Ionic bonding

• Ionic Bond


  Electrostatic attraction between oppositely charged ions.
• Cation


  Positively charged ion formed from metal atoms.
• Anion


  Negatively charged ion formed from non-metal atoms.
• Octet Rule


  Atoms gain noble gas configuration by losing/gaining electrons.
• Group Number


  Predicts ion charge based on outer shell electrons.
• Group 1-3 metals


  Lose electrons to form positive ions. Positive charge=group number
• Group 5-7 (15-17) non-metals


  Gain electrons to form negative ions. Negative charge= 8-group number
• Molecular Ions


  Ions containing covalently bonded atoms.
• Hydroxide Ion


  Molecular ion with formula OH.
• Ammonium Ion


  Molecular ion with formula NH4+.
• Nitrate Ion


  Molecular ion with formula NO3-.
• Sulfate Ion


  Molecular ion with formula SO4^2-.
• Carbonate Ion


  Molecular ion with formula CO3^2-.
• Phosphate Ion


  Molecular ion with formula PO4^3-.
• End in -ide


  Monotomic ion (an ion that contains one atom). Binary ions also apply
• Binary ionic compound


  Ionic compound that contains 2 elements
• End in -ate


  Polyatomic ions
• End in -ite


  Ions with one fewer oxygen atom than ions ending in -ate
• Start with -per


  Ions with one more oxygen atom than ions ending in -ate
• Start with hypo-


  Ions with one fewer oxygen atom than ions ending in -ite
• Roman numerals


  Used to indicate the positive charge (and oxidation number) of the metal ions positive charge.
• Dot and cross diagram rules

  All outer shell electrons must be included. Ionic dot and cross must show each separate ion and it's charge outside square brackets.
• Giant Ionic Lattice


  3D structure of positive and negative ions held in place strongly by the electrostatic attraction between opposite charges.
• Melting Point


  High due to strong ionic bonds in compounds through the structure
• Boiling Point


  High due to extensive ionic bonding throughout the structure
• Electrical Conductivity state of ionic compounds when solid


  Don't conduct electricity when solid. Ions are in a fixed position and are not free to move through the giant ionic lattice.
• Electrical conducivity state of ionic compounds when liquid/in a solution


  Do conduct electricity when liquid/in a solution. Solid lattice has broken down. Ions are free to move in the liquid state or solution.
• Solubility state of ionic compounds


  Ionic compounds dissolve in solvents. Ionic lattice is broken down and polar molecules surround and attract ions within the lattice. Forms an aqueous solution containing separate ions. Forming and ionic solution.
• Ion-Dipole Attraction


  Attraction between ions and polar solvent molecules, which can break down a solid into separate dissolved ions in aqueous solutions.
• Insoluble Ionic Compounds


  Stronger ion-ion attractions than ion-dipole attractions. E.g CaCO3
• Dot and Cross Diagrams

  Visual representation of electron transfer in bonding.