Properties of Metals ( CIE IGCSE Chemistry )

The metallic character diminishes moving left to right across the Periodic Table

Properties of metals

• Conduct heat and electricity
  • This is because metals have delocalised electrons that are able to move through the metal structure
  • This is because the layers of positive metal ions, in the metal structure, are able to slide over each other
  • Usually have high melting and boiling points
    • This is because there is a strong electrostatic attraction between the positive metal ions and delocalised electrons (metallic bond)
    • This strong attraction / bond requires lots of energy to break

    Properties of non-metals

    • Do not conduct heat and electricity
      • This is because all of the electrons are involved in covalent bonding
      • One exception to this is graphite
      • They are not malleable or ductile
      • One exception to this is graphite
      • Many non-metals are gases at room temperature
      • This is because they have weak forces between molecules
      • These weak intermolecular forces do not require a lot of energy to overcome
      • Exceptions to this include diamond and silicon(IV) dioxide

      Chemical properties of metals

      • The chemistry of metals is studied by analysing their reactions with water, dilute acid and oxygen
      • Based on these reactions, a reactivity series of metals can be produced

      Reactions of metals with water

      • Some metals react with water, either warm or cold, or with steam
      • Metals that react with cold water form a metal hydroxide and hydrogen gas

      metal + water → metal hydroxide + hydrogen

      • For example, calcium:
      • Metals that react with steam form a metal oxide and hydrogen gas

      metal + water → metal oxide + hydrogen

      • For example, zinc:

      Zn (s) + H₂O (g) → ZnO (s) + H₂ (g)

      Reactions of metals with acids

      • Most metals react with acids, such as HCl
      • When acids and metals react, the hydrogen atom in the acid is replaced by the metal atom to produce a salt and hydrogen gas

      metal + acid → salt + hydrogen

      • For example, iron:

      Fe (s) + 2HCl (aq) → FeCl₂ (aq) + H₂ (g)

      Reactions of metals with oxygen

      • Unreactive metals, such as gold and platinum, do not react with oxygen
      • Some reactive metals, such as the alkali metals, react easily with oxygen
      • Copper and iron can also react with oxygen, although much more slowly
      • When metals react with oxygen a metal oxide is formed

      metal + oxygen → metal oxide

      • For example, copper:

      2Cu (s) + O₂ (g) → 2CuO (s)