![]() Graphene, single layer graphite arranged in a two-dimensional honeycomb lattice, shows impressive enhancement in these properties, which makes it employable in the manufacturing of fast-charging batteries that are used as a power source in smartphones. The excellent conductivity of graphite due to the presence of free electrons, along with magnificent porosity, durability, lightweight, and low cost, makes it one of the most preferable materials for the manufacturing of anodes for ion batteries. A key component that has paved the way for this success story in the past almost 30 years is graphite, which has served as a lithium-ion host structure for the negative electrode. The modern world of technology is mostly about making gadgets portable and easy to access, which has significantly increased the demand for portable power sources that we call batteries. England enjoyed a monopoly on the production of pencils until a method of reconstituting the graphite powder was found in 1662 in Italy. After the commercialization of graphite as pencil lead, it soon emerged as a preferable material of choice for the manufacturing of cannonballs. ![]() There is a common misconception that pencil contains the element lead however, lead was only used to write or paint in the stone age and there is no evidence that lead was ever used to write on paper. In fact, the word graphite is from the Greek language which translates as “to write.” Graphite leaves the mark on paper by physical abrasion, which can be easily erased with rubber, but they are otherwise resistant to moisture, most chemicals, ultraviolet radiation, and natural aging. Pencil lead is perhaps the most common application of graphite that many of us are aware of. Let’s discuss a few uses of graphite in everyday life. The most prominent attribute of graphite is its stability under standard temperature and pressure conditions, which makes it widely applicable for several uses in daily life. Since graphite displays low adsorption of X-rays and neutrons, it is very valuable in nuclear applications. It is also chemically inert and highly refractory. Although graphite is flexible, it is non-elastic and has high electrical and thermal conductivity. Nonetheless, the lattice structure of the carbon atoms within diamonds contains three-dimensional lattice bonds, whereas graphite contains two-dimensional lattice bonds that make the structure more vulnerable to deformation. Contrary to popular belief, carbon-carbon bonds are stronger in graphite than diamond. Since the bonds between planes are weak, deforming the solid by moving one plane relative to another is easy in graphite. (Graphite’s extremely high melting and boiling points are due to the strong bonding between carbon atoms within each plane.) However, the distance between these atom planes is substantially more than the distance between atoms within the planes. It is made up of extended planes of sp2-hybridized carbon atoms securely bonded to three other carbon atoms. Graphite, anciently known as plumbago, is a crystalline allotrope of carbon, with its atoms arranged in hexagonal structures. These two structurally different arrangements of the same element are known as allotropes. ![]() ![]() While carbon can attach to itself in one manner to form the hardest material called diamond, it can also arrange itself to form one of the softest known substances called graphite. Interestingly, this tetravalent nonmetallic element can exist in several forms and form a variety of compounds. ![]() When we talk about the chemical element carbon, the first thing that may come to our mind is carbon dioxide gas. ![]()
0 Comments
Leave a Reply. |
AuthorWrite something about yourself. No need to be fancy, just an overview. ArchivesCategories |