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Redox reactions, chemical cells and electrolysis - Coggle Diagram

- - - - alkaline manganese cells
      - silver oxide cells
      - zinc-carbon cells
  - - - nickel-metal hydride cells
      - lithium ion cells
      - lead-acid accumulator
- - - - 2 different metal electrode
        
        negative electrode (more reactive)
        
        greater tendency to lose electrons
        
        positive electrode (less reactive)
        
        electrons flows from the negative electrode to the positive electrode through the external circuit
        
        voltage of a chemical cell
        
        can be measured by
        
        multimeter
        
        different reactivity
        
        different tendency/ readiness to lose electrons
      - two half cells
      - salt bridge
        
        completes the circuit
        
        allowing ions to move from one half cell into another
        
        provides ions to balance the charge
      - two half cells
      - porous device
        
        prevents direct mixing of the two electrolytes
        
        allows ions to move from one electrolyte into another
- - - - +ve value
        
        electrons flows from metal X to Cu
        
        metal X is more reactive than Cu
        
        metal X loses electron more readily than Cu
        
        metal X has a higher position than Cu in ECS
      - -ve value
        
        electron flows from Cu to metal X
        
        Cu is more reactive than metal X
        
        Cu loses electron more readily than metal X
        
        Cu has a higher position than metal X in the ECS
- - - - must with + -
        
        eg, +1, -2,+3, -4
  - - - the oxidation number of an element in a simple ion is equal to the charge on the ion
        
        the sum of oxidation number of all elements
        
        in polyatomic ion
        
        equals to the charge on the ion
        
        in a compound
        
        equals to zero
    - - all Grp 1 metals in its cpd, ON = +1
        
        all Grp 2 metals in its cpd, ON = +2
        
        Hydrogen in most of its cpd, ON = +1
        
        fluorine in all of its cpd, ON = -1
        
        chlorine, bromine, iodine in most of its cpd, ON=-1
        
        oxygen in most of its cpd, ON=-2