Account for the differences in the physical and chemical properties of dinitrogen and white phosphorous based on their Lewis structures. Why is red phosphorous stable in air whereas white phosphorous burns violently?

a-The dinitrogeno is a mononuclear diatomic formed by two nitrogen atoms united by a covalent union instead the white phosphorus is a common allotrope of the chemical element phosphorus, nowadays it exists as molecules integrated by four muscles in a tetrahedral structure

b-In addition to its offensive capabilities, white phosphorus is also a highly efficient smoke agent, capable of rapid burning and producing instant smoke screens. For this reason, white phosphorous ammunition is common in infantry smoke grenades and grenade launchers, as well as tank, armored vehicle, cannon, and mortar ammunition.

The incandescent particles of white phosphorus produced in the initial explosion can produce deep, extensive and painful second and third degree burns. Phosphorus burns carry a higher mortality than other types of burns due to the absorption of phosphorus in the body through the areas reached, damaging internal organs such as the heart, liver or kidney.

These weapons are particularly dangerous to personnel because white phosphorus burns unless it is deprived of oxygen or until it is completely consumed, in some cases reaching the burn to the bone. In other cases, burns may be limited to areas where the skin is exposed because phosphorous particles do not completely burn through clothing. According to GlobalSecurity.org, quoted by The Guardian, "White phosphorus causes painful chemical burn damage."

Explanation:

Each chemical component presents different presentations in their orbits, and different amounts of electrons, this makes them act in different ways, some when reacting can be lethal and others not, on the other hand it is important to consider the simplicity of these molecules and the consequences they generate , and this only happens by the forces of their unions.

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