Class 11 Exam > Class 11 Videos > Tetravalency and Hybridisation of Carbon
Tetravalency and Hybridisation of Carbon Video Lecture - Class 11
FAQs on Tetravalency and Hybridisation of Carbon Video Lecture - Class 11
| 1. What is tetravalency of carbon? |  |
Ans. The tetravalency of carbon refers to its ability to form covalent bonds with four other atoms. This is due to carbon having four valence electrons, which allows it to share electrons and form stable compounds with other elements.
| 2. How does hybridization of carbon occur? | |
Ans. Hybridization of carbon occurs when its atomic orbitals mix to form new hybrid orbitals. This process involves the rearrangement of electrons in the valence shell of carbon to create a set of hybrid orbitals with specific geometries, such as sp, sp2, and sp3. These hybrid orbitals enable carbon to form different types of covalent bonds.
| 3. What is the significance of carbon's tetravalency? | |
Ans. Carbon's tetravalency is significant because it allows carbon to form diverse and complex organic compounds. With its ability to form four covalent bonds, carbon can create long chains, branched structures, and rings, giving rise to the vast array of organic molecules found in living organisms and synthetic materials.
| 4. How does hybridization affect the geometry of carbon compounds? | |
Ans. Hybridization greatly influences the geometry of carbon compounds. For example, in sp3 hybridization, carbon forms four sigma bonds, resulting in a tetrahedral geometry. In sp2 hybridization, carbon forms three sigma bonds and one pi bond, leading to a trigonal planar geometry. In sp hybridization, carbon forms two sigma bonds and two pi bonds, resulting in a linear geometry.
| 5. Why is the concept of hybridization important in understanding the properties of carbon compounds? | |
Ans. The concept of hybridization is crucial in understanding the properties of carbon compounds because it helps explain their molecular shapes, bond angles, and reactivity. By knowing the hybridization state of carbon in a molecule, we can predict its geometry and understand how it interacts with other molecules, which is fundamental in fields such as organic chemistry and biochemistry.
Text Transcript from Video
hello friends this video an organic
imaged basic part 2 is brought to you by
exam Viacom no more fear from exam
before we start the whole chapter of
organic chemistry let's start the tetra
valency Oh God and this is the reason
why we have so many carbon compounds so
many common bond that we have a special
branch of science called organic
chemistry because carbon has a good
property to concatenate waveform big
cheese and it's all because of tetra
valency of cover see the atomic number
of carbon is what the atomic number of
carbon is 1/6 so if you see the
electronic configuration is 1s2 2s2 b2
so in the normal state let me write the
normal state the electronic
configuration will be 1s2 2s2 2p6 will
have one 2p why will i have 1 n2 v z VV
m correctly busy that is how it is in
the excited state what will happen is we
have learned about these things in the
previous chapters so this 1 electron
from here will go to P orbitals it will
become 1 s 2 to s 1 to P X 1 u py 1 and
to be z 1 so if you see there are 4
empty so the valence shell has else 4
elements or electrons correct
now since valence L has four electron
and the noble gas configuration and is
it hat it should have eight electrons so
it can either I mean to attain gotta
instability
it can either gain four electron or it
can either lose four liberal correct but
it requires huge energy to either gain
on useful it goes like four electrons on
a joke example sodium has one extra
electron you can easily give an electron
so giving or chlorine if you see
chlorine needs one electron who didn't
has a valence electron seven so chlorine
can easily take one electron and sodium
can easily give one little but exchange
of four electrons is not not a joke it
requires huge huge huge energy correct
so it is this is not possible actually
to gain or lose for electric so this is
not possible this is not possible so
what is the third option the third
option is the sharing of electron
correct sharing is possible maybe one
from this guy one from this guy one from
this guy that is possible right but
actually gaining and losing in on phone
and since gaining and losing involves
finding bond since this is not possible
so in case of carbon will not have only
one
but sharing is possible so will have
covalent
but again if you see right as I have
told the bonds are generally not pure
covalent of your angle it immediate is
covalent bond it will have slight
neglect and that all depends on the
electronegativity difference right
electronegativity differences two point
five or more two point five or more it
does generally I am but in case of most
of this iron chemistry you will see this
covalent
if you see the electronegativity of
carbon as 12.5 this is the
electronegativity of carbon so you can
write the electronegativity or the
commodes if we write here example
hydrogen it is two point one example
oxygen it is three point five for
nitrogen it is three point zero or
chlorine it is three point zero for
sulfur it is 225 so if you see most of
the case and when I talk about a carbon
compound organic compounds carbon forms
born with oxygen nitrogen sulfur
chlorine all these only right so if you
see the electron any difference is not
much but carbon hydrogen agree see two
point five minus two point one at this
point for carbon oxygen also ABC
differences to 0.5 minus three point
where this one carbon nitrogen also if
you see 0.5 minus three that is point
five carbon chlorine also if you see it
is two point five minus three that is
0.5 carbon sulfur two point five minus
0.5 almost zero so since the carbon
compounds organic component we have is
generally formed of carbon hydrogen
oxygen nitrogen sulfur chlorine and the
electrode area difference is not that
much so you see most of them are
covalent compound only one correct so
why this is going on
you can understand this from the
electrode negative negativity difference
point of view also the electronegativity
difference is not that much so they are
covalent also you can say that since it
has four electrons the valence cell it
is very difficult to gain or lose
electrons so it will not form ionic bond
but can share four electrons easily if
you one from this guy one from this guy
one from this van
this guy it will have a happy stable
structure right so it has generally
covalent one function let's talk about
the hybridization carbon so carbon has
three kinds of hybridization sp3
hybridization sp2 and SP all these three
kind of hybridization by cutting example
of sp3 hybridization the example of
meeting
so let's see this hybridization here
this is sp3 hybridization so if you see
in a carbon in the normal state has
electronic configuration of 1 s 2 s 2 2
right so 2 is 2 and compete so what
happens is 1 electron will go from two
ways to 2p this becomes 1 s 2 2 s 1 and
T P so you see this is how this is the
normal state where if you see the has a
us to this to s 2 and this is two feet
it is 2p orbital px py correct so two
electrons the p orbital and two in the Q
s orbitals
I am talking only about diesel this is I
think somewhere there but I have removed
it for simplicity purpose now if you see
this is the electronic injection in the
excited see what will happen is one
electron went to this now if you see
what happens everything is sp3
hybridized right so everything is sp3
hybridized edges you get four orbitals
you got 1 2 3 4 right because sp3 that
means you need s 1 and PC that is four
orbitals so you got four hundreds now
what will happen is this will get SP
three hybridized you see this will get
sp three hybridized this happens when
hydrogen approaches near this carbon so
if you see this become sp3 hybridized
and each of these has 3 electrons one
electron so you see why electron here
one electron here one electron here
multiply in the other green for gains
are from four hydrogen's this is how it
is hope you understand and we have
covered this in the other chapter also
where we talked about the structures of
various atoms yeah then you talk to the
West particularly we have covered this
part so if you see what happened is this
carbon where is the hydrogen approach in
became sp3 hybridized and sp3 hybridized
looks like this with four orbitals each
orbitals has one electron and then it
forms a bond and it won't see s4 with it
you see this is the structure of the
meeting this is the structure la tête
right the other kind of hybrid
then as shown by carbon SBT is sp2 we'll
take the example you so if you see here
the hero's if you see in the normal
state it has two s two and two people
right this is the electronic can be in
the normal state so if you see this is
2s2 and it is stupid
normal state of cover now here what
happens is one electron moves but in
this instead of forming four sp3
orbitals it will form three sp2 orbitals
so you see sp2 that means one s and P P
right so it will form three sp2 orbitals
and one 2p empty orbitals so if you see
the moment hydrogen will approach this
this structure will chain you do SP do
orbitals if you see the moment hydrogen
is approaching what is happening is this
is happening so if you see what happened
is this is my sp2 this is my SP dope
this is my sp2 and this is mine
good luck similarly here also you can
see this is my 2p orbital this is my SPD
this is my SP and this is also my SP
hope you understand what happened here
so here it formed three sp2 orbitals and
one p orbital and then if you see the
carbon is hydrogen is moist and if you
see these P orbitals if you see right
here they form a double bond because
they come - they combine to form a
double bond and if you see this is the
structure here it is a double bond here
why because these P orbitals they
overlap to form a PI bond and thus if
you see here we have sp2 hybridization
similarly carbon also shows SP
hybridization you'll see one more
example in this so if you see the normal
electronic combination is this one s 2 2
s 2 2 P this is a normal neutronic and
the relation we have now what happens is
this is the the same one exactly if you
see 2 s 2 2 people nice to hear the
spherical 1 and P 2 electrons now if you
see one electron went here now instead
of forming
spq it forms to SP orbitals you see and
to MTP is the moment hydrogen will
approach you see here what happens in it
forms to SP orbital and example if you
see this is my SP orbital and this is
the ISP already west power button here
in this and here it forms my PR metal
and so you see this is my 2p orbital
this is my pimp your middle and this is
my SP orbital this best way over right
so we have two SP orbital and to 2p
orbital similarly here also if you see
this is my SPR with you this is my SP
orbital this is my to be in this might
be correct so I have two SP and two
together now if you see hydrogen comes
here and now if you see these guys form
bond because you see this guys from one
bond here right and these guys form are
there so there is a triple bond correct
so that's going to see the structure it
has a triple bond structure so what we
have seen carbon forms SP sp2 and sp3
hybridization correct 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 serene
imaged basic part 2 is brought to you by
exam Viacom no more fear from exam
before we start the whole chapter of
organic chemistry let's start the tetra
valency Oh God and this is the reason
why we have so many carbon compounds so
many common bond that we have a special
branch of science called organic
chemistry because carbon has a good
property to concatenate waveform big
cheese and it's all because of tetra
valency of cover see the atomic number
of carbon is what the atomic number of
carbon is 1/6 so if you see the
electronic configuration is 1s2 2s2 b2
so in the normal state let me write the
normal state the electronic
configuration will be 1s2 2s2 2p6 will
have one 2p why will i have 1 n2 v z VV
m correctly busy that is how it is in
the excited state what will happen is we
have learned about these things in the
previous chapters so this 1 electron
from here will go to P orbitals it will
become 1 s 2 to s 1 to P X 1 u py 1 and
to be z 1 so if you see there are 4
empty so the valence shell has else 4
elements or electrons correct
now since valence L has four electron
and the noble gas configuration and is
it hat it should have eight electrons so
it can either I mean to attain gotta
instability
it can either gain four electron or it
can either lose four liberal correct but
it requires huge energy to either gain
on useful it goes like four electrons on
a joke example sodium has one extra
electron you can easily give an electron
so giving or chlorine if you see
chlorine needs one electron who didn't
has a valence electron seven so chlorine
can easily take one electron and sodium
can easily give one little but exchange
of four electrons is not not a joke it
requires huge huge huge energy correct
so it is this is not possible actually
to gain or lose for electric so this is
not possible this is not possible so
what is the third option the third
option is the sharing of electron
correct sharing is possible maybe one
from this guy one from this guy one from
this guy that is possible right but
actually gaining and losing in on phone
and since gaining and losing involves
finding bond since this is not possible
so in case of carbon will not have only
one
but sharing is possible so will have
covalent
but again if you see right as I have
told the bonds are generally not pure
covalent of your angle it immediate is
covalent bond it will have slight
neglect and that all depends on the
electronegativity difference right
electronegativity differences two point
five or more two point five or more it
does generally I am but in case of most
of this iron chemistry you will see this
covalent
if you see the electronegativity of
carbon as 12.5 this is the
electronegativity of carbon so you can
write the electronegativity or the
commodes if we write here example
hydrogen it is two point one example
oxygen it is three point five for
nitrogen it is three point zero or
chlorine it is three point zero for
sulfur it is 225 so if you see most of
the case and when I talk about a carbon
compound organic compounds carbon forms
born with oxygen nitrogen sulfur
chlorine all these only right so if you
see the electron any difference is not
much but carbon hydrogen agree see two
point five minus two point one at this
point for carbon oxygen also ABC
differences to 0.5 minus three point
where this one carbon nitrogen also if
you see 0.5 minus three that is point
five carbon chlorine also if you see it
is two point five minus three that is
0.5 carbon sulfur two point five minus
0.5 almost zero so since the carbon
compounds organic component we have is
generally formed of carbon hydrogen
oxygen nitrogen sulfur chlorine and the
electrode area difference is not that
much so you see most of them are
covalent compound only one correct so
why this is going on
you can understand this from the
electrode negative negativity difference
point of view also the electronegativity
difference is not that much so they are
covalent also you can say that since it
has four electrons the valence cell it
is very difficult to gain or lose
electrons so it will not form ionic bond
but can share four electrons easily if
you one from this guy one from this guy
one from this van
this guy it will have a happy stable
structure right so it has generally
covalent one function let's talk about
the hybridization carbon so carbon has
three kinds of hybridization sp3
hybridization sp2 and SP all these three
kind of hybridization by cutting example
of sp3 hybridization the example of
meeting
so let's see this hybridization here
this is sp3 hybridization so if you see
in a carbon in the normal state has
electronic configuration of 1 s 2 s 2 2
right so 2 is 2 and compete so what
happens is 1 electron will go from two
ways to 2p this becomes 1 s 2 2 s 1 and
T P so you see this is how this is the
normal state where if you see the has a
us to this to s 2 and this is two feet
it is 2p orbital px py correct so two
electrons the p orbital and two in the Q
s orbitals
I am talking only about diesel this is I
think somewhere there but I have removed
it for simplicity purpose now if you see
this is the electronic injection in the
excited see what will happen is one
electron went to this now if you see
what happens everything is sp3
hybridized right so everything is sp3
hybridized edges you get four orbitals
you got 1 2 3 4 right because sp3 that
means you need s 1 and PC that is four
orbitals so you got four hundreds now
what will happen is this will get SP
three hybridized you see this will get
sp three hybridized this happens when
hydrogen approaches near this carbon so
if you see this become sp3 hybridized
and each of these has 3 electrons one
electron so you see why electron here
one electron here one electron here
multiply in the other green for gains
are from four hydrogen's this is how it
is hope you understand and we have
covered this in the other chapter also
where we talked about the structures of
various atoms yeah then you talk to the
West particularly we have covered this
part so if you see what happened is this
carbon where is the hydrogen approach in
became sp3 hybridized and sp3 hybridized
looks like this with four orbitals each
orbitals has one electron and then it
forms a bond and it won't see s4 with it
you see this is the structure of the
meeting this is the structure la tête
right the other kind of hybrid
then as shown by carbon SBT is sp2 we'll
take the example you so if you see here
the hero's if you see in the normal
state it has two s two and two people
right this is the electronic can be in
the normal state so if you see this is
2s2 and it is stupid
normal state of cover now here what
happens is one electron moves but in
this instead of forming four sp3
orbitals it will form three sp2 orbitals
so you see sp2 that means one s and P P
right so it will form three sp2 orbitals
and one 2p empty orbitals so if you see
the moment hydrogen will approach this
this structure will chain you do SP do
orbitals if you see the moment hydrogen
is approaching what is happening is this
is happening so if you see what happened
is this is my sp2 this is my SP dope
this is my sp2 and this is mine
good luck similarly here also you can
see this is my 2p orbital this is my SPD
this is my SP and this is also my SP
hope you understand what happened here
so here it formed three sp2 orbitals and
one p orbital and then if you see the
carbon is hydrogen is moist and if you
see these P orbitals if you see right
here they form a double bond because
they come - they combine to form a
double bond and if you see this is the
structure here it is a double bond here
why because these P orbitals they
overlap to form a PI bond and thus if
you see here we have sp2 hybridization
similarly carbon also shows SP
hybridization you'll see one more
example in this so if you see the normal
electronic combination is this one s 2 2
s 2 2 P this is a normal neutronic and
the relation we have now what happens is
this is the the same one exactly if you
see 2 s 2 2 people nice to hear the
spherical 1 and P 2 electrons now if you
see one electron went here now instead
of forming
spq it forms to SP orbitals you see and
to MTP is the moment hydrogen will
approach you see here what happens in it
forms to SP orbital and example if you
see this is my SP orbital and this is
the ISP already west power button here
in this and here it forms my PR metal
and so you see this is my 2p orbital
this is my pimp your middle and this is
my SP orbital this best way over right
so we have two SP orbital and to 2p
orbital similarly here also if you see
this is my SPR with you this is my SP
orbital this is my to be in this might
be correct so I have two SP and two
together now if you see hydrogen comes
here and now if you see these guys form
bond because you see this guys from one
bond here right and these guys form are
there so there is a triple bond correct
so that's going to see the structure it
has a triple bond structure so what we
have seen carbon forms SP sp2 and sp3
hybridization correct 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 serene
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Nov 14, 2024 Last updated |
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