What are the difference between graphite and diamond?

Question

Answer

Answer

¶¶Diamond:
1). In diamond each carbon atom is linked to four other carbon atoms to form a three dimensional structure.

2). Diamond is the hardest of all known crystalline substance.

3). It is transparent and shines brilliantly in light.

4). Diamond does not have free electrons hence it is a bad conductor of electricity.

¶¶ Graphite :

1)In graphite, each carbon atom is linked to three other carbon atoms forming a hexagonal structure.

2.)Graphite is a soft, slippery and smooth substance.

3.) It is opaque and has a slight metallic sheen.

4)Graphite does have free electrons hence it is good conductor of electricity.

Answer

In diamond, the carbon atoms have strong bonds in three dimensions, which makes it hard. In graphite the bonds form in flat layers with carbon atoms having strong bonds on the same layer with weaker layers above and below, which makes this graphite weak.Since they are both made of carbon their chemical properties are the same. ... Graphite has a layered sheet-like structure with each layer consisting of hexagonal rings, this is because all carbon atoms are sp2 hybridised. Diamond has a tetrahedral structure since all carbon atoms are sp3 hybridised.Graphite and diamond are two of the most interesting minerals. They are identical chemically – both are composed of carbon (C), but physically, they are very different. Minerals which have the same chemistry but different crystal structures are called polymorphs.

Answer

Answer

Graphite is soft and opaque while as diamond is hard and shiny

Answer

Graphite is conductor but diamond is insulator.

Answer

Diamond: Giant covalent structure, with each carbon covalently bonded to four other carbon atoms in a tetrahedral arrangement to form a rigid structure.

Graphite: It is also Giant covalent structure, with each carbon covalently bonded to three other carbon atoms in a hexagonal arrangement.

Answer

Answer

GRAPHITE IS GOOD CONDUCTOR OF ELECTRICITY.DIAMOND IS BAD CONDUCTOR OF   ELECTRICITY

Answer

Answer

**Graphite and diamond** are both forms of carbon, but they have distinct properties and structures that differentiate them. Let's explore the differences between these two allotropes of carbon:

**1. Atomic Structure:**
- Graphite is composed of layers of carbon atoms arranged in a two-dimensional hexagonal lattice. Each carbon atom forms covalent bonds with three neighboring carbon atoms, creating a sheet-like structure.
- Diamond consists of carbon atoms arranged in a three-dimensional lattice. Each carbon atom forms covalent bonds with four neighboring carbon atoms, resulting in a tetrahedral structure.

**2. Bonding:**
- In graphite, the carbon atoms are bonded together by strong covalent bonds within each layer. However, the layers themselves are held together by weak van der Waals forces, allowing them to slide past each other easily. This gives graphite its lubricating and slippery nature.
- Diamond, on the other hand, has a network of strong covalent bonds in all three dimensions. These bonds are incredibly strong, making diamond the hardest naturally occurring substance.

**3. Physical Properties:**
- Graphite is a grayish-black solid with a relatively low density. It has a soft and slippery texture, making it an excellent lubricant. Graphite is also a good conductor of electricity and heat due to the presence of delocalized electrons in the layers.
- Diamond is a colorless and transparent crystal with a high density. It is the hardest natural substance, making it ideal for cutting tools and industrial applications. Diamond is a poor conductor of electricity as it lacks delocalized electrons.

**4. Uses:**
- Graphite is widely used as a lubricant in various applications, such as in machinery, locks, and pencils. It is also used as a moderator in nuclear reactors and as an electrode in batteries.
- Diamond's exceptional hardness makes it valuable in jewelry and cutting tools. It is also used in industrial applications, such as for drilling, grinding, and polishing. Additionally, diamond has unique optical properties, making it useful in lasers and scientific research.

In conclusion, graphite and diamond have different atomic structures, bonding arrangements, physical properties, and uses. Graphite is layered, soft, and a good conductor, while diamond is three-dimensional, hard, and a poor conductor. These differences result from the distinct arrangements of carbon atoms in each allotrope.

Top Courses for Class 10View all

Science Class 10

Social Studies (SST) Class 10

Mathematics (Maths) Class 10

English Grammar Advanced

English Grammar Basic

Top Courses for Class 10

Top Courses for Class 10

Suggested Free Tests

Related Content

About Class 10

Class 10 Study Material

Class 10 All Subjects

NCERT Textbook Solutions

Other Classes

Important Links

Company