Electrolytes + KMT + IMFs Flashcards
HCl
strong acid
HBr
strong acid
HI
strong acid
HNO3
strong acid
HClO4
strong acid
H2SO4
strong acid
strong acids…
dissociate completely in water to produce ions in solution.. strong electrolye
soluble ionic compounds
strong electrolytes because they dissolve completely
weak electrolytes
dissociate slightly, weak acids and bases bc there are only some ions present
non electrolytes
molecules that stay together when they dissolve in water, covalent compounds with exception to acids
Avogadro’s Law
direct relationship with volume and moles
Boyles’ Law
inverse relationship with pressure and volume
Charles’ Law
direct relationship with temperature and volume
particles are in constant motion. the collisions of the particles with the walls of the container are the cause of the pressure exerted by the gas
true
the molecules in a real gas have finite volumes and do exert forces on each other, thus the real gases do not conform to some of the assumptions of an ideal gas as stated by the kmt
true
The particles are so small compared with the distances between them that the volume of the individual particles can be assumed to be zero.
true
At constant temperature, the lighter the gas molecules, the larger the average velocity.
true
Real gas molecules behave most ideally at low temperature and high pressure.
false
Ideal gas molecules have small volumes and exert weak attractive forces on one another.
false… they are assumed to have zero volume and no attractive forces on one another
average KE is the same when…
..all the temperatures between molecules are the same.. this is not the same with average velocity
a real gas behaves most ideally when..
the container volume is relatively large and the gas molecules are moving relatively quickly
intermolecular force (IMF)
attractions between neighboring molecules which determine physical properties
directly related to IMFs (stronger IMF=higher)
boiling point, melting point, molar heat of vaporization (liquid to gas), molar heat of fusion (melting solid to liquid), molar heat of sublimation (solid to gas)
inversely related to IMFS (stronger IMF =smaller)
vapor pressure (large mm have low vapor pressures, molecules need high energies to escape to the vapor pressure)
enthalpy (heat of anything)
the heat/energy required to melt, vaporize, sublimate
London Dispersion Forces (LDF)
ALL molecules have this force, created from induced instantaneous dipoles (becomes non symmetrical), weakest IMF, increase in strength when increasing mm and when shape is longer
Dipole - Dipole
second weakest, occur due to permanent dipole-dipole attractions, only in polar molecules (strength increases with polarity), line up electrostatically so pos and neg ends near each other (weaker if distance between ends is larger)
hydrogen bonding
third weakest, second strongest strongest covalent IMF, a type and strongest dipole-dipole force, only occurs in H-N, H-F, H-O bonds
electrostatic attraction
strongest IMF, oppositely charged particles attract each other and this attractive force called electrostatic force
