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Structure and properties of graphite

Graphite has a layer structure. In each layer each carbon atom is bound to three others. This results in a two-dimensional network of hexagons. Within each layer there are strong bonds, but between the different layers the bonds are very weak. Thus, the layers can easily be shifted against each other and even separated. This structure is the reason graphite is very soft and is even used as a lubricant. But graphite has other special properties as well:

Electrical conductivity of graphite

The fact that graphite is electrically conductive results from its atomic structure. Each carbon atom in a graphite crystal has four valence electrons, also called outer electrons, which can form bonds with neighboring atoms. However, only three of the four valence electrons enter into a bond, while the fourth electron remains freely mobile and thus allows electricity to be conducted.

Thermal conductivity of graphite

Graphite has excellent thermal conductivity combined with high temperature resistance. Graphite does not have a melting point; it changes from the solid state directly into the gaseous state. This process is called sublimation. In an inert gas atmosphere, graphite becomes plastically deformable starting at a temperature of °C. At temperatures above °C graphite sublimates even without the presence of oxygen.

Chemical resistance of graphite

Graphite is one of the most chemically resistant materials. It is resistant to almost all media of organic chemistry. These typically include the intermediate and/or end products in the petrochemicals, coal refining, plastics industry, the production of paints, coatings, refrigerants and antifreeze, but also in the cosmetics and food industries. Graphite is also resistant to most inorganic media, such as non-oxidizing acids, alkalis, aqueous salt solutions and most technical gases.

Download: Chemical resistance of natural graphite

Uses of Graphite

Graphite is a type of mineral found in metamorphic and igneous rocks. It is usually formed when carbon is subjected to high temperature and pressure in the earth&#;s crust. Graphite is also said to be one of the naturally-occurring forms of crystalline carbon. However, this mineral is an interesting one and is commonly referred to as the mineral of all extremes.

As such, Graphite is soft in nature, it cleaves easily even with light pressure, is greasy and features low specific gravity. Further, this mineral has a black or sometimes greyish colour. It is an excellent conductor of electricity or heat and it can also withstand extreme temperatures. Another significant character of this mineral is that it is chemically inert meaning it is not affected by a majority of reagents and acids.

Graphite is found all over the world in its natural form, and in high quantities as well. However, it is usually classified into three forms namely flake, crystalline, and amorphous depending on the source of the mineral.

Table of Contents

List of Uses of Graphite

Graphite has been used since ancient times. It has a wide range of applications in the modern world too. Let&#;s look at some common uses of graphite below.

• • • • Writing Materials
      • Lubricants
      • Refractory
      • Nuclear Reactors
      • Batteries
      • Graphene Sheets

Writing Materials

The word graphite is from the Greek language which translates as &#;to write&#;. So the most common use of graphite is in making the lead in pencils. This lead is a mixture of clay and graphite which is in an amorphous form.

Lubricants / Repellents

Graphite is one of the main ingredients in lubricants like grease, etc. This mineral reacts with atmospheric water vapour and creates a thin film or layer over the surface applied and thus reduces friction. Graphite is also used in car brakes and clutches.

The powdered form of lump graphite is also used in paints. Why? Well, graphite by nature is water-repellent. So it offers a protective coating on wood and other surfaces.

Refractories

Due to its high tolerance to heat and unchangeability, Graphite is a widely used refractory material. It finds its use in the manufacturing industry and it helps in the production of glass and steel as well as processing of iron.

Nuclear Reactors

Graphite can absorb fast-moving neutrons. As a result, it is used in reactors to stabilize nuclear reactions.

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Electrical Industry

Crystalline flake graphite is used in the manufacturing of carbon electrodes, brushes, and plates needed in dry cell batteries and the electrical industry. Interestingly, natural graphite is also processed into synthetic graphite. This type of graphite is useful in lithium-ion batteries.

Graphene Sheets

Graphite can be used to make graphene sheets. These sheets are said to be 100 times stronger and 10 times lighter than steel. This derivative of graphite is further used in making lightweight and strong sports equipment. Many are considering future applications in the field of medical and aerospace industry.

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Structure and Properties of Graphite

Frequently Asked Questions &#; FAQs

Q1

Why is graphite used in pencil?

This slippery-sheet form is what makes the touch of graphite so sloppy and makes it such a strong writing content. The particles of the carbon sheet readily rub off the pencil centre and onto the page. This property also makes it an excellent dry lubricant for graphite powder.

Q2

What are two uses of graphite?

In pencils and lubricants, graphite is used. It is a strong heat and energy conductor. In electrical devices such as electrodes, batteries, and solar panels, its high conductivity makes it useful.

Q3

Is Graphite an element?

A type of carbon, which is an element, is graphite. The carbon atoms are bound together in graphite and organised into layers. On the right hand of the periodic table, you will find non-metals, and graphite is the only non-metal that is a strong electricity conductor.

Q4

Is graphite a tetrahedral structure?

Every carbon atom is covalently bound to four other carbon atoms at the four corners of the tetrahedron. A simultaneous piling of layers of carbon atoms amounts to the crystal structure of graphite. The carbon atoms lie in fused hexagonal rings inside each layer, which stretch infinitely in two dimensions.

Q5

Is graphite a good conductor of electricity?

In a graphite molecule, each carbon atom&#;s valence electron stays secure, making graphite a strong electricity conductor.

These are some top uses of graphite. To know more about the properties and different types of rocks and minerals you can keep visiting BYJU&#;S or download our app for interesting content and learning experience.

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