Lecture 7 - States of Matter: Gases, Liquids, Solids Flashcards
solid has ______ shape/volume
definite
liquid has _______ shape/volume
indefinite
gas has ________ shape/volume
indefinite
solid has _____ density
high
liquid has _____ density
high
gas has _____ density
very low
solid has ______ compressibility
very low
liquid has _____ compressibility
very low
gas has _____ compressibility
very high
solid has _____ thermal expansion
very small
liquid has _____ thermal expansion
small
gas has _____ thermal expansion
moderate
particles are in constant random motion describes
kinetic energy
particles attract/repel each other describes
potential energy
particles motion ______ with temperature
increases
particles transfer energy through _____
collisions
kinetic energy = ________ = particles ______
disruptive force, far apart
potential energy = _____ = particles _____
cohesive, close together
formula to figure our how much pressure is exerted on a surface
P = (F/A)
p: pressure
f: force
a: area
Boyles Equation
P1V1 = P2V2
Boyles Law:
as pressure increases, volume _______
decreases
Charles Equation
V1/T1 = V2/T2
Charles Law:
as temperature increases, volume ______
increases
Gay-Lussac’s Equation
P1/T1 = P2/T2
Gay Lussac’s Law:
as temperature increases, pressure _____
increases
Combined Gas Equation
(P1V1)/T1 = (P2V2)/T2
empirical gas law
1 mole gas = 22.4 L
What is STP
Standard Temperature = 273 K
Standard Pressure = 1 atm
Ideal Gas Equation
PV = nRT
solid -> liquid
melting
liquid -> gas
evaporation
gas -> liquid
condensation
liquid -> solid
freezing
solid -> gas
sublimation
gas -> solid
deposition
heat is absorbed and the energy of the system increases
endothermic change of state
heat energy is given off and the energy of the system decreases
exothermic change of state
forces that exist between molecules
intermolecular forces
forces within molecules
intramolecular
which is stronger, intermolecular or intramolecular
intramolecular (made of covalent bonds)
exist between polar molecules
dipole-dipole
special type of extra strong dipole-dipole interaction between a hydrogen atom covalently bonded to a small, very electronegative atoms (F, O, or N) and an unshared pair of electrons on another small, very electronegative atom (F, O, N)
hydrogen bonding
how to identify hydrogen bonding
H is bonded to N, O, or F
the amount of heat energy required to convert the solid to liquid
heat of fusion
the amount of heat energy required to convert the liquid to a gas
heat of vaporization
molecules in nonpolar molecular liquids and solids are held together by weak electrostatic forces (larger molecule = stronger force)
London Forces
a weak temporary intermolecular force that occurs between an atom or molecule (polar or nonpolar) and another atom or molecule (polar or nonpolar)
London Force
They results from the temporary uneven e- distribution in molecules at any one moment, thus crating an instantaneous temporary dipole
London Force
They are the weakest type of intermolecular force
London Force
They are important because they occur between all molecules
London Force
Comparing Intermolecular Forces:
- add the the effect of London Forces and are found in polar molecules
Dipole-Dipole
Comparing Intermolecular Forces:
- the strongest intermolecular force and occurs in molecules which have H atoms bonded to F, O, or N atoms
Hydrogen Bonds
Comparing Intermolecular Forces:
- are found in all substances and are the weakest intermolecular force
London Force
List the Intermolecular Forces from strongest to weakest
Hydrogen Bonding > Dipole-Dipole > London
increasing the temperature of a liquid ________ its evaporation rate
increases
molecules that escape (evaporate) from liquid water at room temperature
water vapor
the pressure exerted by a vapor above a liquid when the liquid and vapor are in equilibrium
vapor pressure
the temperature at which the vapor pressure equals the atmospheric pressure
boiling point
