Physics Chap7 Flashcards
Definite volume and definite shape
solids
Attempts to describe all the states of matter and the conversion between states
Kinetic-molecular theory of matter
Solids intermolecular forces are
strong enough to hold molecules rigidly in place with respect to each other
definite volume but no definite shape
liquids
strong enough to hold molecules in a condensed phase, not strong enough to prevent molecules from sliding past each other
intermolecular forces of liquids
fluids have the ability to
flow (liquids and gases)
Neither a definite shape nor volume
gases (will expand to fill the available space)
are essentially zero between molecules
gas intermolecular forces (ideally independent molecules)
what determines how molecules interact?
intermolecular forces (impact the macroscopic properties of a sample directly mostly)
What determines intermolecular forces?
chemical bonding
Molecules, atoms, and oppositely charged are _______ each other, but not to close. ________
attracted(Coulomb’s Law), REPULSION
octet rule
atoms add, remove, or share electrons so as to wind up with 8 VALENCE electrons
formed between metals and nonmetals. metals tend to form cations
ionic compounds
nonmetals tend to form
anions
which is stronger, ionic bonds or covalent bonds?
ionic bonds(almost always solids)
ionic bond results from ________ attraction between _______ charged ions.
coulombic, oppositely
on the periodic table the number of valence electrons is equal to
the group number
covalent bonds result from
sharing of electrons
The intermolecular forces that operate between the molecules in a sample, all of which are caused by how electrons are arranged in the molecule.
VSEPR Theory
What is the most electronegative element?
flourine
If two atoms of identical electronegativity are bonded together, the bond is
non-polar
If two atoms of different electronegativity are bonded together, the bond is
polar, the electrons spend more time around the more electronegative atom (this creates partial charges)
Three main IM forces
dipolar, hydrogen bonding, and London forces
Attraction between the opposite(partial) charges of polar molecules
dipole-dipole attraction
attraction between a hydrogen bonded directly to an O, N, and F and another electronegative atom
hydrogen bonding
attraction between an ionic and a polar molecule
ion dipole attraction
which attraction is important with how we give meds
ion dipole attraction (also with protein binding, albumin and alpha acidic glycoproteins)
what is also known as Vander Waals forces
London forces
result of an instantaneous dipole that is created whenever electrons in a molecule are unevenly distributed.
London Forces, all common matter experiences, larger molecules show more of it.
More intermolecular forces mean what 4 things
-higher boiling and melting points,
higher heats of fusion and vaporization,
lower vapor pressure,
more viscous liquids,
IM forces also affect solubility,
“like dissolves….
“like”
polar compounds dissolve more easily in other _______ compounds
polar. “like dissolves like”
The ultimate in ______ species, are soluble in water, but are generally not soluble in _______ organic solvents such as ether.
polar, nonpolar
what are some nonpolar species
nitrogen, oxygen, and CO2, (relatively insoluble in a polar solvent like water)
Most organic compounds have backbones consisting of hydrogen and carbon. Hydrocarbons are essentially _________. Therefore, most organic compounds are not very soluble in ______.
nonpolar, water.
Substances with ______ IM attractions have _______ surface tensions.
greater, greater
does water have a high or low surface tension?
high
laplaces law
wall surface tension is directly proportional to radius if pressure is the same. tension=radiusxpressure
aneurysms are _______, and radius of aneurysm is divided by
spherical, 2,
soaps are derived directly from fats or oils through a chemical process called
saponification
what is a fatty acid?
a long-chained carboxylic acid having 12-18 carbon atoms.
a soap is the salt of a
fatty acid
when placed into water the surfactant molecule will strive to get the greasy, nonpolar ______ tail away from the ______ water molecules.
hydrocarbon, polar.
what does surfactant disrupt to decrease the surface tension of the water? (monolayers)
disrupt the hydrogen bonding between water molecules
the surfactant molecules stick their polar heads onto the water, while their greasy tails stick out of the surface of water
monolayers
the tails of the surfactant molecules can dissolve in each other to form a double layer.
the nonpolar tails interact with eachother, with the polar heads on the outside interacting with the water molecules
bilayers and basic structure of cell membranes
tails can dissolve in each other forming a sphere, crating a non-polar microenvironment in the water is called
micelles
Viscosity ______ with increasing intermolecular forces.
increases
Substances having ______ IM forces have ______ vapor pressures
greater, lower
The most energetic molecules in a liquid have sufficient kinetic energy to break IM forces and escape into the gas phase. Once the molecules are free as gases, they exert a pressure called
the vapor pressure
vapor pressure is _______ proportional to temp
directly
volatility of a liquid ______ with increasing temp
increases
When there is a balance between vaporization and condensation, a state of ______ ________ exists
dynamic equilibrium
Des has to be heated to ______ roughly to keep in _____ state
2atm, liquid
Is a gas more volatile with a high or low vapor pressure?
high
volatility is
nonquantaitative term that describes the tendency of a liquid to evaporate
what describes the distribution of why vapor pressure increases with temp?
Boltzmann distribution
states the total pressure of a gaseous mixture is the sum of the partial pressures of each of the component gases.
Dalton’s Law of Partial Pressures
vapor pressure is ______ dependent
temperature
liquid to gas
vaporiztion
gas to liquid
condensation
solid to gas
sublimation
gas to solid
deposition
boiling point is _____ at higher elevation
lower, since less atm pressure to overcome
temperature at which the vapor pressure of a liquid equals the ambient pressure
boiling point
