Re: Custom Elements Bureau
Custom element japanese name: kurokongouseki
Custom element english name: carbon release
The element is based on:
The ability to manipulate carbon into different forms in a simalar way as to which elements are. It can be controlled to change its shape and mass to create a wid ranges of elements.
Facts that prove the element to be possible (in the manga context):
Carbon is a naturally abundant nonmetallic element which forms the basis of most living organisms. Carbon is the fourth most abundant element in the universe, and it plays a crucial role in the health and stability of the planet through the carbon cycle. This cycle is extremely complex, and it illustrates the interconnection between organisms on Earth. Most consumers are familiar with the element, along with numerous forms in which it appears.
The atomic number of carbon is six, and the element is identified by the symbol “C” on the periodic table. The structure of carbon molecules is such that the molecules bond readily with a wide range of other elements, forming thousands of compounds. The molecules in carbon also bond with each other in different ways, creating forms of carbon such as diamonds, the hardest substance on Earth, and graphite, one of the softest materials on the planet. The changing personality of carbon, depending on what it bonds with and how, makes it a very unique element.
ll living organisms contain carbon, and as they decay or change, they will continue to contain the element. Coal, limestone, and petroleum, for example, are all fossilized forms of living organisms containing abundant amounts of carbon. Plants and animal life which died millions of years ago were slowly compressed into these substances, and their integral carbon was preserved. This residual carbon is used in everything from jet fuel to children's dolls.
Carbon itself, along with many of its forms, is relatively nonreactive. When it combines with some other elements such as hydrogen, carbon becomes more reactive, and this reactiveness is used to the advantage of industry. In the case of hydrocarbons, the compound is used as a source of energy. The immense versatility of carbon makes it highly useful in a number of industries. Carbon is burned to create fuel, used to filter various substances, and combined with iron to make steel. It also is used as the basis of drawing pencils and charcoals, to make synthetics like plastic, and, in the form of an isotope, as a dating tool for archaeologists.
On its own, carbon is not very dangerous, since it is nontoxic and nonreactive. However, some forms of carbon can be harmful to some organisms, such as carbon monoxide. Carbon may also appear in conjunction with more dangerous elements, or it may generate harmful dust in the case of coal and diamonds. Individual precautions for different forms of carbon vary widely, and it is a good idea to consult a Material Safety Data Sheet (MSDS) if you are concerned about a particular substance.
There are several allotropes of carbon of which the best known are graphite, diamond, and amorphous carbon. The physical properties of carbon vary widely with the allotropic form. For example, diamond is highly transparent, while graphite is opaque and black. Diamond is among the hardest materials known, while graphite is soft enough to form a streak on paper (hence its name, from the Greek word "to write"). Diamond has a very low electrical conductivity, while graphite is a very good conductor. Under normal conditions, diamond has the highest thermal conductivity of all known materials. All the allotropic forms are solids under normal conditions but graphite is the most thermodynamically stable.
All forms of carbon are highly stable, requiring high temperature to react even with oxygen. The most common oxidation state of carbon in inorganic compounds is +4, while +2 is found in carbon monoxide and other transition metal carbonyl complexes. The largest sources of inorganic carbon are limestones, dolomites and carbon dioxide, but significant quantities occur in organic deposits of coal, peat, oil and methane clathrates. Carbon forms more compounds than any other element, with almost ten million pure organic compounds described to date, which in turn are a tiny fraction of such compounds that are theoretically possible under standard conditions.
The different forms or allotropes of carbon (see below) include the hardest naturally occurring substance, diamond, and also one of the softest known substances, graphite. Moreover, it has an affinity for bonding with other small atoms, including other carbon atoms, and is capable of forming multiple stable covalent bonds with such atoms. As a result, carbon is known to form almost ten million different compounds; the large majority of all chemical compounds.[13] Carbon also has the highest melting and sublimation point of all elements. At atmospheric pressure it has no melting point as its triple point is at 10.8 ± 0.2 MPa and 4600 ± 300 K, so it sublimates at about 3900 K.
Carbon sublimes in a carbon arc which has a temperature of about 5800 K. Thus, irrespective of its allotropic form, carbon remains solid at higher temperatures than the highest melting point metals such as tungsten or rhenium. Although thermodynamically prone to oxidation, carbon resists oxidation more effectively than elements such as iron and copper that are weaker reducing agents at room temperature.
Atomic carbon is a very short-lived species and, therefore, carbon is stabilized in various multi-atomic structures with different molecular configurations called allotropes. The three relatively well-known allotropes of carbon are amorphous carbon, graphite, and diamond. Once considered exotic, fullerenes are nowadays commonly synthesized and used in research; they include buckyballs,[19][20] carbon nanotubes,[21] carbon nanobuds[22] and nanofibers.[23][24] Several other exotic allotropes have also been discovered, such as lonsdaleite,[25] glassy carbon,[26] carbon nanofoam[27] and linear acetylenic carbon.[28]
The amorphous form is an assortment of carbon atoms in a non-crystalline, irregular, glassy state, which is essentially graphite but not held in a crystalline macrostructure. It is present as a powder, and is the main constituent of substances such as charcoal, lampblack (soot) and activated carbon.
At normal pressures carbon takes the form of graphite, in which each atom is bonded trigonally to three others in a plane composed of fused hexagonal rings, just like those in aromatic hydrocarbons. The resulting network is 2-dimensional, and the resulting flat sheets are stacked and loosely bonded through weak van der Waals forces. This gives graphite its softness and its cleaving properties (the sheets slip easily past one another). Because of the delocalization of one of the outer electrons of each atom to form a π-cloud, graphite conducts electricity, but only in the plane of each covalently bonded sheet. This results in a lower bulk electrical conductivity for carbon than for most metals. The delocalization also accounts for the energetic stability of graphite over diamond at room temperature.
Some allotropes of carbon: a) diamond; b) graphite; c) lonsdaleite; d–f) fullerenes (C60, C540, C70); g) amorphous carbon; h) carbon nanotube.At very high pressures carbon forms the more compact allotrope diamond, having nearly twice the density of graphite. Here, each atom is bonded tetrahedrally to four others, thus making a 3-dimensional network of puckered six-membered rings of atoms. Diamond has the same cubic structure as silicon and germanium and because of the strength of the carbon-carbon bonds, it is the hardest naturally occurring substance in terms of resistance to scratching. Contrary to the popular belief that "diamonds are forever", they are in fact thermodynamically unstable under normal conditions and transform into graphite.[12] But due to a high activation energy barrier, the transition into graphite is so extremely slow at room temperature as to be unnoticeable.
Under some conditions, carbon crystallizes as lonsdaleite. This form has a hexagonal crystal lattice where all atoms are covalently bonded. Therefore, all properties of lonsdaleite are close to those of diamond.[25]
Fullerenes have a graphite-like structure, but instead of purely hexagonal packing, they also contain pentagons (or even heptagons) of carbon atoms, which bend the sheet into spheres, ellipses or cylinders. The properties of fullerenes (split into buckyballs, buckytubes and nanobuds) have not yet been fully analyzed and represent an intense area of research in nanomaterials. The names "fullerene" and "buckyball" are given after Richard Buckminster Fuller, popularizer of geodesic domes, which resemble the structure of fullerenes. The buckyballs are fairly large molecules formed completely of carbon bonded trigonally, forming spheroids (the best-known and simplest is the soccerball-shaped structure C60 buckminsterfullerene).[19] Carbon nanotubes are structurally similar to buckyballs, except that each atom is bonded trigonally in a curved sheet that forms a hollow cylinder.[20][21] Nanobuds were first published in 2007 and are hybrid bucky tube/buckyball materials (buckyballs are covalently bonded to the outer wall of a nanotube) that combine the properties of both in a single structure.[22]
Of the other discovered allotropes, carbon nanofoam is a ferromagnetic allotrope discovered in 1997. It consists of a low-density cluster-assembly of carbon atoms strung together in a loose three-dimensional web, in which the atoms are bonded trigonally in six- and seven-membered rings. It is among the lightest known solids, with a density of about 2 kg/m3.[29] Similarly, glassy carbon contains a high proportion of closed porosity.[26] But unlike normal graphite, the graphitic layers are not stacked like pages in a book, but have a more random arrangement. Linear acetylenic carbon[28] has the chemical structure[28] -(C:::C)n-. Carbon in this modification is linear with sp orbital hybridization, and is a polymer with alternating single and triple bonds. This type of carbyne is of considerable interest to nanotechnology as its Young's modulus is forty times that of the hardest known material – diamond.[30]
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Some allotropes of carbon: a) diamond; b) graphite; c) lonsdaleite; d–f) fullerenes (C60, C540, C70); g) amorphous carbon; h) carbon nanotube
I believe this to be used in the manga context as its just high level manipulation of earth element to gather carbon atoms and manipulating them with heat to be able to create new isotopes.
Idea behind its creation:
As of 2009, graphene appears to be the strongest material ever tested.[17] However, the process of separating it from graphite will require some technological development before it is economical enough to be used in industrial processes.[18]
The system of carbon allotropes spans a range of extremes:
Synthetic nanocrystalline diamond is the hardest material known.
Graphite is one of the softest materials known.
Diamond is the ultimate abrasive.
Graphite is a very good lubricant.
Diamond is an excellent electrical insulator.
Graphite is a conductor of electricity.
Diamond is the best known naturally occurring thermal conductor
Some forms of graphite are used for thermal insulation (i.e. firebreaks and heat shields)
Diamond is highly transparent.
Graphite is opaque.
Diamond crystallizes in the cubic system.
Graphite crystallizes in the hexagonal system.
Amorphous carbon is completely isotropic.
Carbon nanotubes are among the most anisotropic materials ever produced.
Reading this and seeing how versitile carbon is.
Conditions to be able to use it: Must have mastered earth and fire to be able to control carbon in its basic form and use heat to manipulate the atoms.
Though the user cannon make daimonds as its already someone elses C.e unless they gain permission
Is weak to: Strong fire jutsu due to the bonds being broken, water due to erotion or such.
Is strong against: lightning due to conducters, wind elements, and earth
Co-creators (if any):
Students i passed on this custom element: ? & ?
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~Declined~: Little to no proof that carbon could be used as a element. and please scale back on the book writing
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