Graphite has a giant covalent structure in which: each carbon atom is joined to three other carbon atoms by covalent bonds. the carbon atoms form layers with a hexagonal arrangement of atoms. the layers have weak forces between them. Also, graphite has the following properties
Physical Properties of Graphite
Graphite has a high melting point, similar to that of a diamond. Graphite is a soft, slippery feel, and is used in pencils and as a dry lubricant for things like locks. It has a lower density than diamond. It is insoluble in water and organic solvents – for the same reason that diamond is insoluble.
Graphite has a high melting point, similar to that of a diamond. In order to melt graphite, it isn’t enough to loosen one sheet from another. You have to break the covalent bonding throughout the whole structure.
It is a soft, slippery feel, and is used in pencils and as a dry lubricant for things like locks. You can think of graphite rather like a pack of cards – each card is strong, but the cards will slide over each other, or even fall off the pack altogether. When you use a pencil, sheets are rubbed off and stuck to the paper.
It has a lower density than diamonds. This is because of the relatively large amount of space that is “wasted” between the sheets.
It is insoluble in water and organic solvents – for the same reason that diamond is insoluble. Attractions between solvent molecules and carbon atoms will never be strong enough to overcome the strong covalent bonds in graphite.
Graphite conducts electricity. The delocalized electrons are free to move throughout the sheets. If a piece of graphite is connected into a circuit, electrons can fall off one end of the sheet and be replaced with new ones at the other end.
The material is typically grayish-black in color, opaque, and has a radiant black sheen. It is very soft, cracks with very mild pressure, and has a very low specific gravity. Graphite is a different material because it exhibits the properties of both a metal and a nonmetal.
Although graphite is flexible, it is not elastic and has high electrical and thermal conductivity. These fabulous properties give it a wide range of uses in metallurgy and manufacturing.
Chemical Properties of Graphite
| Color | Steel gray to black |
| Chemical Classification | Native element |
| Streak | Black |
| Luster | Metallic, sometimes earthy |
| Diaphaneity | Opaque |
| Cleavage | Perfect in one direction |
| Mohs Hardness | 1 to 2 |
| Specific Gravity | 2.1 to 2.3 |
| Diagnostic Properties | Color, streak, slippery feel, specific gravity |
| Chemical Composition | C |
| Crystal System | Hexagonal |
What are the main properties of graphite?
Properties of Graphite:
- A greyish-black, opaque substance.
- Lighter than diamond, smooth and slippery to the touch.
- A good conductor of electricity (Due to the presence of free electrons) and a good conductor of heat.
- A crystalline solid
- Very soapy to the touch.
- non-inflammable.
- Soft due to weak Vander wall forces.
- The conductor of electricity.
FAQs
What is so special about graphite?
It is unique in that it has properties of both a metal and a non-metal: it is flexible but not elastic, has a high thermal and electrical conductivity, and is highly refractory and chemically inert. Graphite has a low adsorption of X-rays and neutrons making it a particularly useful material in nuclear applications.
What are the properties of pure 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. Graphite exhibits two crystalline structures; hexagonal (alpha) and rhombohedral (beta).
What are the properties of natural graphite?
Introduction. Natural graphite sheet (NGS) is a compressible, porous, electrically and thermally conductive material that has been used primarily to make sealing gaskets because of its ability to conform to rough surfaces, withstand high temperatures, and resist corrosive fluids.
Why does graphite have unusual properties?
Because of its unusual crystal structure, graphite exhibits many of the properties characteristic of metallic materials such as its ability to conduct electricity. Consequently graphite is also used in the production of electrodes and generator brushes.
Is graphite flammable?
GRAPHITE is non-flammable in bulk form, but combustible. A reducing agent. Mixtures of graphite dust and air are explosive when ignited. Reacts violently with very strong oxidizing agents such as fluorine, chlorine dioxide, and potassium peroxide.