======Thermite======


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**Alternative titles:** Aluminum-Iron Thermite Reaction
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====Summary====                   
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====Procedure====  
  - Fill a metal bucket halfway with sand and create a small depression in the center to capture molten iron.  
  - Place a flower pot in a ring stand directly over the bucket. Cover the hole in the pot with filter paper.  
  - Add about ½ inch of thermite mixture (iron oxide and aluminum powder) into the pot.  
  - Sprinkle a thin layer of red thermite starter powder on top of the main thermite charge.  
  - Insert a strip of magnesium ribbon into the thermite mixture, leaving part exposed.  
  - Ignite the magnesium ribbon with a Bunsen burner flame. Step back as the thermite ignites.  
  - Observe as the reaction produces molten iron and aluminum oxide with a brilliant light.  
  - Once cooled, lift the solidified iron from the sand using tongs.



====Links==== 
Thermite reaction, step by step - Any Excuse for a Chemistry Experiment: 
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Thermite Reaction Demo - osuchemistry: 
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📄 Thermite - University of Washington: [[https://chem.washington.edu/lecture-demos/thermite]]\\

====Variations====
  * Demonstrate different oxide reactants (e.g., copper(II) oxide or manganese dioxide) to show other thermite reactions.  
  * Use small quantities to safely illustrate the principle without excessive heat.  
  * Compare ignition methods - magnesium ribbon fuse vs. pre-lit magnesium dropped into the mixture.



====Safety Precautions====
  * Perform only in a controlled laboratory or outdoor environment.  
  * Molten iron is extremely hot—never attempt to contain it with water or glass.  
  * Use a bucket of sand as the only safe catch material.  
  * Keep all flammable materials (paper, backpacks, screens) far away.  
  * Everyone must wear safety goggles, heat-resistant gloves, and stand well back.  
  * Do not scale up the reaction; excessive amounts are very dangerous.  
  * Only experienced instructors or demonstration technicians should perform this experiment.




====Questions to Consider====
  * Why does aluminum reduce iron oxide so effectively? (Aluminum has a stronger affinity for oxygen than iron, driving the redox reaction.)  
  * What are the products of the thermite reaction? (Molten iron metal and aluminum oxide.)  
  * Why is magnesium ribbon used as a starter? (Its high ignition temperature and strong flame can initiate the thermite reaction, which otherwise requires very high heat to start.)  
  * Why is water never used to contain the molten thermite? (Water reacts violently with molten metal, producing steam explosions.)  
  * What real-world applications use thermite reactions? (Railroad track welding, military incendiaries, and metal cutting in demolition work.)