GENCHEM2 (Chapter 11)

IMF’s List them

London

dipole-dipole

H-bonding

ion-dipole

Heating Curves

Plot of temperature change versus heat added

London IMF’s

“temporary dipole”

Shape vs Size

Dipole-dipole

Polar Molecules

H-bonding

“FON”

ion-dipoles

ionic

Viscosity

resistance to flow (water vs syrup)

Primitive Cubic

8(1/8)=1 atom

Body-centered Cubic

8(1/8)+1=2 atoms

Face-centered Cubic

8(1/8)+6(1/2)=4 atoms

Vapor Pressure

at any temperature some molecules in a liquid have enough energy to escape attraction of the bulk liquid

Volatile Liquids

Liquids which easily evaporate

Critical Pressure

Pressure required for gas liquefaction

Critical Temperature

highest temperature at which a substance can exist as a liquid

Molecular Solid

• consist of atoms or molecules held together by IMF’s

  • dipole-dipole

  • London

  • H-bonds

• Weak intermolecular forces give rise to low melting points

Covalent-Network Solid

• Consist of atoms held together, in larger networks or chains, with covalent bonds

• higher melting points(than molecular solids)

• electorns move freely through the delocalized orbitals

  • diamond

  • graphite

  • quarts (SiO₂₎

Ionic Solids

• consist of ions held together by ionic bonds

• hard, brittle, very high melting points

• ions held together by electrostatic forces of attraction

Metallic Solids

• consist entirely of metal atoms

• soft or hard melting points, good electrical and thermal conductivity, ductile and malleable