Carbon and its importance by jeswant gembali
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Carbon is the sixth element on the periodic table. It has six protons, six neutrons, and four electrons. Carbon occurs naturally in both free and combined states, such as carbon dioxide and carbonate. Carbon is a tetravalent element that forms multiple bonds and catenates, or self-links, allowing it to form long chains and rings. This property of catenation and its ability to form isomers are important to carbon's role in daily life. The three main allotropes of pure carbon are diamond, graphite, and buckminsterfullerene. Diamond has a tetrahedral structure and is the hardest natural material. Graphite has layered structure and is used as lubricant. Buckminsterfullerene
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Carbon exists in several allotropes with different structures and properties. Diamond has a tetrahedral structure where each carbon atom is bonded to four other carbons in a rigid three-dimensional lattice. Graphite has stacked sheets of hexagonal rings where each carbon is sp2 hybridized and bonded to three others in each plane, with the planes held weakly together. Fullerene molecules are hollow spheres, tubes, or ellipsoids composed entirely of carbon, with some rings containing five or seven carbons along with the normal six-carbon hexagonal rings.
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1) Transition elements are found in the d-block of the Periodic Table between Groups 2 and 13, but not all d-block elements are transition elements.
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Carbon has 4 main allotropes - graphite, diamond, fullerene, and graphene. It is the chemical element with atomic number 6 and is a nonmetal. Carbon is widely found in nature and living organisms. Its allotropes have varying properties - diamond is the hardest material, graphite is an electrical conductor, fullerenes are spherical structures, and graphene is a strong two-dimensional material.
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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.
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1. Carbon atoms can form more than 4 bonds through hybridization of orbitals. In methane, carbon's 2s and 2p orbitals hybridize to form 4 equivalent sp3 hybrid orbitals, allowing carbon to form 4 sigma bonds to hydrogen in a tetrahedral structure.
2. In ethene and ethyne, carbon's orbitals hybridize differently to form pi bonds in addition to sigma bonds. Ethene carbons hybridize to form 3 sp2 orbitals and 1 p orbital, allowing 2 sigma bonds and 1 pi bond to other carbons. Ethyne carbons hybridize to form 2 sp orbitals and 2 p orbitals, allowing 1 sigma bond and 1 pi bond to each
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Here is the delocalized structure of the carbonate anion:
O=C=O
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Carbon has 4 main allotropes - graphite, diamond, fullerene, and graphene. It is the chemical element with atomic number 6 and is a nonmetal. Carbon is widely found in nature and living organisms. Its allotropes have varying properties - diamond is the hardest material, graphite is an electrical conductor, fullerenes are spherical structures, and graphene is a strong two-dimensional material.
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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.
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1. Carbon atoms can form more than 4 bonds through hybridization of orbitals. In methane, carbon's 2s and 2p orbitals hybridize to form 4 equivalent sp3 hybrid orbitals, allowing carbon to form 4 sigma bonds to hydrogen in a tetrahedral structure.
2. In ethene and ethyne, carbon's orbitals hybridize differently to form pi bonds in addition to sigma bonds. Ethene carbons hybridize to form 3 sp2 orbitals and 1 p orbital, allowing 2 sigma bonds and 1 pi bond to other carbons. Ethyne carbons hybridize to form 2 sp orbitals and 2 p orbitals, allowing 1 sigma bond and 1 pi bond to each
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Carbon is a nonmetal that is the fourth most abundant element in the human body and is essential to life. It has several allotropes including diamond, graphite, and buckminsterfullerene. Carbon forms covalent bonds and can bond to other carbon atoms to form chains, rings, and complex molecules. Many organic compounds are based on carbon chains and rings that may be saturated or unsaturated. Carbon undergoes many important reactions including combustion, oxidation, and substitution reactions.
X chem ch4_carbon_anditscompounds_topconcepts
1. The document discusses carbon and its compounds, specifically covalent bonds and covalent compounds. It describes the conditions for covalent bond formation and properties of covalent compounds like physical states, solubility, and electrical conductivity.
2. Key concepts include that carbon forms covalent bonds and a large number of compounds due to its tetravalency and ability to catenate. Carbon can form single, double, or triple bonds. Lewis dot structures are used to represent covalent bonding.
3. Hydrocarbons are classified as aliphatic or aromatic. Nomenclature and isomerism of hydrocarbons are also covered. Homologous series have a general molecular formula where successive members differ by -CH
X chem ch4_carbon_anditscompounds_topconcepts
1. The document discusses carbon and its compounds, specifically covalent bonds and covalent compounds. It describes the conditions for covalent bond formation and properties of covalent compounds like physical states, solubility, and electrical conductivity.
2. Key concepts include that carbon forms covalent bonds and a large number of compounds due to its tetravalency and ability to catenate. Carbon can form single, double, or triple bonds. Lewis dot structures are used to represent covalent bonding.
3. Hydrocarbons are classified as aliphatic or aromatic. Nomenclature and isomerism of hydrocarbons are also covered. Homologous series have a general molecular formula where successive members differ by -CH
Carbon can exist in different structural states known as allotropes..pdf
Carbon can exist in different structural states known as allotropes. Two well-known allotropes
are graphite, one of the softest substances, and diamond, the hardest naturally occurring mineral.
Graphite has a crystalline structure in which the carbon atoms are arranged in layers of flat
sheets. Each sheet consists of a network of hexagonal (six-membered) rings in which each
carbon atom is bonded to three other atoms.
Diamond, which is formed in the Earth at very high pressures, adopts a different crystalline
structure. Each carbon atom is bonded to four others, which together form a tetrahedral shape
surrounding the central carbon
Diamond is transparent and hard; it acts as an excellent electrical insulator, and can be used as
an abrasive. By contrast, graphite is opaque and soft. It conducts electricity, and is a good
lubricant. Diamond crystallizes in the cubic system but graphite crystallizes in the hexagonal
system.
Carbon that lacks an overall crystalline structure is known as amorphous carbon. Although it is
possible to produce carbon that is entirely amorphous (non-crystalline), material that is described
as amorphous usually includes small crystals of graphite or diamond. Amorphous carbon is the
main constituent of charcoal, soot (lampblack or carbon black), and activated carbon.
In addition, several exotic allotropes have been synthesized or discovered, including fullerenes,
carbon nanotubes, lonsdaleite, carbon nanofoam, and aggregated diamond nanorods. The carbon
atoms in these allotropes have different structural arrangements.
Fullerene C540. A lattice of five- and six-membered rings of carbon atoms, forming an overall
spherical shape.A fullerene is composed of a sheet of carbon atoms linked together in hexagonal
and pentagonal rings to take the overall form of a hollow sphere or ellipsoid. A spherical
fullerene is also called a buckyball. The most well-known buckyball is Buckminsterfullerene
(containing 60 carbon atoms per sphere), named after Richard Buckminster Fuller, the architect
who developed the geodesic dome.
A carbon nanotube likewise consists of a sheet of carbon atoms linked in hexagonal and
pentagonal rings, but the overall shape is that of a hollow cylinder. Sometimes called a
buckytube, it is classified as part of the fullerene family of carbon compounds.
Lonsdaleite is thought to form when meteoric graphite falls to Earth. The impact\'s heat and
stress transform the graphite into a structure similar to diamond, but graphite\'s hexagonal crystal
lattice is retained. Also known as hexagonal diamond, lonsdaleite is transparent and brownish
yellow in color.
Carbon nanofoam was unexpectedly produced by scientists in Australia in 1997*. It consists of
low-density clusters of carbon atoms that are bonded in six- and seven-membered rings.
Surprisingly, the material is attracted to magnets and can be magnetized at temperatures below -
183°C.
Aggregated diamond nanorods (ADNRs) are denser and harder than diamond, and they ap.
Simple structures of solid state chemistry
The document discusses the crystal structures of various ceramic compounds. It describes common AB compounds which contain equal numbers of cations and anions. Lead oxide (PbO) exists in two polymorphs, a red tetragonal form and a yellow orthorhombic form, which have different crystal structures. Calcium carbide (CaC2) has the sodium chloride structure with calcium and carbide ions in place of sodium and chloride. Chromium(III) oxide (Cr2O3) adopts the corundum structure consisting of a hexagonal close-packed array of oxide ions and two-thirds of the octahedral sites occupied by chromium cations.
Shapes And Bond Angles Of Simple Organic Compounds
The document discusses the structures and bonding in several simple organic compounds and solid materials. It describes:
1) The hybridization of atomic orbitals that gives rise to the tetrahedral structure of methane (CH4) with sp3 hybrid orbitals on carbon and single C-H sigma bonds.
2) The sp2 hybridization in ethene (C2H4) which forms three sp2 hybrid orbitals for C-H and C-C sigma bonds and a perpendicular p orbital for a pi bond between the carbons in the double bond.
3) The delocalized pi bonding and resonance structures in the hexagonal ring structure of benzene.
Similar to Carbon and its importance by jeswant gembali (20)
Carbon can exist in different structural states known as allotropes..pdf
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Shapes And Bond Angles Of Simple Organic Compounds
Shapes And Bond Angles Of Simple Organic Compounds
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The cost of information acquisition by natural selection
Ryan Seamus McGee, Olivia Kosterlitz, Artem Kaznatcheev, Benjamin Kerr, Carl T. Bergstrom
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留信网认证的作用:
1:该专业认证可证明留学生真实身份
2:同时对留学生所学专业登记给予评定
3:国家专业人才认证中心颁发入库证书
4:这个认证书并且可以归档倒地方
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6:个人职称评审加20分
7:个人信誉贷款加10分
8:在国家人才网主办的国家网络招聘大会中纳入资料，供国家高端企业选择人才
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Carbon and its importance by jeswant gembali
- 1. By- Jeswant GembaliBy- Jeswant Gembali
- 2. Position of Carbon in Periodic Table………….
- 3. Carbon Atom’s Electronic structure L-shell (4 e- ) K-shell (2 e- ) Nucleus 6 Neutrons & 6 Protons Atomic No. 6
- 4. Occurrence of Carbon in Nature :- In free state:- In Combined state:- CO2 CO3
- 5. Carbon in daily life:-
- 6. Importance of Carbon:- Tetravalency….. Atomic No. :- 6 Electronic Configuration :- 2,4 Thus, Valency :- 4 c . .. .
- 7. Importance of Carbon:- Multiple Bonds c
- 8. Importance of Carbon:- Catenation (Self- linkage)
- 9. Importance of Carbon:- Isomerism (Property of making Isomers):- Isomers; Same Molecular Formula but different Structure. For eg:- C6H12O6 (Glucose) C6H12O6 (Fructose) Glucose Fructose
- 10. Allotropes of Carbon:- Various forms in which Carbon exists in pure form in Nature. Diamond Properties:- Excellent Brilliance. A Transparent Object. Bad Conductor of Electricity. High Melting Point . Made up of Carbon atoms only. Hardest substance in the World. Can be cut with the help of Another Diamond only.
- 11. Allotropes of Carbon:- Various forms in which Carbon exists in pure form in Nature. Diamond Structure:- Tetrahedral structure. 1C linked with 4C Linked with strong Covalent bonds. A Continuous chain of Carbon atoms.
- 12. Uses of Diamond
- 13. Allotropes of Carbon:- Various forms in which Carbon exists in pure form in Nature. Graphite Properties:- An Opaque Object. Good Conductor of Electricity. High Melting Point . Made up of Carbon atoms only. Liberates Carbon dioxide when heated.
- 14. Allotropes of Carbon:- Various forms in which Carbon exists in pure form in Nature. Graphite Structure:- Structured in Layers. 1C, linked with 3C. Layers, connected with weak Vander wal Forces.
- 15. Graphite in Daily Life….
- 16. Allotropes of Carbon:- Various forms in which Carbon exists in pure form in Nature. Buckminster fullerene Properties:- Black solid at room temperature. Doesn’t conducts electricity. Insoluble in Water. Soluble in Petrol. * Has been named after a great American Architect “Buckminster”
- 17. Allotropes of Carbon:- Various forms in which Carbon exists in pure form in Nature. Buckminster fullerene Structure:- Football shaped Fixed number of Carbon atoms. Eg:- C60 20 Hexagons and 12 Pentagons