Question

ten properties of Graphite .

Answer 1

Physical State 

The mineral graphite is steel gray to black in color and is odorless. It is opaque and has a sub-metallic luster. It is known to have a very soft and greasy texture. It can be broken easily and leaves a black streak on the hand when touched. Although graphite is soft and flexible, it is not elastic in nature.

Structure

This element is crystalline in nature; however, perfect crystals of graphite are rarely found. The carbon atoms in its structure are arranged in a hexagonal manner in a planar, condensed ring system. This gives the graphite crystals a hexagonal shape. Different layers of this element are stacked together and held by weak covalent forces to form a giant covalent structure.

Melting Point

Graphite has a high melting point above 3000ºF, similar to that of diamond―the other allotrope of carbon. Hence, it is stable over a wide range of temperatures.

Density

As there is a lot of vacant space between the graphite sheets held by the weak covalent bonds, and the density of graphite is 2.09 to 2.33 g/cc, which is lower than that of diamond. The measured specific gravity of this element is approximately 2.26 g/cc. However, it depends upon the purity of graphite. Graphite with a higher ash content shows a specific gravity higher than 2.26, while its natural form has a lower specific gravity or density due to the trapped porosity.

Solubility

Graphite is insoluble in water as well as other organic solvents. There are no attractive forces that occur between the solvent molecules and the carbons atoms in its structure, and thus, it fails to dissolve in any of the organic solvents.

Electrical Conductivity

There is a vast delocalization of electrons within the carbon layers of graphite. The delocalized electrons are free to move and are able to conduct electricity, thus, making graphite a good conductor of electricity.

Chemical Properties 

➤ Graphite is chemically inert to almost all chemicals.

➤ It burns completely when heated in oxygen to form carbon dioxide. However, it fails to burn in air, even if it is heated to high temperatures.

➤ When heated in the presence of concentrated sulfuric acid and potassium dichromate, graphite gets oxidized to carbon dioxide.

➤ Due to its chemical inertness and stability at high temperatures, it is widely used as a refractory material.

Uses of Graphite

Manufacture of 'lead' used in pencils

Refractories

Steel making

Lubricant

Making electrodes

Manufacture of polishes and paints

Molds in foundry

This was all about the properties and uses of graphite. The unique properties of this carbon compound are responsible for its use in a variety of applications

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Answer 2

✌️✌️ hey mate,

❄️The physical properties of graphite

➡️has a high melting point, similar to that of diamond.

➡️has a soft, slippery feel, and is used in pencils and as a dry lubricant for things like locks.

➡️has a lower density than diamond.

➡️is insoluble in water and organic solvents - for the same reason that diamond is insoluble.

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