The Condensed State Flashcards
Network Covalent
attractions of valence electrons on atom to the nuclear charge on a neighboring atom
Metallic
metal cation attractions in a sea of electrons
ionic
attractions between cations and anions resulting from an exchange of electrons
Molecular
attractions of partial positive and partial negative charges between discrete molecules. either permanently or temporary, always called inter molecular forces
london dispersion
Temporary dipoles attract very weakly. Strength of LD increases with size and contact area. Everything experiences these. Low melting/boiling points.
Dipole-Dipole
Partial negative charge on one molecule interacts with the partial positive charge on another. Permanent.
Hydrogen bonding
H to F,N,O. Dominant force.
What makes something a conductor
if its electrons are free to move around
metallic structural integrity
malleable and ductile
ionic structural integrity
brittle
network covalent/molecular structural integrity
varies
vapor pressure and imfs
inverse relationship
when do things boil
when vapor pressure is equal to barometric pressure
Size, electron density, polarizability, temporary dipole moment, LD strength
direct
Surface Tension
A liquid tends to shrink itself to get the most of it onto the surface as possible. As IMFs increase, so does surface tension
Capillary action
a substance moving up the sides of the container
structural unit of metallic
metal ions at lattice points with a sea of freely moving electrons
structural unit of ionic
alternating positive and negative ions held in a rigid lattice
structural unit of covalent
independent molecules held together by imfs
structural unit of network covalent
continuous network of atoms convalently bonded to one another
metallic state at room temp
solid
ionic state at room temp (ARE THEY CRYSTALS?)
crystalline solids
covalent state at room temp
solid, liquid, or gas depending on size
network covalent state at room temp
usually solids
metallic electrical conductivity
conducts as solid
ionic electrical conductivity
conducts in liquid and aqueous states, but not solid
molecular / covalent electrical conductivity
not in any conditions
network covalent electrical conductivity
some structures conduct
thermal conductivity of metallics
good
thermal conductivity of ionics
thermal insulator
thermal conductivity of molecular / covalent
poor, most are insulators
network covalent thermal conductivity
somewhat
malleability and ductility of metallic
can be pounded into shapes and drawn into wire
malle. + duct. of ionics
too brittle
malle + duct of covalent
neither
malle + duct of network covalent
too brittle
hardness of metallics
varies
hardness of ionic
hard and brittle
hardness of covalent
typically soft
hardness of network covalent
very hard
enthalphy of fusion/vaporization of metallics
wide range
enthalpy of fusion/vaporization of ionic
typically 10-100 times greater than covalent
enthalpy of fusion/vaporization of network covalent
high, mirroring melting point and boiling point
melt/boil of metallic
wide range
melt/boil of ionic
must overcome ion-ion interactions, so usually high (800-1200ish)
melt/boil of covalent
must overcome weaker dipole-dipole & london dispersion, so much lower than ionic
melt/boil of network covalent
extremely high, 1500-4000
water solubility of metallic
insoluble
water solubility of ionic
depends on relative attraction between ions vs ion-water attraction
water solubility of covalent
smaller polar are soluble, non-polar insoluble
water solubility of network covalent
insoluble
