C6

C6

1. Redox Reactions

   • Electrons transferred
   • Oxidation: loss of electrons
   • Reduction: gain of electrons
   • Oxidising agent accepts electrons
   • Reducing agent donates electrons
   • Chlorine gas passed into iron(II) salt
     • Green to yellow
     • Fe2+ loses electron=Fe3+
     • Chlorine gained electron that Fe2+ lost
     • Chlorines reduced. Iron(II) ion must be reducing agent
   • Displacement Reactions are redox reactions
     • More reactive metal will displace a less reactive metal from its compound
     • Put reactive metal into solution of dissolved metal compound, reactive metal replaces less reactive metal
     • Metal ion gains electrons (reduced)
     • Metal atom loses electrons (oxidised)

2. Rusting of iron

   • iron+oxygen+water=hydrated iron(II) oxide
   • Iron loses electrons when reacting with oxygen
   • Oxygen gains electrons when when reacting with iron
   • Metals combined with other things to prevent rust
   • Oil, grease and paint prevent rusting
   • Coat of tin can protect steel from rust
   • More reactive metals are used to prevent iron rusting

3. Electrolysis

   • Splitting up with electricity
   • electric current passed through a molten or dissolved ionic compound causing it to decompose
   • creates flow of charge through electrolyte
   • positive ions towards cathode
   • negative towards anode