Burning Magnesium

Aim : I want to find out what happens to Magnesium when I burn it.

Hypothesis: I predict that it will turn black and tiny bit not too much melt but not so much.

Method:  1. Get equipment   2. safety goggles  3. put down the heat mat   4. connect the Bunsen burner to the gas tap.    5.  Close the air hole.  6. Ignite the lighter.  7.  Turn on the gas.  8. Open the air hole.  9.  Hold the Magnesium in the scissor tongs.  10. Put the Magnesium  in to the blue flame.  11. observe  What happens.

Variables: Equipment: heat mat , Bunsen burner , Scissor tongs , Magnesium , Lighter ,  Safety goggles

When I burned solid shiny grey magnesium on the Bunsen burner  it formed a bright white light and lasted for 2 - 3 seconds.Then it flashed out.Some sort of white powder was left behind.

Reaction

When magnesium is in its metal form it will burn very easily in air. However, in order to start the reaction (the burning) the magnesium metal needs a source of energy. The flame provides a source of heat so that the magnesium metal atoms can overcome their activation energy. Activation energy is the minimum energy required in order for a chemical reaction to proceed. When the magnesium metal burns it reacts with oxygen found in the air to form Magnesium Oxide. A compound is a material in which atoms of different elements are bonded to one another. Oxygen and magnesium combine in a chemical reaction to form this compound. After it burns, it forms a white powder of the magnesium oxide. Magnesium gives up two electrons to oxygen atoms to form this powdery product. This is an exothermic reaction. An exothermic reaction is a term that describes a chemical reaction in which there is a net release of energy (heat).

2Mg(s)+O2(g)→2MgO(s)+energy(1)$$\begin{array}{}\text{(1)}& 2M{g}_{(s)}+O_{2(g)}\to 2Mg{O}_{(s)}+\text{energy}\end{array}$$

Magnesium is also capable of reducing water to the highly-flammable hydrogen gas, which will be ignited by the excess heat given by the reduction reaction.

Mg(s)+2H2O→Mg(OH)2(s)+H2(g)(2)$$\begin{array}{}\text{(2)}& \mathit{M}{\mathit{g}}_{\mathbf{(}\mathit{s}\mathbf{)}}\mathbf{+}\mathbf{2}{\mathit{H}}_{\mathbf{2}}\mathit{O}\mathbf{\to }\mathit{M}\mathit{g}\mathbf{(}\mathit{O}\mathit{H}{\mathbf{)}}_{\mathbf{2}\mathbf{(}\mathit{s}\mathbf{)}}\mathbf{+}{\mathit{H}}_{\mathbf{2}\mathbf{(}\mathit{g}\mathbf{)}}\end{array}$$

Magnesium also reacts with carbon dioxide to form magnesium oxide and carbon:

Mg(s)+CO2→2MgO(s)+C(s)(3)$$\begin{array}{}\text{(3)}& \mathit{M}{\mathit{g}}_{\mathbf{(}\mathit{s}\mathbf{)}}\mathbf{+}\mathit{C}{\mathit{O}}_{\mathbf{2}}\mathbf{\to }\mathbf{2}\mathit{M}\mathit{g}{\mathit{O}}_{\mathbf{(}\mathit{s}\mathbf{)}}\mathbf{+}{\mathit{C}}_{\mathbf{(}\mathit{s}\mathbf{)}}\end{array}$$

Hence, carbon dioxide fire extinguishers cannot be used for extinguishing magnesium fires either. Burning magnesium is usually quenched by using a Class D dry chemical fire extinguisher, or by covering the fire with sand to remove its air source.

http://chemwiki.ucdavis.edu/Under_Construction/Demonstrations/Burning_Magnesium

Evaluation: other experiments related to this I could do are :
. does all metal burn brightly . how could magnesium burn so quick .why does magnesium burn  with gas.

Results: up above in red.

Discussion:

conclusion: My  hypothesis was that it will turn tiny or melt in to a bunch  of metal I hope you enjoyed my magnesium report. :)