unit 4 Flashcards
gases
low density
indefinite shape
indefinite volume
weak IMF
liquids
high density
indefinite shape
definite volume
moderate IMF
solid
high density
definite shape
definite volume
strong IMF
kinetic molecular theory
explains the states of matter, and is based on the idea that matter is composed of tiny particles that are always in motion
stronger attractive forces between particles =
more they resist moving
solids melt when
heated
gases can be condensed by
decreasing temp
increasing pressure
attractive forces and boiling/melting point relation
stronger attractive forces = higher melting/boiling point
charge and attraction relation
larger charge = stronger attraction
distance and attraction relation
longer distance = weaker attraction
boiling point and IMF relation
higher boiling point = stronger IMF
unequal electron distribution gives
temporary polarity
permanent dipole adds to the
attractive forces between molecules
raises boiling and melting point
polar substances dissolve in
polar substances
non polar substances dissolve in
non polar substances
strongest type of IMF
hydrogen
ion-dipole attraction
ions are attracted to the dipole of polar molecules
strength determines solubility of ionic compounds in water
London dispersion forces are present in
all molecules
dipole-dipole forces are present in
polar molecules
Hydrogen bonding forces are present in
molecules with H bonded to F, O, or N
ion dipole forces are present in
mixtures of ionic compounds and polar compounds
surface tension
Property of liquids that results from the tendency of liquids to minimize their surface area
are molecules more or less stable than molecules in the interior
less
IMF and surface tension relation
stronger IMF = higher surface tension
temperature and surface tension relation
increasing temp = less suface tension
viscosity
resistance of a liquid to flow
IMF and viscosity relation
larger IMF = larger viscosity
IMF and viscosity relation
stronger IMF = higher viscosity
temp and viscosity relation
increasing temp = less viscosity
capillary action
ability of a liquid to flow up a thin tube against the influence of gravity
capillary action forces
cohesive: hold liquid molecules together
adhesive: attracts outer liquid molecules to the tube’s surface
when does capillary action stop?
until gravity counteracts the capillary action forces
What factors cause transitions between the solid and liquid state?
-temperature
-pressure
-heating/cooling
What factors cause transitions between the gas and liquid state?
-temperature
-pressure
-heating/cooling
Describe the relationship between the state of a substance, its temperature, and the strength of its intermolecular forces
solid: as temp increases, they become liquids. strongest IMF.
liquid: as temp increases, they become gases. strong IMF.
gas: lowest IMF
From what kinds of interactions do intermolecular forces originate?
interactions between charges, partial charges and temporary charges on molecules, atoms or ions
Why are intermolecular forces generally much weaker than bonding forces?
Bonding forces are the result of large charges acting over small distances
IMF are the result of smaller charges acting over large distances
What is the dispersion force?
result of fluctuations in electron distribution within molecules or atoms