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Which of the following structures are allotropes of carbon?
1. Diamond
2. Graphite
3. Fullerene
Select the correct answer using the code given below:
- a)1 and 2 only
- b)2 and 3 Only
- c)1 and 3 Only
- d)1, 2 and 3
Correct answer is option 'D'. Can you explain this answer?
Most Upvoted Answer
Which of the following structures are allotropes of carbon? 1. Diamon...
- Diamond and Graphite are formed by carbon atoms, the difference lies in the manner in which the carbon atoms are bonded to one another. In Diamond, each carbon atom is bonded to four other carbon atoms forming a rigid three-dimensional structure.
- In graphite, each carbon atom is bonded to three other carbon atoms in the same plane giving a hexagonal array.
- Fullerenes from another class of carbon allotropes. The first one to be identified was C-60 which has carbon atoms arranged in the shape of a football.
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Which of the following structures are allotropes of carbon? 1. Diamon...
Allotropes of Carbon
Allotropes are different forms of the same element that exist in the same physical state. Carbon, being a versatile element, exhibits different allotropes with distinct structures and properties. The three commonly known allotropes of carbon are diamond, graphite, and fullerene.
1. Diamond:
- Diamond is a crystalline allotrope of carbon.
- It has a three-dimensional network structure, with each carbon atom covalently bonded to four neighboring carbon atoms in a tetrahedral arrangement.
- This strong covalent bonding gives diamond its exceptional hardness and high melting point.
- Diamond is transparent and has a high refractive index, making it a valuable gemstone.
- It is an insulator and does not conduct electricity due to the absence of free electrons.
2. Graphite:
- Graphite is another common allotrope of carbon.
- It has a layered structure, with carbon atoms arranged in hexagonal rings that form stacked layers.
- Each carbon atom in graphite is covalently bonded to three neighboring carbon atoms, creating a planar structure.
- The layers in graphite are held together by weak van der Waals forces, allowing them to slide over each other easily.
- Graphite is soft and slippery due to the weak interlayer bonding.
- It is a good conductor of electricity due to the presence of delocalized electrons in the pi bonds of the carbon atoms.
3. Fullerene:
- Fullerene is a third form of carbon allotrope, discovered in 1985.
- It has a spherical or cage-like structure, consisting of carbon atoms arranged in hexagonal and pentagonal rings.
- The most well-known fullerene is C60, also called buckminsterfullerene or Buckyball, which resembles a soccer ball.
- Fullerene molecules can also form tubes called carbon nanotubes, which have unique mechanical and electrical properties.
- Fullerene and carbon nanotubes have applications in various fields, including electronics, materials science, and medicine.
In conclusion, all three structures mentioned - diamond, graphite, and fullerene - are allotropes of carbon. Each allotrope has distinct properties and applications, making carbon a fascinating element with diverse forms.
Allotropes are different forms of the same element that exist in the same physical state. Carbon, being a versatile element, exhibits different allotropes with distinct structures and properties. The three commonly known allotropes of carbon are diamond, graphite, and fullerene.
1. Diamond:
- Diamond is a crystalline allotrope of carbon.
- It has a three-dimensional network structure, with each carbon atom covalently bonded to four neighboring carbon atoms in a tetrahedral arrangement.
- This strong covalent bonding gives diamond its exceptional hardness and high melting point.
- Diamond is transparent and has a high refractive index, making it a valuable gemstone.
- It is an insulator and does not conduct electricity due to the absence of free electrons.
2. Graphite:
- Graphite is another common allotrope of carbon.
- It has a layered structure, with carbon atoms arranged in hexagonal rings that form stacked layers.
- Each carbon atom in graphite is covalently bonded to three neighboring carbon atoms, creating a planar structure.
- The layers in graphite are held together by weak van der Waals forces, allowing them to slide over each other easily.
- Graphite is soft and slippery due to the weak interlayer bonding.
- It is a good conductor of electricity due to the presence of delocalized electrons in the pi bonds of the carbon atoms.
3. Fullerene:
- Fullerene is a third form of carbon allotrope, discovered in 1985.
- It has a spherical or cage-like structure, consisting of carbon atoms arranged in hexagonal and pentagonal rings.
- The most well-known fullerene is C60, also called buckminsterfullerene or Buckyball, which resembles a soccer ball.
- Fullerene molecules can also form tubes called carbon nanotubes, which have unique mechanical and electrical properties.
- Fullerene and carbon nanotubes have applications in various fields, including electronics, materials science, and medicine.
In conclusion, all three structures mentioned - diamond, graphite, and fullerene - are allotropes of carbon. Each allotrope has distinct properties and applications, making carbon a fascinating element with diverse forms.
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Which of the following structures are allotropes of carbon? 1. Diamond2. Graphite3. FullereneSelect the correct answer using the code given below:a) 1 and 2 onlyb) 2 and 3 Onlyc) 1 and 3 Onlyd) 1, 2 and 3Correct answer is option 'D'. Can you explain this answer?
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