Graphite: Properties, Occurrence and Applications

Graphite is one of the three crystalline forms of the element carbon; the other two being diamond and fullerenes (which include carbon nanotubes and graphene). Graphite occurs naturally in the earth and, under standard conditions, is the most stable form of carbon [1]. This mineral is used in a diverse number of applications from pencils to lubricants and batteries to other more extreme applications, such as nuclear fusion and the Wendelstein 7-X fusion reactor [2].

Here, you will learn about:

  • The properties of graphite
  • Graphite vs diamond
  • How graphite is formed
  • The applications of graphite
  • Graphene and future applications

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Properties of graphite

Graphite is a naturally occurring form of the element carbon (Element 6, symbol C). It is black to steel grey in colour, opaque, and with a distinctive soft lubricative texture [1]. Graphite exhibits two crystalline structures; hexagonal (alpha) and rhombohedral (beta). Both crystalline structures exhibit a high degree of anisotropy, which heavily determine graphite's properties, especially electrical and mechanical [3].

Graphite is recognised for being an excellent conductor of heat and electricity, for exhibiting the highest natural strength and stiffness over all other minerals, for resistance to chemical attack and for withstanding high temperatures (higher than 3600 °C (6500 °F)).

Some of the most relevant physical, thermal, and mechanical properties of graphite are presented in the tables below [4].

Table 1. Properties of graphite.

Physical Properties of Graphite

Crystalline form

Hexagonal, rhombohedral


Black to steel grey

Lattice parameters

a0= 2.46 Å

c0 = 671 Å

Density (at 300 K, 1 atm)

2.26 g/cm3

Atomic volume

5.315 cm3/mol

Triple point

4200 K (3930 °C)

Boiling point

4560 K (4290 °C)

Heat of fusion

46.84 KJ/mol

Heat of vaporisation to monoatomic gas

716.9 KJ/mol

Thermal Properties of Graphite

Standard entropy (at 25°C):

5.697 – 5.743 J/mol*K

Entropy DS298

152.3 J/mol*K

Enthalpy DH298

716.88 KJ/mol

Specific heat capacity (at 25°C)

0.690 – 0.719 kJ/kg*K

Thermal conductivity (at 25°C)

398 W/m*K in ab direction

2.2 W/m*K in c direction

Mechanical Properties of Graphite

Elastic modulus

8 – 15 GPa

Compressive strength

20 – 200 MPa

Flexural strength

6.9 – 100 MPa

Coefficient of thermal expansion

1.2 – 8.2 x10-6 °C

Graphite vs diamond

Graphite and diamond have very different atomic structures. The carbon atoms in diamond are arranged tetrahedrally in a three-dimensional structure composed by an infinite network of atoms. The mechanically strong tetrahedral structure accounts for its excellent properties including extremely high hardness, strength, durability, and thermal conductivity. Diamond is the hardest material on the Mohs scale.

In comparison, the carbon atoms in graphite are arranged in a two-dimensional infinite network of graphene sheets, which are stacked on top of one another to form a three-dimensional structure. This planar structure of graphite accounts for its distinct physical properties. Graphite is widely used in pencils because its layers can easily cleave, or separate. The hardness of graphite is less than 1 on the Mohs scale. Due to its layered structure, graphite has highly anisotropic properties. For example, its thermal conductivity is 398 W/m.K parallel to the layers, yet only 2.2 W/m.K perpendicular to them. Graphite, unlike diamond, is a relatively good electrical conductor and absorber of light [5].

Occurrence of graphite

Graphite is formed when carbon in the Earth’s crust and upper mantle is subjected to high heat and pressure. Most of the graphite found on the Earth’s surface is present at the plate boundaries where deposits of shales and limestone are subjected to heat and pressure by regional metamorphism.

When found in high concentration in rocks, graphite can be mined and crushed until it releases graphite flakes. Some graphite forms from the metamorphism of coal seams, where the seams correspond to the original layer of coal.

Other small amounts form by reaction of carbon compounds during hydrothermal metamorphic processes. In this form, graphite is highly crystalline. 

A very small amount occurs as the primary mineral in igneous rocks such as basalt flow, syenite, and pegmatite. 

Lastly, a small amount of graphite has been found in iron meteorites [6]. 

The world's top graphite-producing countries include China, Brazil, Madagascar, Canada and India.

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Applications of graphite

Some of the most common uses and applications of graphite are:

Writing and art applications

Graphite has been used as writing material since the sixteenth century. Pencils are the oldest and most recognized of its applications and consist of a mixture of graphite flakes and clay as a bonding material.


The carbon atoms form a strong structure arranged in layers and since the bonds between layers are relatively weak, the graphite exhibits a low shear strength when subject to friction. Therefore, graphite can be used as a solid lubricant [7].


Graphite is commonly used as refractory material (meaning it is resistant to decomposition under extreme conditions) due to its high heat conductivity and mechanical stability at high temperatures without suffering chemical changes [8].

Lithium-Ion batteries

The anode in lithium-ion batteries is made from graphite. The graphite anode is manufactured from flake or synthetic graphite [8].

Graphene technology

Graphite can be used as the source material for graphene, which consists of individual carbon layers. For its weight, graphene is stronger than steel [8]. Some authors have referred to it as the “thinnest, strongest, and most conductive material” to electricity and heat [9].

Graphene and its future applications

Research and business are both interested in graphene technology due to its impressive structural and physical characteristics. Graphene technology under development includes medical implants, precise sensors, biosensors, air filters, anti-corrosion coatings and paints, and efficient electronic devices such as smartphones [9].

In 2020, Korean researchers developed a graphene biosensor capable of detecting the COVID-19 virus in under a minute.

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[1] J. P. Rafferty, “Graphite Carbon,” Encyclopedia Britannica,  [Online]. [Accessed April 19, 2020].

[2] J. Hanania, “Graphite,”, University of Calgary, Energy Education, [Online]. [Accessed April 19, 2020].

[3] I. Suarez-Ruiz and J. C. Crelling, Applied Coal Petrology, Elsevier, 2008.

[4] “Graphite,” Earth Science Museum, University of Waterloo, [Online]. Available:, [Accessed May 5, 2020].)

[5] M. Rossi, “How can graphite and diamond be so different if they are both composed of pure carbon?,” Scientific American,  October 9, 2007. [Online]. [Accessed April 19, 2020].

[6] H. M. King, “Graphite,”, [Online], [Accessed April 19, 2020].

[7] H. Wang,  “Graphite Solid Lubrication Materials,” in Encyclopedia of Tribology, Springer, Boston, MA, 2013.

[8] M. Kielmas, “What Are the Uses of Graphite?,” Sciencing, April 05, 2018 [Online]. [Accessed April 19, 2020].

[9] “Graphene applications: what is graphene used for?,”, Metalgrass LTD, Dec. 9 2019 [Online]  [Accessed April 19, 2020]

How was graphite discovered?

At the beginning of the sixteenth century, a significant large deposit of graphite was discovered at a site named Seathwaite Fell in Cumbria, North England. This deposit of graphite was notable for its purity and remains the only deposit of graphite in solid form ever found. To the locals it resembled coal but they found it would not burn. Instead, as it would leave a black mark, they decided to use it for marking sheepskins. Soon, with the involvement of the government of England in the mining operations, graphite became a commodity and its price increased in a short amount of time. The first documented use of graphite in pencils dates from 1565 [a]. The name graphite was given by the German geologist Abraham Gottlob Werner in 1789 from the Greek verb “graphein”, meaning  “to write” [b]. Graphite has been known in the past as “plumbago” or “black lead” [a].

[a] “Graphite,” Earth Science Museum, University of Waterloo, [Online]. Available:, [Accessed May 5, 2020].)

[b] Pierson, H.O., “Handbook of Carbon, Graphite, Diamond, and Fullerenes: Properties, Processing, and Applications”, Noyes Publications, New Jersey, 1993.