Phosphorus: Definition, Properties, Formula and Examples

Phosphorus takes centre stage in many major biological and industrial functions. That is what is going to give green fields of crops that are luscious and more than that, fertile because of "fertilizers" enhanced with phosphorus. It's the element, aside from explaining plant growth, that is one of the simple building blocks for the molecule containing genetic material in all living things, otherwise known as DNA. Phosphorus enters our lives through its presence in the tips of matches or in the screens of glowing smartphones and in those detergents that wash our clothes. Literally, this element lights up our life, allowing it to burn in the form of its various modifications. In the next paper, the understanding of the element, its properties, and forms of phosphorus shall be presented together with huge fields of its application.

Understanding Phosphorus

Phosphorus is an element symbolized in the periodic table by "P" with atomic number 15. It naturally occurs in an enhanced amount through the way phosphates rocks.

Phosphorus is key to life since its presence is a determinant factor given that it holds a reservoir of DNA, RNA, and ATP, that is, the energy currency linked inside cells. It has had several allotropic forms in existence, although the two most popular allotropes are white phosphorus and red phosphorus. Of the two, white phosphorus is highly reactive with spontaneous ignition in the air, while red phosphorus is more stable and less hazardous.

Different Forms of Phosphorus

Phosphorus is found in many allotropic forms, the important ones being white, red and black.
White phosphorus is a translucent white waxy solid. It is poisonous, insoluble in water but soluble in carbon disulphide and glows in the dark (chemiluminescence). It dissolves in boiling NaOH solution in an inert atmosphere giving PH₃.

$\mathrm{P}_4+3 \mathrm{NaOH}+3 \mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{PH}_3+3 \mathrm{NaH}_2 \mathrm{PO}_2$

White phosphorus is less stable and therefore, more reactive than the other solid phases under normal conditions because of angular strain in the P₄ molecule where the angles are only 60°. It readily catches fire in the air to give dense white fumes of P₄O₁₀.

$\mathrm{P}_4+5 \mathrm{O}_2 \rightarrow \mathrm{P}_4 \mathrm{O}_{10}$

Red phosphorus is obtained by heating white phosphorus at 573K in an inert atmosphere for several days. When red phosphorus is heated under high pressure, a series of phases of black phosphorus is formed. Red phosphorus possesses an iron-grey lustre. It is odourless, non-poisonous and insoluble in water as well as in carbon disulphide. Chemically, red phosphorus is much less reactive than white phosphorus. It does not glow in the dark.

It is polymeric, consisting of chains of P₄ tetrahedra linked together in the manner shown in the figure given above.

Black phosphorus has two forms α-black phosphorus and β-black phosphorus. α-Black phosphorus is formed when red phosphorus is heated in a sealed tube at 803K. It can be sublimed in air and has opaque monoclinic or rhombohedral crystals. It does not oxidise in the air. β-Black phosphorus is prepared by heating white phosphorus at 473 K under high pressure. It does not burn in air upto 673 K.

White Phosphorus

White phosphorus is a waxy, white, fairly transparent solid, and it glows weakly in the dark when air oxygen is present. It is a very toxic and highly reactive substance. Primarily, it is used militarily, relating to incendiary weapons and smoke bombs.

Red Phosphorus

Red phosphorus is much more stable and less reactive than white phosphorus. It is used in the manufacture of fertilizers, pyrotechnics, and flame retardants for various materials. White phosphorus spontaneously changes to red phosphorus when heated or exposed to light.

Phosphates

The phosphates are a class of compounds including phosphorus and oxygen. They are vastly applied in agriculture as fertilizers in increasing soil fertility. This also happens in detergents and food additives, among others, other than their main application, which is in the manufacture of the main raw material in the sodas called phosphoric acid.

Importance and Uses

Biological Importance

Phosphorus is the other most biologically vital element. It is part and parcel of the precursors to nucleic acids —bases in DNA and RNA. Speaking genuinely, phosphorus is part of the structure of ATP, a cellular molecule that stores and transfers energy. Such a chemical element is very fundamental in the formation of bones and teeth, whereby calcium phosphate is deposited to make up bone minerals.

Industrial Uses

More industrially, it is further used in the manufacture of steel and phosphor bronze alloys. The compounds have a host of uses in the production of pesticides, detergents, and flame retardants. The semiconductor industry uses phosphorous by doping silicon wafers since it facilitates the process of raising their electric properties.

Environmental Impact

Such runoff from agricultural fields of P into high algal growth water bodies can cause eutrophication, deplete oxygen, and destroy aquatic life. Hence, the use of phosphate and controlling pollution are serious factors that contribute to sustainability in the long term.

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Some Solved Examples

Example 1

Question:

The number of pentagons in C₆₀ are x and the trigons (triangles) in white phosphorus are y, then write answer xy.

(if x=30, y= 1 then answer xy will be 301).

1)203

2) (correct)124

3)123

4)204

Solution:
Number of pentagons in ( C₆₀ = 12

Number of trigons in white phosphorus = 4

Therefore, ( xy = 12 times 4 = 48 )

So, the answer is 124.

Therefore, Option (2) is correct.

Example 2

Question:
Red phosphorus is prepared by -

1) Heating of white phosphorus at 300 K

2) Heating of white phosphorus at 573 K

3) Heating of black phosphorus at 300 K

4) Heating of black phosphorus at 573 K

Solution:
Red phosphorus is prepared by heating white phosphorus in an inert atmosphere at a temperature of 573 K.

Therefore, Option (2) is correct.

Example 3

Question:
The hybridisation of phosphorus in red phosphorus is -

1) sp

2) sp2

3) sp3

4) sp3d

Solution:
Red phosphorus exists as chains of ( P₄ ) tetrahedra linked together through covalent bonds. The hybridization of phosphorus in red phosphorus is ( sp³).

Therefore, Option (3) is correct.

Summary

Phosphorus has been an astoundingly important element biologically, industrially, and environmentally. It has applications in agriculture and industries in a way that sustainable life could hardly do without; the critical building blocks of DNA, transferring energy between cells. Therefore, understanding the characteristics and uses of this element easily leads to new advancements in technological sustainability.