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Liquids, solids, and intermolecular forcesDr. Ashley Faris
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We all know that matter exists as :
D
2)
3)
Solids and liquids are known as--and therefore exert
moderate to strong-
-
on one another .
Our goal : establish
Why do we care ?- We will consider how the structure of particularatom or molecule determines its-
at a given-.
- The state of a sample of matter depends onthe-
of intermolecular forces
( IMF) among the constituent particlesrelative to the amount of-
-
CTE ) in the sample .
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Intermolecular forces :
Thermal Energy :
Trend :
- fixed shape } - indefinite shape- indefinite shape ?
Volume but fixed volume Volume
- high density - high density - low density
in:::::f:÷÷÷÷:f :c:c:::- can be crystalline
- or amorphous
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The-
of the particles that compose a
substance determines the-of the-
that holds the substance together. Which in turndetermines if a substance is a-,
-
,
or- at a given temperature .
I. Dispersion forces-
-
in e- distribution within
molecules and atoms
-
e- exist in a 3- dimensional space outside the nucleus
called-
which is the probability of
finding an e- in that space
- e-
are constantly moving and responding to neighborsnearby
ex :
- usually associated with- molecules or
-
- weakest IMF
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* The strength of the dispersion force depends on
Trend :
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2) Dipole - dipole force- Stronger IMF than dispersion
- polar molecules have--⑧
- strength depends on- --
- strength also depends on - &-
Trend :
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3. Hydrogen bonding- Involves polar molecules with
a)
b)c)
- stronger than dispersionand dipole- dipole IMF
- strength depends on #of H - bonds between
molecules
- dependent on size of molecule
- NOT a covalent bond !
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ex :
~i r it
MW
BP
phaseat RT
strongest IMF
D structure of DNA
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4.
Ion - dipole force
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by Hannah Han
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CHM001B WS11:IntermolecularForces
MissionCollege2|P a g e
Q4.Drawthe3-dimensionalstructureandidentifythedominantintermolecularforceineachmolecule:
a. CBr4
b. CH2Cl2
c. CO2
d. CH3NH2
e. I2
f. CH3OH
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vqorizahoa-nd.VEPressureVaporization :
D Vaporization and vapor pressureTrend :
Temperaturesurface area
IMF
* Liquids that vaporize easily are saidto be-
ex :
Energetics- Takes energy to- molecules
→
ex :
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ex : When we sweat , our bodies are covered in liquid water .As the water evaporates , it absorbs heat from the body,
cooling the skin .
- Heat is released when a gas- to a
liquid .
→
ex :
ex : steam burn
CHM001B WS11:IntermolecularForces
MissionCollege3|P a g e
Q5.Rankthefollowingcompoundsinincreasingboilingpoint(1beingthelowestboilingpoint,4beingthehighestboilingpoint).Explainyouranswer.
octane pentane ethane decane
______ ______ ______ ______
Q6.Rankthefollowingcompoundsinincreasingboilingpoint(1beingthelowestboilingpoint,3beingthehighestboilingpoint).Explainyouranswer.
CH3OH I2 CH2Cl2
______ ______ ______
Q7.Calculatetheamountofheat(inkJ)requiredtovaporize12.4kgofwateratitsboilingpoint.
Q8.Supposethat0.48gofwaterat25°Ccondensesonthesurfaceofa55gblockofaluminumthatisinitiallyat25°C.Iftheheatreleasedduringcondensationgoesonlytowardheatingthemetal,whatisthefinaltemperature(in°C)ofthemetalblock?Thespecificheatcapacityofaluminumis0.903J/g°C.
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Vaporizationi¥fak
µVapor pressure:
Trend :
* When a system in--
is disturbed , the system responds to--
and return to a state of
equilibrium .
Trend :
Boiling point :
Normal boiling point :
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* The relationship between Rap and temperature is-
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LTwo data points equation :
CHM001B WS11:IntermolecularForces
MissionCollege4|P a g e
Q9.Ineachpairofcompounds,picktheonewiththehighervaporpressureatagiventemperature.Explainyourreasoning.
a. CH4orCH3Cl
b. CH3OHorCH2O
c. CH3CH2CH2CH2OHorCH3OH
Q10.Thetablebelowdisplaysthevaporpressureofnitrogenatseveraldifferenttemperatures.Usethedatatodeterminetheheatofvaporizationandnormalboilingpointofnitrogen.
Temperature(K) Pressure(torr)65 130.570 289.575 570.880 102885 1718
y=-711.98x+15.833R²=0.99995
44.55
5.56
6.57
7.58
0.011 0.0115 0.012 0.0125 0.013 0.0135 0.014 0.0145 0.015 0.0155 0.016
lnP
1/T(1/K)
WS11Q10
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OtherphasechangesSublimation :
deposition :ex :
fusion :
freezing :
ex :
D Heating curve for water- The amount of
heat required to achieve a phase change
- The amount of heat required to heat a single phasein which the deposited
heat raises the temperature
in accordancewith the substance
's heat capacity
CHM001B WS11:IntermolecularForces
MissionCollege5|P a g e
Q11.Howmuchheat(inkJ)isevolvedinconverting1.00molofsteamat145°Ctoiceat-50°C?Theheatcapacityofsteamis2.01J/g°C,andthatoficeis2.09J/g°C.
Q12.Considerthephasediagrambelowforiodine.
a. Whatisthenormalboilingpointforiodine?
b. Whatisthemeltingpointforiodineat1atm?
c. Whichstateispresentatroomtemperatureandnormalatmosphericpressure?
d. Whichstateispresentat186°Cand1.0atm?
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CHM001B WS11:IntermolecularForces
MissionCollege5|P a g e
Q11.Howmuchheat(inkJ)isevolvedinconverting1.00molofsteamat145°Ctoiceat-50°C?Theheatcapacityofsteamis2.01J/g°C,andthatoficeis2.09J/g°C.
Q12.Considerthephasediagrambelowforiodine.
a. Whatisthenormalboilingpointforiodine?
b. Whatisthemeltingpointforiodineat1atm?
c. Whichstateispresentatroomtemperatureandnormalatmosphericpressure?
d. Whichstateispresentat186°Cand1.0atm?
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D Phase diagrams- each line (or curve ) represents a set of temperaturesand pressures at which the
substance is in equilibriumbetween the two States on
either side of the line
- triple point :
- critical point :
