Chapter 4: States of Matter

Flashcards covering states of matter, gas laws, intermolecular forces, and solid structures.

Heating

Particles gain kinetic energy, vibrate more vigorously, forces of attraction weaken, particles are further apart.

Cooling

Particles lose kinetic energy, vibrate less vigorously, experience increasing forces of attraction, particles arranged more closely.

Kinetic Theory of Gases Assumptions

Gas molecules move rapidly and randomly, collisions are elastic, distance between molecules is greater than diameter, no forces of attraction/repulsion, temperature related to average kinetic energy.

Boyle's Law

At constant n and T, P is inversely proportional to V.

Gay-Lussac's Law

At constant n and V, P is directly proportional to T.

Charles' Law

At constant n and P, V is directly proportional to T.

Ideal Gas Equation

PV = nRT

Ideal Gas

Volume of molecules is negligible, no forces of attraction/repulsion.

Real Gas

Volume of molecules is not negligible, forces of attraction/repulsion exist.

Deviations from Ideal Gas Behavior

Deviations observed at high pressure and low temperature.

Vapor Pressure

Pressure exerted by a vapor in equilibrium with a liquid in a closed container.

Partial Pressure of a Gas

Each gas in a mixture exerts the pressure it would if it were alone.

Mole fraction

no. of moles of one gas / total no. of moles in a mixture

Properties of Liquids

Liquids have closer distances between molecules and surface tension.

Surface Tension

Cohesive forces between particles, leading to minimization of surface area.

Solids: Crystalline Lattice

Many ionic, metallic, and covalent compounds with a repeating arrangement.

Giant Ionic Lattice

3D arrangement of alternating positive and negative ions held by strong electrostatic forces.

Giant Metallic Lattice

3D arrangement of positive ions surrounded by a sea of delocalized electrons.

Giant Covalent/Molecular Lattice

Structures with a 3D network of covalent bonds throughout.

Graphite Structure

sp² hybridized carbon atoms in planar layers held by weak id-id forces.

Diamond Structure

sp³ hybridized carbon atoms arranged tetrahedrally.

Simple Molecular Lattice

3D arrangement of covalent molecules held together by weak intermolecular forces.

Forces keeping particles together

Ionic bonds, covalent bonds, metallic bonds, temporary-induced dipoles

Steps to explain differences in melting/boiling points

state the structure, state the bonding, compare and contrast the bonding, make the conclusion

Allotropes of Carbon

Diamond, Graphite, Graphene, Carbon nanotubes, Fullerene