Allotropes of carbon: diamond, graphite, graphene

Created by

kashfia k

Cards (74)

How many main allotropes does carbon have?
Three
What are the structures and properties of carbon allotropes?
Diamond:
Structure: Strong, tetrahedral network
Properties: Very hard, non-conductive
Graphite:
Structure: Layers of hexagonal sheets
Properties: Soft, slippery, conducts electricity
Graphene:
Structure: Single layer of hexagonal sheets
Properties: Strong, excellent conductor
What are the main components of the graphite structure shown in the image?
Carbon atoms
Van der Waals forces
Covalent bonds
If the lattice parameter (distance between adjacent atoms/molecules) is $a =$ $0.5 \text{ nm}$ , what is the volume of the unit cell? 
Volume of unit cell = $a^3 =$ $0.5^3 =$ $0.125 \text{ nm}^3$
What type of bonding holds the atoms/molecules together in this crystal lattice?
The atoms/molecules are held together by strong intermolecular forces, likely ionic or covalent bonds
Why is diamond considered very hard?
Due to its strong tetrahedral network
What property distinguishes graphite from diamond?
Graphite is soft and slippery
What are allotropes?
Different forms of the same element
What is the structure shown in the image?
The structure shown is a crystal lattice
It consists of a repeating pattern of atoms or molecules arranged in a 3D grid
How are carbon atoms bonded in diamond?
Through strong covalent bonds in all directions
How are the carbon atoms arranged in the graphite structure?
Carbon atoms are arranged in a hexagonal lattice
The carbon atoms are connected by covalent bonds
The layers of carbon atoms are held together by van der Waals forces
What does the tetrahedral structure of diamond create?
A giant, rigid 3D network
Why is diamond non-conductive?
Because there are no free electrons
How does the structure of graphite contribute to its properties?
The layered structure and weak van der Waals forces allow the layers to slide past each other, making graphite soft and slippery
The delocalized electrons in the covalent bonds allow graphite to conduct electricity
The strong covalent bonds within the layers make graphite very hard and resistant to compression
Why is graphite a good lubricant?
The weak van der Waals forces between the layers allow them to slide past each other easily
How does the graphite structure differ from the structure of diamond?
Graphite has a layered, hexagonal structure, while diamond has a tetrahedral, cubic structure
In graphite, the carbon atoms are sp2 hybridized, while in diamond they are sp3 hybridized
Graphite has delocalized electrons that allow it to conduct electricity, while diamond is an insulator
What are the two main intermolecular forces holding the layers of carbon atoms together in the graphite structure?
Van der Waals forces
If you wanted to use graphite as an electrical conductor, which property of its structure would be most important?
The delocalized electrons in the covalent bonds
How does the structure of graphite differ from the structure of diamond in terms of the hybridization of the carbon atoms?
In graphite, the carbon atoms are sp2 hybridized, while in diamond they are sp3 hybridized
How are carbon atoms arranged in diamond's structure?
Arranged in a regular, repeating pattern
Extends throughout the crystal
What type of bonds connect atoms within each layer of graphite?
Strong covalent bonds
What is the reason for diamond's non-conductivity?
No free electrons to carry electricity
How are the carbon atoms arranged in graphite layers?
In a hexagonal pattern
Why can graphite easily slide apart in layers?
Due to weak Van der Waals forces
What physical properties does the structure of graphite impart?
It makes graphite soft and slippery
What forces hold the layers of graphite together?
Weak Van der Waals forces
What is the structure of graphite primarily composed of?
Layers of carbon atoms
Why is graphite a good lubricant?
The weak van der Waals forces between the layers allow them to slide past each other easily
How does the graphite structure differ from the structure of diamond?
Graphite has a layered, hexagonal structure, while diamond has a tetrahedral, cubic structure
In graphite, the carbon atoms are sp2 hybridized, while in diamond they are sp3 hybridized
Graphite has delocalized electrons that allow it to conduct electricity, while diamond is an insulator
What are the two main intermolecular forces holding the layers of carbon atoms together in the graphite structure?
Van der Waals forces
How does the structure of graphite contribute to its properties?
The layered structure and weak van der Waals forces allow the layers to slide past each other, making graphite soft and slippery
The delocalized electrons in the covalent bonds allow graphite to conduct electricity
The strong covalent bonds within the layers make graphite very hard and resistant to compression
How many carbon atoms are bonded to each carbon atom in diamond?
Four
If you wanted to use graphite as an electrical conductor, which property of its structure would be most important?
The delocalized electrons in the covalent bonds
How do the properties of graphite relate to its structure?
Layers and weak forces enable softness and conductivity
What is a key structural feature of graphite?
Layers
Why is graphite used in pencil lead?
Its layers detach easily when writing
How does graphite conduct electricity?
Covalent bonds create free electrons in layers
What is the structure shown in the image?
The image shows a graphene sheet, which is a two-dimensional lattice of carbon atoms arranged in a hexagonal pattern.
How does the structure of graphite differ from the structure of diamond in terms of the hybridization of the carbon atoms?
In graphite, the carbon atoms are sp2 hybridized, while in diamond they are sp3 hybridized
How could graphene be used in electronic devices?
Transistors and integrated circuits
Transparent conductive coatings
Flexible electronics
Sensors