View source for Melting point

{{short description|Temperature at which a solid turns liquid}}
{{for|the EP by Zerobaseone|Melting Point (EP)}}
{{for|the physical processes that take place at the melting point|Melting|Freezing|Crystallization}}
{{Redirect|Freezing point|other uses}}
[[File:Melting ice thermometer.jpg|thumb|Ice cubes put in water will start to melt when they reach their melting point of 0&nbsp;[[Celsius|°C]]]]
The '''melting point''' (or, rarely, '''liquefaction point''') of a substance is the [[temperature]] at which it changes [[state of matter|state]] from [[solid]] to [[liquid]]. At the melting point the solid and liquid [[phase_(matter)|phase]] exist in [[Thermodynamic equilibrium|equilibrium]]. The melting point of a substance depends on [[pressure]] and is usually specified at a [[Standard conditions for temperature and pressure|standard pressure]] such as 1 [[Atmosphere (unit)|atmosphere]] or 100 [[Pascal (unit)|kPa]].

When considered as the temperature of the reverse change from liquid to solid, it is referred to as the '''freezing point''' or '''crystallization point'''. Because of the ability of substances to [[Supercooling|supercool]], the freezing point can easily appear to be below its actual value. When the "characteristic freezing point" of a substance is determined, in fact, the actual methodology is almost always "the principle of observing the disappearance rather than the formation of ice, that is, the [[#Melting point measurements|melting point]]."<ref>{{cite journal |last1=Ramsay |first1=J. A. |title=A New Method of Freezing-Point Determination for Small Quantities |journal=Journal of Experimental Biology |date=1 May 1949 |volume=26 |issue=1 |pages=57–64 |doi=10.1242/jeb.26.1.57 |pmid=15406812 |url=http://jeb.biologists.org/cgi/pmidlookup?view=long&pmid=15406812 }}</ref>

==Examples==
{{further|List of elements by melting point}}
[[File: Carboxylic.Acids.Melting.&.Boiling.Points.jpg|thumb|upright=1.3|Melting points (in blue) and boiling points (in pink) of the first eight [[carboxylic acids]] (°C)]]

For most substances, [[melting]] and [[freezing]] points are approximately equal. For example, the melting and freezing points of [[mercury (element)|mercury]] is {{Convert|234.32|K|C F|lk=on|abbr=out}}.<ref>[[#Haynes|Haynes]], p. 4.122.</ref> However, certain substances possess differing solid-liquid transition temperatures. For example, [[agar]] melts at {{Convert|85|C|F K}} and solidifies from {{Convert|31|C|F K}}; such direction dependence is known as [[hysteresis]]. The melting point of ice at 1 atmosphere of pressure is very close<ref>The melting point of purified water has been measured as 0.002519 ± 0.000002 °C, see {{cite journal|author1=Feistel, R. |author2=Wagner, W. |name-list-style=amp |year = 2006 |title = A New Equation of State for H<sub>2</sub>O Ice Ih |journal = Journal of Physical and Chemical Reference Data|volume = 35|issue = 2 |pages = 1021–1047 |doi = 10.1063/1.2183324|bibcode = 2006JPCRD..35.1021F }}</ref> to {{Convert|0|C|F K}}; this is also known as the ice point. In the presence of [[Nucleation|nucleating substances]], the freezing point of water is not always the same as the melting point. In the absence of nucleators water can exist as a [[Supercooling|supercooled]] liquid down to {{Convert|-48.3|C|F K}} before freezing.<ref>{{Cite journal |last=Kringle |first=Loni |last2=Thornley |first2=Wyatt A. |last3=Kay |first3=Bruce D. |last4=Kimmel |first4=Greg A. |date=2020-09-18 |title=Reversible structural transformations in supercooled liquid water from 135 to 245 K |url=https://www.science.org/doi/10.1126/science.abb7542 |journal=Science |language=en |volume=369 |issue=6510 |pages=1490–1492 |doi=10.1126/science.abb7542 |issn=0036-8075|arxiv=1912.06676 }}</ref>

The metal with the highest melting point is [[tungsten]], at {{Convert|3414|C|F K}};<ref>[[#Haynes|Haynes]], p. 4.123.</ref> this property makes tungsten excellent for use as [[electrical filament]]s in [[incandescent lamp]]s. The often-cited [[carbon]] does not melt at ambient pressure but [[sublimation (physics)|sublimes]] at about {{Convert|3700|C|F K|sigfig=2}}; a liquid phase only exists above pressures of {{Convert|10|MPa|atm|abbr=on}} and estimated {{Convert|4,030-4,430|C|F K}} (see [[:File:Carbon basic phase diagram.png|carbon phase diagram]]). [[Hafnium carbonitride]] (HfCN) is a [[refractory]] compound with the highest known melting point of any substance to date and the only one confirmed to have a melting point above {{Convert|4273|K|C F}} at ambient pressure. Quantum mechanical computer simulations predicted that this alloy (HfN<sub>0.38</sub>C<sub>0.51</sub>) would have a melting point of about 4,400 K.<ref>{{cite journal|author1= Hong, Q.-J. |author2=van de Walle, A. |year = 2015 | title = Prediction of the material with highest known melting point from ab initio molecular dynamics calculations | journal = Phys. Rev. B | volume = 92 |issue = 2 | pages = 020104(R) | doi = 10.1103/PhysRevB.92.020104 |bibcode=2015PhRvB..92b0104H |doi-access = free }}</ref> This prediction was later confirmed by experiment, though a precise measurement of its exact melting point has yet to be confirmed.<ref>{{cite journal |last1=Buinevich |first1=V.S. |last2=Nepapushev |first2=A.A. |last3=Moskovskikh |first3=D.O. |last4=Trusov |first4=G.V. |last5=Kuskov |first5=K.V. |last6=Vadchenko |first6=S.G. |last7=Rogachev |first7=A.S. |last8=Mukasyan |first8=A.S. |title=Fabrication of ultra-high-temperature nonstoichiometric hafnium carbonitride via combustion synthesis and spark plasma sintering |journal=Ceramics International |date=March 2020 |volume=46 |issue=10 |pages=16068–16073 |doi=10.1016/j.ceramint.2020.03.158 |s2cid=216437833 }}</ref>  At the other end of the scale, [[helium]] does not freeze at all at normal pressure even at temperatures arbitrarily close to [[absolute zero]]; a pressure of more than twenty times normal [[atmospheric pressure]] is necessary.

{| class="wikitable sortable collapsible"
! colspan=4 |List of common chemicals
|-
!Chemical{{efn-ur|name=fn10}}
! data-sort-type="number" | [[Density]] {{nowrap|1=({{nobold|1={{sfrac|[[Gram|g]]|[[Cubic centimetre|cm<sup>3</sup>]]}}}})}}
! data-sort-type="number" | Melt {{nowrap|1=({{nobold|[[Kelvin|K]]}})}}<ref>{{cite journal|last1=Holman|first1=S. W.|last2=Lawrence|first2=R. R.|last3=Barr|first3=L.|title=Melting Points of Aluminum, Silver, Gold, Copper, and Platinum|journal=Proceedings of the American Academy of Arts and Sciences|date=1 January 1895|volume=31|pages=218–233|doi=10.2307/20020628|jstor=20020628}}</ref> 
! data-sort-type="number" | [[Boiling point|Boil]] {{nowrap|1=({{nobold|K}})}}
|-
| Water @STP || 1 || {{convert|0|C|K|disp=number}} || {{convert|100|C|K|disp=number}}
|-
| [[Solder]] (Pb60Sn40) ||   || {{convert|188|C|K|disp=number}} || 
|-
| [[Cocoa butter]] || || {{convert|34.1|C|K|disp=number}} || -
|-
| [[Paraffin wax]] || 0.9 || {{convert|37|C|K|disp=number}} || {{convert|370|C|K|disp=number}}
|-
| [[Hydrogen]] || 0.00008988 || {{sort|0014|14.01}} || 20.28
|-
| [[Helium]] || 0.0001785 || {{sort|0.1|—}}{{efn-ur|name=fn6}} || 4.22
|-
| [[Beryllium]] || 1.85 || {{sort|1560|1,560}} || 2,742
|-
| [[Carbon]] || 2.267 || {{sort|0.1|—}}{{efn-ur|name=fn11}}<ref name=rsc/> || 4,000{{efn-ur|name=fn11}}<ref name=rsc>{{cite web|url=https://www.rsc.org/periodic-table/element/6/carbon|title=Carbon|website=rsc.org}}</ref>
|-
| [[Nitrogen]] || 0.0012506 || {{sort|0063|63.15}} || 77.36
|-
| [[Oxygen]] || 0.001429 || {{sort|0054|54.36}} || 90.20
|-
| [[Sodium]] || 0.971 || {{sort|0371|370.87}} || 1,156
|-
| [[Magnesium]] || 1.738 || {{sort|0923|923}} || 1,363
|-
| [[Aluminium]] || 2.698 || {{sort|0933.5|933.47}} || 2,792
|-
| [[Sulfur]] || 2.067 || {{sort|0388.4|388.36}} || 717.87
|-
| [[Chlorine]] || 0.003214 || {{sort|0171.6|171.6}} || 239.11
|-
| [[Potassium]] || 0.862 || {{sort|0336.5|336.53}} || 1,032
|-
| [[Titanium]] || 4.54 || {{sort|1941|1,941}} || 3,560
|-
| [[Iron]] || 7.874 || {{sort|1811|1,811}} || 3,134
|-
| [[Nickel]] || 8.912 || {{sort|1728|1,728}} || 3,186
|-
| [[Copper]] || 8.96 || 1,357.77 || 2,835
|-
| [[Zinc]] || 7.134 || {{sort|0693|692.88}} || 1,180
|-
| [[Gallium]] || 5.907 || {{sort|0302.9|302.9146}} || 2,673
|-
| [[Silver]] || 10.501 || 1,234.93 || 2,435
|-
| [[Cadmium]] || 8.69 || {{sort|0594.22|594.22}} || 1,040
|-
| [[Indium]] || 7.31 || {{sort|0429.75|429.75}} || 2,345
|-
| [[Iodine]] || 4.93 || {{sort|0386.85|386.85}} || 457.4
|-
| [[Tantalum]] || 16.654 || 3,290 || 5,731
|-
| [[Tungsten]] || 19.25 || 3,695 || 5,828
|-
| [[Platinum]] || 21.46 || 2,041.4 || 4,098
|-
| [[Gold]] || 19.282 || 1,337.33 || 3,129
|-
| [[Mercury (element)|Mercury]] || 13.5336 || {{sort|0234.43|234.43}} || 629.88
|-
| [[Lead]] ||  11.342 || {{sort|0600.61|600.61}} || 2,022
|-
| [[Bismuth]] || 9.807 || {{sort|0544.7|544.7}} || 1,837
|-
|- class="sortbottom"
| colspan=13 |<div class="mw-collapsible mw-collapsed">
Notes<!-- Footnotes are defined here -->
<div class="mw-collapsible-content">{{notelist|group=upper-roman|refs=
{{efn-ur|name=fn6|Helium does not solidify at a pressure of one atmosphere. Helium can only solidify at pressures above 25 atmospheres, which corresponds to a melting point of absolute zero.}}
{{efn-ur|name=fn10|Z is the standard symbol for [[atomic number]]; C is the standard symbol for [[heat capacity]]; and χ is the standard symbol for [[electronegativity]] on the Pauling scale.}}
{{efn-ur|name=fn11|Carbon does not melt at any temperature under standard pressure, instead it sublimes around 4,100 K}}
}}</div></div>
|}

==Melting point measurements==
{{main|Melting-point apparatus}}
[[File:Koflerbank.jpg|thumb|Kofler bench with samples for calibration]]
Many [[laboratory techniques]] exist for the determination of melting points.
A [[Kofler bench]] is a metal strip with a temperature gradient (range from room temperature to 300&nbsp;°C). Any substance can be placed on a section of the strip, revealing its thermal behaviour at the temperature at that point. [[Differential scanning calorimetry]] gives information on melting point together with its [[enthalpy of fusion]].

[[File:Krüss M5000.jpg|thumb|upright|Automatic digital melting point meter]]
A basic melting point apparatus for the analysis of crystalline solids consists of an [[oil bath]] with a transparent window (most basic design: a [[Thiele tube]]) and a simple magnifier. Several grains of a solid are placed in a thin glass tube and partially immersed in the oil bath. The oil bath is heated (and stirred) and with the aid of the magnifier (and external light source) melting of the individual crystals at a certain temperature can be observed. A metal block might be used instead of an oil bath. Some modern instruments have automatic optical detection.

The measurement can also be made continuously with an operating process. For instance, oil refineries measure the freeze point of diesel fuel "online", meaning that the sample is taken from the process and measured automatically. This allows for more frequent measurements as the sample does not have to be manually collected and taken to a remote laboratory.{{cn|date=May 2023}}

===Techniques for refractory materials===
For refractory materials (e.g. platinum, tungsten, tantalum, some carbides and nitrides, etc.) the extremely high melting point (typically considered to be above, say, 1,800&nbsp;°C) may be determined by heating the material in a black body furnace and measuring the black-body temperature with an optical [[pyrometer]]. For the highest melting materials, this may require extrapolation by several hundred degrees. The spectral radiance from an incandescent body is known to be a function of its temperature. An optical pyrometer matches the radiance of a body under study to the radiance of a source that has been previously calibrated as a function of temperature. In this way, the measurement of the absolute magnitude of the intensity of radiation is unnecessary. However, known temperatures must be used to determine the calibration of the pyrometer. For temperatures above the calibration range of the source, an extrapolation technique must be employed. This extrapolation is accomplished by using [[Planck's law]] of radiation. The constants in this equation are not known with sufficient accuracy, causing errors in the extrapolation to become larger at higher temperatures. However, standard techniques have been developed to perform this extrapolation.{{cn|date=May 2023}}

Consider the case of using gold as the source (mp = 1,063&nbsp;°C). In this technique, the current through the filament of the pyrometer is adjusted until the light intensity of the filament matches that of a black-body at the melting point of gold. This establishes the primary calibration temperature and can be expressed in terms of current through the pyrometer lamp. With the same current setting, the pyrometer is sighted on another black-body at a higher temperature. An absorbing medium of known transmission is inserted between the pyrometer and this black-body. The temperature of the black-body is then adjusted until a match exists between its intensity and that of the pyrometer filament. The true higher temperature of the black-body is then determined from Planck's Law. The absorbing medium is then removed and the current through the filament is adjusted to match the filament intensity to that of the black-body. This establishes a second calibration point for the pyrometer. This step is repeated to carry the calibration to higher temperatures. Now, temperatures and their corresponding pyrometer filament currents are known and a curve of temperature versus current can be drawn. This curve can then be extrapolated to very high temperatures.

In determining melting points of a refractory substance by this method, it is necessary to either have black body conditions or to know the [[emissivity]] of the material being measured. The containment of the high melting material in the liquid state may introduce experimental difficulties. Melting temperatures of some refractory metals have thus been measured by observing the radiation from a black body cavity in solid metal specimens that were much longer than they were wide. To form such a cavity, a hole is drilled perpendicular to the long axis at the center of a rod of the material. These rods are then heated by passing a very large current through them, and the radiation emitted from the hole is observed with an optical pyrometer. The point of melting is indicated by the darkening of the hole when the liquid phase appears, destroying the black body conditions. Today, containerless laser heating techniques, combined with fast pyrometers and spectro-pyrometers, are employed to allow for precise control of the time for which the sample is kept at extreme temperatures. Such experiments of sub-second duration address several of the challenges associated with more traditional melting point measurements made at very high temperatures, such as sample vaporization and reaction with the container.

==Thermodynamics==
[[File:Melting curve of water.svg|thumb|upright=1.45|Pressure dependence of water melting point.]]
For a solid to melt, [[heat]] is required to raise its temperature to the melting point. However, further heat needs to be supplied for the melting to take place: this is called the [[heat of fusion]], and is an example of [[latent heat]].{{cn|date=May 2023}}

From a thermodynamics point of view, at the melting point the change in [[Gibbs free energy]] (ΔG) of the material is zero, but the [[enthalpy]] (''H'') and the [[entropy]] (''S'') of the material are increasing (ΔH, ΔS > 0). Melting phenomenon happens when the Gibbs free energy of the liquid becomes lower than the solid for that material. At various pressures this happens at a specific temperature. It can also be shown that:

: <math>\Delta S = \frac {\Delta H} {T}</math>

Here ''T'', ''ΔS'' and ''ΔH'' are respectively the temperature at the melting point, change of entropy of melting and the change of enthalpy of melting.

The melting point is sensitive to extremely large changes in [[pressure]], but generally this sensitivity is orders of magnitude less than that for the [[boiling point]], because the solid-liquid transition represents only a small change in volume.<ref>The exact relationship is expressed in the [[Clausius–Clapeyron relation]].</ref><ref>{{cite web |url= http://mpec.sc.mahidol.ac.th/RADOK/physmath/PHYSICS/j10.htm |title= J10 Heat: Change of aggregate state of substances through change of heat content: Change of aggregate state of substances and the equation of Clapeyron-Clausius |access-date= 19 February 2008 |archive-date= 28 February 2008 |archive-url= https://archive.wikiwix.com/cache/20080228000000/http://mpec.sc.mahidol.ac.th/RADOK/physmath/PHYSICS/j10.htm |url-status= dead }}</ref> If, as observed in most cases, a substance is more dense in the solid than in the liquid state, the melting point will increase with increases in pressure. Otherwise the reverse behavior occurs. Notably, this is the case of water, as illustrated graphically to the right, but also of Si, Ge, Ga, Bi. With extremely large changes in pressure, substantial changes to the melting point are observed. For example, the melting point of silicon at ambient pressure (0.1 MPa) is 1415&nbsp;°C, but at pressures in excess of 10 GPa it decreases to 1000&nbsp;°C.<ref>Tonkov, E. Yu. and Ponyatovsky, E. G. (2005) ''Phase Transformations of Elements Under High Pressure'', CRC Press, Boca Raton, p. 98 {{ISBN|0-8493-3367-9}}</ref>

Melting points are often used to characterize organic and inorganic compounds and to ascertain their [[wiktionary:Purity|purity]]. The melting point of a pure substance is always higher and has a smaller range than the melting point of an impure substance or, more generally, of mixtures. The higher the quantity of other components, the lower the melting point and the broader will be the melting point range, often referred to as the "pasty range". The temperature at which melting begins for a mixture is known as the ''[[Solidus_(chemistry)|solidus]]'' while the temperature where melting is complete is called the ''[[liquidus]]''. Eutectics are special types of mixtures that behave like single phases. They melt sharply at a constant temperature to form a liquid of the same composition. Alternatively, on cooling a liquid with the eutectic composition will solidify as uniformly dispersed, small (fine-grained) mixed crystals with the same composition.

In contrast to crystalline solids, [[glass]]es do not possess a melting point;
on heating they undergo a smooth [[glass transition]] into a [[viscous liquid]].
Upon further heating, they gradually soften, which can be characterized by certain [[softening point]]s.

==Freezing-point depression==
{{main|Freezing-point depression|Supercooling}}

The freezing point of a [[solvent]] is depressed when another compound is added, meaning that a [[Solution (chemistry)|solution]] has a lower freezing point than a pure solvent. This phenomenon is used in technical applications to avoid freezing, for instance by adding salt or ethylene glycol to water.{{cn|date=May 2023}}

==Carnelley's rule==
In [[organic chemistry]], '''Carnelley's rule''', established in 1882 by [[Thomas Carnelley]], states that ''high [[molecular symmetry]] is associated with high melting point''.<ref>{{cite journal |title= Melting Point and Molecular Symmetry |journal= [[Journal of Chemical Education]] |page= 724 |volume= 77 |issue= 6 |year= 2000 |doi= 10.1021/ed077p724 |author1=Brown, R. J. C.  |author2=R. F. C. |name-list-style=amp |bibcode = 2000JChEd..77..724B }}</ref> Carnelley based his rule on examination of 15,000 chemical compounds. For example, for three [[structural isomer]]s with [[molecular formula]] C<sub>5</sub>H<sub>12</sub> the melting point increases in the series [[isopentane]] −160&nbsp;°C (113 K) [[n-pentane]] −129.8&nbsp;°C (143 K) and [[neopentane]] −16.4&nbsp;°C (256.8 K).<ref>[[#Haynes|Haynes]], pp. 6.153–155.</ref> Likewise in [[xylene]]s and also [[dichlorobenzene]]s the melting point increases in the order [[arene substitution patterns|meta, ortho and then para]]. [[Pyridine]] has a lower symmetry than [[benzene]] hence its lower melting point but the melting point again increases with [[diazine]] and [[triazine]]s. Many cage-like compounds like [[adamantane]] and [[cubane]] with high symmetry have relatively high melting points.

A high melting point results from a high [[heat of fusion]], a low [[entropy of fusion]], or a combination of both. In highly symmetrical molecules the crystal phase is densely packed with many efficient intermolecular interactions resulting in a higher enthalpy change on melting.
[[image:Si(tms)4.png|thumb|right|180 px|Like many high symmetry compounds, [[tetrakis(trimethylsilyl)silane]] has a very high melting point (m.p.) of 319-321 °C.  It tends to sublime, so the m.p. determination requires that the sample be sealed in a tube.<ref name=Gilman>{{cite journal|title= Tetrakis(trimethylsilyl)silane|author1=Gilman, H. |author2=Smith, C. L. |journal=Journal of Organometallic Chemistry|year=1967|volume=8|issue=2 |pages=245–253|doi=10.1016/S0022-328X(00)91037-4}}</ref>]]

==Predicting the melting point of substances (Lindemann's criterion)==
An attempt to predict the bulk melting point of crystalline materials was first made in 1910 by [[Frederick Lindemann]].<ref name="Lindemann1910">{{cite journal |author=Lindemann FA |title=The calculation of molecular vibration frequencies |journal=Phys. Z. |volume=11 |year=1910 |pages=609–612 |author-link=Frederick Lindemann}}</ref> The idea behind the theory was the observation that the average amplitude of thermal vibrations increases with increasing temperature. Melting initiates when the amplitude of vibration becomes large enough for adjacent atoms to partly occupy the same space. The '''Lindemann criterion''' states that melting is expected when the vibration [[root mean square amplitude]] exceeds a threshold value.

Assuming that all atoms in a crystal vibrate with the same frequency ''ν'', the average thermal energy can be estimated using the [[equipartition theorem]] as<ref name=Sorkin>Sorkin, S., (2003), [http://phycomp.technion.ac.il/~phsorkin/thesis/thesis.html Point defects, lattice structure, and melting] {{Webarchive|url=https://web.archive.org/web/20161005221157/http://phycomp.technion.ac.il/~phsorkin/thesis/thesis.html |date=5 October 2016 }}, Thesis, Technion, Israel.</ref>
:<math>
 E = 4\pi^2 m \nu^2~u^2 = k_{\rm B} T
 </math>
where ''m'' is the [[atomic mass]], ''ν'' is the [[frequency]], ''u'' is the average vibration amplitude, ''k''<sub>B</sub> is the [[Boltzmann constant]], and ''T'' is the [[Thermodynamic temperature|absolute temperature]]. If the threshold value of ''u<sup>2</sup>'' is ''c<sup>2</sup>a<sup>2</sup>'' where ''c'' is the [[Lindemann index|Lindemann constant]] and ''a'' is the [[atomic spacing]], then the melting point is estimated as
:<math>
 T_{\rm m} = \cfrac{4\pi^2 m \nu^2 c^2 a^2}{k_{\rm B}} .
 </math>
Several other expressions for the estimated melting temperature can be obtained depending on the estimate of the average thermal energy. Another commonly used expression for the Lindemann criterion is<ref name=Hofmann>{{cite book|author=Philip Hofmann|title=Solid state physics: an introduction|url=https://books.google.com/books?id=XfIpxi4kcM4C&pg=PA67|access-date=13 March 2011|year=2008|publisher=Wiley-VCH|isbn=978-3-527-40861-0|page=67}}{{Dead link|date=August 2023 |bot=InternetArchiveBot |fix-attempted=yes }}</ref>
:<math>
 T_{\rm m} = \cfrac{4\pi^2 m \nu^2 c^2 a^2}{2k_{\rm B}} .
 </math>
From the expression for the [[Debye frequency]] for ''ν'',
:<math>
 T_{\rm m} = \cfrac{2\pi m c^2 a^2 \theta_{\rm D}^2 k_{\rm B}}{h^2}
 </math>
where ''θ''<sub>D</sub> is the [[Debye temperature]] and ''h'' is the [[Planck constant]]. Values of ''c'' range from 0.15 to 0.3 for most materials.<ref name=Nelson>Nelson, D. R., (2002), [https://books.google.com/books?id=YtYFAqswRzUC Defects and geometry in condensed matter physics], Cambridge University Press, {{ISBN|0-521-00400-4}}</ref>

== Melting point prediction==
In February 2011, [[Alfa Aesar]] released over 10,000 melting points of compounds from their catalog as [[open data]]. This dataset has been used to create a [[random forest]] model for melting point prediction which is now freely available.<ref name=LangGuha>[http://www.qsardb.org/repository/predictor/10967/104?model=rf Predict melting point from SMILES]. Qsardb.org. Retrieved on 13 September 2013.</ref> Open melting point data are also available from ''[[Nature Precedings]]''.<ref name=Williams>{{cite journal |last1=Bradley |first1=Jean-Claude |last2=Lang |first2=Andrew |last3=Williams |first3=Antony |last4=Curtin |first4=Evan |title=ONS Open Melting Point Collection |journal=Nature Precedings |date=11 August 2011 |doi=10.1038/npre.2011.6229.1 |doi-access=free }}</ref> High quality data mined from patents and also models<ref name=OCHEM>[http://ochem.eu/article/99826 OCHEM melting point models]{{Dead link|date=February 2024 |bot=InternetArchiveBot |fix-attempted=yes }}. ochem.eu. Retrieved on 18 June 2016.</ref> developed with these data were published by Tetko ''et al''.<ref name=Tetko>{{cite journal | doi = 10.1186/s13321-016-0113-y | title = The development of models to predict melting and pyrolysis point data associated with several hundred thousand compounds mined from PATENTS | journal = Journal of Cheminformatics | volume = 8 | year = 2016 | last1 = Tetko | first1 = Igor V | last2 = m. Lowe | first2 = Daniel | last3 = Williams | first3 = Antony J | pages = 2 | pmc = 4724158 | pmid=26807157 | doi-access = free }}</ref>

== Melting point of the elements ==
{{main|Melting points of the elements (data page)}}
{{Periodic table (melting point)}}

==See also==
{{colbegin}}
* [[Boiling point]]
* [[Congruent melting]]
* [[Hagedorn temperature]]
* [[Hafnium carbonitride]], a compound with the highest known melting point
* [[List of elements by melting point]]
* [[Melting points of the elements (data page)]]
* [[Phase diagram]]
* [[Simon–Glatzel equation]]
* [[Slip melting point]]
* [[Triple point]]
* [[Zone melting]]
{{colend}}

== References ==

=== Citations ===
{{Reflist}}

=== Sources ===
{{refbegin}}
; Works cited
* {{cite book |ref = Haynes |editor-last = Haynes |editor-first = William M. |year = 2011 |title = CRC Handbook of Chemistry and Physics |edition = 92nd |publisher = CRC Press |isbn = 978-1439855119 }}
{{refend}}

==External links==
* [https://archive.org/details/meltingboilingpo01carnuoft Melting and boiling point tables vol. 1] by Thomas Carnelley (Harrison, London, 1885–1887)
* [https://archive.org/details/meltingboilingpo02carnuoft Melting and boiling point tables vol. 2] by Thomas Carnelley (Harrison, London, 1885–1887)
* [http://ochem.eu/article/99826 Patent mined data]{{Dead link|date=February 2024 |bot=InternetArchiveBot |fix-attempted=yes }} Over 250,000 freely downloadable  melting point data. Also downloadable at [https://figshare.com/articles/Melt-ing_Point_and_Pyrolysis_Point_Data_for_Tens_of_Thousands_of_Chemicals/2007426 figshare]

{{State of matter}}
{{Use dmy dates|date=October 2015}}

{{DEFAULTSORT:Melting Point}}
[[Category:Atmospheric thermodynamics]]
[[Category:Physical quantities]]
[[Category:Phase transitions]]
[[Category:Threshold temperatures]]