Molecular Structure of White Phosphorus

Oct 13, 2025 by windailys.com 20 views

The Chemistry of White Phosphorus: Understanding its Properties and Reactions

White phosphorus is a highly reactive and toxic chemical compound made up of four phosphorus atoms. It is a waxy, white solid that is highly flammable and can ignite spontaneously in air at room temperature. In this article, we will delve into the properties and reactions of white phosphorus, including its molecular structure, chemical reactions, and safety precautions.

Molecular Structure of White Phosphorus

White phosphorus consists of a molecule made up of four phosphorus atoms. The molecular formula for white phosphorus is P4, indicating that it is composed of four phosphorus atoms. The phosphorus atoms in white phosphorus are bonded together in a tetrahedral arrangement, with each phosphorus atom bonded to three other phosphorus atoms.

Chemical Reactions of White Phosphorus

White phosphorus is highly reactive and can undergo a variety of chemical reactions. One of the most common reactions of white phosphorus is its combustion in pure oxygen to produce tetraphosphorus decaoxide. This reaction is represented by the following equation:

${ P_4(s) + 5 O_2(g) \rightarrow P_4 O_{10}(s) }$

In this reaction, the white phosphorus reacts with oxygen to form a solid product called tetraphosphorus decaoxide. This reaction is highly exothermic, releasing a large amount of heat energy.

Safety Precautions when Handling White Phosphorus

White phosphorus is a highly toxic and flammable chemical compound that requires special handling and safety precautions. When handling white phosphorus, it is essential to wear protective clothing, including gloves, goggles, and a face mask. The substance should be handled in a well-ventilated area, away from any open flames or sparks.

A 1.00 g piece of phosphorus is burned in a flask filled with pure oxygen. The reaction is represented by the following equation:

${ P_4(s) + 5 O_2(g) \rightarrow P_4 O_{10}(s) }$

To solve this problem, we need to determine the number of moles of phosphorus that are present in the 1.00 g sample. We can do this by using the molar mass of phosphorus, which is 30.97 g/mol.

Calculating the Number of Moles of Phosphorus

The number of moles of phosphorus can be calculated using the following formula:

${ n = \frac{m}{M} }$

where n is the number of moles, m is the mass of the substance, and M is the molar mass.

Plugging in the values, we get:

${ n = \frac{1.00 \text{ g}}{30.97 \text{ g/mol}} = 0.0323 \text{ mol} }$

Determining the Number of Moles of Oxygen

To determine the number of moles of oxygen that are required to react with the phosphorus, we need to use the balanced equation for the reaction. From the equation, we can see that 5 moles of oxygen are required to react with 1 mole of phosphorus.

Therefore, the number of moles of oxygen required to react with the 0.0323 mol of phosphorus is:

${ n = 5 \times 0.0323 \text{ mol} = 0.1615 \text{ mol} }$

Calculating the Mass of Oxygen Required

The mass of oxygen required can be calculated using the molar mass of oxygen, which is 32.00 g/mol.

Plugging in the values, we get:

${ m = n \times M = 0.1615 \text{ mol} \times 32.00 \text{ g/mol} = 5.17 \text{ g} }$

In conclusion, white phosphorus is a highly reactive and toxic chemical compound that requires special handling and safety precautions. Its molecular structure consists of four phosphorus atoms bonded together in a tetrahedral arrangement. The chemical reactions of white phosphorus include its combustion in pure oxygen to produce tetraphosphorus decaoxide. When handling white phosphorus, it is essential to wear protective clothing and handle the substance in a well-ventilated area.

"White Phosphorus" by Wikipedia
"Chemical Reactions of White Phosphorus" by Chemistry LibreTexts
"Safety Precautions when Handling White Phosphorus" by ScienceDirect

National Institute for Occupational Safety and Health (NIOSH)
Occupational Safety and Health Administration (OSHA)
American Chemical Society (ACS)
Frequently Asked Questions about White Phosphorus =====================================================

Q: What is white phosphorus?

A: White phosphorus is a highly reactive and toxic chemical compound made up of four phosphorus atoms. It is a waxy, white solid that is highly flammable and can ignite spontaneously in air at room temperature.

Q: What are the properties of white phosphorus?

A: White phosphorus is a highly reactive and toxic chemical compound that is highly flammable and can ignite spontaneously in air at room temperature. It has a molecular formula of P4 and a molar mass of 123.88 g/mol.

Q: What are the safety precautions when handling white phosphorus?

A: When handling white phosphorus, it is essential to wear protective clothing, including gloves, goggles, and a face mask. The substance should be handled in a well-ventilated area, away from any open flames or sparks.

Q: What are the chemical reactions of white phosphorus?

A: White phosphorus can undergo a variety of chemical reactions, including its combustion in pure oxygen to produce tetraphosphorus decaoxide. This reaction is represented by the following equation:

${ P_4(s) + 5 O_2(g) \rightarrow P_4 O_{10}(s) }$

Q: What is the molecular structure of white phosphorus?

A: The molecular structure of white phosphorus consists of four phosphorus atoms bonded together in a tetrahedral arrangement.

Q: What is the molar mass of white phosphorus?

A: The molar mass of white phosphorus is 123.88 g/mol.

Q: What is the density of white phosphorus?

A: The density of white phosphorus is 1.823 g/cm3.

Q: What are the uses of white phosphorus?

A: White phosphorus has a variety of uses, including in the production of matches, fireworks, and other pyrotechnic devices.

Q: What are the hazards of white phosphorus?

A: White phosphorus is highly toxic and can cause severe burns and other injuries if not handled properly. It is also highly flammable and can ignite spontaneously in air at room temperature.

Q: How should white phosphorus be stored?

A: White phosphorus should be stored in a well-ventilated area, away from any open flames or sparks. It should be kept in a sealed container and handled with care.

Q: What are the regulations regarding the handling and storage of white phosphorus?

A: The handling and storage of white phosphorus are regulated by various government agencies, including the Occupational Safety and Health Administration (OSHA) and the Environmental Protection Agency (EPA).

Q: What are the environmental concerns associated with white phosphorus?

A: White phosphorus can contaminate soil and water if not handled properly. It can also cause environmental damage if released into the atmosphere.

Q: How can white phosphorus be disposed of?

A: White phosphorus should be disposed of in accordance with local and national regulations. It should be handled and stored with care, and disposed of in a sealed container.

In conclusion, white phosphorus is a highly reactive and toxic chemical compound that requires special handling and safety precautions. Its properties, chemical reactions, and uses are discussed in this article, along with the safety precautions and regulations regarding its handling and storage.