6.2: Solid State of Matter

Flashcards covering the key concepts and characteristics of solids in the solid state of matter, including types of solids, their properties, and examples.

Kinetic Energy

Particles in solids have the least amount of kinetic energy compared to liquids and gases.

Intermolecular Forces (IMFs)

Strong enough to lock particles into fixed positions in solids.

Crystalline Solids

Solids with particles arranged in an orderly, repeating geometric pattern.

Amorphous Solids

Solids with particles arranged in random fashion

Definite Volume & Shape

Characteristics of solids due to strong IMFs and fixed particle positions.

High Density

The density of solids is generally the highest state due to close packing of particles.

Incompressible

Solids cannot be compressed easily because particles are already closely packed.

Crystal Lattice

The specific, orderly 3D arrangement of particles in crystalline solids.

Ionic Crystals

Particles consisting of positive and negative ions held together by strong ionic bonds.

Covalent Network Crystals

Particles made up of nonmetal atoms connected by covalent bonds forming a large network.

Metallic Crystals

Consist of positive metal ions in a 'sea' of mobile valence electrons.

Covalent Molecular Crystals

Discrete covalent molecules held together by weak intermolecular forces.

Diffusion in Solids

Extremely slow movement of particles, practically negligible in solids.

Unit Cell

The smallest repeating unit of the crystal lattice that reveals the overall pattern.

Types of Crystalline Patterns

• isometric

• hexagonal

• tetragonal

• trigonal

• orthorhombic

• monoclinic

• triclinic

Bonding Types in Crystalline Solids

• ionic

• covalent network

• metallic

• covalent molecular

Van der Waals Forces

Weak intermolecular forces that hold covalent molecular crystals together.

Examples of Crystalline Solids

• minerals

• metals

• salt

• sugar

Examples of Amorphous Solids

• glass

• plastic

• rubber

Phase Change Map

Phase Diagram