Diamond. Diamond, graphite and buckyballs are examples of the variety of ways carbon atoms can join together, and are particularly interesting because they contain only carbon atoms. The factor for the differences in firmness as well as various other physical homes can … Graphite has a lower density than diamond. Diamond- 4 carbon-carbon bonds; Graphite- layers-between layers there are free electrons; Graphite-lubricates-layers can slide over easily; Overall comparison. Image source 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. and graphite. Diamond is hard due to strong covalent bonds present in it. In diamond the atoms are arranged in a three dimensional lattice, while in graphite they are joined together in an array of planar six membered rings, arranged in layers. Diamond (left) and graphite (right) are both made of carbon atoms, but arranged in different ways. These layers are held together by much wealer van der Wall's forces, therefore the crystals of graphite soft and slippery. electricity. but the difference is that the bond between atoms is different for diamond ,graphite … By Rudina El Dokani Science 9 (1) Mrs. Nicholl Tuesday December 17th Compare and contrast the properties of diamond and graphite Why do Diamonds and Graphite have such different properties? Experts are waiting 24/7 to provide step-by-step solutions in as fast as 30 minutes! This is because of the relatively large amount of space that is "wasted" between the sheets. are different forms of the element. Diamond and also graphite are chemically the same, both made up of the element carbon, however, they have entirely different atomic and also crystal frameworks. so they are made of the same atom. Want to see the step-by-step answer? Check out a sample Q&A here. The difference between the three naturally occurring allotropes is the structure and bonding of the atoms within the allotropes; diamond enjoying a diamond lattice crystalline structure, graphite having a honeycomb lattice structure, and amorphous carbon (such … Both occur naturally. * In a Graphite, carbon atoms are bounded together in a flat layers by an strong covalent bonds in a regular haxagon. In Diamond each carbon atom bonds to 4 other carbon atoms, Whilst, in Graphite, each carbon atom bonds to 3 other carbon atoms. List three differences and two similarities between diamond and graphite. Answer:Similarity: either: both contain carbon atoms; or: both have strong covalent bonds between the atomsDifference: either: graphite structure has layers whereas diamond structure does not; or: graphite contains WEAK intermolecular forces BETWEEN LAYERS whereas diamond only has strong covalent bonds between atoms[would include a diagram of the two structures in the answer] check_circle Expert Answer. Both graphite and diamond are forms of carbon. Diamond atoms have a rigid 3 dimensional structure with each atom carefully loaded with each other as well as connected to 4 other carbon atoms. See Answer. actually graphite , diamond, fullerene are allotrope of carbon. carbon. Both can be made artificially. These electrons are free to move between the layers in graphite, so graphite can conduct. Thus, diamond bears more of a tetrahedral structure, whereas graphite takes the form of layers. Diamond and graphite. 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