Graphite: Difference between revisions

Latest revision as of 14:22, 21 February 2025

Graphite[edit]

Graphite is an allotrope of carbon. It is a naturally occurring form of crystalline carbon and is known for its use in pencils and as a lubricant. Graphite is one of the softest materials and is also a good conductor of electricity.

Structure[edit]

Graphite has a layered, planar structure. In each layer, the carbon atoms are arranged in a hexagonal lattice. The layers are held together by weak van der Waals forces, allowing them to slide over each other easily, which accounts for graphite's lubricating properties.

The covalent bonds within the layers are strong, making the layers themselves very stable. This structure also contributes to graphite's electrical conductivity, as electrons can move freely within the layers.

Properties[edit]

Graphite is known for its high thermal and electrical conductivity, chemical inertness, and lubricating properties. It is opaque and has a metallic luster. Graphite is also resistant to heat and can withstand temperatures up to 3000°C in a vacuum.

Occurrence[edit]

Graphite occurs naturally in metamorphic rocks such as marble, schist, and gneiss. It is also found in igneous rocks and meteorites.

Uses[edit]

Graphite is used in a variety of applications, including:

Pencils: Graphite is mixed with clay to form the "lead" in pencils.
Lubricants: Due to its slippery nature, graphite is used as a dry lubricant in applications where "wet" lubricants cannot be used.
Electrodes: Graphite is used in electrolysis and battery electrodes due to its conductivity.
Nuclear reactors: Graphite is used as a moderator in nuclear reactors.

Phase Diagram[edit]

Graphite is stable under standard conditions, but it can transform into diamond at high pressures and temperatures. The phase diagram of carbon shows the conditions under which graphite and diamond are stable.

Pressure-Volume Relationship[edit]

The pressure-volume relationship of graphite is important in understanding its behavior under different conditions, such as in high-pressure environments.

Related Pages[edit]

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-'''Graphite''' is a naturally occurring form of crystalline carbon. It is a native element mineral found in metamorphic and igneous rocks. Graphite is extremely soft, cleaves with very light pressure, and has a very low specific gravity. In contrast, it is extremely resistant to heat and nearly inert in contact with almost any other material. These properties give it a diverse range of uses in metallurgy and manufacturing.
+== Graphite ==
-==Properties of Graphite==
+[[File:Graphite-233436.jpg|thumb|right|Graphite sample]]
-Graphite is a mineral that is very soft. On the Mohs hardness scale, it falls between 1 and 2. Because of its softness and streak, graphite is used in pencils and was used in the past for writing on slate. Graphite has a gray to black streak. It is opaque and metallic in luster. It is flexible but not elastic, which means it can be bent but will not spring back to its original shape. It is also a good conductor of electricity. This makes it useful in such items as batteries and solar panels.
-==Occurrence and Production of Graphite==
+'''Graphite''' is an [[allotrope]] of [[carbon]]. It is a naturally occurring form of crystalline carbon and is known for its use in pencils and as a lubricant. Graphite is one of the softest materials and is also a good conductor of electricity.
-Graphite occurs in metamorphic rocks as a result of the reduction of sedimentary carbon compounds during metamorphism. It also occurs in igneous rocks and in meteorites. Minerals associated with graphite include quartz, calcite, micas, iron meteorites, and tourmalines.
-Graphite is not mined in the United States, but U.S. production of synthetic graphite in 2010 was 134,000 t (147,000 short tons). The top three producers of graphite are China, India, and Brazil.
+== Structure ==
-==Uses of Graphite==
+[[File:Graphite-layers-side-3D-balls.png|thumb|left|Graphite layers side view]]
-Graphite has a wide range of uses in industry. It is used in the manufacture of pencils, lubricants, paint, steelmaking, batteries, and conductive coatings. It is also used in the nuclear industry and in brake linings.
-==Health Effects of Graphite==
+Graphite has a layered, planar structure. In each layer, the carbon atoms are arranged in a [[hexagonal]] lattice. The layers are held together by weak [[van der Waals forces]], allowing them to slide over each other easily, which accounts for graphite's lubricating properties.
-Graphite dust can cause irritation of the eyes and can cause the skin to become dry and cracked. Long term exposure can cause lung damage. However, graphite is not considered a carcinogen.
+[[File:Graphite-layers-top-3D-balls.png|thumb|right|Graphite layers top view]]
+The [[covalent bond]]s within the layers are strong, making the layers themselves very stable. This structure also contributes to graphite's electrical conductivity, as electrons can move freely within the layers.
+== Properties ==
+Graphite is known for its high thermal and electrical conductivity, chemical inertness, and lubricating properties. It is opaque and has a metallic luster. Graphite is also resistant to heat and can withstand temperatures up to 3000°C in a vacuum.
+[[File:Graphite-unit-cell-3D-balls.png|thumb|left|Graphite unit cell]]
+== Occurrence ==
+Graphite occurs naturally in [[metamorphic rock]]s such as [[marble]], [[schist]], and [[gneiss]]. It is also found in [[igneous rock]]s and [[meteorites]].
+[[File:Kimmirut_Graphite.jpg|thumb|right|Graphite from Kimmirut, Canada]]
+== Uses ==
+Graphite is used in a variety of applications, including:
+* [[Pencil]]s: Graphite is mixed with clay to form the "lead" in pencils.
+* [[Lubricant]]s: Due to its slippery nature, graphite is used as a dry lubricant in applications where "wet" lubricants cannot be used.
+* [[Electrode]]s: Graphite is used in [[electrolysis]] and [[battery]] electrodes due to its conductivity.
+* [[Nuclear reactor]]s: Graphite is used as a moderator in nuclear reactors.
+== Phase Diagram ==
+[[File:Carbon_basic_phase_diagram.png|thumb|left|Carbon phase diagram]]
+Graphite is stable under standard conditions, but it can transform into [[diamond]] at high pressures and temperatures. The phase diagram of carbon shows the conditions under which graphite and diamond are stable.
+== Pressure-Volume Relationship ==
+[[File:Graphite-pV.svg|thumb|right|Graphite pressure-volume relationship]]
+The pressure-volume relationship of graphite is important in understanding its behavior under different conditions, such as in high-pressure environments.
+== Related Pages ==
-==See Also==
 * [[Carbon]]
-* [[Metamorphic Rocks]]
+* [[Diamond]]
-* [[Igneous Rocks]]
+* [[Allotropy]]
-* [[Mohs Hardness Scale]]
+* [[Van der Waals force]]
+* [[Hexagonal lattice]]
+[[Category:Allotropes of carbon]]
 [[Category:Minerals]]
-[[Category:Metallurgy]]
+[[Category:Conductive materials]]
-[[Category:Manufacturing]]
-[[Category:Health]]
-{{stub}}
-<gallery>
-File:Graphite_ambient_STM.jpg|Graphite
-File:Graphite-layers-side-3D-balls.png|Graphite
-File:Graphite-layers-top-3D-balls.png|Graphite
-File:Graphite-unit-cell-3D-balls.png|Graphite
-File:Carbon_basic_phase_diagram.png|Graphite
-File:Graphite-pV.svg|Graphite
-File:Kimmirut_Graphite.jpg|Graphite
-File:Orgy_of_the_Growl_Devils_“_Graphited_Wood_Grease”_1908_ad_-_Electric_railway_review_(IA_electricrailwayr19amer)_(page_50_crop).jpg|Graphite
-File:Crane’s_Servants_Friend_series_no._3.jpg|Graphite
-File:Pencils_hb.jpg|Graphite
-File:CaC6structure.jpg|Graphite
-File:Naturalis_Biodiversity_Center_-_Museum_-_Exhibition_Nature_theatre_08_-_Graphite,_large_stone.jpg|Graphite
-</gallery>