Carbon is a non-metallic element with several unique properties that make it essential in both organic and inorganic chemistry.

• Allotropic Forms: Carbon exists in several forms, including diamond, graphite, and fullerene, each with distinct physical properties.
• Hardness: Diamond is the hardest natural substance known, while graphite is soft and slippery.
• Electrical Conductivity: Graphite conducts electricity, whereas diamond is an insulator.
• Melting Point: Carbon has a very high melting point (~3550°C for diamond).
• Density: Varies with allotrope; diamond is dense, graphite is less dense.
• Non-Metallic Nature: Carbon does not exhibit metallic properties like malleability or ductility.
• Insolubility: Carbon is insoluble in water and most common solvents.
• Catenation: Carbon atoms can bond to each other to form long chains, branched chains, and rings.

Carbon reacts with other elements and compounds under specific conditions. Its chemical properties can be categorized as follows:

• Reaction with Oxygen:
  • Carbon burns in oxygen to produce carbon dioxide or carbon monoxide:

  C + O₂ → CO₂

  2C + O₂ → 2CO (limited oxygen)

• Reaction with Hydrogen:
  • Carbon reacts with hydrogen at high temperatures to form hydrocarbons:

  C + 2H₂ → CH₄ (methane)

• Reaction with Halogens:
  • Carbon reacts with halogens on heating to form carbon halides:

  C + 2Cl₂ → CCl₄

• Reaction with Steam:
  • Carbon reacts with steam at high temperatures to produce water gas:

  C + H₂O → CO + H₂

• Reaction with Metal Oxides:
  • Carbon reduces metal oxides to metals:

  CuO + C → Cu + CO

• Reaction in a Charcoal Pot:
  • When placed in a closed charcoal pot and heated, carbon reacts with limited oxygen to produce carbon monoxide and heat:

  2C + O₂ → 2CO

  • This reaction is exothermic and is the principle used in charcoal stoves for cooking and heating.
• Reaction with Acids and Alkalis:
  • Carbon does not react with acids or alkalis under normal conditions, showing chemical inertness.