IMFs

electricity conducting

charged particles, particles must be able to move freely

substitutional

similar atomic radii

interstitial

different atomic radii

network covalent

graphite, diamond, glass, quartz, SiO2, SiC, Si

Stronger IMF = ___ boiling point

Higher

LDF

nonpolar + nonpolar

Dipole-Dipole

polar + polar and only non-metals

Hydrogen bonding

polar and O, N, F

Dipole-Induced Dipole

Nonpolar + polar

Ion-Induced Dipole

Nonpolar + Ion

Ion-Dipole

Polar + Ion

Polarizability

ability to form an induced dipole

lattice energy

energy needed to separate ions in ionic compounds

larger charges = 

more attraction = more energy required to separate the ions

smaller radii = 

more attraction = more energy required to separate the ions

Bond energy

energy required to break a bond (energy is released when a bond is formed)

bond length vs bond energy

larger bond length = smaller bond energy

lattice energy vs size

larger lattice energy when smaller ion size (stronger coulombic attraction)

linear structure vs. spherical structure

linear structure = more IMFs, spherical structure = least IMFs because reduced surface area for interactions

vapor pressure

stronger IMFs = lower vapor pressure (harder for molecules to transition into gas phase)

lattice energy increases when…

IMF increases

Ionic

metal and nonmetal + ion-dipole

covalent network

nonmetals

molecular (covalent)

nonmetal

metallic

metals