Solid

• Solids


  Have definite shape and volume, unlike liquid and gas
• Diamond is known as the hardest natural substance to exist in the world
• Solids

  • Some are soft and can be easily manipulated
  • Others are brittle and strong resistance to shape
• Describe the difference in structure of crystalline and amorphous solids


  STEM_GC11IMF-IIIa-c-104
• Kinetic Molecular Theory of Solids

  A simple microscopic model that explains the three different phases (solid, liquid, and gas) of matter and how they can change from one phase to another
• Kinetic Theory of Matter

  All matter is composed of particles that have a certain amount of energy to make them move at different speeds depending on temperature
• Temperature


  The average kinetic energy of particles in a system
• Solids


  • Intermolecular forces between neighboring particles are held together by strong covalent or ionic bonding
  • Noncompressible due to lack of spaces between them
  • Definite shape and volume
• Solids

  • Can appear in different forms
  • Two main categories: crystalline solids, amorphous solids
• Crystalline Solids


  • Solids in which the atoms, ions, or molecules are arranged in a definite repeating pattern
  • Held together by uniform, strong intermolecular forces
• Crystalline Solids


  • Silicon dioxide (SiO2), also known as quartz
• Crystalline Solids

  • The orderly arrangement of atoms: highly regular shapes
  • Examples: quartz and sodium chloride
• Amorphous Solids

  • From the Greek words for "without form"
  • Lacks the order found in crystalline solids
  • Structures at the atomic level similar to the structures of liquids
• Amorphous Solids

  • Obsidian (typically KAlSi3O8)
• Amorphous Solids

  • Atoms, ions, or molecules have little freedom to move unlike in liquids
  • Do not have well-defined shapes of a crystal
  • Examples: obsidian (volcanic glass) and rubber
• Crystalline solids consist of particles in an organized form, while the particles of amorphous solids are not formed in an orderly manner
• Properties of Solids


  • Characteristic properties that are distinguishable from other states of matter
  • Dependent on the composition of solids
• Melting Point


  The temperature at which a solid loses its definite shape and is converted to a liquid
• Freezing Point


  The temperature at which a liquid changes to a solid
• Melting/Freezing Point

  At this temperature, solid and liquid forms of a substance are in equilibrium with each other
• Crystalline Solids


  • Have a precise melting point
• Amorphous Solids

  • Melt over a wide range of temperature
• Stronger interaction


  Has a higher melting point
• Melting Point


  • Cristobalite melts at 1713 oC, while soda-lime glass, the most prevalent type of glass, can melt between 550 oC and 1450 oC
• Heat of Fusion


  The quantity of heat necessary to melt a solid
• Solids with stronger intermolecular forces


  • Have higher values of heat of fusion
• Crystalline Solids


  • Heat of fusion is fixed and definite
• Amorphous Solids


  • No precise value for heat of fusion
• Sublimation


  The process of direct passage from solid to vapor phase, bypassing the liquid state
• Deposition


  The reverse process of sublimation (vapor to solid phase)
• Malleability


  The ability of a solid to undergo compressive stress without breaking
• Metals are highly malleable and can be shaped through forging, rolling, extrusion, and indenting
• Ductility

  • The ability of a solid to undergo tensile stress
  • Can be measured
  • Describes the extent to which the solid can be stretched without fracture
• Most of the time, malleability and ductility properties coexist
• Malleable and ductile solids

  • Silver and gold
  • Gold is known to be the most malleable and ductile