1h metallic bonding

• Metallic bonding


  Electrostatic attraction between positive metal ions and delocalised electrons
• Metallic crystals have a giant structure of positive ions surrounded by a "sea" of delocalised electrons
• Giant metallic lattice


  • Layers (malleable, ductile)
  • Uniform (layers)
  • 3D (shape in 3D)
  • Delocalised electrons
• Bonding


  • Strong (high melting point)
  • Electrostatic attraction
• Marginal utility


  The additional utility (satisfaction) gained from the consumption of an additional product
• Metals are ductile


  They can be drawn out/stretch
• Metals are malleable


  They can be bent/shaped
• Layers that can slide over each other in 3 dimensions
• Metals conduct electricity and heat well
• Delocalised electrons are free to move
• Common properties of metals

  • Ductile
  • Malleable
  • Conducts electricity
  • Conducts heat
• Transition metals have higher strength compared to other metals
• Copper is used to make the base of saucepans
• Copper is ductile and used for electrical cables
• Properties to look for in making knives and forks include resistance to corrosion, high melting point, malleability, and ductility
• Common formulae include Carbon dioxide (CO₂), Water (H₂O), and Sodium chloride (NaCl)
• Common chemical names and formulas

  • Carbon dioxide (CO₂)
  • Carbon monoxide (CO)
  • Water (H₂O)
  • Ammonia (NH₃)
  • Glucose (C₆H₁₂O₆)
  • Sodium chloride (NaCl)
  • Hydrochloric acid (HCl)
  • Sulphuric acid (H₂SO₄)
  • Nitric acid (HNO₃)
  • Sodium hydroxide (NaOH)
  • Potassium hydroxide (KOH)
  • Calcium carbonate (CaCO₃)
  • Sulphur dioxide (SO₂)
  • Nitrogen dioxide (NO₂)
  • Hydrogen gas (H₂)
  • Oxygen gas (O₂)
  • Nitrogen gas (N₂)
  • Copper sulphate (CuSO₄)
  • Chlorine gas (Cl₂)
  • Bromine liquid (Br₂)
  • Iodine solid (I₂)
  • Calcium hydroxide (Ca(OH)₂)
  • Methane (CH₄)
  • Copper (II) oxide (CuO)
  • Copper carbonate (CuCO₃)
• Group charges


  • Group 1 (1+)
  • Group 2 (2+)
  • Group 3 (3+)
  • Group 4 (Does not form ions)
  • Group 5 (3-)
  • Group 6 (2-)
  • Group 7 (1-)
  • Group 8 (Does not bond)
• Positive ions form by losing electrons
• Negative ions form by gaining electrons
• Formula is neutral
• Brackets are used in formulas only if you have more than one ion and the ion is in it