Solids have a definite shape and volume, with particles that are tightly packed and not easily compressible. The particles vibrate about fixed positions and have strong intermolecular forces. At the melting point, vibrations overcome interactions holding particles in fixed positions, transforming the solid to a liquid. Sublimation is the direct transition from solid to gas without an intermediate liquid phase. Crystalline solids have an orderly repeating structure while amorphous solids lack order. Different types of crystalline solids include ionic held by electrostatic forces, molecular held by dispersion forces, and metallic held by delocalized electrons.

1. STATES OF MATTER
SOLID

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.