Fireworks get many of their colors from heated metal compounds. When atoms in these compounds gain energy and then release it, they emit light at characteristic wavelengths. Different elements produce different colors, while the firework’s design controls when and where the colors appear.
Heat excites atoms
A firework’s burning mixture heats color-producing compounds. Energy raises electrons in atoms to higher states; as they return to lower-energy states, they emit light. The wavelengths emitted determine the colors people see. [1]
Different elements give different colors
Common examples include strontium compounds for red, barium compounds for green, and copper compounds for blue. The exact shade also depends on temperature, chemical formulation, and how cleanly the compounds emit their light. [2]
The burst pattern is a separate design
The colored “stars” are arranged inside the shell. Their positions and timing influence the visible pattern—such as a sphere, ring, or willow-like trail—while the compounds determine much of the color.
Why can some fireworks look white or gold?
Some effects come from hot metal particles or mixtures that emit a broad range of visible wavelengths, which can appear white, gold, or silver.
Sources and evidence
- American Chemical Society — What’s in fireworks, and what produces those colorful explosions? ↗
Explains that modern firework colors use metal chlorides and gives examples of color-producing compounds.
- American Chemical Society — Further Exploration: Fireworks ↗
Describes metal salts in firework stars as the source of colored light.
Sources consulted: 15 October 2026. Written with AI assistance and checked against the linked references; not independently reviewed by a subject specialist. Sources do not endorse this article. See our editorial policy.
Revision: Initial publication; the explanation was checked against linked institutional, medical, or scientific references. This article was prepared with AI assistance and has not received independent expert review.