CH # 6 State of matter : Solids One liner

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  1. Solids have fixed particles with strong forces, making them rigid and hard to compress.
  2. Solids have a definite shape and volume.
  3. Particles in solids vibrate about their mean position.
  4. Intermolecular forces in solids are strong, holding particles in fixed positions.
  5. Solids have a high density due to close packing of particles.
  6. Solids diffuse very slowly due to restricted particle movement.
  7. Solids expand little when heated.
  8. Solids melt at a specific temperature, turning into liquid.
  9. Some solids sublime, changing directly from solid to vapor.
  10. Crystalline solids have a definite geometrical shape and sharp melting points.
  11. Amorphous solids lack a regular arrangement of particles and have no sharp melting point.
  12. Crystal lattice is a 3D structural arrangement of particles in a crystalline solid.
  13. Unit cell is the smallest repeating pattern of a crystal lattice.
  14. NaCl has a face-centered cubic (FCC) structure with a 1:1 ratio of Na⁺ and Cl⁻ ions.
  15. Lattice energy is the energy released when an ionic solid forms from gaseous ions.
  16. Lattice energy decreases with increasing ion size and increases with higher ionic charge.
  17. Ionic solids are hard, brittle, and have high melting points.
  18. Ionic solids conduct electricity in molten/aqueous state.
  19. Covalent solids (diamond, graphite) have strong covalent bonds and high melting points.
  20. Covalent solids are generally poor conductors.
  21. Metallic solids have a “sea” of delocalized electrons, making them malleable and ductile.
  22. Metallic solids are good conductors of heat and electricity.
  23. Molecular solids have weak intermolecular forces and low melting points.
  24. Molecular solids are poor conductors.
  25. Crystal symmetry is determined by plane, axis, and center of symmetry.
  26. Crystalline solids exhibit anisotropy, with physical properties varying with direction.
  27. Isomorphism occurs when different solids have the same crystalline structure.
  28. Polymorphism is when a compound exists in multiple crystal structures.
  29. Allotropy is when an element exists in different crystal structures (e.g., diamond and graphite).
  30. Transition temperature is the point where two allotropes coexist.
  31. Ionic solids’ shape is influenced by ionic association and radius ratio.
  32. Graphite is a layered structure with weak van der Waals forces.
  33. Diamond is the hardest substance with a tetrahedral structure.
  34. Lattice energy values predict solubility and stability of ionic compounds.
  35. Ionic compounds with smaller lattice energy and greater hydration energy are more soluble in water.
  36. Born-Haber cycle calculates lattice energy indirectly.