Class 11 Exam > Class 11 Videos > L2 : London or dispersion force - states of matter, Class 11
L2 : London or dispersion force - states of matter, Class 11 Video Lecture
FAQs on L2 : London or dispersion force - states of matter, Class 11 Video Lecture
| 1. What are dispersion forces? |  |
Ans. Dispersion forces, also known as London forces, are the weakest intermolecular forces that exist between non-polar molecules. These forces arise due to temporary fluctuations in the electron distribution within a molecule, creating temporary dipoles. These temporary dipoles induce similar dipoles in neighboring molecules, resulting in an attractive force between them.
| 2. How do dispersion forces affect the states of matter? | |
Ans. Dispersion forces play a crucial role in determining the physical properties of substances and their states of matter. In gases, the weak dispersion forces allow molecules to move freely, resulting in a low boiling point and compressibility. In liquids, stronger dispersion forces cause molecules to be closer together, leading to a higher boiling point and viscosity. In solids, the strongest dispersion forces result in a fixed arrangement of molecules, leading to a high melting point and rigidity.
| 3. What factors influence the strength of dispersion forces? | |
Ans. The strength of dispersion forces depends on the size and shape of molecules. Larger molecules have more electrons, leading to stronger dispersion forces. Similarly, molecules with a larger surface area have more contact points for dispersion forces, making them stronger. The distance between molecules also affects the strength of dispersion forces, with closer molecules experiencing stronger attractions.
| 4. How do dispersion forces compare to other intermolecular forces? | |
Ans. Dispersion forces are generally weaker than other intermolecular forces such as dipole-dipole interactions and hydrogen bonding. However, they are present in all molecules, regardless of polarity, whereas dipole-dipole interactions and hydrogen bonding only occur in polar molecules. Therefore, dispersion forces are the primary intermolecular forces in non-polar substances.
| 5. Can dispersion forces be overcome? | |
Ans. Yes, dispersion forces can be overcome by providing enough energy to break the temporary attractions between molecules. This can occur through the application of heat, resulting in a phase change from solid to liquid or liquid to gas. Additionally, dispersion forces can be weakened or eliminated by introducing other intermolecular forces, such as polarity or hydrogen bonding, which can compete with dispersion forces for molecule-molecule interactions.
Text Transcript from Video
hello friends this video on states of
matter part 2 is brought to you by exam
Viacom no more fear from exam if you're
watching the video please make sure that
you have watched part 1 so we'll start
with intermolecular force so they told
intermolecular force our force of
attraction or repulsion between
interacting particles atoms are one and
some of these interactive attractive and
repulsive intramolecular forces all
Wonderwall force so all the force which
you have I'll show you different inner
force you have intermolecular force you
add all these things all those force you
can get wonder one forces or this are
called wonder one force cumulative
actually so they're various types of on
drama throws the first force is called a
London force named after the scientist
who discovered it and then you have
something called a dipole-dipole force
and in dipole-dipole force we have some
called hydrogen is a special kind of
dipole-dipole force we'll explain that
and then we have called type 1 and in
use i before so we have actually three
types of von der Waal forces London
forces dipole-dipole and by : induced I
will explain these chumps right please
note here that the attractive force
between the ion and a Bible are ion
dipole force and they are not one
durable force please note I on dipole
force is not one or one force so in
whatever form a only three types London
force dipole-dipole and dipole induce
dipole emotion okay
and as I told intermolecular force are
responsible for physical properties so
physical properties is a boiling point
bending point viscosity and surface
tension can be determined by
intermolecular correct so before we even
start with different in the force list
understand on its recap let's take a
recap on the poorer and mantle
molecule size we already know that but
let's do that we can be able to study
this in past classes so polar molecules
here there is no net charge and on each
of the atom in the molecule there is no
net charge no charge or delta charge in
any atom and mostly this is because the
symmetry actually there is no net charge
example if you see does not need child
and carbon or hydrogen here also there
is no nitrogen on bone of fluorine here
or say we see nitrogen nitrogen the
symmetry there is no no charge oxygen
also you see because symmetry there is
known and charged but if you see there's
something called polar molecules where
individual atoms may have some charge
because of the difference in
electronegativity and lack of similarity
example if you see h2o oxygen will have
slight negative charge and hydrogen will
have slight positive charge right slight
charge is noted by the symbol example a
chapati PC since flowing is more electro
negativity negative chlorine will get
slightly de Chardin H will give slight
positive charge because fluorine will
attract electron to watch itself here
also if you see o 3 for this two oxygen
molecules has applied negative charge
and this has plus charged and we have
discussed this when you discuss a little
structure if you are not comfortable in
this you can watch my video on the
structure of atom last video and s3 also
if you see they are slight poorer
actually they have some dipole and there
there there are some polar molecules
like so with this in mind we if we know
what is polar and normally the polar
molecule let's start with the London
dispersion the London force or the
dispersion watch so they are generally
temporary in nature so will they explain
that so and these are generally by the
nonpolar molecules this London London
for London force is exhibited by Norman
pure molecules and they are temporary
right and they are because of the
movement of electrons in the molecule
this change example example I have
bought two molecules 202 molecules right
I have an automatical here one of the
molecule here so I am talking about the
intermolecular force and rahim would
force between these two molecules and if
you see the normal load two molecules I
am just drawing the liver structure the
electrons are evenly distributed so my
two pairs of electrons are shared and if
you see two electrons four electrons
each are evenly distributed across
oxygen here also same thing my two pair
for four electrons are evenly
distributed across this oxygen but if
you see even as I do this in my
electrons this is my atom right and then
I have various shells I have this s
right like this very shells I have pick
up every shells at the end the electron
keeps moving from keep jumping here and
there and there is a big probability
cloud here right because the electron is
not static it keeps moving jumping here
there so it may happen sometime then
these electrons spend more time in this
direction so what happens these
electrons spend more time in this
direction since this direction has got
more electron is slightly degree charge
and the series likely positive charge
since this has got slightly degree
charged this negative charge will repel
the electrons here and we get slight
positive charge here so it is sliced
partly this will be negative
similarly if there is a nearby like
oxygen here also since it has got
negative charge and it will repel the
electrons here so the electrons will
move here ready bit here right this side
and this will also gets like positive
charges like nature right see the
electrons jumps around here and there
sometimes may happen the temporary fault
in this particular molecule the
electrons are in this direction more the
electron density is more in this
direction
may happen because it jumps around here
there just like that so since it may
move it may be in this direction a
little bit more so it gets like a
negative charge and this will get
slightly positive charge this negative
charge will induce positive charge here
it will because this will repel the
electron here and again you get slightly
positive charge a is like killing a
Charlie Sheen it is slightly negative
charge it will ripple the electrons here
the electrons will go this side
so if you see consequently what we are
getting is plus minus plus minus plus
minus and then there will be force of
attraction between them right and this
force of attraction is something but
mylanta London and London force or
dispersion foot and please note this
happens in nonpolar molecules and they
are temporary but he is happening it
like that there billions of molecules in
a in decibels in a class water and this
course come into play it goes off comes
into play but it keeps happening example
it may be that there are some 10 lacs
molecules and out of that always a good
number of molecules are getting packed
in due to non unforced and that's why it
has importance just now that it's not
important it is important because they
are the millions of molecules in a
energy in a glass of water agency but
out of that good number of molecules I
think at any given point of time good
number of molecules take part in this
kind of cycle they are a in this force
so this force to exist but it is not
that it is always between this two
Monica's it's keep changing rates and
sometimes it is in this part something
is in this part and this is this part if
I'm talking about a tongue or quarter
let us understand some more thing on the
dispersion force it was proposed by sama
business London and that's how the deal
came and it is a temporary force and
this is always force of
she liked the always attractive and the
interaction energy is inversely
proportional to vi power of distance
between two interacting party so if you
see the force or energy is directly in
inversely proportional to our six where
R is the distant true body and these
four sign point only for short distance
the slight positive slightly in each
other also temporary there they are
there's their existing only for short
distance right and these all depends on
the polarizability of the particle how
easily a atom in a molecule can be
polarized so this force depend on the
magnitude of that because if water
molecule and knock see is easy to rise
it sorry water I can't take because
water is a non-polar thing I take polar
money
so if oxygen molecule and NOx is easily
polarizable it will have strong
dispersal if I take some other molecule
some one reporter molecule and there is
not easily polarizable that you have we
this question or so the magnitude
depends on the polarizability of the
particle how easily you can polarize the
particle thank you visit exam viacom to
watch free education videos try free
online tests get the best quality study
materials study from the best tutors and
mentors and much more thanks and sorry
matter part 2 is brought to you by exam
Viacom no more fear from exam if you're
watching the video please make sure that
you have watched part 1 so we'll start
with intermolecular force so they told
intermolecular force our force of
attraction or repulsion between
interacting particles atoms are one and
some of these interactive attractive and
repulsive intramolecular forces all
Wonderwall force so all the force which
you have I'll show you different inner
force you have intermolecular force you
add all these things all those force you
can get wonder one forces or this are
called wonder one force cumulative
actually so they're various types of on
drama throws the first force is called a
London force named after the scientist
who discovered it and then you have
something called a dipole-dipole force
and in dipole-dipole force we have some
called hydrogen is a special kind of
dipole-dipole force we'll explain that
and then we have called type 1 and in
use i before so we have actually three
types of von der Waal forces London
forces dipole-dipole and by : induced I
will explain these chumps right please
note here that the attractive force
between the ion and a Bible are ion
dipole force and they are not one
durable force please note I on dipole
force is not one or one force so in
whatever form a only three types London
force dipole-dipole and dipole induce
dipole emotion okay
and as I told intermolecular force are
responsible for physical properties so
physical properties is a boiling point
bending point viscosity and surface
tension can be determined by
intermolecular correct so before we even
start with different in the force list
understand on its recap let's take a
recap on the poorer and mantle
molecule size we already know that but
let's do that we can be able to study
this in past classes so polar molecules
here there is no net charge and on each
of the atom in the molecule there is no
net charge no charge or delta charge in
any atom and mostly this is because the
symmetry actually there is no net charge
example if you see does not need child
and carbon or hydrogen here also there
is no nitrogen on bone of fluorine here
or say we see nitrogen nitrogen the
symmetry there is no no charge oxygen
also you see because symmetry there is
known and charged but if you see there's
something called polar molecules where
individual atoms may have some charge
because of the difference in
electronegativity and lack of similarity
example if you see h2o oxygen will have
slight negative charge and hydrogen will
have slight positive charge right slight
charge is noted by the symbol example a
chapati PC since flowing is more electro
negativity negative chlorine will get
slightly de Chardin H will give slight
positive charge because fluorine will
attract electron to watch itself here
also if you see o 3 for this two oxygen
molecules has applied negative charge
and this has plus charged and we have
discussed this when you discuss a little
structure if you are not comfortable in
this you can watch my video on the
structure of atom last video and s3 also
if you see they are slight poorer
actually they have some dipole and there
there there are some polar molecules
like so with this in mind we if we know
what is polar and normally the polar
molecule let's start with the London
dispersion the London force or the
dispersion watch so they are generally
temporary in nature so will they explain
that so and these are generally by the
nonpolar molecules this London London
for London force is exhibited by Norman
pure molecules and they are temporary
right and they are because of the
movement of electrons in the molecule
this change example example I have
bought two molecules 202 molecules right
I have an automatical here one of the
molecule here so I am talking about the
intermolecular force and rahim would
force between these two molecules and if
you see the normal load two molecules I
am just drawing the liver structure the
electrons are evenly distributed so my
two pairs of electrons are shared and if
you see two electrons four electrons
each are evenly distributed across
oxygen here also same thing my two pair
for four electrons are evenly
distributed across this oxygen but if
you see even as I do this in my
electrons this is my atom right and then
I have various shells I have this s
right like this very shells I have pick
up every shells at the end the electron
keeps moving from keep jumping here and
there and there is a big probability
cloud here right because the electron is
not static it keeps moving jumping here
there so it may happen sometime then
these electrons spend more time in this
direction so what happens these
electrons spend more time in this
direction since this direction has got
more electron is slightly degree charge
and the series likely positive charge
since this has got slightly degree
charged this negative charge will repel
the electrons here and we get slight
positive charge here so it is sliced
partly this will be negative
similarly if there is a nearby like
oxygen here also since it has got
negative charge and it will repel the
electrons here so the electrons will
move here ready bit here right this side
and this will also gets like positive
charges like nature right see the
electrons jumps around here and there
sometimes may happen the temporary fault
in this particular molecule the
electrons are in this direction more the
electron density is more in this
direction
may happen because it jumps around here
there just like that so since it may
move it may be in this direction a
little bit more so it gets like a
negative charge and this will get
slightly positive charge this negative
charge will induce positive charge here
it will because this will repel the
electron here and again you get slightly
positive charge a is like killing a
Charlie Sheen it is slightly negative
charge it will ripple the electrons here
the electrons will go this side
so if you see consequently what we are
getting is plus minus plus minus plus
minus and then there will be force of
attraction between them right and this
force of attraction is something but
mylanta London and London force or
dispersion foot and please note this
happens in nonpolar molecules and they
are temporary but he is happening it
like that there billions of molecules in
a in decibels in a class water and this
course come into play it goes off comes
into play but it keeps happening example
it may be that there are some 10 lacs
molecules and out of that always a good
number of molecules are getting packed
in due to non unforced and that's why it
has importance just now that it's not
important it is important because they
are the millions of molecules in a
energy in a glass of water agency but
out of that good number of molecules I
think at any given point of time good
number of molecules take part in this
kind of cycle they are a in this force
so this force to exist but it is not
that it is always between this two
Monica's it's keep changing rates and
sometimes it is in this part something
is in this part and this is this part if
I'm talking about a tongue or quarter
let us understand some more thing on the
dispersion force it was proposed by sama
business London and that's how the deal
came and it is a temporary force and
this is always force of
she liked the always attractive and the
interaction energy is inversely
proportional to vi power of distance
between two interacting party so if you
see the force or energy is directly in
inversely proportional to our six where
R is the distant true body and these
four sign point only for short distance
the slight positive slightly in each
other also temporary there they are
there's their existing only for short
distance right and these all depends on
the polarizability of the particle how
easily a atom in a molecule can be
polarized so this force depend on the
magnitude of that because if water
molecule and knock see is easy to rise
it sorry water I can't take because
water is a non-polar thing I take polar
money
so if oxygen molecule and NOx is easily
polarizable it will have strong
dispersal if I take some other molecule
some one reporter molecule and there is
not easily polarizable that you have we
this question or so the magnitude
depends on the polarizability of the
particle how easily you can polarize the
particle thank you visit exam viacom to
watch free education videos try free
online tests get the best quality study
materials study from the best tutors and
mentors and much more thanks and sorry
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Jan 02, 2025 Last updated |
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