======Burning Magnesium Ribbon======


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**Materials: **{{$demo.materials_description}}\\
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**Safety: **{{$demo.safety_description}}\\
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**Alternative titles:** Bright Light Magnesium Reaction
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====Summary====                   
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====Procedure====  
  - Cut a strip of magnesium ribbon about 10 cm (4 inches) long.  
  - Hold the ribbon securely with a pair of tongs.  
  - Place the ribbon into the hottest part of a lighter or Bunsen burner flame until it ignites.  
  - Step back slightly and observe the bright white light as the magnesium burns and forms a white powder of magnesium oxide.  
  - Allow the ash to cool before disposal.



====Links==== 
Burning magnesium ribbon - DonoChem: 
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Chemistry Demo: Burning Magnesium - Dr. B's Chemistry: 
{{youtube>bXh2FlvqA8c?}}\\

📄 Burning Magnesium - LibreTexts Chemistry: [[https://chem.libretexts.org/Ancillary_Materials/Demos_Techniques_and_Experiments/Lecture_Demonstrations/Burning_Magnesium]]\\


====Variations====
  * Compare burning magnesium ribbon to burning other metals such as iron wool.  
  * Place burning magnesium in a controlled container of carbon dioxide to show that it continues to burn, forming magnesium oxide and carbon.


====Safety Precautions====
  * Wear safety goggles with UV protection; the bright flame produces ultraviolet light that can damage eyes.  
  * Do not look directly at the burning magnesium; view indirectly.  
  * Keep away from combustible materials.  
  * Handle with tongs; do not touch magnesium during or after burning.  
  * Do not attempt to extinguish magnesium with water or carbon dioxide, as these can intensify the fire. Use only Class D fire extinguishers or cover with dry sand.  
  * Do not allow children to perform this experiment.




====Questions to Consider====
  * Why is magnesium able to burn so brightly in air? (Magnesium atoms release large amounts of energy when reacting with oxygen, forming MgO.)  
  * What type of reaction is burning magnesium? (A combustion reaction and also a redox reaction: magnesium is oxidized, oxygen is reduced.)  
  * Why can’t water or carbon dioxide be used to extinguish a magnesium fire? (Magnesium reacts with water to release hydrogen gas, and with CO2 to release carbon—both reactions intensify the fire.)  
  * What is the balanced equation for burning magnesium in air? (2Mg(s) + O2(g) → 2MgO(s).)  
  * Why is the reaction exothermic? (Energy is released as strong ionic bonds form between Mg2+ and O2− ions in magnesium oxide.)