Eutectic point

Equilibrium phase diagram for a binary system. The eutectic point is the point at which the liquid phase L borders directly on the solid phase α + β.

The melting point of a mixture of two or more solids (such as an alloy) depends on the relative proportions of its ingredients. A eutectic or eutectic mixture is a mixture at such proportions that the melting point is a local temperature minimum, which means that all the constituents crystallize simultaneously at this temperature from molten liquid solution. Such a simultaneous crystallization of a eutectic mixture is known as a eutectic reaction, the temperature at which it takes place is the eutectic temperature, and the composition and temperature at which it takes place is called the eutectic point.

The term comes from the Greek eutektos, meaning "easily melted".^[1]

The equilibrium phase diagram at the right displays a simple binary system composed of two components, A and B, which has a eutectic point. The phase diagram plots relative concentrations of A and B along the horizontal axis, and temperature along the vertical axis. The eutectic point is the point at which the liquid phase L borders directly on the solid phase α + β (a homogeneous mixture composed of both A and B), representing the minimum melting temperature of any possible alloy of A and B.

Not all binary system alloys have a eutectic point: those that form a solid solution at all concentrations, such as the gold-silver system, have no eutectic. An alloy system that has a eutectic is often referred to as a eutectic system, or eutectic alloy.

Solid products of a eutectic reaction can often be identified by their lamellar structure, as opposed to the dendritic structures commonly seen in non-eutectic solidification. The same conditions that force the material to form lamellae can instead form an amorphous solid if pushed to an extreme.

Metallic eutectics

The term is often used in metallurgy to describe the alloy of two or more component materials having the relative concentrations specified at the eutectic point. When a non-eutectic alloy solidifies, its components crystallize at different temperatures, exhibiting a plastic melting range. A eutectic alloy solidifies at a single, sharp temperature. The phase transformations that occur while solidifying a given alloy can be understood by drawing a vertical line from the liquid phase to the solid phase on a phase diagram.

Some uses include:

• eutectic alloys for soldering, composed of tin (Sn), lead (Pb) and sometimes silver (Ag) or gold (Au).
• casting alloys, such as aluminium-silicon and cast iron (at the composition for an austenite-cementite eutectic in the iron-carbon system).
• brazing, where diffusion can remove alloying elements from the joint, so that eutectic melting is only possible early in the brazing process.
• temperature response, i.e. Wood's metal and Field's metal for fire sprinklers.
• non-toxic mercury replacements, such as galinstan.
• experimental glassy metals, with extremely high strength and corrosion resistance.
• eutectic alloys of sodium and potassium (NaK) that are liquid at room temperature and used as coolant in experimental fast neutron nuclear reactors.

Other eutectic mixtures

Sodium chloride and water form a eutectic mixture. It has a eutectic point of −21.2 C^[2] and 23.3%^[3] salt by mass. The eutectic nature of salt and water is exploited when salt is spread on roads to aid snow removal, or mixed with ice to produce low temperatures (for example, in traditional ice cream making).

Lidocaine and prilocaine, both solids at room temperature, form a eutectic that is an oil with a 16°C melting point, used in EMLA (Eutectic Mixture of Local Anesthetic) preparations.

Minerals may form eutectic mixtures in igneous rocks,^[4] giving rise to characteristic intergrowth textures such as that of granophyre.

Some inks are eutectic mixtures, allowing inkjet printers to operate at lower temperatures.^[5]

Other critical points

Eutectoid

When the solution above the transformation point is solid, rather than liquid, an analogous eutectoid transformation can occur. For instance, in the iron-carbon system, the austenite phase can undergo a eutectoid transformation to produce ferrite and cementite (iron carbide), often in lamellar structures such as pearlite and bainite. This eutectoid point occurs at 727°C (1340.6 ºF) and about 0.83% carbon^[6]; alloys of nearly this composition are called high-carbon steel, while those which have less carbon are termed mild steel. The process analogous to glass formation in this system is the martensitic transformation.

Iron-carbon phase diagram, showing the euctectoid transformation between austenite (γ) and pearlite.

Peritectic

Peritectic transformations are also similar to eutectic reactions. Here, a liquid and solid phase of fixed proportions react at a fixed temperature to yield a single solid phase. Since the solid product forms at the interface between the two reactants, it can form a diffusion barrier and generally causes such reactions to proceed much more slowly than eutectic or eutectoid transformations. Because of this, when a peritectic composition solidifies it does not show the lamellar structure that you find with eutectic solidification.

Such a transformation exists in the iron-carbon system, as seen near the upper-left corner of the figure. It resembles an inverted eutectic, with the δ phase combining with the liquid to produce pure austenite at 1495 °C and 0.17 mass percent carbon.

References

1. ^ Merriam-Webster (2003), Merriam-Webster's collegiate dictionary (11th ed.), Merriam-Webster, p. 432, ISBN 9780877798095, http://books.google.com/books?id=O78rzaI2XmUC&pg=RA1-PA432 .
2. ^ Muldrew, Ken; Locksley E. McGann (1997). "Phase Diagrams". Cryobiology—A Short Course. University of Calgary. http://www.ucalgary.ca/~kmuldrew/cryo_course/cryo_chap6_1.html. Retrieved 2006-04-29. 
3. ^ Senese, Fred (1999). "Does salt water expand as much as fresh water does when it freezes?". Solutions: Frequently asked questions. Department of Chemistry, Frostburg State University. http://antoine.frostburg.edu/chem/senese/101/solutions/faq/saltwater-ice-volume.shtml. Retrieved 2006-04-29. 
4. ^ Fichter, Lynn S. (2000). "Igneous Phase Diagrams". Igneous Rocks. James Madison University. http://csmres.jmu.edu/geollab/Fichter/IgnRx/Phasdgrm.html. Retrieved 2006-04-29. 
5. ^ Davies, Nicholas A.; Beatrice M. Nicholas (1992). "Eutectic compositions for hot melt jet inks". US Patent & Trademark Office, Patent Full Text and Image Database. United States Patent and Trademark Office. http://patft.uspto.gov/netacgi/nph-Parser?Sect1=PTO2&Sect2=HITOFF&p=1&u=/netahtml/search-bool.html&r=1&f=G&l=50&co1=AND&d=ptxt&s1=5298062.WKU.&OS=PN/5298062&RS=PN/5298062. Retrieved 2006-04-29. 
6. ^ Iron-Iron Carbide Phase Diagram Example

• Sadoway, Donald (2004). "Phase Equilibria and Phase Diagrams" (pdf). 3.091 Introduction to Solid State Chemistry, Fall 2004. MIT Open Courseware. http://ocw.mit.edu/NR/rdonlyres/Materials-Science-and-Engineering/3-091Fall-2004/6ECFB930-9D59-4DD5-A872-FE48002587B0/0/notes_10.pdf. Retrieved 2006-04-12. 

Bibliography

• Mortimer, Robert G. (2000). Physical Chemistry. Academic Press. ISBN 0-12-508345-9. 
• Reed-Hill, R.E.; Reza Abbaschian (1992). Physical Metallurgy Principles. Thomson-Engineering. ISBN 0-534-92173-6. 
• Easterling, Edward (1992). Phase Transformations in Metals and Alloys. CRC. ISBN 0-7487-5741-4. 
• Askeland, Donald R.; Pradeep P. Phule (2005). The Science and Engineering of Materials. Thomson-Engineering. ISBN 0-534-55396-6. 

See also

• Azeotrope
• Solid solution
• Phase diagram
• Freezing point depression
• Hypoeutectic alloy