Structure and bonding of carbon

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Diamond: Structure and Bonding

Diamond and graphite are allotropes of carbon: both contain only carbon atoms but have different bonding arrangements, making them physically completely different.
In diamond, each carbon atom forms four covalent bonds with four other carbon atoms, creating a giant covalent tetrahedral structure.
All the covalent bonds in diamond are identical, very strong, and there are no intermolecular forces between separate molecules.
All outer shell electrons of each carbon atom are held in the four covalent bonds, so there are no freely moving particles to carry charge.
Diamond has a very high melting point because its giant covalent structure has strong covalent bonds that need lots of energy to break.
Diamond is extremely hard and dense due to its strong covalent bonds and each carbon atom being bonded to four others.
Diamond's hardness makes it useful in cutting tools like drills; it is the hardest naturally occurring mineral but is brittle and can be smashed with a hammer.

Diamond's giant covalent network

Graphite: Structure and Bonding

In graphite, each carbon atom forms three covalent bonds with three other carbon atoms, forming layers of hexagonal rings.
One electron per carbon atom is delocalised (free to move) and exists between the layers, allowing graphite to conduct electricity.
The covalent bonds within the layers are very strong, but the layers are held together by weak intermolecular forces, so they can slide over each other.
Graphite is soft and slippery because its layers can slide over each other, making it useful as a lubricant and in pencils.
Graphite has a high melting point because it has a giant covalent structure with strong covalent bonds needing lots of energy to break.
Graphite can be used to make inert electrodes for electrolysis, important in the extraction of metals such as aluminium.
Graphite is similar to metals in that it has delocalised electrons; it does not conduct because of free ions.

Graphite layers and delocalised electrons

Graphene: Structure and Properties

Graphene is a single layer of graphite, just one atom thick, consisting of a sheet of carbon atoms covalently bonded in a continuous hexagonal layer.
It is essentially a 2D molecule and has very unusual properties that make it useful in composites and electronics.
Graphene is extremely strong due to its unbroken pattern and strong covalent bonds between carbon atoms; even stitched patches remain the strongest material.
It is also amazingly light, transparent (absorbs 2.3% of visible light), and flexible—it can be twisted, pulled and curved without breaking.
Graphene conducts heat and electricity because it has delocalised electrons that can move along its surface; it moves electrons 200 times faster than silicon.
Its transparency gives it potential for making computer screens of the future.

Graphene: one carbon layer

Fullerenes: Structure and Uses

Fullerenes are carbon allotropes consisting of molecules with hollow tubes or spheres.
Their structures are based on interlocking hexagonal rings, but may also contain rings of five or seven carbon atoms.
Fullerenes can trap other molecules by forming around them, making them useful for targeted drug delivery systems.
They have a huge surface area, useful for trapping catalyst molecules so catalysis can take place.
Some fullerenes are excellent lubricants and are used in industrial processes.
The first fullerene discovered was Buckminsterfullerene (C60), a hollow sphere of 60 carbon atoms forming 20 hexagons and 12 pentagons, shaped like a football.
Buckminsterfullerene was discovered as a component of soot and its discovery won the 1996 Nobel Prize in Chemistry.

Buckminsterfullerene C60

Carbon Nanotubes

Carbon nanotubes are cylindrical fullerenes made by rolling a sheet of graphene into a cylinder.
They have very high length to diameter ratios and high tensile strength, resisting breaking or stretching.
Like graphene, nanotubes can conduct electricity, making them useful in composites, specialised materials, electronics and nanotechnology.
Their properties make them useful for nanotechnology, electronics and materials.

Carbon nanotubes

Comparing Diamond, Graphite and Graphene

Diamond is hard and does not conduct; graphite is soft, slippery and conducts; graphene is a single layer of graphite that is strong, flexible and conducts.
Diamond has a giant covalent structure with each carbon bonded to four others; graphite has layers with each carbon bonded to three others.
Graphite conducts because of delocalised electrons between layers; diamond does not because all outer electrons are held in covalent bonds.
Graphite is soft because its layers slide over each other (weak intermolecular forces); diamond is hard because its rigid covalent network prevents movement.
Graphene is similar to graphite in that it is a layer of hexagonal carbon rings, but different because it is only one atom thick.
Both diamond and graphite have high melting points due to strong covalent bonds needing lots of energy to break.

Carbon allotropes: diamond and graphite

Common Misconceptions to Avoid

Graphite does not conduct because of free ions; it conducts because of delocalised electrons.
Each carbon atom in graphite forms three bonds, not four.
Graphene is a single layer of graphite, not the same as bulk graphite.
Diamond does not conduct electricity even though it is a giant structure.
The layers in graphite are not held together by covalent bonds; they are held by weak intermolecular forces.

Carbon allotropes: common misconceptions

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1.Which bonding is found in diamond, graphite and fullerenes?
Easy
- AIonic
- BCovalent
- CMetallic
- DCoordinate
2.Which substance cannot conduct electricity?
Easy
- ADiamond
- BBuckminsterfullerene
- CGraphite
- DNanotubes
3.In graphite, each carbon atom is bonded to how many other carbon atoms?
Medium
- ATwo
- BThree
- CFour
- DFive
4.Why can graphite conduct electricity?
Medium
- AGraphite has delocalised electrons
- BGraphite has layers of atoms that can slide over each other
- CGraphite has a giant structure
- DGraphite has strong covalent bonds
5.Which statement about diamond is correct?
Medium
- AIt is a hard substance with a low melting point
- BEach carbon atom is bonded to three others with strong covalent bonds
- CIt has a giant structure and conducts electricity
- DIt has a high melting point with each carbon bonded to four others
6.Which of the following is not a property of carbon nanotubes?
Medium
- AHigh tensile strength
- BHigh melting point
- CPoor conductor of electricity
- DStrong covalent bonds
7.Which of the following are properties of Buckminsterfullerene? (select all that apply)
Medium
- AStrong metallic bonds
- BA hollow shape
- CEach carbon is bonded to four other carbon atoms
- DHigh melting point
- EStrong covalent bonds
- FPoor conductor of electricity
8.Graphite is slippery because it has weak covalent bonds between its layers.
Easy
True or false?

더 많은 문제

9.Graphene is a single layer of graphite that is one atom thick.
Easy
True or false?
10.Match each carbon allotrope to its structure.
Medium
- Diamond
- Graphite
- Graphene
- Buckminsterfullerene
- A single layer of graphite one atom thick
- A hollow sphere of 60 carbon atoms
- A giant covalent structure where each carbon bonds to four others
- Layers of hexagonal rings with delocalised electrons between the layers
11.Match each carbon allotrope to the correct description of its structure.
Easy
- Diamond
- Graphite
- Graphene
- Buckminsterfullerene
- A giant covalent lattice where each carbon bonds to four others in a tetrahedral arrangement
- Layers of hexagonal rings where each carbon bonds to three others, with weak forces between layers
- A single one-atom-thick layer of graphite
- A hollow sphere of 60 carbon atoms made of 20 hexagons and 12 pentagons
12.Arrange these carbon structures in order of increasing number of other carbon atoms each carbon is bonded to, starting with the lowest.
Medium
- Graphite
- Graphene
- Diamond
13.Which of the following statements about graphene are correct? (select all that apply)
Medium
- AIt is a single layer of graphite one atom thick
- BIt is extremely strong but very light
- CIt conducts electricity because it has delocalised electrons
- DIt is a good electrical insulator
- EIt is made of hollow spheres of carbon atoms
14.Which of the following are properties of carbon nanotubes? (select all that apply)
Medium
- AHigh tensile strength
- BResistant to breaking or stretching
- CCan conduct electricity
- DPoor conductor of electricity
- EHollow cylindrical shape
15.A student heats a 2.0 g sample of diamond to 5000 °C. Diamond melts at temperatures above 4800 °C. Which statement explains why so much energy is needed to melt diamond?
Medium
- AWeak intermolecular forces between layers must be overcome
- BStrong covalent bonds between carbon atoms must be broken
- CDelocalised electrons must be removed from the structure
- DIonic bonds between carbon ions must be broken
16.Graphite is used as an electrode in the extraction of aluminium. Which property makes graphite suitable for this use?
Medium
- AIt is soft and slippery
- BIt has a low melting point
- CIt conducts electricity and is inert
- DIt is transparent and flexible
17.Graphene is described as a 2D molecule. Which statement best explains why it is described in this way?
Medium
- AIt is made of carbon atoms arranged in a single layer one atom thick
- BIt is a hollow sphere made of carbon atoms
- CIt is a cylinder rolled from a sheet of carbon atoms
- DIt is a giant covalent structure with carbon atoms bonded in three dimensions
18.Fullerenes are molecules of carbon atoms with hollow shapes.
Easy
True or false?
19.Match each carbon allotrope to its correct use.
Medium
- Diamond
- Graphite
- Graphene
- Carbon nanotubes
- Cutting tools such as drills
- Lubricant and electrodes
- Electronics and composites
- Nanotechnology and specialised materials
20.Which of the following statements about carbon nanotubes are correct? (select all that apply)
Hard
- AThey are cylindrical fullerenes
- BThey have a high length to diameter ratio
- CThey have high tensile strength
- DThey are poor conductors of electricity
- EThey can be used in nanotechnology
21.Graphite can conduct electricity because it has delocalised electrons between its layers.
Medium
True or false?
22.Match each property to the correct carbon allotrope.
Medium
- Extremely hard
- Slippery and conducts electricity
- Single layer, transparent and flexible
- Hollow sphere used for drug delivery
- Diamond
- Graphite
- Graphene
- Buckminsterfullerene
23.Diamond conducts electricity because it is a giant covalent structure.
Easy
True or false?
24.Arrange these steps to describe how graphite conducts electricity, starting with the first step.
Hard
- Each carbon atom forms three covalent bonds
- One electron per carbon atom is delocalised
- Delocalised electrons are free to move between layers
- The moving electrons carry charge through the structure
25.A student is given a sample of an unknown carbon allotrope. They find that it is a solid, it does not conduct electricity, and it scratches glass. Which of the following statements about this sample are correct? (select all that apply)
Medium
- AIt is diamond.
- BIt is graphite.
- CIt has a giant covalent structure.
- DEach carbon atom forms three covalent bonds.
- EIt has delocalised electrons.
26.A student sets up an electrolysis circuit using graphite electrodes. Which property of graphite makes it suitable for this use?
Medium
- AIt has a high melting point.
- BIt is soft and slippery.
- CIt conducts electricity and is inert.
- DIt is a giant covalent structure.
27.In graphite, the layers are held together by strong covalent bonds.
Medium
True or false?
28.A student heats a 2.0 g sample of graphite to 5000 °C. Graphite sublimes at around 3600 °C. Which statement explains why so much energy is needed to sublime graphite?
Hard
- AGraphite has weak intermolecular forces between layers.
- BGraphite has strong covalent bonds within its layers that need a lot of energy to break.
- CGraphite has delocalised electrons that absorb energy.
- DGraphite has a low density.
29.Which term describes elements that can exist in different physical forms while in the same state?
Easy
- AIsotopes
- BAllotropes
- CIsomers
- DPolymers
30.Which of the following is a fullerene?
Easy
- ADiamond
- BGraphite
- CBuckminsterfullerene
- DSilicon dioxide
31.Graphene is best described as:
Medium
- AA single layer of graphite one atom thick
- BA hollow sphere of 60 carbon atoms
- CA giant covalent structure of carbon atoms bonded to four others
- DA cylinder of rolled-up diamond
32.Which statement about the bonding in graphite is correct?
Medium
- AEach carbon atom forms four covalent bonds, and all electrons are localised
- BEach carbon atom forms three covalent bonds, and one electron per atom is delocalised
- CEach carbon atom forms two covalent bonds, and two electrons per atom are delocalised
- DEach carbon atom forms three covalent bonds, and all electrons are localised
33.Which of the following statements about fullerenes are correct? (select all that apply)
Medium
- AThey are molecules of carbon with hollow shapes
- BThey are based on hexagonal rings but may also contain five- or seven-membered rings
- CThey are giant covalent structures like diamond
- DBuckminsterfullerene was the first fullerene to be discovered
- EThey cannot be used to trap other molecules
34.Which of the following are properties of graphene? (select all that apply)
Medium
- AIt is extremely strong
- BIt is transparent
- CIt is flexible
- DIt conducts electricity
- EIt is a good electrical insulator
35.Graphite is slippery because the weak forces between its layers allow the layers to slide over each other.
Easy
True or false?
36.Diamond conducts electricity because it has delocalised electrons.
Easy
True or false?
37.Match each carbon allotrope to its correct description.
Medium
- Diamond
- Graphite
- Graphene
- Buckminsterfullerene
- Each carbon bonded to four others in a giant covalent structure
- Layers of hexagonal rings with delocalised electrons between layers
- A single layer of graphite one atom thick
- A hollow sphere of 60 carbon atoms
38.Which statement about the bonding in diamond is correct?
Medium
- AEach carbon atom forms four covalent bonds with other carbon atoms
- BEach carbon atom forms three covalent bonds with other carbon atoms
- CDiamond contains delocalised electrons between layers
- DDiamond is held together by weak intermolecular forces
39.Which of the following is a use of fullerenes?
Medium
- AAs a lubricant
- BIn targeted drug delivery
- CAs a cutting tool
- DAs an electrode in electrolysis
40.Which of the following statements about graphite are correct? (select all that apply)
Medium
- AEach carbon atom forms three covalent bonds to other carbon atoms.
- BThe layers are held together by strong covalent bonds.
- CThere is one delocalised electron per carbon atom.
- DThe layers can slide over each other because of weak intermolecular forces.
- EGraphite is a poor conductor of electricity.
41.Complete the sentence about the melting points of diamond and graphite.
Medium
Their melting points are ____ due to strong covalent bonds needing lots of ____ to break.
42.How many carbon atoms are joined together in one molecule of Buckminsterfullerene?
Medium
43.Give the electronic configuration of a carbon atom.
Easy
44.Name the first fullerene that was discovered.
Medium
45.Buckminsterfullerene is made of 60 carbon atoms. How many carbon atoms are there in 3 molecules of Buckminsterfullerene?
Medium
46.Complete the sentence about the bonding in graphene.
Medium
In graphene, each carbon atom is bonded to ____ other carbon atoms, and the delocalised ____ allow it to conduct electricity.
47.What term is used to describe elements that can exist in different physical forms while in the same state?
Medium
48.Complete the sentences about the structure of graphite.
Medium
Graphite is made from layers of ____ rings. The layers are held together by weak ____ forces, so they can slide over each other.
49.A carbon nanotube has a length of 1.0 × 10^-6 m and a diameter of 1.0 × 10^-9 m. Calculate its length to diameter ratio.
Medium
50.In one molecule of Buckminsterfullerene, how many carbon atoms are joined together?
Medium
51.How many covalent bonds does each carbon atom form in diamond?
Easy
52.How many covalent bonds does each carbon atom form in graphite?
Easy
53.Explain why diamond is extremely hard.
Hard
54.Explain why graphite is soft and slippery.
Hard
55.Explain why graphite is soft and slippery, but diamond is extremely hard.
Hard
56.Explain why graphene is such a strong material and how it is able to conduct electricity.
Hard
57.Explain why diamond has a very high melting point.
Hard
58.How many carbon atoms are joined together in one molecule of Buckminsterfullerene?
Medium
- A60
- B66
- C54
- D72
59.Buckminsterfullerene is made of 60 carbon atoms. How many carbon atoms are there in 3 molecules of Buckminsterfullerene?
Medium
- A198 atoms
- B216 atoms
- C162 atoms
- D180 atoms
60.A carbon nanotube has a length of 1.0 × 10^-6 m and a diameter of 1.0 × 10^-9 m. Calculate its length to diameter ratio.
Medium
- A900
- B1200
- C1000
- D1100
61.In one molecule of Buckminsterfullerene, how many carbon atoms are joined together?
Medium
- A60
- B54
- C72
- D66
62.How many covalent bonds does each carbon atom form in diamond?
Easy
- A5
- B6
- C3
- D4
63.How many covalent bonds does each carbon atom form in graphite?
Easy
- A3
- B2
- C5
- D4

플래시카드

What are allotropes of carbon?

Different physical forms of the same element, carbon, that contain only carbon atoms but have different bonding arrangements, such as diamond and graphite.

How many other carbon atoms does each carbon atom bond to in diamond?

Four. Each carbon atom forms four strong covalent bonds, giving a tetrahedral arrangement.

What is the structure of diamond?

A giant covalent structure in which each carbon atom is covalently bonded to four other carbon atoms, with all bonds identical and very strong.

Why does diamond have a very high melting point?

It has a giant covalent structure with strong covalent bonds between carbon atoms, and these need lots of energy to break.

Why is diamond extremely hard?

Each carbon atom is bonded to four other carbon atoms by strong covalent bonds in a rigid giant covalent structure, so the structure is very hard and dense.

Why does diamond not conduct electricity?

All of the outer shell electrons in each carbon atom are held in the four covalent bonds, so there are no freely moving particles to carry a charge.

Give one use of diamond and the property that makes it suitable.

It is used in cutting tools like drills because it is extremely hard.

How many other carbon atoms does each carbon atom bond to in graphite?

Three. Each carbon atom forms three covalent bonds, forming layers of hexagonal rings.

What happens to the fourth outer electron of each carbon atom in graphite?

It becomes a delocalised electron, free to move along and between the layers and carry charge.

Why does graphite conduct electricity?

Each carbon atom is bonded to three others, leaving one delocalised electron per carbon atom; these free electrons can move through the structure and carry charge.

Why is graphite soft and slippery?

It is arranged in layers; the atoms within a layer are joined by strong covalent bonds, but there are only weak intermolecular forces between the layers, so the layers can slide over each other.

Are the layers in graphite held together by covalent bonds?

No. There are no covalent bonds between the layers; they are held together only by weak intermolecular forces.

Give two uses of graphite and explain each.

It is used in pencils and as a lubricant because its layers slide over each other, and it is used to make inert electrodes for electrolysis because it conducts electricity.

What is graphene?

A single layer of graphite — a sheet of carbon atoms covalently bonded in a continuous hexagonal layer, only one atom thick, so it is essentially a 2D molecule.

Why is graphene extremely strong?

It has an unbroken pattern of strong covalent bonds between the carbon atoms, so it resists breaking even when patches are stitched together.

Why does graphene conduct electricity?

It has delocalised electrons which can move along its surface, allowing it to conduct electricity.

State three properties of graphene.

It is extremely strong but very light, it conducts heat and electricity, and it is transparent and flexible.

Give two uses of graphene.

It is useful in electronics (such as future computer screens) and in making composite materials.

What are fullerenes?

Molecules of carbon atoms with hollow shapes, based on hexagonal rings but which may also contain rings of five or seven carbon atoms.

What is Buckminsterfullerene?

The first fullerene to be discovered, with the formula C60: 60 carbon atoms joined into 20 hexagons and 12 pentagons forming a hollow sphere shaped like a football.

Give two properties of Buckminsterfullerene.

It has a hollow shape and strong covalent bonds, and it is a poor conductor of electricity.

Why is Buckminsterfullerene slippery with a low melting point?

It is made of individual hollow molecules held together only by weak intermolecular forces, which are easily overcome and allow the molecules to slide over each other.

Give two uses of fullerenes.

They can be used for targeted drug delivery, by trapping molecules inside their hollow shapes, and as catalysts, because their huge surface area can trap catalyst molecules.

What is a carbon nanotube?

A cylindrical fullerene formed by rolling a sheet of graphene, with a very high length to diameter ratio.

Why are carbon nanotubes useful for making badminton rackets?

They have high tensile strength and are resistant to breaking or stretching, and they are very light.

Give two uses of carbon nanotubes.

They are useful in electronics and nanotechnology, and in composites and specialised materials, because they conduct electricity and have high tensile strength.

What type of bonding is found in diamond, graphite, graphene and fullerenes?

Covalent bonding — they are all giant covalent or molecular covalent structures made only of carbon atoms.

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