Bonding and Structures

• Ions

  Charged particle formed when an atom gains or loses an electron
• Molecular Ion

  Charged particle containing more than one atom
• Charge when an atom loses an electron

  1+
• Charge when an atom gains an electron

  1-
• Metals form

  Positive Ions
• Non-Metals form

  Negative Ions
• Ionic Bonding

  Strong electrostatic attraction between cations and anions
• Ionic Bonding is typical of

  Metal Compounds
• Covalent bonding

  The sharing of a pair of electrons between two non-metal ions
• Diatomic Molecule

  Formed when two atoms are covalently bonded
• Molecule

  Two atoms chemically bonded together by a covalent bond
• Metallic Bonding

  The attraction between positive ions in a regular lattice and the delocalised electrons
• Alloy


  Mixture of two or more elements, at least on of which is a metal and the resulting mixture has metallic properties
• Properties of Ionic Compounds

  High Melting Points

  Brittle

  Hard

  Soluble in Water

  Conducts electricity when molten or aqueous

  Cannot conduct as a solid
• Molecular Covalent Properties

  Low Melting and Boiling Points

  Cannot Conduct electricity

  Insoluble in water
• Diamond Properties

  Hard

  Each Carbon atom is bonded to 4 others

  High Melting and Boiling points

  Cannot conduct electricity
• Graphite Properties

  Each carbon atom is bonded to 3 others

  Soft and Slippery

  Conducts electricity

  High Melting and boiling points
• Covalent Bond

  
• Ionic Bond

  
• Metallic Bond

  
• Metallic Properties

  High Melting and boiling points

  Can conduct electricity and heat

  Hard and dense

  Malleable

  Ductile
• Graphine Properties


  1 atom thick

  Strong

  Can conduct electricty
• Allotropes

  Allotropes are different forms of the same element in the same physical state