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Diamond and graphite are allotropes of carbon. In diamond, each carbon atom is bonded to four other carbon atoms, forming a solid three-dimensional structure; In graphite, on the other hand, carbon atoms are bonded to each other in a two-dimensional plane, forming large, flat plates that are stacked on top of each other. These sheets slide easily over each other; This is why graphite is a good lubricant. The reason why graphite leaves marks on paper is that these thin sheets of atoms separate from graphite and accumulate on the paper. Apart from diamond and graphite, carbon also has artificial allotropes such as natural, glassy carbon such as hexagonal diamond, fullerenes clustered diamond nanorods, carbon nanofoam, linear acetylenic carbon (LAC). Amorphous carbon is an allotrope of carbon that does not have a distinctive structure or form of its own. Coal is in this form.

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Rhombic sulfur (S); It consists of S8 molecules. It is bright yellow in color, odorless. It is insoluble in water. Its crystals are diamond-shaped. Stable up to 95.5°C.
Monoclinic sulfur; It consists of S8 Molecules. Dull yellow color, odorless, insoluble in water. The crystals are needle-shaped. Stable up to 119°C.
Liquid sulfur; It consists of S8 molecules. It is light yellow in color and odorless, insoluble in water. It does not show crystal structure. It is fluid at 160°C. At this temperature, S8 rings open and long spiral chain molecules are formed.
sulfur vapor; As the temperature increases, the molecules move away from each other. Sulfur vapor contains S8, S6, S4, S2 molecules.

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Phosphorus exists in nature in three different forms. These different forms are called allotropes. These are white phosphorus, red phosphorus and black phosphorus.

White phosphorus is the most common allotrope of phosphorus in nature. It is crystalline and melts at 44.25 °C. Its most important features are that it glows in the dark and is very conspicuous. In contact with air, it ignites and burns with white fumes. That's why they're in bottles of water. White phosphorus is used for insect and rat poison, fog and grenades.

Red phosphorus is made up of sunlight and heat from white phosphorus. White phosphorus is not easily ignited, radiant and not accidental. Melting is much higher. Red phosphorus matches are used.

Black phosphorus is covered by the airless effect of white. It is required for the production of black phosphorus fillings.

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Tin has two main allotropes, alpha-tin and beta-tin. It is gray or alpha-tin stable at low temperatures and has a cubic crystal structure similar to silicon and germanium. It turns white or beta-tin when heated above 13.2 °C. White tin has a tetragonal crystalline structure. When cooled, it slowly turns into a gray form, a condition known as tin disease. This conversion is affected by the presence of impurities such as aluminum and zinc and can be prevented by the addition of antimony or bismuth.