Solids

• a nearly incompressible state of matter with a well-defined shape. solid
• the units(atoms, molecules, ions) making up the solid are inclose contact and reside in fixed positions or sites
• Type of Solid:

  consists of atoms and molecules held together by IMFA. Molecular Solid
• Type of Solid:

  consists of positive cores of metal atoms held together by metallic bonding. Metallic solid
• Type of Solid:

  composed of anions/cations held together by ionic bonds. Ionic solid
• Type of Solid:

  consists of atoms held together by large networks of covalent bonds. covalent network solid
• Physical properties such as melting point, hardness, and electrical conductivity are related to solid structure.
• Hardness depends on how easily the structural units can be moved relative to one another.
• Low melting point, soft/brittle and nonconductive. Molecular
• melting point varies, hardness also varies but malleable and shaped by hammering, conductive. Metallic
• high-very high melting point, hard/brittle (fractures easily), nonconductive as a solid but conductive as a liquid. Ionic
• very high melting point, very hard, usually nonconductive. covalent networks
• has a disordered structure and lacks a well-defined arrangement of basic units. amorphous solid
• an amorphous solid obtained by cooling a liquid rapidly enough that its basic units are “frozen” in random positions before they can assume a crystalline arrangement. glass
• The ordered structure of a crystal. crystal lattice
• UNIT CELL TYPES:

  atoms/ions are at the corners only. Simple cubic
• UNIT CELL TYPES:

  1 atom/ion surrounded by atoms/ions at the corner. body-centered cubic
• UNIT CELL TYPES:

  atoms/ions at the center of the 6 faces with the corner atoms/ions. face-centered cubic
• How many atom/s per body-centered cubic cell? 2 atoms