As all of you know, diamonds are anything but affordable, and graphite is — well, pretty cheap. Some of you might not have seen this big of a difference coming — but just remember how much does a graphite pencil cost. Well, the amount of graphite that goes inside your average pencil would be worth a staggering times more if it was a diamond heart.
Given the fact that there are only limited amounts of these materials, some of you might pose a valid question of the prices rising. Last year, Turkey ranked as the country with the most reserves of graphite that were around 90 million metric tons. China has around 73 million, and Brazil has around 70 million metric tons of graphite in reserves.
That might put into perspective how widely available this material is, especially when compared to a diamond. Russia is the country with the biggest reserves of diamonds in the world, with over million carats in their reserves. When you look at this data, you can clearly see that the difference in the reserves is also one of the largest ones — literally. And the rarity of a particular material plays a huge role in determining its price and value.
As you probably know, scarcity is one of the most significant factors for anything naturally formed on — or in — the Earth, such as gas, gold, and diamonds. The first thing that binds these two together is the fact that they both originate, or are a derivate, of pure carbon. The only difference is those processes that we talked about earlier.
It is known that graphite can be converted into diamond when subjected to high pressure and high temperatures. Similarities Between Graphite and Diamonds Carbon. Both graphite and diamonds are made out of pure carbon.
Covalent Bonds. The bonds that hold the carbon to each other are covalent bonds. High Melting Points. The melting points of both graphite and diamond are very high.
Naturally Occuring. Expert Answer: Both graphite and diamond are forms of carbon. As such, they are said to be allotropes of carbon. Both occur naturally.
Both are produced in the earth in geothermal processes. Both can be made artificially. Both are normally solids and highly stable. Diamond is a form of carbon in which each carbon atom is joined to four other carbon atoms, forming a giant covalent structure. As a result, diamond is very hard and has a high melting point. It does not conduct electricity as there are no delocalised electrons in the structure.
Integrated with its tendency to be clear, this causes the anemic, clear appearance of the majority of diamond. Blue diamonds come from boron pollutants, yellow diamond from nitrogen contamination, brownish diamonds from latticework defects, and environment-friendly diamonds from radiation direct exposure. Diamond have a hardness far surpassing compared to that of any other substance understood to us.
It has a very high level of openness and dispersion or 'fire'. As a result of its hardness a lot of the diamonds which are mined are made use of for industrial objective as well as few are taken right into gems.
Graphite is a non-metal. Both Diamond and also Graphite are a crystalline kind of carbon Both are made of pure carbon. They are the same in the chemical structure, they vary a whole lot in the physical make-up.
On the Moh s array, Diamond rates as 10 making it the hardest mineral as compared to Graphite, which is the softest. Thus, based upon the physical buildings, they are utilized for various functions. Also, as a result of the rarity, a Diamond is far more expensive than Graphite. Although they are made from the exact same component Carbon , a Diamond differs from Graphite in the atomic structure. In Diamonds, the atoms are carefully packed with together with each atom connected to various other carbon atoms as compared to Graphite where the bonds in between the layers are weak.
This is the reason why Diamonds have a extremely solid as well as inflexible framework. Both are pure carbon, however vary in crystalline framework because they are adhered differently. A carbon atom has 4 electrons that are unpaired as well as can develop bonds by pairing with electrons from various other atoms. When it comes to diamond and graphite we are speaking about just various other atoms of carbon.
In Diamond, all of the electrons are matched an covalent bonds to other carbon atoms. The diamond framework is hard to envision in 3 dimensional room, however very easy to see in a 3 dimensional version.
An average atom is about 0. If you have a nice x-ray source that provides a very specific wavelength of light, and you also have a very nice crystal, you can get very nice diffraction patterns. This technique is known as single-crystal x-ray diffraction. Darker spots come from heavier atoms higher atomic weights and lighter spots are due to lighter atoms. You cannot tell, though, what element is what.
Carbon atoms and nitrogen atoms, for example, are hard to tell apart in x-ray diffraction. You would need some additional measurements to confirm which elements make up your solid substance. Now: does it matter how atoms are arranged in a solid?
The answer here too is: Yes! The best example of this is carbon. We all know that carbon is one of the most important elements in our planet; all living things contain carbon. Pure carbon is known to us as diamond, if arranged one way in three dimensions; and graphite if arranged in another.
In diamond, all the carbon atoms have strong chemical bonds to four other carbon atoms, making perfect tetrahedra on and on throughout the crystal. In graphite, all the carbon atoms have strong chemical bonds to three other carbon atoms, making sheets that look like chicken wire; weak forces hold the sheets together in stacks that can slide past each other easily. Clearly the properties of diamond and graphite are very different.
Diamond is one of the hardest materials known, is transparent to light, and does not conduct electricity at all. Graphite is soft, gray, and can conduct electricity reasonably well.
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