science of fireworks
Survey of the Sciences
Unit 4: The Science of Fireworks
7-7-14/7-14-14
What is a firework? An explosive or combustible used for display. In the 19th century the introduction of new ingredients such as magnesium and aluminum greatly heightened the brilliance of such displays. There are two main classes of fireworks, force-and-spark and flame. In force and spark compositions, potassium nitrate, sulfur, and finely ground charcoal are used, with additional ingredients that produce various types of sparks. In flame compositions, such as the stars that shoot out of rockets, potassium nitrate, salts of antimony, and sulfur maybe be used. For colored fire, potassium chlorate or potassium perchlorate is combined with a metal salt that determines the color. Inside each firework are small packets filled with chemicals, mainly metal salts and metal oxides, which react to produce an array of colors. When heated, the atoms of each element in the mix absorb energy causing its electrons to rearrange from their lowest energy state to a higher excited state. As the electrons plummet back down to their lower energy state the excess energy gets emitted as light.
Each element releases a different amount of energy and this energy is what determines the color or wavelength of the light that is emitted. For instance, when sodium nitrate is heated, electrons in the sodium atoms absorb the energy and get excited. When electrons come down from the high they release their energy, about 200 kilojoules per molecule, or the energy of yellow light. The recipe that creates blue includes varying amounts of copper chloride compounds and red comes from strontium and lithium salts. Like paints, secondary colors can be made by mixing the ingredients of their primary color relatives. A mixture of copper and strontium makes purple. Pure colors require pure ingredients. Careful formulation is required so that too much smoke or residue does not mask color. As with other things you get
Unit 4: The Science of Fireworks
7-7-14/7-14-14
What is a firework? An explosive or combustible used for display. In the 19th century the introduction of new ingredients such as magnesium and aluminum greatly heightened the brilliance of such displays. There are two main classes of fireworks, force-and-spark and flame. In force and spark compositions, potassium nitrate, sulfur, and finely ground charcoal are used, with additional ingredients that produce various types of sparks. In flame compositions, such as the stars that shoot out of rockets, potassium nitrate, salts of antimony, and sulfur maybe be used. For colored fire, potassium chlorate or potassium perchlorate is combined with a metal salt that determines the color. Inside each firework are small packets filled with chemicals, mainly metal salts and metal oxides, which react to produce an array of colors. When heated, the atoms of each element in the mix absorb energy causing its electrons to rearrange from their lowest energy state to a higher excited state. As the electrons plummet back down to their lower energy state the excess energy gets emitted as light.
Each element releases a different amount of energy and this energy is what determines the color or wavelength of the light that is emitted. For instance, when sodium nitrate is heated, electrons in the sodium atoms absorb the energy and get excited. When electrons come down from the high they release their energy, about 200 kilojoules per molecule, or the energy of yellow light. The recipe that creates blue includes varying amounts of copper chloride compounds and red comes from strontium and lithium salts. Like paints, secondary colors can be made by mixing the ingredients of their primary color relatives. A mixture of copper and strontium makes purple. Pure colors require pure ingredients. Careful formulation is required so that too much smoke or residue does not mask color. As with other things you get
References: About.com/chemistry Firework. (2014). Encyclopedia Britannica Live science.com