Explain why the type of metal used in creating fireworks determines the colour seen when the fireworks are set off. Discuss what occurs within the metal atoms.
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The type of metal used in creating fireworks plays a crucial role in determining the color seen when the fireworks explode. This is because the color of the light emitted by a material is closely related to the specific arrangement and energy levels of the atoms within the material.
When a firework explodes, the heat generated by the initial ignition causes the atoms in the metal to absorb energy. This energy excites the outermost electrons of the metal atoms, making them jump to higher energy levels or even become completely detached from the atom. However, this excited state is unstable, and the electrons rapidly return to their original energy levels.
As the electrons fall back to their original energy levels, they release the excess energy in the form of light. The specific amount and frequency of energy emitted determines the color of the light. Different metals have different electron configurations and energy level structures, leading to distinct colors when they emit light.
For example, when copper is used in fireworks, it emits blue or green light. Copper atoms have a specific arrangement of electrons in their outer energy level, which causes them to emit light in the blue or green part of the electromagnetic spectrum. Similarly, other metals like strontium produce red light, barium produces green light, and sodium produces yellow light.
In conclusion, the specific arrangement and energy levels of the atoms within a metal determine the color of light it emits when used in fireworks. By selecting different metals, firework creators can produce a range of vibrant colors to enhance the visual spectacle.