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batteries containers of chemicals waiting to be converted to electricity the chemical reaction does not take place until the two reactions are connected (you turn it on) typically create 1.5 to 9 volts

McGraw Hill Flash animation

the oxidation and reduction reactions are separated electrodes (two different strips of metals) are placed in each electrolyte (solution that conducts electricity)

electrons move through a wire connecting the two electrodes salt bridge connects the reactions

chemical energy changes electrical to energy through a spontaneous redox reaction greater the difference in reactivity of metals means greater the voltage the more reactive metal (higher on the activity series) is the negative electrode (anode) oxidation occurs here causing loss of e- ex) Zn (s)  Zn 2+ (aq) + 2e - the less reactive metal (lower on the activity series) is the positive electrode (cathode) reduction occurs here causing the gain of e- ex) Cu 2+ (aq) + 2e -  Cu (s)

ions move through a salt bridge connecting the two electrolyte solutions to keep the ions created from building up in either of the solutions