Carbon allotropes
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Allotropes of carbon Carbon is capable of forming many allotropes due to its valency. Well known forms of carbon include diamond and graphite. In recent decades many more allotropes and forms of carbon have been discovered and researched including ball shapes such as buckminsterfullerene and sheets such as graphene. Larger scale structures of carbon include nanotubes, nanobuds and nanoribbons. Other unusual forms of carbon exist at very high temperature or extreme pressures.
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Carbon and its allotropes
Carbon exists in different allotropes including diamond and graphite. Diamond and graphite have very different physical properties despite being made of the same element carbon. This is because the arrangement of carbon atoms differs between the two allotropes, with diamond having the carbon atoms arranged in a tightly bound 3D structure while graphite has the carbon atoms arranged in stacked planar sheets.
Allotropic forms of carbon
There are three main allotropic forms of carbon: diamond, graphite, and fullerene. Diamond has a tetrahedral structure with each carbon atom covalently bonded to four other carbons. It is extremely hard, transparent, and a poor conductor of electricity. Graphite has stacked hexagonal layers with each carbon covalently bonded to three others; the fourth electron is delocalized, giving graphite a metallic luster and making it a conductor. Fullerene (C60) has a soccer ball-like structure of carbon atoms.
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Coordinate covalent bonds involve one atom contributing both electrons to form a bond that cannot be distinguished from a regular covalent bond. Metallic bonds are depicted by the electron sea model where positive metal ions are immersed in a sea of delocalized and mobile electrons. Network covalent solids have atoms bonded covalently forming very hard, high melting point materials that are poor conductors such as diamond. Allotropes of carbon include diamond, graphite, amorphous carbon, fullerenes, carbon nanotubes, buckyballs, and lonsdaleite which each have different bonding structures and properties.
Allotropes of carbon
This is a really good presentation on allotropes of carbon. one must watch this ppt which can be easily edited. thank you
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Allotropes of Carbon.ppt
Carbon can form different allotropes by bonding in different ways, including diamond, graphite, buckyballs, and nanotubes. Diamond has each carbon atom bonded to four others in a rigid three-dimensional structure, giving it properties like hardness and high melting point. Graphite has layers of carbon atoms bonded together in flat sheets that can slide past each other, making it slippery and able to conduct electricity. Buckyballs and nanotubes are spherical and tube-shaped fullerenes with delocalized electrons that result in high conductivity and strength.
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Carbon and its allotropes
Carbon exists in different allotropes including diamond and graphite. Diamond and graphite have very different physical properties despite being made of the same element carbon. This is because the arrangement of carbon atoms differs between the two allotropes, with diamond having the carbon atoms arranged in a tightly bound 3D structure while graphite has the carbon atoms arranged in stacked planar sheets.
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There are three main allotropic forms of carbon: diamond, graphite, and fullerene. Diamond has a tetrahedral structure with each carbon atom covalently bonded to four other carbons. It is extremely hard, transparent, and a poor conductor of electricity. Graphite has stacked hexagonal layers with each carbon covalently bonded to three others; the fourth electron is delocalized, giving graphite a metallic luster and making it a conductor. Fullerene (C60) has a soccer ball-like structure of carbon atoms.
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Coordinate covalent bonds involve one atom contributing both electrons to form a bond that cannot be distinguished from a regular covalent bond. Metallic bonds are depicted by the electron sea model where positive metal ions are immersed in a sea of delocalized and mobile electrons. Network covalent solids have atoms bonded covalently forming very hard, high melting point materials that are poor conductors such as diamond. Allotropes of carbon include diamond, graphite, amorphous carbon, fullerenes, carbon nanotubes, buckyballs, and lonsdaleite which each have different bonding structures and properties.
Allotropes of carbon
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Carbon can form different allotropes by bonding in different ways, including diamond, graphite, buckyballs, and nanotubes. Diamond has each carbon atom bonded to four others in a rigid three-dimensional structure, giving it properties like hardness and high melting point. Graphite has layers of carbon atoms bonded together in flat sheets that can slide past each other, making it slippery and able to conduct electricity. Buckyballs and nanotubes are spherical and tube-shaped fullerenes with delocalized electrons that result in high conductivity and strength.
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The name ‘carbon’ is derived from the Latin
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Carbon allotropes
- 1. ALLOTROPES OF CARBON PRESENTED BY- VINITHA V
- 2. KERALA UNIVERSITY COLLEGE OF TEACHER EDUCATION,KOLLAM
- 3. ALLOTROPE DEFINITION •Allotropy or allotropism is the property of some chemical elements to exist in two or more different forms, known as allotropes of these elements. Allotropes are different structural modifications of an element.
- 4. ALLOTROPES OF CARBON •Diamond •Graphite •“Bucky balls” or buckminsterfullerene •Carbon nanotube
- 6. DIAMOND • Diamond word means “unbreakable“ in Greek, is a metastable allotrope of carbon, where the carbon atoms are arranged in a variation of the face-centered cubic crystal structure called a diamond lattice.
- 7. DIAMOND • Each carbon atom is bonded to 4 others to form a giant covalent network or lattice • Is bond is of the same length and equally strong so the carbon atoms are sp3 hybridized • As all the electrons are localised (fixed in position), diamond is exceptionally hard and it does not conduct electricity
- 8. DIAMOND Each carbon atom is bonded to 4 others to form a giant covalent network or lattice
- 9. PROPERTIES OF DIAMOND • Very high melting point • Doesn’t conduct electricity • Good conductor of heat. • Very hard. • Fluorescence under UV light and X-ray.
- 10. GRAPHITE Graphite, meaning "writing stone“ in Greek is a semi metal, native element mineral. Graphite is the most stable form of carbon under standard conditions.
- 11. GRAPHITE • Each carbon atom is bonded to 3 other carbon atoms to give layers of hexagonal rings • As each bond is the same, the carbon atoms are sp2 hybridised • The remaining p orbital electron is delocalised to form weak bonds between the layers • The covalent layer lattice has all sigma bonds
- 12. GRAPHITE Each carbon atom is bonded to 3 other carbon atoms to give layers of hexagonal rings
- 13. PROPERTIES OF GRAPHITE • Because of the layers, graphite is an excellent lubricant as the layers can slide over each other • Graphite is also a good conductor of electricity because of the delocalised electrons e.g. carbon rods, lead pencils
- 14. BUCKMINSTERFULLERENE • Is one member of a family of spherical carbon molecules sometimes called “buckyballs” • Has the formula C60 • The C atoms are arranged in hexagons and pentagons to give a geodesic spherical structure similar to a football
- 15. BUCKMINSTERFULLERENE • Like in graphite, each carbon atom is bonded to 3 others
- 16. BUCKMINSTERFULLERENE • Like in graphite, each carbon atom is bonded to 3 others • Each carbon atom is sp2 hybridized • There are also delocalized electrons, hence C60 can conduct electricity slightly
- 17. CARBON NANOTUBE • Carbon nanotubes (CNTs) are allotropes of carbon with a cylindrical nanostructure.
- 18. CARBON NANOTUBE • They have a hollow structure with the walls formed by one-atom-thick sheets of carbon, called graphene. • The chemical bonding of nanotubes is composed entirely of sp2 bonds, similar to those of graphite. • Carbon nanotubes are the strongest and stiffest materials yet discovered in terms of tensile strength and elastic modulus.