Differentiate between diamond and graphite?

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Answer

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Answer

The difference between diamond and carbon is given below.

Diamond *Graphite
It has crystalline nature
*It has layered structure
Each C is sp3 hybridzed and forms 4 covalent bonds with neighboring C atoms.
*Each C atom is sp2 hybridized and forms 3 sigma bonds with 3 other C atoms. Fourth electron forms pi bond.
The geometry is tetrahedral.
*The geometry is planar
C-C bond length is 154 pm
*C-C bond length is 141.5 pm
It has rigid covalent boning which is difficult to break.
*It is soft. Its layers can be separated easily.
It is an electrical insulator.
*It is good conductor of electricity.

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Both Diamond and also Graphite are a crystalline kind of carbon (Both are made of pure carbon). ... In Diamonds, the atoms are carefully packed with together with each atom connected to various other carbon atoms as compared to Graphite where the bonds in between the layers are weak.

Answer

Diamond.

It doesn't conduct electricity.
Hard and have shiny look.
One carbon atom is connected with other 4 carbon atom.
Have high melting point.

GRAPHITE

Conduct electricity.
Brittle and dull appearance.
One carbon atom is connected with other 3 carbon atom.
Have low melting point.

HOPE HELP U

Answer

Differentiation between Diamond and Graphite:

Introduction:
Diamond and graphite are two allotropes of carbon, meaning they are different forms of the same element. Despite being made up of carbon atoms, they possess distinct physical and chemical properties due to their unique structures. This article aims to highlight the differences between diamond and graphite.

1. Structure:
- Diamond: Diamond has a three-dimensional crystal lattice structure. Each carbon atom is covalently bonded to four other carbon atoms in a tetrahedral arrangement, forming a rigid network of carbon atoms. This arrangement gives diamond its exceptional hardness and makes it the hardest known natural substance.
- Graphite: Graphite, on the other hand, has a layered structure. Carbon atoms are arranged in sheets of hexagonal rings, with each carbon atom bonded to three others. The layers are held together by weak van der Waals forces. These layers can slide over each other easily, which gives graphite its characteristic slippery and lubricating properties.

2. Physical Properties:
- Diamond:
- Hardness: Diamond is the hardest known natural substance, scoring 10 on the Mohs scale of mineral hardness.
- Transparency: Diamonds are transparent and allow light to pass through, making them highly valued as gemstones.
- Electrical Conductivity: Diamond is an insulator and does not conduct electricity.
- Graphite:
- Softness: Graphite is relatively soft and can be easily scratched with a fingernail.
- Opacity: Graphite is opaque and does not allow light to pass through.
- Electrical Conductivity: Graphite is a good conductor of electricity due to the presence of delocalized electrons within the layers.

3. Chemical Properties:
- Diamond: Diamond is extremely stable and does not react with most chemicals. It is resistant to acids and bases and requires high temperatures to burn.
- Graphite: Graphite is less stable and can react with certain chemicals under appropriate conditions. It can burn at lower temperatures compared to diamond.

Applications:
- Diamond: Due to its exceptional hardness, diamond is primarily used as a gemstone in jewelry. It also has industrial applications in cutting, grinding, and drilling tools.
- Graphite: Graphite is commonly used as a lubricant in various applications, including machinery and automotive components. It is also used in pencils due to its ability to leave marks on paper.

In conclusion, diamond and graphite exhibit significant differences in structure, physical properties, chemical properties, and applications. Diamond possesses a three-dimensional lattice structure, is extremely hard, transparent, and an insulator. On the other hand, graphite has a layered structure, is soft, opaque, and a good conductor of electricity. Understanding these distinctions is crucial for their respective applications and utilization in various industries.

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