2. Properties of Solid
Solids have a definite shape and a definite
volume.
Particles of solids are tightly packed, not easily
compressible
Molecules still move but only vibrate about a
fixed position.
Intermolecular forces are strong
3. Melting Point
• the temperature where a solid turns into a
liquid.
• at the melting point, the disruptive vibrations
are strong enough to overcome the interactions
holding them in a fixed position
4. Sublimation
• process of transformation directly from
the solid phase to the gaseous phase without
passing through an intermediate liquid phase
• endothermic phase transition that occurs at
temperatures and pressures below a
substance's triple point in its phase diagram.
5. Classification of Solids
Crystalline Solids
• a solid material whose
constituent atoms, molecules, or ions are
arranged in an orderly, repeating
pattern extending in all three spatial
dimensions.
Amorphous Solids
• lack an ordered internal structure atoms are
randomly arranged
6. • In a crystal, the particles are arranged in a
orderly, repeating, three-dimensional
pattern called a crystal lattice
• A crystal lattice a three-dimensional form that
determines the shape of individual units of
crystal.
7. Types of Crystalline Solids
Ionic Solids
• made up of positive and
negative ions and held together
by electrostatic attractions.
• characterized by very high
melting points and brittleness
and are poor conductors in the
solid state
Examples: Sodium Chloride, Zinc
Sulphide, Calcium Fluoride
8. Molecular Solids
• Made up of atoms or
molecules held together by
London dispersion forces,
dipole-dipole forces, or
hydrogen bonds.
• Characterized by low
melting points and
flexibility
Examples: sugar, ice(water),
dry ice
9. Atomic (Covalent-Network) Solids
• Made up of atoms connected by covalent bonds; the
intermolecular forces are covalent bonds as well.
• Characterized as being very hard with very high melting
points and being poor conductors.
Examples: Diamond, quartz, graphite
10. Metallic Solids
• are held together by a high density of shared,
delocalized electrons, resulting in metallic
bonding.
• Characterized by high melting points, can range
from soft and malleable to very hard, and are
good conductors of electricity.
