An electrochemical cell is like a magic box that turns chemical energy into electrical energy and vice-versa. They're split into two main types

Voltaic Cells (Primary & Secondary Cells, and Fuel Cells)

• These are like little power plants. They convert chemical energy into electrical energy.

  Did you know? 🤓

  • The batteries you find in everyday gadgets, like your remote control, are voltaic cells!

Electrolytic Cells

• These are the opposite of voltaic cells. They take electrical energy and use it to make a chemical change happen.

Electrons are little particles that buzz around in chemical reactions. In redox reactions, electrons move from a substance that's being oxidized (giving away electrons) to a substance that's being reduced (taking electrons). These reactions can create energy, which we can harness for electricity.

Cool Fact: 🌟 Nearly all spontaneous redox reactions give off heat and can be used to make electricity.

Back in the day, an Italian scientist named Luigi Galvani found that by touching a frog leg with two different metals, he could make it twitch (like it's dancing)! Another scientist, Alessandro Volta, showed that you don't need frog legs to make electricity - just chemical reactions. And thus, the battery was born!

Different metals can undergo redox reactions. The one that's more reactive gives away its electrons, while the less reactive one takes those electrons. This can be seen in a reaction between zinc and copper ions. It looks something like this

Zn (s) + Cu²⁺(aq) → Zn²⁺ (aq) + Cu (s)

Breaking it down: Zn (s) → Zn²⁺ (aq) + 2e⁻
Cu²⁺ (aq) + 2e⁻ → Cu (s)

Remember, anode is where oxidation happens (loses electrons), while cathode is where reduction happens (gains electrons). An easy way to remember this: RED CAT (REDuction at CAThode).