MCQ Detailed View

The making of matchsticks is a classic example of applied chemistry. The main substance used in their production is phosphorus, which plays a vital role in the ignition process. Without phosphorus, the simple striking of a matchstick would not produce a flame.

In the earliest days, matchsticks were made with white phosphorus, which is highly reactive and ignites at low temperatures. However, it was extremely dangerous because it could cause accidental fires and severe health problems such as “phossy jaw” in factory workers. For this reason, white phosphorus was later banned.

Modern matchsticks use red phosphorus, which is safer and more stable. Red phosphorus is generally applied on the striking surface of the matchbox, not directly on the match head. When the match is struck against the box, a small portion of red phosphorus converts into white phosphorus due to friction and heat, which then ignites.

The match head itself usually contains a mixture of chemicals. Sulphur or antimony trisulfide acts as additional fuel, while potassium chlorate provides oxygen for combustion. Binders like starch and coloring agents are also added. Together, these substances ensure that the match burns steadily after ignition.

The striking surface of a matchbox contains powdered glass (to increase friction), red phosphorus, and an adhesive to hold the material together. The controlled reaction between the match head and the striking surface makes ignition safe and reliable.

In summary, phosphorus is the main element responsible for the functioning of matchsticks. It is used in combination with sulfur, oxidizers, and binders to create a safe, dependable, and long-lasting product. This chemical principle is a simple yet powerful example of how chemistry impacts our daily lives.