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This document discusses the allotropic forms of carbon. It introduces carbon allotropes as different crystalline forms of an element. The main carbon allotropes discussed are diamond, graphite, and fullerenes. Diamond is the hardest natural material due to its covalent bonding structure. Graphite is composed of stacked graphene layers and is the most stable carbon allotrope. Fullerenes are closed-cage molecules composed entirely of carbon, such as buckyballs. The document provides examples of uses for some carbon allotropes and briefly mentions a few less common allotropes.
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Carbon and its compounds
Myself being as a class 10 CBSE student; I understand the difficulties faced by the students.
so refer this presentation to have a well understanding over a difficult chapter.
PLEASE DO FOLLOW ME FOR FURTHER UPDATES!!
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Diamond and graphite are two allotropes of carbon that differ significantly in their physical properties. Diamonds form under high temperature and pressure deep in the Earth's mantle, while graphite forms through the metamorphism of carbonaceous sediments. Despite being made of the same element, diamond is transparent, extremely hard, and thermally conductive, while graphite is black, soft, and electrically conductive. Both have important industrial applications, with diamond used in cutting and optics and graphite used in pencils, lubricants, and batteries.
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1) New ligands were synthesized from benzyl azide and methyl propiolate or dimethylacetylene dicarboxylate to form 1-benzyl-1H-1,2,3-triazole-4-carboxylic acid and 1-benzyl-1H-1,2,3-4,5-dicarboxylic acid for use in metal binding complexes.
2) The ligands were reacted with various transition metal salts like Ag+, Fe2+, Fe3+, Zn2+, Co2+, Mn2+, Cr3+, and Ni2+ to form colored precipitates that were analyzed using spectroscopy to study complex formation.
3) Preliminary
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1. Carbon exists in three allotropic forms: diamond, graphite, and fullerenes.
2. Diamond is extremely hard due to its rigid, three-dimensional covalent network structure where each carbon atom is bonded to four others in a tetrahedral shape. It is formed under high temperature and pressure deep in the Earth.
3. Diamond has many uses such as cutting, grinding, drilling, and jewelry due to its properties including hardness, high melting point, thermal conductivity, and brilliance when cut and polished. Synthetic diamonds are also produced for industrial applications.
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Perovskites solar cells
Perovskite solar cells are a promising photovoltaic technology that has seen rapid increases in efficiency from 3.8% in 2009 to 19.3% in 2014. Perovskites have a unique crystal structure and can be prepared through various methods like spin coating and inkjet printing. They offer benefits such as high absorption, tunable bandgaps, and flexibility. However, challenges remain around stability issues from oxygen, moisture, UV light and heat that can be addressed through material engineering and encapsulation. With further research into replacing lead and improving stability, perovskite solar cells have the potential to become a leading solar technology of the future.
Carbon diamond vs gerahpit
Diamond and graphite are both made of carbon but have different properties due to their molecular structure. Diamond has a rigid 3D structure that makes it the hardest natural material. Graphite has layered sheets that allow for movement, making it softer. While diamond is an insulator, graphite can conduct electricity due to delocalized electrons between layers.
Fullerene
Fullerenes are spherical or tubular molecules composed entirely of carbon, with the best known being buckminsterfullerene (C60). C60 is highly symmetric, resembling the pattern of a soccer ball with 12 pentagons and 20 hexagons. While the sp2 carbon bonds give fullerenes stability, there is also some angle strain due to the curved structure. Fullerenes can be made more stable through electrophilic addition that changes some carbons to sp3 hybridization. Potential applications of fullerenes include cancer treatment by attaching drugs to their surface, use as superconductors, and inhibiting HIV enzymes.
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Fullerenes
The document discusses fullerenes, which are hollow carbon structures made of pentagons and hexagons. It provides a brief history of their discovery in 1985 and describes their structure as spheres like soccer balls made of 12 pentagons and various hexagons. The most famous fullerene is buckminsterfullerene (C60), which contains 60 carbon atoms arranged in 20 hexagons and 12 pentagons. The document outlines the hybridization, bonding, and geometry of C60 and other fullerenes. It concludes by discussing some applications of fullerenes in areas like antioxidants, drug delivery, solar cells, and more.
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Carbon and its compounds
Myself being as a class 10 CBSE student; I understand the difficulties faced by the students.
so refer this presentation to have a well understanding over a difficult chapter.
PLEASE DO FOLLOW ME FOR FURTHER UPDATES!!
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Carbon and its compounds
Carbon being the most versatile element on this earth is also the most important element for mankind. Carbon (from Latin: carbo "coal") is a chemical element with the symbol C and atomic number 6. It is nonmetallic and tetravalent—making four electrons available to form covalent chemical bonds. It belongs to group 14 of the periodic table. Carbon makes up only about 0.025 percent of Earth's crust.
Carbon
Carbon exists in several allotropes with different properties. Diamond and graphite are two major allotropes. Diamond is very hard while graphite is soft and slippery. Other allotropes include nanotubes, graphene, buckminsterfullerene, and amorphous carbon. Carbon undergoes substitution, addition, and oxidation reactions. It is essential for life but can also have harmful health effects if inhaled in certain forms like coal dust. Applications of carbon include uses in jewelry, lubricants, batteries, and tires due to its various properties.
Carbon
Carbon belongs to the group IV of the periodic table.
It has four electrons in its outermost orbit, so its valency is four.
Carbon is a non-metal.
Why so many Carbon Compounds in nature
Because carbon is chemically unique.
Only carbon atoms have the ability to combine with themselves to form long chains
The number of carbon compounds is larger than that of all other elements put together.
Occurrence of carbon
The name ‘carbon’ is derived from the Latin
word ‘carbo’ meaning coal. Carbon is found in
nature in free as well as compound state. Carbon in
the free state is found as diamond and graphite, and
in the combined state in the following compounds.
1. As carbon dioxide and in the form of carbonates
such as calcium carbonate, marble, calamine
(ZnCO3)
2. Fossil fuel – coal, petroleum, natural gas
3. Carbonaceous nutrients – carbohydrates,
proteins, fats
4. Natural fibres – cotton, wool, silk
Properties of carbon
Allotropic nature of Carbon
Allotropy - Some elements occur in nature in more than one form. The chemical properties
of these different forms are the same but their physical properties are different. This
property of elements is called allotropy. Like carbon, sulphur and phosphorus also exhibit
allotropy.
Allotropes of carbon
A. Crystalline forms
1. A crystalline form has a regular and definite arrangement of atoms.
2. They have high melting points and boiling points.
3. A crystalline form has a definite geometrical shape, sharp edges and plane surfaces.
Carbon
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.
Carbon and it's compounds - part 2
This slide is for the students of class X CBSE. This will surely help them for their board examinations
carbon_comp.ppt
This document discusses carbon and its compounds. It notes that carbon has four valence electrons and can form long chains, allowing it to combine with many other elements. This results in a vast number of carbon compounds in nature. Specifically, it discusses the allotropes of carbon - diamond and graphite. While chemically identical, they have very different physical properties due to variations in atomic arrangement. Hydrocarbons, compounds of carbon and hydrogen, are also discussed. The simplest, methane, is examined as are saturated hydrocarbons called alkanes and unsaturated versions like alkenes and alkynes.
Hello-bachho.pptx
Carbon is a non-metallic element that is essential for all organic life. It has an atomic number of 6 and exists in several allotropes including graphite, diamond, and buckyballs. Carbon is the backbone of organic molecules like DNA, proteins, and carbohydrates. It also plays a critical role in the carbon cycle by which carbon is exchanged between living organisms. The document then discusses the physical and chemical properties of carbon and its allotropes in more detail.
Carbon
This document discusses carbon and its compounds. Carbon has four electrons in its outer orbit and can form four covalent bonds, giving it a valency of four. It is a non-metal that occurs naturally in two allotropes - diamond and graphite. While diamond and graphite are chemically identical, consisting entirely of carbon, they have very different physical properties due to differences in how the carbon atoms are arranged. Carbon has the unique ability to form long chains, providing a backbone for other atoms to attach to, resulting in the vast number and variety of carbon compounds found in nature, including hydrocarbons.
carbon_comp.ppt
This document discusses carbon and its compounds. Carbon has four electrons in its outer orbit and can form four covalent bonds, giving it a valency of four. It is a non-metal that occurs naturally in two allotropes - diamond and graphite. While diamond and graphite are chemically identical, consisting entirely of carbon, they have very different physical properties due to differences in how the carbon atoms are arranged. Carbon has the unique ability to form long chains, providing a backbone for other atoms to attach to, resulting in a huge number and variety of carbon compounds known as hydrocarbons.
Carbon and Its Compounds
Carbon is a key element that forms the basis of many important compounds due to its ability to bond with other carbon atoms and elements. It exists in several allotropes with varying properties, including diamond and graphite. Carbon can form single, double, and triple bonds with other atoms, allowing it to create large, complex molecules through catenation. Saturated carbon compounds contain only single bonds, while unsaturated compounds contain double or triple bonds. Functional groups and structural isomers give compounds unique reactivity and properties. Important carbon compounds discussed include ethanol, ethanoic acid, soaps, and detergents.
LESSON PLAN 3d Carbon.pdf
Carbon has 8 main allotropes including diamond, graphite, fullerene, carbon nanotubes, and amorphous carbon. Diamond is the hardest known mineral that forms in a cubic crystal lattice. Graphite is soft and used in pencils as it forms in hexagonal planes. Fullerenes like C60 buckyballs were discovered in 1985 and are hollow spherical structures that can be used in nanotechnology. Carbon nanotubes are stronger than diamonds and can conduct heat well. Amorphous carbon is found in coal and soot and does not have a defined crystal structure. The different allotropes of carbon have a variety of applications including industrial uses, electronics, medicine, and more.
Class 10 chemistry Carbon and its compounds.pdf
Carbon is a unique element that can form large numbers of compounds. It has four valence electrons and forms covalent bonds, allowing it to link together in chains, branches, and rings. There are three main allotropes of carbon: diamond, graphite, and fullerene. Diamond has a three-dimensional crystalline structure that makes it very hard, while graphite has stacked hexagonal layers that allow for conductivity. Carbon forms the basis of all known life and many important compounds like fuels, plastics, and organic chemicals.
Carbon comp
Carbon has four electrons in its outer orbit giving it a valency of four. It is a non-metal that can form long chains by combining with itself, providing a backbone to which other atoms can attach in various ways. In nature, carbon exists as two allotropes, diamond and graphite, which differ physically in properties like appearance, hardness, and conductivity despite being chemically identical. Hydrocarbons are compounds of carbon and hydrogen that are the main component of petroleum, and include saturated compounds like alkanes as well as unsaturated compounds with double or triple bonds between carbons like alkenes and alkynes.
Carbon allotropes
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.
Nano materials
Fullerenes are a third allotrope of carbon that are cage-like molecules formed by heating graphite in an inert gas. The most common fullerene is C60, which has a soccer ball shape. Fullerenes are highly stable, insoluble in water but soluble in organic solvents. They have applications in optics, electronics, medicine, and as antioxidants or catalysts.
Carbon nanotubes are cylindrical nanostructures composed of graphite sheets rolled at specific angles, determining the nanotube's properties. Single-walled nanotubes are single graphene sheets rolled into cylinders while multi-walled nanotubes contain multiple concentric graphene cylinders. Carbon nanotubes have excellent thermal and electrical
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Presentation (
- 1. ALLOTROPIC THEORY PRESENT BY – DIKSHA SUNIL DHIWAR. S.Y.B.SC.B.ED. SUBJECT INORGANIC AND ORGANIC CHEMISTRY (322)
- 2. INTRODUCTION •When an element exists in more than one crystalline form, those forms are called Allotropes; two most common Allotropes of carbon are diamond and graphite.
- 3. ALLOTROPES OF CARBON • Eight allotropes of carbon a)diamond b)graphite c)lonsdaleite d)C 60 e)C540,Fullerite f)C70, g)amorphous carbon, h)zig-zag single-walled carbon nanotube. • Carbon is capable of forming many allotropes (structurally different forms of the same element ) due to its valency. • Diamond, graphite, and fullerenes are three allotropes of pure carbon.
- 4. DIAMOND • Diamond is a well known allotrope of carbon. The hardness and high dispersion of light of diamond make it useful for both industrial applications and jwelry. Diamond is the hardest known natural mineral.
- 5. GRAPHITE • In graphite each carbon atom uses only 3 of its 4 outer energy level electrons in covalently bonding to three other carbon atom contributes one electron to a delocalized system of electrons that is also a part of the chemical bonding . • Graphite is the most stable allotrpe of carbon.
- 6. FULLERENE • A fullerene is an allotropes of carbon whose molecule consists of carbon atoms connected by single and double bonds so as to form a closed mesh, with fused rings of five to seven atoms. • Cylindrical fullerenes are also called carbon nanotubes or buckytubes.
- 7. EXAMPLES AND USES OF CARBONS ALLOTROPES • Graphite • - Soft, black, solid, • - Used in batteries ( for its conductivity ) and in pencils • - Most stable forms of carbon .
- 8. EXAMPLES AND USES OF CARBONS ALLOTROPES • Fullerene • -Group of ball-like and tube-like structures • -Discovered in 1985 • -Molecules composed 100% of carbon. • -Study but scientists are trying to use it in medical purposes.
- 9. MORE OF ALLOTROPES OF CARBON 1. Carbon Nanofoam 2. Carbon Nanotube 3. Lonsdaleite 4. Ceraphite Allotrope.