A is ζEn, and the average energy transferred is ζEn/2, where: 2 4 1 A ζ A For a neutron hitting an 56 Fe nucleus, ζ = 0.069. Taking the neutron to have an energy of 1 MeV, the average energy transferred to an iron atom (the expected energy of the PKA, Ep) would be Ep = 3.45 10 4 eV. The average number of atoms displaced per PKA is Ep/2Ed, where Ed is the energy required to displace an atom from its lattice site. For -Fe, Ed ≈ 40 eV, so that the number of displaced atoms is 431. The accumulated damage in irradiated material can be characterised as the average number of displacements per atom (dpa). The rate of damage of course depends on the incident neutron FH44 Course F: Materials under Extreme Conditions FH44 flux, and also on the relevant collision cross-sections (which describe the probability of different nuclear reactions occurring). Typical damage rates (measured as displacements per atom per second, dpa s -1 ) range from 10 -9 dpa s -1 in thermal reactors to 10 -5 dpa s -1 in the first wall of proposed fusion reactors. Over the lifetime of a component in a nuclear fission reactor, each atom could be displaced as many as 100 times. Clearly such extreme conditions can have profound effects on the microstructure of the alloys involved. These effects include dissolution of precipitates, changes in their morphology, and appearance of non-equilibrium phases. Here, we will focus on the effects on the main crystal lattice. 3.4 Principal types of damage We have seen that each PKA generates excess populations of vacancies and interstitials in the displacement cascade. In principle, the vacancies and interstitials might recombine directly to restore the equilibrium structure, but they are too widely separated. Interstitial atoms have higher excess energies than vacancies and they are also more mobile. They quickly disappear at dislocations and grain boundaries acting as sinks. Dislocations act as sinks for interstitials through the process of negative climb (FH22), without any need for vacancy migration. As a result displacement cascades are left with an excess of vacancies. The effects on the structure of the irradiated solid depend on temperature, with dislocation loops forming at lower temperatures, and voids forming at higher temperatures. 3.4.1 Dislocation loops Dislocation loops can form at lower temperatures (T < 0.2 Tm, where Tm is the absolute melting temperature of the irradiated alloy). In a face-centred cubic metal (for example the austeniticstainless steel cladding of fuel rods), interstitial atoms can condense as monolayer discs between the close-packed {111} planes of the crystal, forming an interstitial loop. Vacancies likewise can condense as discs between {111} planes, forming a vacancy loop, and the lattice above and below the vacancy disc closes in. Both types of dislocation loop disrupt the ABCABC stacking sequence of the close-packed planes, resulting in a stacking fault. Interstitial loop Vacancy loop FH45 Course F: Materials under Extreme Conditions FH45 In these dislocation loops, the Burgers vector is normal to the planes and of magnitude equal to the interplanar spacing (± a/3<111>). The dislocation is sessile (unable to glide). The formation of vacancy-type and interstitial-type loops under irradiation gives an increase in dislocation density, analogous to that obtained on cold-working. However, as irradiation continues, a steady-state dislocation density is reached when the rate of damage equals the rate at which defects are annealed out (due to local heating of the material). The steady-state dislocation density depends on damage rate and temperature. Typical dislocation densities in austenitic stainless steels: Annealed: 1012 m-2 Cold-worked: 1015 to 1016 m-2 Irradiated: (6 ± 3) 1014 m-2 (at steady state) This figure shows dislocation density as a function of irradiation dose in annealed and cold-worked austenitic stainless steels, irradiated at 500°C. The irradiation drives the dislocation density to the same steady-state value, independent of the starting value. A cold-worked material can actually show a decrease in dislocation density on irradiation. 3.4.2 Voids Irradiation at higher temperatures (T > 0.2 Tm), leads to cavities or voids. Once voids are nucleated they grow easily; the interstitials formed in displacement cascades are absorbed mainly at dislocations and the vacancies mainly join the voids. Void nucleation and growth under irradiation have the feature, not often encountered in metallurgical precipitation, that the precipitating species (vacancies) are under continual production; without this, voids already produced would largely disappear on annealing. The formation of voids leads to swelling, which is the most studied type of radiation damage. In austenitic stainless steels, the steady-state swelling rate is ~1% per dpa. The maximum reported swelling under neutron irradiation is 88% (i.e. almost doubling the volume). FH46 Course F: Materials under Extreme Conditions FH46 These images show void swelling at different temperatures in an austenitic stainless steel at ~1.41027 neutrons/m2, equivalent to ~70 dpa. In each case, the total volume of the voids is approximately the same. However, at low temperatures, many small voids are seen, whereas at high temperatures, fewer larger voids are seen. This arises due to a balance of nucleation and growth (as seen in course C). From the first observations of void formation in 1967, it was recognised that this is a particularly important form of radiation damage, leading to swelling and distortion of irradiated components. It can cause hardening of irradiated alloys and associated embrittlement and loss of ductility. The development of voids on grain boundaries shortens creep life. This image shows swelling (~10% linear, 33% by volume) of a stainless steel cladding tube irradiated at 1.5×10 27 neutrons/m 2 , equivalent to ~75 dpa, at 510°C. Note that all relative proportions are preserved during swelling. 3.4.3 Structural changes on irradiation We have seen that in typical structural alloys, there are major microstructural effects of irradiation, but the crystal lattice itself is rather stable, continual repair processes counteracting damage rates. In contrast, some minerals containing radioactive U or Th, are amorphised by the internal bombardment resulting from decay processes. These metamict glassy minerals can show faceted forms inherited from their crystalline precursors, and may crystallise on heating. Whether damage or repair processes dominate is largely dependent on damage rate and temperature. FH47 Course F: Materials under Extreme Conditions FH47 4. Life under extreme conditions 4.1 Extremophiles Extremophiles are organisms that have adapted to be able to survive (and in fact thrive) in physically or chemically extreme conditions that would be detrimental to most life on Earth. Many extremophiles are simple single-cell organisms, but others are much more complex. For example, in course E, you learnt about several extremophiles: plants that can survive extremely dry conditions (by forming glasses rather than mineral crystals – EH49) fish that can survive very cold conditions because their blood plasma contains antifreeze proteins (EH50) frogs that can survive cold conditions because ice nucleating agents promote the formation of ice outside their cells rather than inside (EH50-51). There are many classes of extremophiles including: Acidophiles are adapted to life at pH 3 or below Alkaliphiles are adapted to life at pH 9 or above Thermophiles thrive at temperatures between 45°C and 122°C Psychrophiles survive at temperatures of -15°C or lower for long periods Halophiles require high concentrations of salt (> 0.2 M) for growth Piezophiles are adapted to life at high pressures (such as underground or deep in the ocean) Xerophiles can grow in extremely dry conditions Radioresistant extremophiles are resistant to high levels of ionising radiation (UV or nuclear radiation) Many extremophiles fall under more than one category and are termed polyextremophiles. For example, there are worms and shrimps that live in or near deep ocean thermal vents (where there are high temperatures, high pressures and extreme pH), and many types of bacteria thrive in geothermal areas and hot springs (where there are high temperatures and very low pH). FH48 Course F: Materials under Extreme Conditions FH48 4.2 Tardigrades Perhaps the most impressive example of a polyextremophile is the Tardigrade (from the Italian “Tardigrada”, meaning “slow stepper”), otherwise known as the waterbear (from their original German name “kleiner Wasserbär”). Tardigrades can reversibly suspend their metabolism, dehydrate and go into a state of crytobiosis which makes them able to survive: Temperatures from just above absolute zero, to well above the boiling point of water Pressures as low as the vacuum of outer space (hey are the first known animal to survive in outer space) and six times higher than those found in the deepest ocean trenches Ionising radiation at doses hundreds of times higher than the lethal does for a human Going without food or water for more than 10 years Drying out to the point where they contain less than 3% water Tardigrades have 8 legs and are typically about 0.5 mm long. There are over 1000 different species, and they are found all over the world, from the Himalayas to the deep sea, and from the polar regions to the equator). (from Wikipedia commons) (From www.nps.gov) FH49 Course F: Materials under Extreme Conditions FH49 4.3 Applications of extremophiles 4.3.1 Hydrogen peroxide removal: Thermus brockianus Hydrogen peroxide is used in industrial
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