is Carbon60 an allotropic form of carbon?
464354
Yes.  It is one example of a buckminsterfullerene (or fullerene or buckyball), which is one carbon allotrope.  Carbon has many other allotropes, including: diamond, graphite, and carbon nanotubes.\n\nBruce (below), "allotrope" does not mean "isotope."
233938
im highly sceptical on that, because the bond angle of carbon is different from other chemicals, but if one was to be formed, i would imagine silicone or germanium would form it, although, silicone forms stronger bonds, which cant bend that easily, I THINK... not perticularly true... just an assumption on my part
702126
because....\n1) all organic compunds are made of carbon...\n2) the interatomic interaction is made up of covalent bond which is very strong....\n\nand only saturated compounds are stable... not all....\n"saturated" means the bonds between 2 carbon atoms are ALWAYS single bonds...
839410
This compound is an amine.  You can identify it by the NH2 (amine group) at the end.  You did a fair job with the structure considering the limits of the text here.  I am sure you realize that two of your carbons do not have the correct number of bonds.
953266
carbon can be found in a gaseous state (which you'll almost never encounter) and in a liquid state (which you'll also never encounter).  the only states that are useful are its 4 solid states: diamond, graphite (the stuff that pencil lead is made of), buckyballs (which are basically balls of carbon atoms bonded together in a soccer-ball-like pattern), and carbon nanotubes (which are sheets of carbon atoms wrapped up into tubes).
844956
Zero.  Carbon has 4 valence electrons, so it likes to form 4 bonds to give it a stable octet.  C is the central atom in CBr4, and since it's hooked up with 4 things, it's happy, and got nothing left over.  CCl4, CF4, and CH4 are similar to it in that respect.
643513
It is energetically more stable for carbon atoms to have the configuration of graphite at atmospheric pressure.  However, under lots of pressure, it obviously favors diamond.  It doesn't change back because even though it is more favorable to be graphite, it is much harder for carbon to do the changing necessary.  It's like, dropping a ball, if you drop it inside a 20 story building, it'll still only hit the floor in front of you.  It would have less potential energy on the 1st floor, but it would have to have lots more energy than it does to get there.
762916
In the proposed structure for C60(fullerenes), each vertex of the truncated icosahedron is occupied by a carbon atom, and each carbon is three-connected to other carbon atoms by one double bond and two single bonds. Carbon atoms with this kind of connectivity are usually referred to as "sp carbons" because the orbitals used to sigma-bond the three adjacent carbons are hybrids of the 2s orbital and the two 2p orbitals (2p and 2p). The remaining 2p orbital (2p) is responsible for the pi-bond.\n\nUsually, an sp carbon and its three neighboring atoms are all coplanar. This is the case, for example, in graphite where there are infinite planar sheets of sp carbons arranged in edge-sharing hexagons. The p orbitals all lie parallel to each other and perpendicular to the graphite plane, generating a sea of - electron density above and below the plane.\n\nIn graphite, the C-C bonds are all equal in length and intermediate between normal single and double bonds. This "delocalization" can be explained by noting that graphite has many different but equivalent "resonance structures". (The resonance structures differ only in the placement of the double bonds.) \nthe proposed structure for C60 is not planar! The angle between a p axis and a C-C bond vector is 101.6° (as compared to 90° in planar graphite) . The bowl-shape or concavity at each sp carbon center introduces some strain into the molecule. However, the high symmetry distributes that strain evenly across the entire structure.\n\n# Other Fullerenes\n\nThe truncated icosahedron is not the only possible fullerene-type structure. There are, in fact, many other hollow cage structures that can be constructed using only pentagons and hexagons (Kroto, 1987). Interestingly, each of these structures contains exactly twelve pentagons, while the number of hexagons is arbitrary. The pentagons are necessary for closure. (Recall that graphite, which consists only of fused hexagons, is essentially a planar sheet. While this sheet may warp and bend, it can never close.) The number of vertices in closed fullerene-type structures is necessarily even.\n\nThe smallest possible fullerene would be C20, containing twelve pentagons and zero hexagons. However, such a structure would possess a great deal of strain, because the local topology at each carbon center would be highly non-planar. Other possible fullerenes include C28, C32, C50, and C70. Because the molecular strain tends to be concentrated in the five-membered rings that are responsible for closure, structures that avoid contiguous (edge-sharing) pentagons are particularly stable. It turns out that C and C are the smallest carbon clusters for which this can be achieved.\n\n# Other Possible Structures for C60\n\nWhile the truncated icosahedron structure for C60 is elegant and aesthetically-pleasing, it is important to bear in mind that when it was proposed, there was only one piece of supporting experimental evidence - an unusually large peak at 720 in the mass spectrum. Other C60 cluster structures, including the following three, were possible.\n\n   1. Planar graphite fragments.\n      The problem with this type of structure is that it contains many unsatisfied valences, and it is not clear why C60 should be any more stable than any other cluster size.\n   2. Cyclic polyalkynes.\n      In this structure, there are no unsatisfied valences but the stability of C60 vs. other cluster sizes is not easily rationalized.\n   3. Other fullerenes, i.e., other hollow cage structures with different atom arrangements.\n      These would necessarily be less highly symmetric than the truncated icosahedron and would less effectively distribute strain evenly around the molecule. \n\nGiven these possible, albeit less attractive, alternatives, it was crucial to obtain additional experimental evidence for the structure of C60.
650823
Carbon, Hydrogen, and Oxygen.
150301
Graphite is the most stable form of C. It has a gleaming appearenc and is quite brittle. It has a low elting point as well...
889370
carbon has no free electrons available\nso it cannot conduct electricitys\nin case of germanium and si they have d orbits in the outer shell and they have greater mobility
232315
Gases are either loose molecules or loose atoms that has insufficient intermolecular forces to maintain cohesion.  In a system with a gas, the reasons why they can be compressed is that between the particles are spaces of voids which aren't filled with anything.  Thus, the particles collide with each other at a less frequent rate than the same particles in a liquid or solid.  \n\nThe compressed state of any substance will form a phase of the material where it is configured in the least energy position.  For carbon, at room pressure it would be at a sliding hexagonal position which is stable.  For carbon at higher temperatures, it converts to a face centered cubic (FCC) lattice which would be the most relaxed position at that pressure.  For diamonds at STP, they are undergoing transformation at an extremely low rate to graphite.  Thus, reinforcing the part about them liking the arrange themselves to be most relaxed at a certain condition.\nWhy?  Intermolecular forces already are strong enough to cause the particles to stick together.  Outside factors such as pressure and temperature causes them to rearrange themselves to fit a more appropriate formation that is most relaxing and least energetic.  Therefore, they cannot be compressed more than they should, but they can change their crystal lattice formation to occupy the most comforatable position.
439535
Diamond, Graphite, and Buckministerfullerene are all types of carbon, which means that they are arrangements of carbon atoms with only carbon-carbon bonds. \n\nYou are made of organic compounds with carbon-oxygen, olefin, carbon-hydrogen, oxygen-phosphoros, etc bonds. The carbon that exists within you is the same carbon in diamond or bucky balls; It's just bound in a different way.
732587
There are all kinds of different materials lumped under the generic heading of "plastics".  The variations run into hundreds, perhaps even thousands of compounds!\n\nFor example, there's nylon.  The most familiar form, nylon 66, is a copolymer of adipic acid or adipoyl chloride and hexamethylene diamine.  But I can substitue various hydrocarbon chains in those two components to make nylon 55, nylon 65, nylon 48, nylon 83, etc.\n\nThen there are the families of polyaramid polymers, and polyester polymers, and polycarbonates, and . . . .\n\nNobody will ever be able to give you an exhaustive list here.  Try looking up some books on polymer chemistry at your library.
417185
Carbon (C), Hydrogen (H), and Oxygen (O)
696413
1. Diamonds and graphite are a form of carbon.\n\n2. Ammonia is made using the Haber process.\n\nLook here for details\nhttp://www.ausetute.com.au/haberpro.html\n\nIt is used as a fertilizer, explosives, chemicals\n\n3. Ozone in the upper atmosphere act as a filter for UV rays, which are harmful to life.\n\n4. Halogens have an outer orbital that will be filled if they add one electron\n\n5. Noble gases have an outer orbital that is completelly filled.
260431
R-O-CH3 \n\n R is any carbon based group. I wish I had chem draw on this computer, but the structure is actually bent due to the symmetry (this involves group theory - a linear algebra based idea in quantum mechanics) of the orbitals involved in bonding. Its bent for the same reasons that water is bent, now your teachers may say that water is bent due to electronic repulsions but if thats true how come they draw the lone pairs so close to eachother??? Its because its not true, and its part of VSEPR theory which is just a practicle method of teaching structure to people who dont know too much physics, math, and chemistry.