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Chapter 14: Problem 6

Give an account of the various allotropes of phosphorus.

Short Answer

Expert verified
The main allotropes of phosphorus include white, red, black, and violet phosphorus. The white one is a waxy white solid with tetrahedral P4 molecules, it glows in the dark. Red phosphorus is less reactive, doesn't glow and is made of chains of linked P4 tetrahedra. Black phosphorus is the least reactive, having a layered structure similar to graphite and each atom is coordinated to three others. Violet Phosphorus is a polymeric structure made by annealing red phosphorus above 550 degrees Celsius.

Step by step solution

01

Discussing White Phosphorus

White Phosphorus is the most common allotrope and it is typically used in industry. It is a waxy white solid, which glows in the dark due to slow oxidation. Its structure is made up of P4 molecules, where each P atom is connected to the others through single bonds, forming a tetrahedral shape.
02

Discussing Red Phosphorus

Red Phosphorus is much less reactive than white phosphorus and does not glow in the dark. Its structure is made of chains of linked P4 tetrahedra. Red phosphorus can be obtained by heating white phosphorus at high temperatures or under sunlight.
03

Discussing Black Phosphorus

Black Phosphorus is the least reactive allotrope and the most stable under standard conditions. It has a layered structure, quite similar to graphite. Each phosphorus atom in black phosphorus is coordinated to three others.
04

Discussing Violet Phosphorus

Violet Phosphorus is a form of phosphorus that can be produced by day-long annealing of red phosphorus above 550 degrees Celsius. It has a complex polymeric structure.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

White Phosphorus
White Phosphorus is one of the most well-known forms of phosphorus. It appears as a waxy solid and is recognized for its ability to glow faintly in the dark. This glow comes from its slow oxidation when exposed to air. An interesting aspect of white phosphorus is its molecular structure, which consists of P4 tetrahedra. Within this tetrahedral structure, each phosphorus atom is bonded to three others, forming a distinct three-dimensional shape.
  • Highly reactive
  • Used industrially in the manufacture of chemicals like phosphoric acid
  • Can spontaneously ignite in air, making it dangerous to handle without water or inert gases
Despite its dangerous reactivity, white phosphorus has significant industrial applications, primarily because it serves as a precursor to many phosphorus compounds.
Red Phosphorus
Red Phosphorus is another important allotrope of phosphorus and is characterized by its stability compared to white phosphorus. It doesn鈥檛 glow in the dark, making it much safer to handle than its white counterpart. Structurally, red phosphorus consists of a network of linked P4 tetrahedra that form long chains.
  • Less reactive than white phosphorus
  • Commonly used in safety matches, fireworks, and as a flame retardant
  • Can be produced by heating white phosphorus
Red phosphorus is favored for uses where stability is essential, as its reduced reactivity lowers the risk of hazardous scenarios.
Black Phosphorus
Black Phosphorus stands out among its peers due to its stability and layered, graphite-like structure. It is the least reactive of all phosphorus allotropes and is stable under standard conditions. In black phosphorus, the atoms are arranged in layers where each atom is bonded to three others in a much more ordered fashion.
  • Appears as a black crystalline solid
  • Has potential applications in electronics, similar to graphene, due to its semiconductive properties
  • Formed from high-pressure processing of white phosphorus
Its unique properties make black phosphorus a subject of interest in technological and material science research, particularly for the next-generation electronic devices.
Violet Phosphorus
Violet Phosphorus is the least well-known allotrope and boasts a complex polymeric structure. It is produced through the process of high-temperature annealing of red phosphorus, typically above 550 degrees Celsius.
  • Limited industrial applications compared to other allotropes
  • Research interest due to its distinct structure
  • Less reactive, similar to red and black phosphorus
Though violet phosphorus is not as prevalent in industrial applications as the other allotropes, its unique characteristics offer exciting potential for further study to uncover new uses and properties.

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Most popular questions from this chapter

Give an account of the preparation and properties of the following substances. (a) Hydrazoic acid (b) Phosphoric acid (c) White arsenic

Discuss the structure of the following: (a) \(\mathrm{HNO}_{2}\) (b) \(\mathrm{N}_{2} \mathrm{H}_{4}\) (c) \(\mathrm{H}_{3} \mathrm{PO}_{3}\) (d) \(\mathrm{PH}_{3}\) (e) \(\mathrm{PCl}_{5}\)

Give reasons for the following: (a) \(\mathrm{NCl}_{3}\) is hydrolysed but \(\mathrm{NF}_{3}\) is stable. (b) \(\mathrm{PCl}_{5}\) is known but \(\mathrm{NCl}_{5}\), does not exist. (c) Bismuth shows mainly +III oxidation states. (d) Nitrogen shows-III oxidation state.

Discuss the oxidising action of dilute and conc. nitric acid with the help of suitable examples.

Discuss the comparative account of the properties of the trihalides of Group 15 elements.
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