Seminar o nm aterial enginering
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The document summarizes key information about three materials: aluminum oxide, silicon carbide, and diamond. It discusses their crystal structures, properties like hardness and thermal conductivity, common processing methods, and applications. Aluminum oxide is used as an abrasive and refractory material. Silicon carbide is very hard and used for abrasives, armor, and power electronics. Diamond is the hardest known material and used in drilling, cutting, and jewelry due to its optical properties.
Seminar o nm aterial enginering
- 1. SEMINAR ON MATERIAL ENGINEERING PRESENTED BY TUSHAR ANEYRAO ROLL NO:16 M.TECH. (CAD-CAM)
- 2. • Properties processing and application of: – Aluminium oxide – Silicon carbide – Diamond •
- 3. Aluminum oxide (Al2O3) • Aluminum oxide is an amphoteric oxide with the chemical formula Al2O3. It is commonly referred to as alumina (α-alumina), aloxide, or corundum in its crystalline form, as well as many other names, reflecting its widespread occurrence in nature and industry. • Its most significant use is in the production of aluminum metal, although it is also used as an abrasive owing to its hardness and as a refractory material owing to its high melting point. There is also a cubic γ-alumina with important technical applications
- 4. FIGURE: ALUMINIUM OXIDE (α-Al2O3) CRYSTAL STRUCTURE
- 5. PROPERTIES • Hard, wear-resistant • Excellent dielectric properties from DC to GHz frequencies • Resists strong acid and alkali attack at elevated temperatures • Good thermal conductivity • Excellent size and shape capability
- 6. PROPERTIES • High strength and stiffness • Available in purity ranges from 94%, an easily metallizable composition, to 99.5% for the most demanding high temperature applications.
- 7. • Aluminium oxide is an electrical insulator but has a relatively high thermal Conductivity (30 Wm−1K−1) for a ceramic material. In its most commonly occurring crystalline form, called corundum or α- aluminium oxide, its hardness makes it suitable for use as an abrasive and as a component in cutting tools. • Aluminium oxide is responsible for the resistance of metallic aluminium to weathering. Metallic aluminium is very reactive with atmospheric oxygen, and a thin passivation layer of alumina (4 nm thickness) forms on any exposed aluminium surface.
- 8. • This layer protects the metal from further oxidation. The thickness and properties of this oxide layer can be enhanced using a process called anodizing. A number of alloys, such as aluminium bronzes, exploit this property by including a proportion of aluminium in the alloy to enhance corrosion resistance. The alumina generated by anodising is typically amorphous, but discharge assisted oxidation processes such as plasma electrolytic oxidation result in a significant proportion of crystalline alumina in the coating, enhancing it shardnes. • Aluminium oxide is completely insoluble in water. However it is an amphoteric substance, meaning it can react with both acids and bases, such as hydrochloric acid and sodium hydroxide. • Al2O3 + 6 HCl → 2 AlCl3 + 3 H2O • Al2O3 + 6 NaOH + 3 H2O → 2 Na3Al(OH)6
- 9. PROCESSING • Aluminium hydroxide minerals are the main component of bauxite, the principal ore of aluminium. A mixture of the minerals comprise bauxite ore, including gibbsite (Al(OH)3), boehmite (γ- AlO(OH)), and diaspore (α-AlO(OH)), along with impurities of iron oxides and hydroxides, quartz and clay minerals. Bauxites are found in laterites. Bauxite is purified by the Bayer process: Al2O3 + 3 H2O → 2 Al(OH)3
- 10. • Except for SiO2, the other components of bauxite do not dissolve in base. Upon filtering the basic mixture, Fe2O3 is removed. When the Bayer liquor is cooled, Al(OH)3 precipitates, leaving the silicates in solution. The solid is then calcined (heated strongly) to give aluminium oxide: 2 Al(OH)3 → Al2O3 + 3 H2O
- 11. APPLICATION: • As a filler – Being fairly chemically inert and white, alumina is a favored filler for plastics. • As a catalyst and catalyst support – Alumina catalyses a variety of reactions that are useful industrially. In its largest scale application, alumina is the catalyst in the Claus process for converting hydrogen sulfide waste gases into elemental sulfur in refineries. It is also useful for dehydration of alcohols to alkenes
- 12. APPLICATION • Gas purification and related absorption applications – Alumina is widely used to remove water from gas streams • As an abrasive – It is widely used as an abrasive, including as a much less expensive substitute for industrial diamond.
- 13. MISCELLANEOUS USES • Gas laser tubes • Wear pads • Seal rings • High temperature electrical insulators • High voltage insulators • Furnace liner tubes • Thread and wire guides • Electronic substrates • Ballistic armor • Abrasion resistant tube and elbow liners • Thermometry sensors • Laboratory instrument tubes and sample holders • Instrumentation parts for thermal property test machines • Grinding media
- 14. SILICON CARBIDE • Silicon carbide (SiC), also known as carborundum, is a compound of silicon and carbon with chemical formula SiC. It occurs in nature as the extremely rare mineral moissanite. • Silicon carbide exists in about 250 crystalline forms. The polymorphism of SiC is characterized by a large family of similar crystalline structures called polytypes.
- 16. • Alpha silicon carbide (α-SiC) is the most commonly encountered polymorph; it is formed at temperatures greater than 1700 °C and has a hexagonal crystal structure (similar to Quartzite). • The beta modification (β-SiC), with a zinc blende crystal structure (similar to diamond), is formed at temperatures below 1700 °C. Until recently, the beta form has had relatively few commercial uses, although there is now increasing interest in its use as a support for heterogeneous catalysts, owing to its higher surface area compared to the alpha form
- 17. • Pure SiC is colorless. The brown to black color of industrial product results from iron impurities. The rainbow-like luster of the crystals is caused by a passivation layer of silicon dioxide that forms on the surface
- 18. PROCESSING • The simplest manufacturing process is to combine silica sand and carbon in an Acheson graphite electric resistance furnace at a high temperature, between 1600 and 2500 °C. • Fine SiO2particles in plant material (e.g. rice husks) can be converted to SiC by heating in the excess carbon from the organic material. The silica fume, which is a byproduct of producing silicon metal and ferrosilicon alloys, also can be converted to SiC by heating with graphite at 1500 °C.
- 19. APPLICATION • Abrasive and cutting tools: – In manufacturing, it is used for its hardness in abrasive machining processes such as grinding, honing,water-jet cutting and sandblasting. Particles of silicon carbide are laminated to paper to create sandpapers and the grip tape on skateboards.
- 20. APPLICATION • Structural material: – It is used for high temperature gas turbines. Also, silicon carbide is used in composite armor (e.g.Chobham armor), and in ceramic plates in bulletproof vests. Dragon Skin, which is produced by Pinnacle Armor, uses disks of silicon carbide. • Automobile parts: – Silicon-infiltrated carbon-carbon composite is used for high performance "ceramic" brake discs, as it is able to withstand extreme temperatures. The silicon reacts with the graphite in the carbon-carbon composite to become carbon-fiber-reinforced silicon carbide (C/SiC).
- 21. APPLICATION • Power electronic devices: – Silicon carbide is a semiconductor in research and early mass-production providing advantages for fast, high-temperature and/or high-voltage devices. First devices available were Schottky diodes, followed by Junction-gate FETs and MOSFETs for high-power switching.
- 22. MISCELLANEOUS APPLICATION • Thin filament pyrometry • Heating elements • Nuclear fuel particles • Nuclear fuel cladding • Jewelry • Steel production • Catalyst support
- 23. DIAMOND • Diamond is the allotrope of carbon in which the carbon atoms are arranged in the specific type of cubic lattice called diamond cubic. • Diamond is an optically isotropic crystal that is transparent to opaque. • Owing to its strong covalent bonding, diamond is the hardest naturally occurring material known.
- 24. PROPERTIES • HARDNESS AND CRYSTAL STRUCTURE – Diamond is the hardest known naturally occurring material, scoring 10 on the Mohs scale of mineral hardness. – Diamond is extremely strong owing to the structure of its carbon atoms, where each carbon atom has four neighbors joined to it with covalent bonds.
- 25. PROPERTIES – Diamonds crystallize in the diamond cubic crystal system and consist of tetrahedrally, covalently bonded carbon atoms. – A second form called lonsdaleite, with hexagonal symmetry, has also been found, but it is extremely rare and forms only in meteorites or in laboratory synthesis.
- 26. PROPERTIES • TOUGHNESS: – Unlike hardness, which only denotes resistance to scratching, diamond's toughness or tenacity is only fair to good. – Toughness relates to the ability to resist breakage from falls or impacts. Because of diamond's perfect and easy cleavage, it is vulnerable to breakage. – A diamond will shatter if hit with an ordinary hammer.
- 27. PROPERTIES – As with any material, the macroscopic geometry of a diamond contributes to its resistance to breakage. Diamond has a cleavage plane and is therefore more fragile in some orientations than others. Diamond cutters use this attribute to cleave some stones, prior to faceting.
- 28. PROPERTIES • OPTICAL PROPERTIES – Color:Diamonds occur in various colors — black, brown, yellow, gray, white, blue, orange, purple to pink and red. Colored diamonds contain crystallographic defects, including substitutional impurities and structural defects, that cause the coloration. – Luster:The luster of a diamond is described as 'adamantine', which simply means diamond-like.
- 29. – Fluorescence:Diamonds exhibit fluorescence, that is, they emit light of various colors and intensities under long-wave ultra-violet light. • Thermal stability: – Being a form of carbon, diamond oxidizes in air if heated over 700 °C. – In absence of oxygen, e.g. in a flow of high- purity argon gas, diamond can be heated up to about 1700 °C
- 31. THE FOUR BASIC STEPS FOR DIAMOND CUTTING 1. Planning – Planning is a crucial step in diamond manufacturing because during this stage the size and relative value of the cut stones that the rough will produce are determined. – A person called a planner decides where to mark the diamond rough for fashioning into the most profitable polished gem(s).
- 32. 2. Cleaving or sawing – Once the planner decides where the diamond should be cut, the diamond is either manually cleaved or sawed. Sawing can be done with a diamond- coated rotary saw or a laser.
- 33. 3. Bruting – Bruting forms the basic face-up outline of a round diamond to prepare it for faceting. – During the bruting phase the diamond being bruted is spun on a rotating lathe while another diamond is forced against it, gradually forming the rounded outline. Essentially, one diamond is used to shape the other.
- 34. 4. Polishing – Polishing is the final stage of the cutting process, giving the diamond its finished proportions. – The first and perhaps most crucial polishing stage is blocking. – This step lays the foundation for the potential of the diamond's performance because it establishes the diamond's basic symmetry
- 35. APPLICATION • Used as a cutting tool for materials marble, granite and hard wood. • Used as cutting tool for shaping of engine blocks. • Synthetic diamonds are used in machinery. • As shapes of synthetic diamonds can be controlled they are widely used as tools in many machining processes.
- 36. APPLICATION • The fact that it can absorb high levels of heat(5 TIMES GREATER THAN COPPER) means that it can be used to reduce the friction in many engineering parts. • Including the diamond as a 'heat sink' helps in extending the life of the machinery since it avoids wear and tear due to friction and heat. • 'Slices' of synthetic diamonds are also be used for other industrial and surgical tools.
- 37. REFFERENCES • http://en.wikipedia.org/wiki/Silicon_carbide • http://www.britannica.com/EBchecked/topic/544369/s ilicon-carbide • http://en.wikipedia.org/wiki/Aluminium_oxide • P. Patnaik (2002). Handbook of Inorganic Chemicals. McGraw-Hill.ISBN 0-07-049439-8 • anse, A.J.A. (2007). "Global Rough Diamond Production Since 1870". Gems & Gemology 43 (2): 98– 119. doi:10.5741/GEMS.43.2.98 • eorge E. Harlow (1998). The nature of diamonds. Cambridge University Press. p. 34. ISBN 0-521-62935-7
- 38. THANK YOU!