GCSE›AQA GCSE Chemistry›Mind mapsIonic Bonding and Ionic CompoundsAQA GCSE Chemistry: Mind mapStudy pack PDFAlso for this subtopic:Revision notesFlashcardsSubtopic testCover factsWhat is it?Metal transfers electrons to non-metalMetal loses electrons: cation (+)Non-metal gains electrons: anion (−)Both get a full outer shellAttraction between opposite ions is the bondIon chargesGroup 1: +1, Group 2: +2, Group 3: +3Group 6: −2, Group 7: −1Non-metals: count back from Group 8FormulaeBalance charges to zeroMgX2+\ce{Mg^2+}MgX2+ needs two ClX−\ce{Cl-}ClX−: MgClX2\ce{MgCl2}MgClX2AlX3+\ce{Al^3+}AlX3+ and OX2−\ce{O^2-}OX2− give AlX2OX3\ce{Al2O3}AlX2OX3Leave charges out of final formulaIonic bondinggiant ionic latticesNa+Cl-Mg2+LatticeRegular repeating 3D arrangement of ionsNo individual moleculesIn NaCl each ion has 6 neighboursPropertiesHigh melting point: strong electrostatic forcesSolid: does not conduct, ions fixedMolten or dissolved: conducts, ions free to moveMany dissolve in waterBrittle: like charges align and repelExam tipsConducts via ions, not electronsSay ions are free to moveNever write MgCl for magnesium chlorideHigher ion charge, higher melting point