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Magnesium Burning. Magnesium metal burns in air producing intense light. Demonstration. The reaction was initiated in a flame The reaction produced intense light The magnesium reacted with the oxygen and nitrogen in the atmosphere to form solid products. Purpose.

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magnesium burning

Magnesium Burning

Magnesium metal burns in air producing intense

light

demonstration
Demonstration
  • The reaction was initiated in a flame
  • The reaction produced intense light
  • The magnesium reacted with the oxygen and nitrogen in the atmosphere to form solid products
purpose
Purpose
  • To observe a metal while it burns
concepts
Concepts

1. Combustion Reactions

2. Combination Reactions

3. Energy

1 combustion reactions
1. Combustion Reactions
  • “Burning” reactions
  • Usually organic substances
      • wood
      • paper
  • By definition a combustion reaction is the exothermic reaction of a substance, usually with oxygen (but not always)
  • Light typically is also a product of the reaction
  • Metals also burn!
2 combination reactions
2. Combination Reactions
  • General form
    • A + B C
  • In this demonstration
    • 2 Mg + O2 MgO
    • 3 Mg + N2 Mg3N2
  • The oxygen and nitrogen occur naturally in the atmosphere
    • O2 is 21% of air
    • N2 is 78% of air
3 energy
3. Energy
  • Two types of energy are produced in this demonstration
    • heat energy DHf MgO = -601.83 kJ/mole (kiloJoules per mole)
        • this is said to be the ‘heat of formation’ for MgO
        • the negative sign indicates the formation is exothermic
    • light energy
        • approximately 10% of the energy of combustion occurs as light in this demonstration
        • more light than any other known reaction
conclusions
Conclusions
  • When the energy of activation was applied magnesium burst into flame
  • Magnesium burned with the intense production of light and heat
  • The reaction was a combination reaction which used gaseous components from the atmosphere
comments
Comments
  • This is a redox reaction in addition to a combination and combustion reaction
    • Mg begins as oxidation number 0
    • In both magnesium oxide and magnesium nitride the oxidation number of magnesium is 2+
    • magnesium has lost electrons therefore has been oxidized
  • Flashbulbs contain magnesium filaments