Intermolecular Forces
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Transcript Intermolecular Forces
Two things affect intermolecular forces:
› Charge
› Distance
Bigger distance equals LESS attraction!
More charge equals MORE attraction!
Coulomb’s Law
› F ~ charge/distance2
› Distance has more effect since it is squared.
Bonds are permanent attractions, IMF’s
are temporary
Covalent
› Sharing of electrons in permanent tug of
war.
Ionic
› Stealing electrons and then being attracted
by opposite charges
Ion Dipole
Hydrogen Bonding
Dipole-Dipole
London Dispersion forces
Between an ion and a dipole!
› Ion = permanently charged particle
› Dipole = a polar molecule
Almost exclusively seen in aqueous
solutions.
Between two dipoles!
› Dipoles are polar molecules
that have no net charge, but
the charge is distributed
unequally.
› Positive end of one attracts
negative end of the other.
ALL covalent compounds experience
this force.
› It is between the electrons in one atom and
the nucleus of another atom.
› More mass and/or more atoms means more
dispersion forces.
›
More mass doesn’t cause an increase in LDF!
›
More mass infers that there are more P and N,
which MEANS there are more electrons.
It is an increase in the number of e- which
causes a larger e- density which leads to a
stronger temporary dipole.
You can use molar mass to figure it out since a
larger molar mass implies a bigger density but
you can't use the words molar mass in your
justification in a Free Response Question
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Occurs in molecules in which hydrogen is
having FON!
› The most electronegative atoms are F, O
and N. With a hydrogen, there is excessive
polarization.
› This excessive polarization attracts the lone
pair of electrons.
Strongest:
Ion-Dipole
(very strong)
Hydrogen Bonding (strong)
Dipole-Dipole
Dispersion Forces (very weak)
More IMF’s or stronger IMF’s affect the
following properties:
› Boiling point
› Melting Point
› Viscosity (thickness)
› Vapor Pressure
› Surface tension
Stronger IMF
› Higher boiling point
Weaker IMF
› Lower boiling point
Compare CS2 to CO2
Both are linear
Both are nonpolar covalent
Both have LDF
CS2 has stronger LDF – larger molecule
means larger e- density
Stronger IMF
› Higher melting point
Weaker IMF
› Lower melting point
Think of red rover…
Compare HBr to Cl2
Both are liner
HBr has LD, Dipole
Cl2 has LD, nonpolar
HBr has stronger IMF – higher melting
point
Stronger IMF
› Higher viscosity
Weaker IMF
› Lower viscosity
More attached to each other, the hard
to flow, like solids vs. liquids.
Compare CH3OCH3 to CH3CH2OH
CH3OCH3 LD, Dipole
CH3CH2OH LD, HB
Therefore CH3CH2OH has stronger IMF and
a higher viscosity
Stronger IMF
› Lower vapor pressure
Weaker IMF
› Higher vapor pressure
Again…think red rover.
Compare H2S to H2O2
H2S LD, Dipole
H2O2 LD, HB
H2O2 has stronger IMF therefore lower
vapor pressure
Resistance of a liquid to increase in its
surface area
Stronger IMF
› Higher surface tension
Weaker IMF
› Lower surface tension
Compare H2CO to H2O
H2CO
H2 O
LD, Dipole
LD, HB
Hydrogen bonding is a stronger IMF than
Dipole, therefore H2O has a stronger
surface tension
Stronger IMF
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Higher boiling point
Higher melting point
Higher viscosity
Higher surface tension
Lower vapor pressure
Weaker IMF
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Lower boiling point
Lower melting point
Lower viscosity
Lower surface tension
Higher vapor pressure