Thermite Reaction: The metal dioxide and metal powder make up thermite, which is a pyrotechnic composition. Thermite undergoes an exothermic reduction-oxidation (redox) reaction when ignited by heat or chemical reaction. In general, this kind of plant is not explosive, but it can create brief bursts of high temperature and heat in a small space. Likewise, black powder’s action is similar to that of fuel-oxidizer mixtures.

Thermites come in a variety of compositions. The following materials are used as fuels: aluminum, magnesium, titanium, zinc, silicon, and boron. The low cost and high boiling point of aluminum make it a common metal. Oxidizers include bismuth(III) oxide, boron(III) oxide, silicon(IV) oxide, chromium(III) oxide, manganese(IV) oxide, iron(III) oxide, iron(II,III) oxide, copper(II) oxide, and lead(II,IV) oxide.

In thermite welding, the process is also known as the Goldschmidt process. Incendiary weapons and disabling munitions are also used for thermometers. Pyrotechnic initiators similar to thermite are commonly used in fireworks.

What Is a Thermite Reaction in Chemistry?

An interesting chemical reaction you can try is the thermite reaction. It’s basically the same thing as burning metal, except much more quickly than with normal oxidation. A practical application (e.g., welding) of this elementary reaction is easy to accomplish. Despite the reaction being highly exothermic and potentially dangerous, don’t be afraid to try it. However, use proper safety precautions.

Thermite Reaction
Thermite Reaction

Iron oxide is normally added to the aluminum powder to produce thermite. Binders (e.g., dextrin) are usually mixed into these reactants to keep them from separating, although you can mix the materials right before ignition without a binder. A thermometer will be able to tell when it has reached its ignition temperature, but don’t grind the ingredients together. The following are needed:

  • 50 g of finely powdered Fe2O3
  • 15 g of aluminum powder

You can recover aluminum powder from the inside of an Etch-a-Sketch if you cannot find aluminum powder. A blender or spice mill can also be used to blend aluminum foil. You must be careful! There is a toxic element in aluminum. Avoid inhaling the powder or touching your skin with your bare hands. Clean your clothes as well as any instruments that may have been exposed to the electricity. In comparison to the solid metal, you come in contact with every day, aluminum powder is much more reactive.

Both rust and magnetite contain iron oxide. Magnetite can be found on beaches by running a magnet through the sand. (For instance, rust from a skillet can also contribute to iron oxide.)

It is only a matter of choosing the right source of heat to ignite the mixture once you have it.

Perform the Thermite Reaction

  • It takes a lot of heat to initiate the thermite reaction due to its high ignition temperature.
  • A propane or MAPP gas torch can be used to light the mixture. It is important to use caution when using gas torches because they provide reliable, consistent heat. The reaction tends to be sensitive to your proximity.
  • Fuse can be made from magnesium strips.
  • Sparklers can be used to light the mixture. Sparklers are one of the cheapest and easiest options, but they don’t provide constant heat. To light a sparkler, use a large one instead of a small colored one.
  • The mixture can be ignited with a lighter or matchbook if you are using powdered iron (III) oxide and aluminum. Avoid flash burns by using tongs.
  • The liquid metal can be picked up using tongs after the reaction has ended. Place the metal into the water but do not pour water on it.
  • Depending on which metals you used, the thermite reaction involves a chemical reaction involving oxidation or burning.

The Thermite Reaction Chemical Reaction

In addition to black or blue iron oxide (Fe3O4), red iron (III) oxide (Fe2O3), manganese oxide (MnO2), chromium oxide (Cr2O3), and copper (II) oxide can all be used. Metals are almost always oxidized by aluminum.

The typical chemical reaction is:

Fe2O3 + 2Al → 2Fe + Al2O3 + heat and light

The reaction is both an oxidation-reduction reaction and an example of combustion. Oxidation of one metal reduces its oxide. Adding another source of oxygen can increase the rate of the reaction. A spectacular display results from performing the thermite reaction on a bed of dry ice (solid carbon dioxide).


Because of its high temperature and difficulty in stopping the reaction once it is initiated, thermite usage is extremely hazardous. During the reaction, small streams of molten iron escape over considerable distances, melting metal containers and igniting their contents. Furthermore, flammable metals with very low boiling points, such as zinc (with a boiling point of 907 °C, about 1,370 °C below the temperature at which thermite burns), could potentially spray superheated boiling metal violently into the air, for some reason, thermite is contaminated with organics, hydrated oxides and other compounds able to produce gases upon heating or reaction with thermite components, the reaction products may be sprayed.

A mixture of thermite and air, given enough empty spaces, can also be sprayed if it burns fast enough and contains enough air. The following reasons make it desirable to use relatively crude powders with moderate reactions so that hot gases can escape the reaction zone.

By pouring new thermite over hot, freshly ignited slag, for example, one can accidentally preheat thermite before ignition. A lit piece of preheated thermite can burn almost instantly, releasing light and heat at a much higher rate than normal, causing burns and eye damage at a distance that would otherwise be fairly safe.

Thermite can form accidentally when workers use ferrous metals to grind and cut wheels using abrasive materials. Aluminum can react with these oxides violently in this situation; this creates an explosion risk.

Mixing water with thermite or pouring water onto burning thermite can cause a steam explosion, spraying hot fragments in all directions.

One of the thermite’s main ingredients was also used to coat or dope the Hindenburg, probably contributing to its fiery demise, due to its properties in reflecting heat and insulating heat. This was a theory put forward by the former NASA scientist Addison Bain and later tested on a small scale by the scientific reality-TV show MythBusters with semi-inconclusive results (it was proven not to be the fault of the thermite reaction alone, but instead conjectured to be a combination of that and the burning of hydrogen gas that filled the body of the Hindenburg).

Another video found on the Internet was also tested by the MythBusters program, in which a quantity of thermite was ignited while sitting atop several blocks of ice, causing a sudden explosion. As far as 50m from the explosion point, they found chunks of ice. Jamie Hyneman speculated that the mixture may have been aerosolized, perhaps by steam, causing it even faster to burn.

As well as being skeptical about one theory, he also voiced skepticism about another one: the idea that the reaction separated hydrogen from oxygen in the ice and caused it to ignite. In this explanation, aluminum molten at high temperatures reacts with water to cause an explosion. In high temperatures, aluminum releases hydrogen and oxidizes, releasing oxygen in the process.  

Thermite Reaction Safety Notes

During thermite reactions, the temperature rises rapidly. You can also damage your eyes from looking at the very bright light produced by the reaction in addition to getting burned if you get too close to it or have material ejected from it. Fire-safe surfaces should only be used for thermite reactions. Try to ignite the reaction from a far distance, while wearing protective clothing.