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Solids (Crystalline Solid:
A solid that contains atoms at the lattice…
Solids
Crystalline Solid:
A solid that contains atoms at the lattice points
picture: 
website: https://chemistry.tutorvista.com/inorganic-chemistry/crystalline-solid.html
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covalent network solids: substances such as diamond, silicon, and graphite. They have a very high boiling point, don't conduct electricity, have a very tough external shell because of the need to break very strong covalent bonds, and is insoluble in water. Graphite solids are kept together by having each of its carbon atoms use three of their electrons to form three bonds with three close atoms. The fourth electron is in the bonding level. It becomes delocalized over the whole sheet of atoms in a layer and is free to wander throughout the layer. And there is no relation from one sheet to another. The atoms within the sheet are held together by strong covalent bonds. The sheets are held together by van der Waals dispersion forces. As each electron moves around, dipoles are set up around the sheets that induce other dipoles in the sheets above and below it. Ref: https://chem.libretexts.org/Core/Inorganic_Chemistry/Crystal_Lattices/Lattice_Basics/Covalent_Network_Solids
Metallic solids: Metallic solids are solids composed of metal atoms held together by metallic bonds. They have a sea of electrons. Because of this, metals are soft and malleable, meaning they can be pounded into sheets. They are also ductile, which means they can be made into wires. Examples of metallic solids are gold, copper, and zinc. Ref: https://ch301.cm.utexas.edu/section2.php?target=imfs/solids/metallic-solids.html
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Atomic Solids
Network Solids: A network solid is a chemical compound where the atoms are bonded covalently in a continuous network. In a network solid there are no individual molecules and the entire crystal is the molecule. Website: http://www.kentchemistry.com/links/bonding/network.htm
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Carbon Network Solids: Solids that are made when carbon atoms join together in a larger crystal structure. The two main occur forms are graphite and diamond. There are naturally and synthetic forms of carbon networks known to scientists.
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Diamond:Diamond has a giant molecular structure. Each carbon atom is covalently bonded to four other carbon atoms. A lot of energy is needed to separate the atoms in diamond. This is because covalent bonds are strong, and diamond contains very many covalent bonds.Picture: Website:http://sciencesolve.blogspot.com/2015/09/diamond-structure.html
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Metallic Solids: Metallic solids are solids composed of metal atoms that are held together by metallic bonds picture:
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atomic solids consist of atoms that are held together by weak dispertion forces. picture:
Amorphous Solids:
A solid that lacks orders that are characteristics of crystals picture:
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glass
borosilicate: main components are SiO2, B203
soda-lime silicate: main components are SiO2, Na2O, CaO
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