Redox Reactions & Metal Extraction | Interactive Chemistry model

Choose a metal extraction

MetalView

Metal species before extraction

→

Metal after reduction

Simplified reactivity series

More reactive ⟵ K Ca Al Zn Fe Cu ⟶ Less reactive
Metals above carbon generally require electrolysis; metals below carbon can often be chemically reduced.

Extraction method

Metal is...

Oxidation-state change

Electrons gained per metal atom

Reducing process

Why this method?

Metal	Typical ore/species	Metal oxidation state	Typical extraction
Al	Al₂O₃	+3	Electrolysis
Zn	ZnO	+2	Reduction with carbon/CO
Fe	Fe₂O₃	+3	Reduction with CO in blast furnace
Cu	CuO (model reaction)	+2	Reduction; low reactivity aids extraction

Metal Extraction Redox Model

The Python model stores each metal's oxidation state and extraction route. It calculates the number of electrons that each metal ion must gain to become a neutral metal atom.

# Redox and metal extraction model

metals = {
    "iron": {
        "symbol": "Fe",
        "oxidation_state": 3,
        "ore": "Fe2O3",
        "method": "reduction with CO",
        "reaction":
            "Fe2O3 + 3CO -> 2Fe + 3CO2"
    },

    "aluminium": {
        "symbol": "Al",
        "oxidation_state": 3,
        "ore": "Al2O3",
        "method": "electrolysis",
        "reaction":
            "2Al2O3 -> 4Al + 3O2"
    },

    "zinc": {
        "symbol": "Zn",
        "oxidation_state": 2,
        "ore": "ZnO",
        "method": "reduction with carbon/CO",
        "reaction":
            "ZnO + CO -> Zn + CO2"
    },

    "copper": {
        "symbol": "Cu",
        "oxidation_state": 2,
        "ore": "CuO",
        "method": "chemical reduction",
        "reaction":
            "2CuO + C -> 2Cu + CO2"
    }
}

metal = metals["iron"]

charge = metal["oxidation_state"]

print("Ore:", metal["ore"])
print("Method:", metal["method"])
print("Reaction:", metal["reaction"])

print()
print("Reduction half-equation:")

print(
    metal["symbol"]
    + str(charge)
    + "+"
    + " + "
    + str(charge)
    + "e- -> "
    + metal["symbol"]
)

print(
    "Oxidation state:",
    "+" + str(charge),
    "-> 0"
)

print(
    "Electrons gained:",
    charge
)

# Example for iron:
#
# Fe3+ + 3e- -> Fe
#
# Iron gains electrons,
# therefore iron is reduced.
#
# In the blast furnace:
#
# Fe2O3 + 3CO
# -> 2Fe + 3CO2
#
# Carbon monoxide acts as
# the reducing agent.

Reduction and Reactivity

A highly reactive metal forms a very stable compound, so carbon may not remove its oxygen effectively. Electrical energy is therefore used to force reduction during electrolysis.

For less reactive metals, a reducing agent such as carbon or carbon monoxide can remove oxygen from the metal compound.