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How intermolecular forces affect boiling points - The Solid State Video
FAQs on How intermolecular forces affect boiling points - The Solid State
| 1. How do intermolecular forces affect boiling points? |  |
Ans. Intermolecular forces play a crucial role in determining the boiling point of a substance. Stronger intermolecular forces result in higher boiling points, as more energy is required to overcome these forces and convert the substance from a liquid to a gas state.
| 2. What are the types of intermolecular forces that affect boiling points? | |
Ans. The types of intermolecular forces that affect boiling points include hydrogen bonding, dipole-dipole forces, and London dispersion forces. Hydrogen bonding is the strongest intermolecular force and leads to the highest boiling points, followed by dipole-dipole forces, and then London dispersion forces.
| 3. How does hydrogen bonding affect boiling points? | |
Ans. Hydrogen bonding is a strong intermolecular force that occurs between a hydrogen atom bonded to a highly electronegative atom (such as oxygen, nitrogen, or fluorine) and a lone pair of electrons on another electronegative atom. The presence of hydrogen bonding leads to higher boiling points, as it requires more energy to break these strong bonds and convert the substance from a liquid to a gas state.
| 4. Can you explain dipole-dipole forces and their effect on boiling points? | |
Ans. Dipole-dipole forces occur between the positively charged end of one polar molecule and the negatively charged end of another polar molecule. These forces are weaker than hydrogen bonding but still contribute to higher boiling points compared to substances with only London dispersion forces. The stronger the dipole-dipole forces, the higher the boiling point.
| 5. How do London dispersion forces influence boiling points? | |
Ans. London dispersion forces, also known as van der Waals forces, are the weakest intermolecular forces. They occur between all molecules, whether polar or nonpolar, due to temporary shifts in electron distribution. London dispersion forces increase with the size and shape of the molecules, resulting in higher boiling points for substances with larger and more complex molecules.
Text Transcript from Video
well this part of the IP chemistry
syllabus is a real mess but I'm gonna do
my best for you when all the videos are
done there'll be nothing missing so
hydrogen fluoride and hydrogen chloride
well those are two halogens there and if
I write down the boiling points the
hydrogen fluoride has a higher boiling
point than hydrogen chloride so it needs
more energy to pull hydrogen fluoride
apart from each other so the liquid
phase into the gas now both of these
molecules have dipoles but the dipole
and hydrogen fluoride is much stronger
that's why it's harder to boil it needs
more energy to boil it now the special
sort of strong dipole is called a
hydrogen bond and those are stronger
than regular dipole-dipole interactions
so hydrogen bond is a special dipole
it's special because it's stronger so if
I had two hydrogen fluorides there the
hydrogen bond will be between for
example a hydrogen on one molecule and
are flowing on another those dotted
lines represent one hydrogen bond there
are special sort of dipole why are they
special they're strong fo and n are the
three elements that bond with hydrogen
to make hydrogen bonds that's tie for
rain that's how I remember it fun buck
my cup tie for rain is fall
Arabic for rain is that won't
help you so let's look at water and
hydrogen sulfide hydrogen bonds in water
and only dipole-dipole in hydrogen
sulfide does have a dipolar bent
molecule and there is some attraction
between one hydrogen sulfide and the
next but it's not as strong as the
hydrogen bond on water so the boiling
point of water is a hundred and hydrogen
sulfide well that's kind of the eggy
smell that you might have when you break
wind and that's a gas well at least I
hope it's I guess jeez
so let's look at ethanol and that isn't
ether there now you don't need to know
the name of the ether on the right and I
can't remember it you don't need to know
it now these are isomers they have the
same formula but I had
and structures so these are gonna have
different boiling points ethanol you can
see has the ability to make hydrogen
bonds but that ether there no hydrogen
bonds there is no hydrogen connected to
fluorine oxygen or nitrogen now in
yellow that oxygen hydrogen bond that
isn't a hydrogen bond don't fall for
that the hydrogen bonds are between one
molecule and another molecule their
intermolecular not entrap molecular
those are covalent we're not going to
break those when we boil it we just have
carbon oxygen and hydrogen left so the
ethanol has hydrogen bonds they're a
special sort of dipole they're stronger
and so that explains what ethanol has
the higher boiling point the ether also
has a dipole but there are no hydrogen's
connected to oxygen nitrogen or fluorine
so there's no hydrogen bonds in ether
all right then so let's look down Group
five here's a little thing for you if
you were to drop dead in a swamp then
the phosphorus in your bones and the
anaerobic environment of the swamp would
form the chemical ph3 which vib wants
you to know about
it's a reducing environment hydrogen's
are added now pH three will react with
itself as it passes through the soil to
form dye phosphorus tetrahydrate which
spontaneously lights up and explodes on
contact with air leaving a white smoke
behind this white smoke is tetra
phosphorus Dec oxide I guess that's why
people might think there could be a
ghost you know that's one of the ways
that when people die in swamps they
might think there's a ghost wish a big
flash jeez all right then so this one's
again pretty obvious as hydrogen bonds a
beating dipole-dipole all the ones we've
done so far specifically mentioned in
the syllabus so let me just draw that
out for you
the hydrogen bonds are between the
hydrogen in one molecule and the
nitrogen in the next molecule those two
dashed yellow lines represent a hydrogen
bond
these three chemicals well the top one
is propane
it's an alkane the second one is ethanol
and the final one is ethanol now they're
molar masses are about the same the top
one only has van der waals the middle
ones dipole-dipole from that c double
bond o and hydrogen bond on the final
one so how do you think the pattern of
the boiling points is going to go or the
lowest boiling point is at the top and
the highest is at the bottom
syllabus is a real mess but I'm gonna do
my best for you when all the videos are
done there'll be nothing missing so
hydrogen fluoride and hydrogen chloride
well those are two halogens there and if
I write down the boiling points the
hydrogen fluoride has a higher boiling
point than hydrogen chloride so it needs
more energy to pull hydrogen fluoride
apart from each other so the liquid
phase into the gas now both of these
molecules have dipoles but the dipole
and hydrogen fluoride is much stronger
that's why it's harder to boil it needs
more energy to boil it now the special
sort of strong dipole is called a
hydrogen bond and those are stronger
than regular dipole-dipole interactions
so hydrogen bond is a special dipole
it's special because it's stronger so if
I had two hydrogen fluorides there the
hydrogen bond will be between for
example a hydrogen on one molecule and
are flowing on another those dotted
lines represent one hydrogen bond there
are special sort of dipole why are they
special they're strong fo and n are the
three elements that bond with hydrogen
to make hydrogen bonds that's tie for
rain that's how I remember it fun buck
my cup tie for rain is fall
Arabic for rain is that won't
help you so let's look at water and
hydrogen sulfide hydrogen bonds in water
and only dipole-dipole in hydrogen
sulfide does have a dipolar bent
molecule and there is some attraction
between one hydrogen sulfide and the
next but it's not as strong as the
hydrogen bond on water so the boiling
point of water is a hundred and hydrogen
sulfide well that's kind of the eggy
smell that you might have when you break
wind and that's a gas well at least I
hope it's I guess jeez
so let's look at ethanol and that isn't
ether there now you don't need to know
the name of the ether on the right and I
can't remember it you don't need to know
it now these are isomers they have the
same formula but I had
and structures so these are gonna have
different boiling points ethanol you can
see has the ability to make hydrogen
bonds but that ether there no hydrogen
bonds there is no hydrogen connected to
fluorine oxygen or nitrogen now in
yellow that oxygen hydrogen bond that
isn't a hydrogen bond don't fall for
that the hydrogen bonds are between one
molecule and another molecule their
intermolecular not entrap molecular
those are covalent we're not going to
break those when we boil it we just have
carbon oxygen and hydrogen left so the
ethanol has hydrogen bonds they're a
special sort of dipole they're stronger
and so that explains what ethanol has
the higher boiling point the ether also
has a dipole but there are no hydrogen's
connected to oxygen nitrogen or fluorine
so there's no hydrogen bonds in ether
all right then so let's look down Group
five here's a little thing for you if
you were to drop dead in a swamp then
the phosphorus in your bones and the
anaerobic environment of the swamp would
form the chemical ph3 which vib wants
you to know about
it's a reducing environment hydrogen's
are added now pH three will react with
itself as it passes through the soil to
form dye phosphorus tetrahydrate which
spontaneously lights up and explodes on
contact with air leaving a white smoke
behind this white smoke is tetra
phosphorus Dec oxide I guess that's why
people might think there could be a
ghost you know that's one of the ways
that when people die in swamps they
might think there's a ghost wish a big
flash jeez all right then so this one's
again pretty obvious as hydrogen bonds a
beating dipole-dipole all the ones we've
done so far specifically mentioned in
the syllabus so let me just draw that
out for you
the hydrogen bonds are between the
hydrogen in one molecule and the
nitrogen in the next molecule those two
dashed yellow lines represent a hydrogen
bond
these three chemicals well the top one
is propane
it's an alkane the second one is ethanol
and the final one is ethanol now they're
molar masses are about the same the top
one only has van der waals the middle
ones dipole-dipole from that c double
bond o and hydrogen bond on the final
one so how do you think the pattern of
the boiling points is going to go or the
lowest boiling point is at the top and
the highest is at the bottom
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Apr 19, 2026 Last updated
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