Open Access Articles- Top Results for Silicon nitride

Silicon nitride

Silicon nitride
Sample of silicon nitride
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Preferred IUPAC name
Silicon nitride
Other names
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12033-89-5 7pxY
ChemSpider 2341213 7pxY
EC number 234-796-8
Jmol-3D images Image
MeSH Silicon+nitride
PubChem Template:Chembox PubChem/format
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Molar mass Lua error in Module:Math at line 495: attempt to index field 'ParserFunctions' (a nil value). g·mol−1
Appearance grey, odorless powder
Density 3.2 g/cm3, solid
Melting point Script error: No such module "convert".[1] (decomposes)
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Main hazards When heated to decomposition, silicon nitride may emit toxic fumes of ammonia and ozone. Contact with acids may generate flammable hydrogen gas.[1]
EU classification not listed
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Other anions
silicon carbide, silicon dioxide
Other cations
boron nitride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Silicon nitride is a chemical compound of the elements silicon and nitrogen, with the formula Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom. It is a white, high-melting-point solid that is relatively chemically inert, being attacked by dilute HF and hot [[Sulfuric acid|Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom]]. It is the most thermodynamically stable of the silicon nitrides. Hence, Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom is the most commercially important of the silicon nitrides[3] and is generally understood as what is being referred to where the term "silicon nitride" is used.


The material is prepared by heating powdered silicon between 1300 °C and 1400 °C in an atmosphere of nitrogen:

3 Si + 2 Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom

The silicon sample weight increases progressively due to the chemical combination of silicon and nitrogen. Without an iron catalyst, the reaction is complete after several hours (~7), when no further weight increase due to nitrogen absorption (per gram of silicon) is detected. In addition to Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom, several other silicon nitride phases (with chemical formulas corresponding to varying degrees of nitridation/Si oxidation state) have been reported in the literature, for example, the gaseous disilicon mononitride (Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atom); silicon mononitride (SiN), and silicon sesquinitride (Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom), each of which are stoichiometric phases. As with other refractories, the products obtained in these high-temperature syntheses depends on the reaction conditions (e.g. time, temperature, and starting materials including the reactants and container materials), as well as the mode of purification. However, the existence of the sesquinitride has since come into question.[4]

It can also be prepared by diimide route:[5]

Template:Chem/atomTemplate:Chem/atom + 6 Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom + 4 Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atom(s)    at 0 °C
3 Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom + Template:Chem/atomTemplate:Chem/atom + 3 Template:Chem/atomTemplate:Chem/atom(g)    at 1000 °C

Carbothermal reduction of silicon dioxide in nitrogen atmosphere at 1400–1450 °C has also been examined:[5]

3 Template:Chem/atomTemplate:Chem/atom + 6 C + 2 Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom + 6 CO

The nitridation of silicon powder was developed in the 1950s, following the "rediscovery" of silicon nitride and was the first large-scale method for powder production. However, use of low-purity raw silicon caused contamination of silicon nitride by silicates and iron. The diimide decomposition results in amorphous silicon nitride, which needs further annealing under nitrogen at 1400–1500 °C to convert it to crystalline powder; this is now the second-most important route for commercial production. The carbothermal reduction was the earliest used method for silicon nitride production and is now considered as the most-cost-effective industrial route to high-purity silicon nitride powder.[5]

Electronic-grade silicon nitride films are formed using chemical vapor deposition (CVD), or one of its variants, such as plasma-enhanced chemical vapor deposition (PECVD):[5][6]

3 Template:Chem/atomTemplate:Chem/atom(g) + 4 Template:Chem/atomTemplate:Chem/atom(g) → Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom(s) + 12 Template:Chem/atomTemplate:Chem/atom(g)
3 Template:Chem/atomTemplate:Chem/atom(g) + 4 Template:Chem/atomTemplate:Chem/atom(g) → Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom(s) + 12 HCl(g)
3 Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom(g) + 4 Template:Chem/atomTemplate:Chem/atom(g) → Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom(s) + 6 HCl(g) + 6 Template:Chem/atomTemplate:Chem/atom(g)

For deposition of silicon nitride layers on semiconductor (usually silicon) substrates, two methods are used:[6]

  1. Low pressure chemical vapor deposition (LPCVD) technology, which works at rather high temperature and is done either in a vertical or in a horizontal tube furnace,[7] or
  2. Plasma-enhanced chemical vapor deposition (PECVD) technology, which works at rather low temperature and vacuum conditions.

The lattice constants of silicon nitride and silicon are different. Therefore tension or stress can occur, depending on the deposition process. Especially when using PECVD technology this tension can be reduced by adjusting deposition parameters.[8]

Silicon nitride nanowires can also be produced by sol-gel method using carbothermal reduction followed by nitridation of silica gel, which contains ultrafine carbon particles. The particles can be produced by decomposition of dextrose in the temperature range 1200–1350 °C. The possible synthesis reactions are:[9]

Template:Chem/atomTemplate:Chem/atom(s) + C(s) → SiO(g) + CO(g)    and
3 SiO(g) + 2 Template:Chem/atomTemplate:Chem/atom(g) + 3 CO(g) → Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom(s) + 3 Template:Chem/atomTemplate:Chem/atom(g)    or
3 SiO(g) + 2 Template:Chem/atomTemplate:Chem/atom(g) + 3 C(s) → Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom(s) + 3 CO(g).


Silicon nitride is difficult to produce as a bulk material—it cannot be heated over 1850 °C, which is well below its melting point, due to dissociation to silicon and nitrogen. Therefore, application of conventional hot press sintering techniques is problematic. Bonding of silicon nitride powders can be achieved at lower temperatures through adding additional materials (sintering aids or "binders") which commonly induce a degree of liquid phase sintering.[10] A cleaner alternative is to use spark plasma sintering where heating is conducted very rapidly (seconds) by passing pulses of electric current through the compacted powder. Dense silicon nitride compacts have been obtained by this techniques at temperatures 1500–1700 °C.[11][12]

Crystal structure and properties

Blue atoms are nitrogen and grey are silicon atoms

There exist three crystallographic structures of silicon nitride (Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom), designated as α, β and γ phases.[13] The α and β phases are the most common forms of Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom, and can be produced under normal pressure condition. The γ phase can only be synthesized under high pressures and temperatures and has a hardness of 35 GPa.[14][15]

The α- and β-Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom have trigonal (Pearson symbol hP28, space group P31c, No. 159) and hexagonal (hP14, P63, No. 173) structures, respectively, which are built up by corner-sharing Template:Chem/atomTemplate:Chem/atom tetrahedra. They can be regarded as consisting of layers of silicon and nitrogen atoms in the sequence ABAB... or ABCDABCD... in β-Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom and α-Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom, respectively. The AB layer is the same in the α and β phases, and the CD layer in the α phase is related to AB by a c-glide plane. The Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom tetrahedra in β-Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom are interconnected in such a way that tunnels are formed, running parallel with the c axis of the unit cell. Due to the c-glide plane that relates AB to CD, the α structure contains cavities instead of tunnels. The cubic γ-Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom is often designated as c modification in the literature, in analogy with the cubic modification of boron nitride (c-BN). It has a spinel-type structure in which two silicon atoms each coordinate six nitrogen atoms octahedrally, and one silicon atom coordinates four nitrogen atoms tetrahedrally.[12]

The longer stacking sequence results in the α-phase having higher hardness than the β-phase. However, the α-phase is chemically unstable compared with the β-phase. At high temperatures when a liquid phase is present, the α-phase always transforms into the β-phase. Therefore, β-Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom is the major form used in Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom ceramics.[16]


In general, the main issue with applications of silicon nitride has not been technical performance, but cost. As the cost has come down, the number of production applications is accelerating.[17]

Automobile industry

One of the major applications of sintered silicon nitride is in automobile industry as a material for engine parts. Those include, in diesel engines, glowplugs for faster start-up; precombustion chambers (swirl chambers) for lower emissions, faster start-up and lower noise; turbocharger for reduced engine lag and emissions. In spark-ignition engines, silicon nitride is used for rocker arm pads for lower wear, turbocharger for lower inertia and less engine lag, and in exhaust gas control valves for increased acceleration. As examples of production levels, there is an estimated more than 300,000 sintered silicon nitride turbochargers made annually.[5][10][17]


Si3N4 bearing parts

Silicon nitride bearings are both full ceramic bearings and ceramic hybrid bearings with balls in ceramics and races in steel. Silicon nitride ceramics have good shock resistance compared to other ceramics. Therefore, ball bearings made of silicon nitride ceramic are used in performance bearings. A representative example is use of silicon nitride bearings in the main engines of the NASA's Space Shuttle.[18][19]

Since silicon nitride ball bearings are harder than metal, this reduces contact with the bearing track. This results in 80% less friction, 3 to 10 times longer lifetime, 80% higher speed, 60% less weight, the ability to operate with lubrication starvation, higher corrosion resistance and higher operation temperature, as compared to traditional metal bearings.[17] Silicon nitride balls weigh 79% less than tungsten carbide balls. Silicon nitride ball bearings can be found in high end automotive bearings, industrial bearings, wind turbines, motorsports, bicycles, rollerblades and skateboards. Silicon nitride bearings are especially useful in applications where corrosion, electric or magnetic fields prohibit the use of metals. For example, in tidal flow meters, where seawater attack is a problem, or in electric field seekers.[10]

Si3N4 was first demonstrated as a superior bearing in 1972 but did not reach production until nearly 1990 because of challenges associated with reducing the cost. Since 1990, the cost has been reduced substantially as production volume has increased. Although Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom bearings are still 2–5 times more expensive than the best steel bearings, their superior performance and life are justifying rapid adoption. Around 15–20 million Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom bearing balls were produced in the U.S. in 1996 for machine tools and many other applications. Growth is estimated at 40% per year, but could be even higher if ceramic bearings are selected for consumer applications such as in-line skates and computer disk drives.[17]

High-temperature material

Silicon nitride thruster. Left: Mounted in test stand. Right: Being tested with Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom propellants

Silicon nitride has long been used in high-temperature applications. In particular, it was identified as one of the few monolithic ceramic materials capable of surviving the severe thermal shock and thermal gradients generated in hydrogen/oxygen rocket engines. To demonstrate this capability in a complex configuration, NASA scientists used advanced rapid prototyping technology to fabricate a one-inch-diameter, single-piece combustion chamber/nozzle (thruster) component. The thruster was hot-fire tested with hydrogen/oxygen propellant and survived five cycles including a 5-minute cycle to a 1320 °C material temperature.[20]


Silicon nitride has many orthopedic applications.[21][22] The material is also an alternative to PEEK (polyether ether ketone) and titanium, which are used for spinal fusion devices.[23][24] It is silicon nitride’s hydrophilic, microtextured surface that contributes to the materials strength, durability and reliability compared to PEEK and titanium.[22][23][25]

Metal working and cutting tools

The first major application of Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom was abrasive and cutting tools. Bulk, monolithic silicon nitride is used as a material for cutting tools, due to its hardness, thermal stability, and resistance to wear. It is especially recommended for high speed machining of cast iron. Hot hardness, fracture toughness and thermal shock resistance mean that sintered silicon nitride can cut cast iron, hard steel and nickel based alloys with surface speeds up to 25 times quicker than those obtained with conventional materials such as tungsten carbide.[10] The use of Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom cutting tools has had a dramatic effect on manufacturing output. For example, face milling of gray cast iron with silicon nitride inserts doubled the cutting speed, increased tool life from one part to six parts per edge, and reduced the average cost of inserts by 50%, as compared to traditional tungsten carbide tools.[5][17]


Silicon nitride is often used as an insulator and chemical barrier in manufacturing integrated circuits, to electrically isolate different structures or as an etch mask in bulk micromachining. As a passivation layer for microchips, it is superior to silicon dioxide, as it is a significantly better diffusion barrier against water molecules and sodium ions, two major sources of corrosion and instability in microelectronics. It is also used as a dielectric between polysilicon layers in capacitors in analog chips.[26]

Silicon nitride deposited by LPCVD contains up to 8% hydrogen. It also experiences strong tensile stress, which may crack films thicker than 200 nm. However, it has higher resistivity and dielectric strength than most insulators commonly available in microfabrication (1016 Ω·cm and 10 MV/cm, respectively).[6]

Not only silicon nitride, but also various ternary compounds of silicon, nitrogen and hydrogen (SiNxHy) are used insulating layers. They are plasma deposited using the following reactions:[6]

2 Template:Chem/atomTemplate:Chem/atom(g) + Template:Chem/atomTemplate:Chem/atom(g) → 2 SiNH(s) + 3 Template:Chem/atomTemplate:Chem/atom(g)
Template:Chem/atomTemplate:Chem/atom(g) + Template:Chem/atomTemplate:Chem/atom(g) → SiNH(s) + 3 Template:Chem/atomTemplate:Chem/atom(g)

These SiNH films have much less tensile stress, but worse electrical properties (resistivity 106 to 1015 Ω·cm, and dielectric strength 1 to 5 MV/cm).[6][27]

Silicon nitride is also used in xerographic process as one of the layer of the photo drum.[28] Silicon nitride is also used as an ignition source for domestic gas appliances.[29] Because of its good elastic properties, silicon nitride, along with silicon and silicon oxide, is the most popular material for cantilevers — the sensing elements of atomic force microscopes.[30]


The first reported preparation was in 1857 by Henri Etienne Sainte-Claire Deville and Friedrich Wöhler.[31] In their method, silicon was heated in a crucible placed inside another crucible packed with carbon to reduce permeation of oxygen to the inner crucible. They reported a product they termed silicon nitride but without specifying its chemical composition. Paul Schuetzenberger first reported a product with the composition of the tetranitride, Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom, in 1879 that was obtained by heating silicon with brasque (a paste made by mixing charcoal, coal, or coke with clay which is then used to line crucibles) in a blast furnace. In 1910, Ludwig Weiss and Theodor Engelhardt heated silicon under pure nitrogen to produce Template:Chem/atomTemplate:Chem/atomTemplate:Chem/atomTemplate:Chem/atom.[32] E. Friederich and L. Sittig made Si3N4 in 1925 via carbothermal reduction under nitrogen, that is, by heating silica, carbon, and nitrogen at 1250–1300 °C.

Silicon nitride remained merely a chemical curiosity for decades before it was used in commercial applications. From 1948 to 1952, the Carborundum Company, Niagara Falls, New York, applied for several patents on the manufacture and application of silicon nitride.[5] By 1958 Haynes (Union Carbide) silicon nitride was in commercial production for thermocouple tubes, rocket nozzles, and boats and crucibles for melting metals. British work on silicon nitride, started in 1953, was aimed at high-temperature parts of gas turbines and resulted in the development of reaction-bonded silicon nitride and hot-pressed silicon nitride. In 1971, the Advanced Research Project Agency of the US Department of Defense placed a US$17 million contract with Ford and Westinghouse for two ceramic gas turbines.[33]

Even though the properties of silicon nitride were well known, its natural occurrence was discovered only in the 1990s, as tiny inclusions (about 2 µm × 0.5 µm in size) in meteorites. The mineral was named nierite after a pioneer of mass spectrometry, Alfred O. C. Nier.[34] This mineral might have been detected earlier, again exclusively in meteorites, by Soviet geologists.[35]


  2. ^ Refractive index database.
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  7. ^ "Crystec Technology Trading GmbH, Comparison of vertical and horizontal tube furnaces in the semiconductor industry". Retrieved 2009-06-06. 
  8. ^ "Crystec Technology Trading GmbH, deposition of silicon nitride layers". Retrieved 2009-06-06. 
  9. ^ Ghosh Chaudhuri, Mahua; Dey, Rajib; Mitra, Manoj K.; Das, Gopes C.; Mukherjee, Siddhartha (2008). "A novel method for synthesis of α-Si3N4 nanowires by sol-gel route". Science and Technology of Advanced Materials 9: 5002. Bibcode:2008STAdM...9a5002G. doi:10.1088/1468-6996/9/1/015002. 
  10. ^ a b c d "Silicon Nitride – An Overview". Retrieved 2009-06-06. 
  11. ^ Nishimura, T.; Xu, X.; Kimoto, K.; Hirosaki, N.; Tanaka, H. (2007). "Fabrication of silicon nitride nanoceramics—Powder preparation and sintering: A review". Science and Technology of Advanced Materials 8 (7–8): 635. Bibcode:2007STAdM...8..635N. doi:10.1016/j.stam.2007.08.006. 
  12. ^ a b Peng, Hong (2004). Spark Plasma Sintering of Si3N4-based Ceramics: Sintering mechanism-Tailoring microstructure-Evaluating properties (PhD thesis). Stockholm University. ISBN 978-91-7265-834-9. [page needed]
  13. ^ "Crystal structures of Si3N4". Retrieved 2009-06-06. 
  14. ^ Jiang, J. Z.; Kragh, F.; Frost, D. J.; Ståhl, K.; Lindelov, H. (2001). "LETTER TO THE EDITOR: Hardness and thermal stability of cubic silicon nitride". Journal of Physics: Condensed Matter 13 (22): L515. Bibcode:2001JPCM...13L.515J. doi:10.1088/0953-8984/13/22/111. 
  15. ^ "Properties of gamma-Si3N4". Retrieved 2009-06-06. [self-published source?]
  16. ^ Zhu, Xinwen; Sakka, Yoshio (2008). "TOPICAL REVIEW: Textured silicon nitride: Processing and anisotropic properties". Science and Technology of Advanced Materials 9 (3): 3001. Bibcode:2008STAdM...9c3001Z. doi:10.1088/1468-6996/9/3/033001. 
  17. ^ a b c d e Richerson, David W.; Freita, Douglas W. "Ceramic Industry". Opportunities for Advanced Ceramics to Meet the Needs of the Industries of the Future. Oak Ridge National Laboratory. OCLC 692247038. 
  18. ^ "Ceramic Balls Increase Shuttle Engine Bearing Life". NASA. Retrieved 2009-06-06. 
  19. ^ "Space Shuttle Main Engine Enhancements". NASA. Retrieved 2009-06-06. 
  20. ^ "Silicon Nitride Rocket Thrusters Test Fired Successfully". NASA. Retrieved 2009-06-06. 
  21. ^ Olofsson, Johanna; Grehk, T. Mikael; Berlind, Torun; Persson, Cecilia; Jacobson, Staffan; Engqvist, Håkan (2012). "Evaluation of silicon nitride as a wear resistant and resorbable alternative for total hip joint replacement". Biomatter 2 (2): 94–102. PMID 23507807. doi:10.4161/biom.20710. 
  22. ^ a b Mazzocchi, M; Bellosi, A (2008). "On the possibility of silicon nitride as a ceramic for structural orthopaedic implants. Part I: Processing, microstructure, mechanical properties, cytotoxicity". Journal of Materials Science: Materials in Medicine 19 (8): 2881–7. PMID 18347952. doi:10.1007/s10856-008-3417-2. 
  23. ^ a b Webster, T.J.; Patel, A.A.; Rahaman, M.N.; Sonny Bal, B. (2012). "Anti-infective and osteointegration properties of silicon nitride, poly(ether ether ketone), and titanium implants". Acta Biomaterialia 8 (12): 4447–54. PMID 22863905. doi:10.1016/j.actbio.2012.07.038. 
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  25. ^ Arafat, Ahmed; Schroën, Karin; De Smet, Louis C. P. M.; Sudhölter, Ernst J. R.; Zuilhof, Han (2004). "Tailor-Made Functionalization of Silicon Nitride Surfaces". Journal of the American Chemical Society 126 (28): 8600–1. PMID 15250682. doi:10.1021/ja0483746. 
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  33. ^ Carter, C. Barry and Norton, M. Grant (2007). Ceramic Materials: Science and Engineering. Springer. p. 27. ISBN 0-387-46270-8. 
  34. ^ Lee, M. R.; Russell, S. S.; Arden, J. W.; Pillinger, C. T. (1995). "Nierite (Si3N4), a new mineral from ordinary and enstatite chondrites". Meteoritics 30 (4): 387. Bibcode:1995Metic..30..387L. doi:10.1111/j.1945-5100.1995.tb01142.x. 
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Further reading

  • R. C. Sangster (2005). Formation of Silicon Nitride: From the 19th to the 21st Century – Materials Science Foundations (monograph series). 22–24. Trans. Tech. Publications. ISBN 0-87849-492-8. 
  • V.I. Belyi and L.L. Vasilyeva (1988). Silicon Nitride in Electronics. Elsevier, Nederlands. ISBN 978-0444426895. 
  • Ziegler, G.; Heinrich, J.; Wötting, G. (1987). "Relationships between processing, microstructure and properties of dense and reaction-bonded silicon nitride". Journal of Materials Science 22 (9): 3041. Bibcode:1987JMatS..22.3041Z. doi:10.1007/BF01161167. 
  • Veprek, S.; Reiprich, S. (1995). "A concept for the design of novel superhard coatings". Thin Solid Films 268: 64. Bibcode:1995TSF...268...64V. doi:10.1016/0040-6090(95)06695-0. 

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