Carbon : An important element

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Symbol: C, Atomic number: 6, Atomic mass: 12, Electron configuration: 2,4, Valency: 4, Non-metallic element. Carbon forms four covalent bonds due to its electron configuration.

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Allotropy is the property where some elements occur in nature in more than one form. These forms have the same chemical properties but different physical properties. Example: Carbon exists as diamond,

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Diamond: 3D tetrahedral structure, hardest natural substance, bad conductor of electricity, density 3.5 g/cm³. Graphite: Layered hexagonal structure, soft and slippery, good conductor of electricity,

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In graphite, each carbon atom is bonded to only 3 other carbon atoms, leaving free electrons that can move within the layers, making it conductive. In diamond, all 4 electrons of each carbon are invol

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Fullerene is an allotrope of carbon with molecules in the form of buckyballs and buckytubes. The first example is C₆₀ (Buckminsterfullerene). It was discovered by Harold Kroto, Robert Curl, and Richar

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1. Glass cutting and rock drilling machines 2. Ornaments and jewelry 3. Diamond knives in eye surgery 4. Diamond dust for polishing other diamonds 5. Radiation-resistant windows in space equipment and

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1. Peat: <60% carbon (first stage) 2. Lignite: 60-70% carbon (second stage) 3. Bituminous coal: 70-90% carbon (third stage) 4. Anthracite: ~95% carbon (purest form, hardest)

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Hydrocarbons are compounds made only of carbon and hydrogen. Saturated hydrocarbons have only single bonds (e.g., methane CH₄, ethane C₂H₆). Unsaturated hydrocarbons have multiple bonds (e.g., ethene