The boiling point of carbon, an element that is not metallic, is determined by its allotrope. Carbon exhibits various allotropes, such as graphite and diamond, each possessing distinct physical characteristics. Graphite, comprising layers of carbon atoms organized in a hexagonal lattice, lacks a boiling point because it directly transitions from a solid to a gas through sublimation. Conversely, diamond, composed of carbon atoms arranged in a three-dimensional lattice, also lacks a boiling point as it undergoes direct sublimation. Consequently, carbon, in its pure elemental form, does not possess a boiling point.
The boiling point of carbon, a nonmetallic element, depends on its allotrope. Carbon has multiple allotropes, including graphite and diamond, each with different physical properties. Graphite, which consists of layers of carbon atoms arranged in a hexagonal lattice, does not have a boiling point since it sublimes directly from a solid to a gas. On the other hand, diamond, which is composed of carbon atoms arranged in a three-dimensional lattice, also does not have a boiling point as it undergoes direct sublimation. Therefore, carbon does not have a boiling point in its pure elemental form.
The boiling point of carbon is approximately 4,827 degrees Celsius (8,740 degrees Fahrenheit).
