What are the differences between amorphous and crystalline solids?
Amorphous: No long-range order, rapid cooling | Crystalline: Repeating pattern, definite melting point.
Compare and contrast diamond and graphite.
Diamond: $sp^3$ hybridized, insulator, hardest naturally occurring substance. | Graphite: $sp^2$ hybridized, conductor, layers can slide, soft.
Compare substitutional and interstitial alloys.
Substitutional: Atoms replace each other in lattice. | Interstitial: Smaller atoms fit in spaces between larger atoms.
Compare intermolecular and intramolecular forces in molecular solids.
Intermolecular: Weak forces between molecules, determine melting/boiling points. | Intramolecular: Strong covalent bonds within molecules.
Compare the conductivity of metallic and ionic solids.
Metallic: Good conductors due to delocalized electrons. | Ionic: Conduct only when molten or in solution due to mobile ions.
Compare the melting points of molecular and covalent network solids.
Molecular: Low melting points due to weak IMFs. | Covalent network: High melting points due to strong covalent bonds.
What is the effect of delocalized electrons in metallic solids?
Good electrical conductivity, thermal conductivity, and shiny appearance.
What is the effect of strong electrostatic forces in ionic solids?
High melting points and brittle nature.
What is the effect of weak IMFs in molecular solids?
Low melting and boiling points.
What is the effect of a network of strong covalent bonds in covalent network solids?
High melting points and hardness.
What is the effect of rapid cooling on solid formation?
Formation of amorphous solids.
What is the effect of higher charges and smaller ion sizes on ionic attractions?
Stronger electrostatic attractions, leading to higher melting points.
Define ionic solids.
Solids held together by electrostatic forces between cations and anions.
Define metallic solids.
Solids held together by metallic bonds between metal atoms, with electrons in a 'sea'.
Define covalent network solids.
Solids held together by a vast network of covalent bonds.
Define molecular solids.
Solids held together by weak intermolecular forces (IMFs).
Define amorphous solids.
Solids with no long-range, repeating structure.
Define crystalline solids.
Solids with particles arranged in a repeating pattern.
Define crystal lattice.
The geometrical pattern of points on which crystalline solids are arranged.
Define unit cell.
The smallest repeating unit of the crystal lattice.
Define substitutional alloy.
Atoms of one element replace atoms of another in the lattice.
Define interstitial alloy.
Smaller atoms fit into the spaces between larger atoms.
