Unveiling the Mysteries of the Melting Point of a Diamond

The melting point of a diamond certainly isn’t a common discussion, which makes it all the more interesting. Diamonds are famous for their glitter as well as their hardness. Naturally, they are not devoid of other extraordinary properties, say, like physical properties. Out of all the wonderful features a diamond possesses, the melting point of a diamond is one which strikingly captures the attention of a lot of researchers and scientists, and so it has been a debated topic for such a long time. What happens to a diamond when it is exposed to conditions that can melt its atomic bonds and deeply pressurize the bonds inside the carbon? In today’s article, I will be diving deeper into articulating and analyzing the scientific theories that revolve around the concept of diamonds and their near-impossible melting temperature. I will explain the intense heat and pressure and the atomic structure that ultimately works on bringing such an awe-inspiring form of material into existence. Get ready for an interesting thesis of the captivating world we live in and the very principles of both physical science and nature that shape our understanding of earth science.

Can Diamonds Be Melted?

Indeed, diamonds can be melted, however, it requires meticulous circumstances. A diamond can melt at about 4,027 degrees Celsius (7,280 degrees Fahrenheit), but at normal atmospheric conditions, it also vaporizes into carbon gas. Melting a diamond without vaporization requires immense systems of pressure, like those present deep within the earth. This transformation allows the diamond to change into liquid without disintegrating into other forms of carbon. This phenomenon underscores the distinct and powerful structural resilience of a diamond as a material, which is made of carbon in its hardest form.

Understanding the Structure of Diamond

Diamonds are made up of carbon atoms arranged in a three-dimensional lattice structure. Each carbon atom is bonded to four other carbon atoms through strong covalent bonds, forming a solid three-dimensional model that resembles a pyramid. This is the reason why diamonds are extremely hard, have elevated thermal conductivity, and exhibit enhanced optical clarity. The strong and compact internal structure significantly reduces internal weaknesses, so carbon structures are considered one of the hardest materials, which is also a factor for their higher melting point. This astonishing structure, along with the strength of the bonds, makes diamonds extremely rigid.

Why Diamonds Cannot Melt in Lava

Diamonds are incapable of melting in lava because the conditions needed to sever their atomic bonds and the diamonds’ melting points are unparalleled. Since diamonds are practically carbon, they require a pressure of approximately 4,027 degrees Celsius (7,280 degrees Fahrenheit) for their melting point, but under ordinary atmospheric pressure, they don’t melt; they sublime directly into gas around 3,547 degrees Celsius (6,416 degrees Fahrenheit).

Lava ranges from approximately 700 to 1,200 degrees Celsius (1,292 to 2,192 degrees Fahrenheit), depending on the type of lava. Even the most extreme surface flowing lava on Earth is nowhere near the temperature required to shatter the rigid covalent bonds of diamonds. These covalent bonds, which are arranged in a tetrahedral crystal lattice configuration, are some of the strongest bonds known to man, thus further fortifying the stability of diamonds under severe conditions.

Also, for a diamond to melt, it would need both exceedingly high temperatures and enormous pressure, such as what is found deep within the earth’s mantle where diamonds are formed. The surface does not offer these conditions. Rather than melting, with lava, a diamond with sufficient oxygen might slowly oxidize and degrade, turning into carbon dioxide gas. This illustrates the astounding strength, both physically and chemically, that diamonds possess on Earth.

The Role of Pressure in Melting Diamonds

In preventing diamonds from melting under natural conditions, pressure is perhaps the most vital factor. At room temperature and standard atmospheric pressure, diamonds remain stable due to the strong covalent bonds between the carbon atoms within the crystalline lattice. However, in industrial settings or controlled laboratory settings, diamonds require a combination of pressures above 5 GigaPascals (GPa) and temperatures near 4,000 Kelvin (K) to achieve a molten state. This is roughly 50,000 times the pressure of Earth’s atmosphere at sea level.

Such extreme pressure closely matches the conditions deep within the Earth’s mantle where diamonds naturally form. The temperature and pressure ranging from 1100 °C to 1400 °C at the depth within the Earth’s mantle of 150 to 200 kilometers ensure that carbon crystallizes into diamond rather than existing in other allotropes like graphite. The combination of these extreme temperatures and pressures is precisely the reason that diamonds can only be subjected to melting or significant structural changes in highly specialized experimental environments or the deepest geological formations on Earth.

What is the Melting Point of a Diamond?

The Highest Melting Point Among Materials

Because of the extreme hardness, it possesses the highest melting point, approximately 3550 degrees Celcius or 6422 degrees Fahrenheit, of any known natural material. This number does change significantly at different pressure conditions, however. For instance, the pressure within the Earth’s mantle allows for the melting point of diamond to exceed 4000 degrees Celcius or 7232 degrees Fahrenheit. This remarkable liability can be attributed to the crystal lattice structure and bonding framework of the diamond, which is greatly covalently bonded.

Not only does this trait showcase diamonds durability, but it also makes it agreeable for other applications that require a high thermal resistance material. Some areas where it is used directly are cutting tools or in high-performance electronics. In addition to this, it can withstand degradation unlike any other material at elevated temperatures, which makes it useful to fields where most conventional substances fail. While diamonds’ extreme attributes drive research into the use of the substance for high-pressure technology, its thermal conductivity further adds to other uses in the circuitry.

Comparing Graphite and Diamond

Diamonds and graphite are two vastly different substances about physical and chemical properties. This is because diamonds have a different atomic structure compared to graphite. The carbon atoms in graphite form hexagonal crystalline structures, and they generate layers that are stacked on top of each other. These layers are soft and can slide on each other easily due to weak van der Waals forces that hold them together. This allows graphite to be lubricative and soft. On the other hand, the carbon atoms in a diamond are arranged in a tetrahedral lattice structure in which each carbon atom covalently bonds with four other carbon atoms. This creates a dense network of rigid carbon atoms. This is the reason why diamonds have unparalleled hardness and high mechanical strength.

Graphite serves many purposes, like electrodes, batteries, and even lubricants, due to the free electrons in their structure. This makes graphite an excellent electrical conductor. Contrary to graphite, diamonds have exceptional insulating properties. However, they are renowned for being a thermal conductor, due to their extremely high thermal conductivity value that exceeds 2000 W/m·K. This makes diamonds essential for heat dissipation in high-performance systems.

Graphite is relatively available and cheap from an industrial point of view, making it suitable for use in steel, pencils, and refractories. Natural and synthetic diamonds are much rarer and more expensive, mostly employed in high-end cutting devices, abrasives, and laser optical systems. Regardless of these materials’ differences, enhanced methods of synthetic production are broadening the scope of both materials, providing numerous industry-specific solutions.

Factors Affecting the Melting Point of Diamond

The melting point of diamonds is determined by several of the following key conditions:

• Pressure: Diamonds, in order to retain their crystalline structure at high temperatures, need to be subjected to extremely high pressures. In the presence of atmospheric pressure, diamonds do not melt, rather, transform into graphite.
• Temperature: If there is a controlled amount of pressure, then diamonds can be melted at temperatures higher than 4,000 Kelvin (close to 6,740 °F).
• Purity of the diamond: Impurities contained within the diamond lattice may affect its melting behavior thus altering the temperature at which certain structural changes take place.

These reasons mark the remarkable stability of a diamond’s atomic structure and the extreme conditions needed for the melting of a diamond.

Can Lava Melt a Diamond?

Exploring Temperature and Pressure Conditions

The carbon atoms in a diamond are bonded together in a stable crystal lattice which makes diamonds extremely durable. That structure gives diamonds the ability to survive the most extreme conditions without succumbing to break down easily. When determining if something like lava can melt a diamond, one must consider the temperature and pressure conditions because diamonds are known to be incredibly hard and nearly impossible to melt.

Depending on the type, lava tends to have a temperature range between 1200 to 2200 degrees Fahrenheit, which is between 650 to 1200 degrees Celsius. While cycles of extreme heat exist, these temperatures are considerably lower than the melting point of a pure diamond, which is roughly 4,027 degrees C or 7,280 degrees F under normal barometric pressure. The bold temperature difference suggests that lava, in all its molten glory, does not stand a chance at melting diamonds in ordinary conditions.

The melting point of diamonds is likely to be influenced by the high-pressure scenarios found deep within the earth’s mantle. There is most certainly strong pressure in areas like mantle plume regions, but that pressure needs to be accompanied by extreme temperature conditions in order for carbon-based materials to function properly. Still, even with these scenarios, studies suggest the conditions needed to melt diamonds are far beyond anything a volcanic site can naturally incur.

Therefore, the interplay between a diamond’s thermal stability and the relatively low temperature of lava guarantees that diamonds will not be damaged in these situations. This extraordinary material can only be melted under very high temperatures and pressure, which can only be artificially done, such as in laser cutting or in specialized industrial settings.

Why is Diamond the Hardest Substance

The reason diamond withstands scratching is due to its distinguished crystal structure, called a covalent network. Within a diamond crystal, a carbon atom is covalently bonded to four additional carbon atoms, creating a tetrahedral lattice. The position of the atoms in a diamond crystal lattice structure is fixed with respect to each other, which renders the crystal more or less incompressible; this is also known as a diamond lattice. The value of a diamond’s bond strength within the lattice, which is approximately 347 kJ/mol, is what enables it to be determined as the hardest naturally occurring substance.

In the Meric system’s grade of hardness, a diamond has a score of 10, which denotes the highest level. This indicates that diamond is capable of scratching every other material, even those deemed hard sapphires and rubies, which are 9 on the Mohs hardness scale. Also, diamond surpasses most other materials as it has an indentation hardness of about 60-120 GPa with the Vickers hardness testing method.

The uncommon nature of a diamond’s hardness does not stop at its occurrence in nature. Diamonds created by humans, using processes like High Pressure, high temperature (HPHT) or Chemical Vapor Deposition (CVD), can achieve comparable, if not greater, hardness due to environmental conditions that mimic crystal-forming processes found in nature. These synthetic diamonds are frequently used in industry, like cutting, grinding, and drilling, due to their high durability and resistance to wear.

Other factors like temperature and pressure also help in stabilizing the hardness of a diamond. A diamond’s equilibrium or bottom point is far beneath the earth’s surface at 900-1,300°F (500-700°C), where the temperature and pressure reach a staggering 725,000 pounds per square inch (over 5GPa). These extreme conditions help a diamond achieve its robust lattice formation instead of shifting into a softer material like graphite, which is a carbon compound that’s more stable under standard conditions.

Other than this, there’s ongoing research indicating that the hardness of a diamond has no limits. Some studies suggest that nanocrystalline diamonds contain greater mechanical properties due to having a smaller grain size which reduces imperfections. With these new findings, it’s clear that diamonds will continue to be a useful material for science technology and industry due to their unparalleled characteristics.

The Substance That Challenges Lava

Tungsten is frequently at the top of the list when dealing with elements that can endure extreme conditions such as molten lava, considering SEM images shows its astonishing melting point to be 6192°F or 3422°C. As one of the most heat stubborn elements present, its thermal stability makes tungsten extremely useful in aerospace and manufacturing industries, due to its unrivaled value at high temperatures.

Aside from Tungsten’s ability to withstand heat, one of its most head-turning properties is its exceptional tensile strength. Possessing a high density of nearly 19.25 g/cm³ enables these remarkable properties to make tungsten extremely useful in high-stress environments. Due to these characteristics, tungsten alloys are commonly used in the construction of burn-resistant rocket nozzles and protective reentry systems for spacecraft.

These boundaries are accompanied by an even more staggering value, which comes from an alloy of tungsten and carbon called tungsten carbide. With a melting point a bit lower than pure tungsten, its significantly stiffer state, around 9 on the Mohs scale, enables it to be widely used in drilling and mining tools that can withstand extremely abrasive environments. These characteristics show us why tungsten is trusted more than any other material for extreme applications, such as contact with molten lava or industrial furnaces. As scientists continue to unlock the potential of tungsten through material science, they are constantly redefining its use in extreme conditions.

How is Diamond Melted in Laboratories?

The Process of Burning and Melting a Diamond

One of the most thermally stable natural materials is a diamond, which is formed from crystanline carbon. Because of the unique physical and chemical properties of diamonds, such as their extreme hardness and high sublimation point, the processes of burning or melting a diamond becomes very complex. However, while controlled laboratory conditions, both diamond burning and melting is achievable through certain methods.

Diamond burning involves igniting the diamond in an oxygen atmosphere at 1562°F (850°C), which causes it to burn. A diamond will also burn when exposed to high temperatures, like a laser, or being surrounded by an oxygen-rich environment. During the process, the diamond undergoes burning, which permits its carbon atoms to react with oxygen to yield carbon-dioxide gas. Shefl combustion will occur, meaning that no products will remain. In a laboratory setting, researchers aim to burn the diamond in rather safe manner by using vacuum chambers or controlled oxidation environments to prevent any excess oxygen from flowing in.

Melting a diamond requires very specific conditions as it cannot turn into liquid form under standard atmospheric pressure. Instead, diamonds turn ino liquid when the temperature is raised to 7092°F (3936°C). With the aid of sophisticated tools, diamonds undergo immense pressure which allow them to melt, such as diamond anvil cells which work by applying over 10 GPa (megapascals) of pressure.

While conducting scientific research, these methods assist the scholars in comprehending the atomic arrangement, as well as the thermal stability of diamonds. The outcomes hold major importance in materials science and fields that need strong carbon materials.

Creating Liquid Diamond in Controlled Settings

Experimental Practices and Procedures

The process of obtaining liquid diamonds necessitates a combination of pressure and temperature that needs to be simulated in labs. Studies show that diamonds start to flow at a maximum of 10 GPa (gigapascals) of pressure and at above 4000 K (kelvin). These procedures are done using diamond anvil cells (DACs), which can compress sample pieces to unfathomable pressures. In order to control the temperatures more efficiently, laser heating systems are affixed to the DACs so that the sample is heated to the right temperature for it to turn to a liquid.

Every experiment is fused with spectroscopic approaches, which monitor and track the changes in the diamond structure throughout the experiment. The tracking indicates a shift from the solid crystalline form to a more disordered liquid form and a change in the bonding and density. This high-energy state of carbon displays unique properties, including exceptional electrical conductivity and structural fluidity, which makes it suitable for a variety of applications.

Liquid Diamonds Possible Uses

The study of liquid diamonds offers possibilities in high-pressure physics, liquid electronics, and materials science. It has unique properties, which could mean that liquid diamonds can be achieved in the creation of new super-hard coatings and electronic systems that operate under extreme conditions. Additionally, studying carbon at such extreme pressures aids in understanding the core components of many planets, such as the gas giants Jupiter and Saturn, where these conditions may exist.

These experiments are aimed at extreme conditions of material science. They are very useful not only in the practical world, but in theoretical modeling as well.

Advanced Techniques for Melting Diamonds

To melt diamonds, one has to create high temperature and pressure extremes. This is usually done with high-pressure devices like diamond anvil cells associated with laser systems that offer focused heating. To transmute diamond to its liquid form, the temperature must surpass 4,000 Kelvin, with pressure of approximately 10 to 20 GPa. These settings help ensure precision and control so that researchers can observe the material’s behavior under those conditions.

Why Does Diamond Turn into Graphite?

Understanding the Phase Diagram of Carbon

From the phase diagram of carbon, we observe that diamond changes to graphite at specific temperature and pressure. Under standard atmospheric pressure, graphite is the most stable form of carbon. Although diamond is metastable, it requires a high energy barrier for structural transformation. Under increased temperature and lower pressure, however, thermodynamic stability is achieved, and diamond reverts to graphite. This illustrates the effect of environmental conditions on the structural phases of carbon and how diamonds can form under extreme conditions.

The Transition from Diamond to Graphite

The conversion of diamond to graphite is thermodynamically favorable due to a free energy reduction because graphite is the most stable carbon allotrope under standard conditions. It is mainly a function of temperature and pressure. Research suggests that the conversion is easiest for diamonds at elevated temperatures of 1500 – 2000 degrees Celsius and pressures below 2 GPa, conditions which lie outside the stability field for diamonds.

The atomic-level detail involves the breaking of bonds between the sp³ hybridized carbons in the diamond lattice and their donning of the sp² planar hybrid arrangement characteristic of graphite. This energy barrier is surpassed by vibrational energy at elevated temperatures that ease the kinetic stability associated with diamonds. This rearrangement results in the formation of other disordered intermediate phases indicative of the complex nature of the transition.

Trace impurities and defects in the diamond lattice are known to disrupt the structure and speed up the change. Experimental data supports these claims. This demonstrates the role of external catalysts and other imperfections of the lattice in these phase shifts. With each step in computational modeling, further understanding of the energetic pathways and diamond’s behavior under different environmental conditions evolves.

Implications of High Temperature and Pressure

The use of heat treatment under high temperature and pressure (HTHP) greatly impacts the field of material science, especially when it comes to the synthesis and modification of substances such as diamonds, graphites, and other carbon compounds. The carbon lattice can undergo additional significant changes in structure given roughly 1500°C and using over 5 GPa of pressure. These unfavorable conditions are crucial to the industrial synthesis of diamonds as they allow for tailored attribute graphite conversion to diamonds, and the enhanced melting diamonds have numerous other uses.

The study on HTHP conditions has shown that there is a need for specific parameters to enable phase shifts, but also for the size of the crystals, their shapes, and even the amount of defects within the crystals of synthetic materials. Observed phenomena include better optical and mechanical properties of the diamonds, as well as stronger resistance to damages from thermal event such as explosions, windows, and other hostile controllable environments, thanks to the precise control of the temperature gradient that decreases the formation of defects. The refinement of the multi-anvil press and the diamond anvil cell has allowed precise condition replication, enabling scientists to have better control over these features.

Insights from recent studies indicate that heating carbon to more than 2000°C and applying a force of nearly 7 GPa triggers its structural transition to diamond lattices, maximizing its hardness and thermal conductivity. These insights highlight the need for a better understanding of the thermodynamic and kinetic boundaries of these processes and for life technologies that can support and monitor HTHP conditions. Such understanding is critical not only in the engineering of advanced materials but also in natural materials like those found in the Earth’s mantle.

Frequently Asked Questions (FAQs)

Q: Which material has the highest melting point, and how does a diamond fare? 

A: Among all metals, tungsten holds the record for the highest melting point of roughly 3422 °C; however, under high pressure conditions, diamonds surpass this, with an estimated melting point at around 4500 degrees Celsius. That said, diamonds actually do not melt at normal atmospheric pressure levels but instead combust around 700-800°C, transforming directly to carbon dioxide and carbon monoxide. The exceptional melting point of diamonds is attributed to their crystal structure, where carbon atoms bond covalently to four neighboring carbon atoms in a tetrahedral lattice. The energy required to break such bonds is enormous.

Q: What happens to a diamond when it is warmed to extreme temperatures? 

A: If a diamond is heated to extremely high temperatures, around 700°C – 800°C, while oxygen is present in the atmosphere, it will not melt but turn into carbon dioxide as it burns. However, if a diamond is heated to approximately 4500°C and high pressure (around 10 GPA) is applied, it can melt and turn into liquid carbon. This process is remarkably difficult, as diamonds are the hardest substance on Earth. This transition is seldom witnessed in nature because it’s exceptionally hard to maintain such extreme conditions. In most environments, diamonds will oxidize before reaching the melting point.

Q: What are the basic physical characteristics that are responsible for the unique melting characteristics of diamonds?

A: Melting diamonds is a very uncommon occurrence due to several striking physical features that emerge when heat is applied. To begin, a diamond is an atomically rigid structure consisting of a three-dimensional network of carbon atoms linked together via covalent bonds. This structure offers significant strength, and thus, a substantial amount of energy is needed to break it apart. Another reason why it is rare to find a melted diamond is because of its high thermal conductivity. This allows the stone to dissipate heat instead of absorbing it, which would facilitate melting. A third reason would be the bonds formed through the diamond structure’s electron configuration, which is extremely stable. Collectively, these features explain why diamonds can withstand enormously high temperatures, consequently classifying it as one of the most thermally resistant naturally occurring materials on Earth.

Q: What measures do scientists employ to study the melting of diamonds, considering they give off carbon dioxide when heated?

A: Scientists try to manage the oxidation state (where diamonds turn into carbon dioxide) of their environment by studying diamond melting in the absence of oxygen at very high pressures, particularly utilizing z machines to mimic these scenarios. They possess instruments such as diamond anvil cells with laser heating systems that can simultaneously apply over 10 GPa pressure and 4,500°C temperature. Some researchers use computer simulations to represent the behavior of carbon under such extreme conditions. Also, they may analyze diamonds encased in inert gas or void chambers to stop oxidation reactions for viewing phase changes.

Q: How does burning a diamond differ from melting it?

A: The process of burning a diamond involves the oxidation of the carbon atoms in the diamond structure. Oxygen reacts with and sheds two carbon atoms from the diamond structure, resulting in exothermic energy as carbon dioxide is produced. Combustion sets in at 700-800°C in air, representing a change in state where carbon bonds are destroyed and new bonds to oxygen are formed. In contrast, melting is a phase change where the solid diamond would melt into liquid carbon and remain compositionally pure carbon. There’s no burning a diamond at that temperature. The theoretical melting point of diamonds is much higher than the temperature of burning diamonds, explaining why jewelers can identify real gemstones using flame tests without risking damage to genuine stones.

Q: Is it possible for other planets to have diamond oceans due to differing atmospheric pressure?

A: Theoretical models suggest that with the right combination of high pressure, high temperature, and carbon content, certain planets and some exoplanets might have the capacity to host liquid carbon or ‘diamond rain. Gas giants like Uranus and Neptune could have certain layers that, under extreme conditions, may host carbon in the form of *liquid diamonds*, also known as ‘diamond oceans’ and ‘diamond rain’. To consider the existence of true liquid diamond oceans, the planets would need an atmospheric pressure thousands of times greater than Earth’s, along with 4500 degree celsius temperature, and no oxidising elements to convert the carbon into compounds instead of leaving it as pure carbon. Even though the existence of such exotic diamond oceans is very fascinating, finding concrete evidence for it is still a long shot.

Q: Why does diamond have the most corrosion resistance to gemstones in comparison to other gemstones?

A: The reason for a diamond’s high resistance to corrosion lies in the fact that it is a form of carbon with a highly stable tetrahedral crystal lattice structure. This structure has no weak bonds or reactive sites that acids or other corrosive materials could attack. Pots and pans that contain metal ions are complex structures and minerals, but diamond has a homogeneous composition of pure carbon with strong covalent bonds. This means that it is omn chemically inert to most acids and bases. When combined with exceptional engineering properties such as turbulence and toughness, the diamond retains its core brilliance for centuries. Exposed to environmental conditions that gemstones cannot withstand, while enduring years of wear, the diamond still evades erosion.

Q: Which temperature and pressure conditions allow for the melting of diamonds in laboratory environments?

A: In laboratory settings, diamonds are said to be ‘melted’ under very severe conditions of somewhere around 4500 degree Celsius and 10 GPa(roughly 100,000 atmospheres). These conditions are only met using extreme precision tools like laser-heated diamond anvil cells or high-pressure tools alongside intense heating mechanisms. If there is not enough pressure, diamonds will transform into graphite and then oxidize into carbon dioxide instead of melting. The difficulty in attaining and sustaining such conditions explains why, despite a lot of scientific interest in the properties of carbon in its liquid state, diamonds are rarely produced or studied.

Q: How do scientists measure the melting point of diamonds while considering their extreme temperature requirements?

A: The melting point of diamonds can be measured using some methods like a laser-heated diamond anvil cell, which can apply high pressure (greater than 10 GPa) and temperatures of 4500 degrees Celsius. Scientists use X-ray diffraction, which reveals different crystal structures, to monitor phase transitions, along with other spectroscopic techniques that measure shifts in atomic configurations and even direct inspection using specialized optical systems. Computer simulations have also become very important, allowing scientists to virtually test the behavior of carbon atoms under intense conditions without having to actually do any physical experiments. These methods together have greatly improved our understanding of melthing points of diamonds.

Reference Sources

1. “Laser-flash Sealing of Melting Diamond in a Diamond Cell”

• Authors: L. Yang et al.
• Journal: High Pressure Research
• Published Date: 2022-12-27
• Citation Token: (Yang et al., 2022, pp. 1–14)
• Summary: This work analyses how diamond melts under high pressure with the use of laser-flash heating techniques. The authors performed experiments to test the melting temperature of diamonds at different pressures up to 50 GPa. It was discovered that the melting point of diamond is particularly sensitive to pressure and that it is much higher than previously accepted values. The study used in-situ x-ray diffraction and electron microscopy to observe the phase changes and melting processes of diamond to understand the characteristics of carbon at extreme conditions.

2. “High-pressure melting experiments of Fe3S and a thermodynamic model of the Fe–S liquids for the Earth’s core”  

• By Samuel Thompson et al.
• Published In: Journal of Physics: Condensed Matter
• Date of Publication: July 19, 2022
• Citation Token: (Thompson et al. 2022)
• Summary: This research was undertaken with iron sulfide as the center focus. However, this study also looks into the melting of diamond in high-pressure environments. The authors performed high-pressure melting experiments alongside developing a thermodynamic model to explain the melting points of a number of materials, diamond included. Their results indicate that the melting point of diamond is susceptible to changes due to pressure, as well as other elements modifying its environmental conditions.

3. Melting point

4. Diamond