- List the physical characteristics of each
- Explain the organization of carbon atoms for each
Explore carbon and graphite on the interactive website below. After you have an understanding of the organization of the carbon atoms for both, find fullerenes and
- Explain how the carbon atoms are organized and
- List some properties and uses of fullerenes.
Diamond- Hard, very strong, hardest substance on earth, crystalline structure, transparent
ReplyDeleteGraphite- Very soft, flakey, flexible, great conductor
Organization of Carbon Atoms - The organization of the diamond and graphite atoms is very different. The difference between the two is that the diamond is in more of a cluster formation, compared to the graphite which is in a layered formation.
Organization of Carbon Atoms in the fullerenes- The organization of the fullerenes is that it is arranged so that has equal patterns throughout. Its shape is circular, making it very durable.
Fullerenes
Circular, Only carbon, Hollow
Graphite physical attributes- weaker material than diamond.
ReplyDelete- layered material and formed in sheets.
- flexible and good conductor.
Diamond physical attributes- very strong material, especially compared to graphite.
- high melting point unlike graphite.
- crystalline structure.
Although both Graphite and Diamond are both made up of 100% carbon, they both have very different attributes. This is because their molecular structures are very different. In graphite, atoms and their covalent bonds are very strong in their own layers, but they are not strongly bonded to the other layers. This makes a weak substance with strong individual layers. Diamond on the other hand has intertwined atoms and bonds with each layer, so nothing is left weak, and the entire substance is very strong.
Fullerenes- Fullerenes are made up of just 60 carbon atoms and arranged spherically, hollow, and intertwined. Fullerenes can be use, mainly, to create the circular or hexagonal carbon shapes that make up nanotubes. Nanotubes can be used as insulators, semiconductors, or conductors, depending on their makeup.
Graphite: weak, soft, flaky, layered, etc.
ReplyDeleteDiamond: hardest substance, strong, durable, etc.
Graphite and Diamond are both composed of the same type of atom: Carbon atoms. However, Graphite is very weak and flaky, whereas Diamond is strong and durable. This is due to the differences in molecular structures. A Diamond's structure is more organized and layered, making it stronger. However, the organization of graphite atoms is more random than that of Diamond's.
A fullerene is a molecule that holds an organized and pattern-based structure of carbon atoms. The shape of a fullerene is a circle/hexagon that is hollow.
Diamonds: solid, hard, 4 directions of cleavage, broad color range, high melting point, very low reactivity to chemicals, rare, durable, transparent over a large range of wavelengths
ReplyDeleteA diamond’s carbon atoms are bonded together in a three-dimension frame like structure. They are all the same distance from the other carbon atoms and there is “a rigid network of bonds within the crystal” (worldofmolecules.com).
Graphite: soft, slippery, black silver colour, metallic or dull luster, opaque, 1-2 hardness, 1 direction cleavage, flaky
The carbon atoms in graphite are in a sheet like structure (only 2 dimensional), where the atoms lie in a plane, weakly bonded to the sheets above and below. They are organized with strong covalent bonds in each layer while weak forces lay between them. This makes it easier for the layers of atoms to slide over each other.
Fullerenes:
The fullerenes’ carbon atoms’ structure represents that of a soccer ball. It is “hollow, spherical, and arranged in interlocking hexagons and pentagons” (worldofmolecules.com). Fullerenes are being used in drug delivery for diseases like cancer and AIDs, and in nanotechnology. In nanotubes, they can be “insulators, semiconductors, or conductors” and they are very flexible.
Diamond physical characteristics:
ReplyDelete• Very, very hard and durable
• Many different colors
• Very low reactivity to chemicals
• High melting point
• Resistant to compression
• Electrical insulator
• Abrasive
• Transparent
• Crystallizes in the Isometric system
The carbon atoms of a diamond are bonded together very tightly, almost in connecting stacks.
Graphite:
• Soft
• High-strength in composites
• Conducts electricity
• Good lubricant
• Opaque
• Stable at surface temperatures and pressures
• Crystallizes in the hexagonal form
The carbon atoms are bonded in sheets which allow it to slide. When the sheets are rolled into fibers and the fibers are twisted into threads, the bonds are very strong.
Fullerene:
The carbon atoms in fullerene are bonds in a spherical form.
Uses: They have the potential to be used for delivering drugs to treat cancer, AIDS, and other diseases. They can also be used in nanotechnology. In nanotubes they can act as "insulators, semiconductors, or conductors."
Graphite
ReplyDelete• Weaker than diamond
• Formed in sheets
• Layered
• Good conductor
• Flexible
Diamond
• Extremely strong
• Crystal structure
• High melting point
Graphite and Diamond are both materials made from carbon. Graphite is a weaker substance than diamond because it uses layers. Although the individual layers may be very strong the bond between the layers is not. In diamond though all the components are strongly intertwined making it a overall very strong substance.
Fullerenes – These are made up of 60 carbon atoms and made up in a sphere. They are also hollow and intertwined with itself like diamonds. Fullerenes are often used to make nano tubes. Nano tubes can be used as insulators semi conductors or conductors. There use all depends on there make up.
Physical characteristics of Diamond:
ReplyDelete• Variety of colour
• Solid, hard and durable
• Transparent
• Electrical insulator
• High Melting point
Physical characteristics of Graphite:
• Soft
• Conducts electricity
• Lubricant
• Metallic grey and black
• Stable at surface temperatures
• Non-transparent
Organization of carbon atoms of Diamonds: bonds are very tight and strong, equidistant from each other, Organized into layers
Organization of carbon atoms of Graphite: looser bonds, allow more flexibility, randomly organized
Fullerenes: soccer-ball shaped, hexagonal, hollow and intertwined with self, commonly used to make nanotubes.
Diamond:
ReplyDeletePhysical-
Hard, Strong, high melting point, Transparent
The carbon atoms of a diamond are bonded very closely together.
Graphite:
Physical-
Weak, soft, Conducts electricity, Metallic grey and black
The carbon atoms of graphite are bonded in sheets. The structure of graphite and diamonds is what makes them either weak or strong.
The carbon atoms in fullerenes are hollow, arranged in interlocking pentagons and hexagons.
Graphite is weak, stiff, flakey, and is easily broken.
ReplyDeleteDimond is hard, strong, high melting point, transparent, and is not easily broken.
In graphite the atoms are not strongly bonded to the other layers. That is why the graphite is so weak. On the other hand, diamond has strong atoms and bonds with each layer. That is why teh diamond is so strong.
Fullerenes!
A molecule that hold a very neat and organized structure of carbon atoms, and the shape is a circle and it is hollow.
Diamond is hard, very strong, melts at a high temperature, is a good conductor of electricity, and is not broken easily.
ReplyDeleteGraphite is weak, easily broken, metallic grey or black.
Diamond atoms are bonded together strongly which is the reason diamond is so strong and hard. Graphite has loosely bonded atoms, making it soft and weak.
Fullerenes
A molecule that is attached with pentagons or hexagons intertwined, often used for nano tubes.