3.2 ap chem properties of solids

What vapor pressure, melting point, and boiling point do ionic solids tend to have

Low vapor pressure, high melting point, and high boiling points

What results in higher lattice energy in ionic solids

Smaller ions and/or ions with higher charges

When do ionic solids conduct electricity

Only when the ions are mobile

Why are ionic solids typically brittle

Due to repulsion of like charges caused by one layer sliding across another

Why are 3d covalent network solids rigid and hard

Because the covalent bond angles are fixed

Examples of covalent network solids

Diamond, silicon dioxide, silicon carbide, graphite

Why do molecular solids not conduct electricity

Due to their valence electrons being tightly held within their covalent bonds and lone pairs of each molecule

Key qualities of metallic solids

Conductivity, malleability and ductility

Why are metallic solids conductive

Due to metallic bonds being a packed lattice of cations surrounded by a sea of moving electrons

Ionic solid conduction state

Ionic solids are poor conductors of heat and electricity

Molecular solids conduction state

Molecular solids are poor conductors of heat and electricity

Covalent solid conduction state

Covalent solids are poor conductors of heat and electricity but many exceptions exist

Metallic solid conduction state

Metallic solids are good conductors of heat and electricity

Ionic solid relative melting point

Relatively high melting point

Molecular solid relative melting point

Low melting point

Covalent solid relative melting point

High melting point

Metallic solid relative melting point

Melting point depends strongly on electron config

Ionic solid hardness

Ionic solids are hard but brittle

Molecular solid hardness

Molecaular solids are soft

Covalent solid hardness

Covalent solids are very hard and brittle

Metallic solid hardness

Metallic solids are easily deformed under stress due to ductility and malleability

Luster of ionic, molecular, and covalent solids

Dull surface

Luster of metallic solids

Lustrous

Order of increasing strength of solids

Molecular solids < Ionic solids < Metallic solids < Covalent solids