hybridization of atomic orbitals and spsp2
sp3 hybridization of carbon firstly let me teach you that what is hybridization well the
word hybridization means mixture for example when you mix salt plus water you get a mixture
when you mix sugar plus water you get a mixture similarly consider two atomic orbitals s orbital
and p orbital when these two orbitals mix are combined together they form hybrid orbitals
this noted down that hybridization is the mixture or combination of atomic orbitals just like the
mixture of salt and water are mixture of sugar and water in this lecture for simplicity i
would often use mixture of atomic orbitals which would mean hybridization of atomic orbitals
i do so so that you could easily understand it hence we define hybridization as when different
atomic orbitals of same or nearly same energy combined together to form new hybrid orbitals is
called hybridization for example the energy of s orbital is smaller than p orbital but nearly they
have the same energy so they combine together to form hybrid orbitals here you must learn that why
we need to study hybridization of atomic orbitals well hybridization of atomic orbitals teach us two
important concepts it shows us molecular geometry or shape of the molecules secondly it shows us
the bonding of atomic orbitals you will learn more about the molecular geometry and bonding of atomic
orbitals in this lecture secondly why atomic orbitals are hybridized or why hybridization take
place well there are different theories which explain this concept but i am going to explain
it very easily consider two types of atoms a atom and b atom that a atom has two orbitals s orbital
and p orbital while b atom have only one orbital like s orbital now let a atom react with two atoms
of b to form a molecule we can see that there is ss bond between a atom and b atom while here is
sp bond between a atom and b atom we can see that ss bond is totally different from sp bond it means
that a atom form two types of bonds with the same atom of b which is impossible not understandable
and hundred percent wrong thus to solve this issue we look at the hybridization of atomic
orbitals or mixture of atomic orbitals now s orbital and p orbital would combine together to
form two hybrid orbitals known as sp orbitals here this is sp orbital and this is also sp orbital
hence this sp orbital of air atom will form covalent bond with s orbital of b atom and this
sp orbital of a atom will also form covalent bond with s orbital of this b atom so this is now ssp
bond and this is also ssp bond now we can say that a atom form ssp bond with b atom which is
possible understandable and 100 percent right also remember that hybridization of atomic
orbitals does not take place in every molecule for example no hybridization occurs
in the atomic orbitals of molecules like h2 hcl h2s etc now let me explain the
hybridization of atomic orbitals of carbon firstly learning sp3 hybridization of a carbon
atom sp3 hybridization means that in this mixture of atomic orbitals there is one s orbital and
three p orbitals so there are total four orbitals present in sp3 hybridization here is 25 percent
s character and 75 percent peak character present in the sp3 hybridization now have
1s and 3p orbitals combined together to form sp3 hybridization for example consider a carbon
atom in the ground state we know that there are six electrons present in carbon atom and one is
there are two electrons and two s there are two electrons while n2p there is one electron in the
x orbital and one electron in the y orbital now let's consider the excited state of a carbon
atom there are two electrons in the 1s orbital while the one electron and 2s jump into z orbital
of 2pe this is the excited state of a carbon atom the 1s orbital is already complete having 2
electrons so this 2s orbital and 3 orbitals of 2p x y z mix are combined together to form four
hybrid orbitals thus i will place these unpaired four electrons in these four hybrid orbitals
remember that they must have the same spin this is the first sp3 orbital this is the second
sp3 orbital this is the third sp3 orbital and this is the fourth sp3 orbital so we have four
hybrid orbitals sp3 each having one electron now it is sp3 hybridization that teach us
the geometry of carbon and its molecule for example carbon has this type of geometry
and sp3 hybridization this is one sp3 orbital this secant third and fourth sp3 orbitals and each
orbital having single electron the bond angle in sp3 hybridization is 109.5 degree and the ship
of sp3 hybridization of carbon is tetrahedral noted down that these four sp3 hybrid orbitals
are called degenerate orbitals it means that they all have the same energy also let me
give you an example of sp3 hybridization of a carbon and a molecule like methane ch4 now
consider sp3 hybridization in this carbon atom we know that there are four unpaired electrons
present in it according to valence bond theory rvt unpaired electrons are needed to form
covalent bond so four hydrogen atoms will share their single valence electron with
the electron of hybrid orbitals of a carbon and we get ch4 thus this is the shape and
geometry of methane ch4 in which carbon has sp3 hybridization so note down this example
secondly let me teach you sp2 hybridization sp2 hybridization means that in this mixture of
atomic orbitals there is one s orbital and two p orbitals hence there are total three
orbitals present in sp2 hybridization or there is 33 percent s character and 67 percent
peak character present in sp2 hybridization now how these orbitals 1s and 2s combine together
in sp2 hybridization well again consider carbon in a ground state we know that 1s has 2 electrons 2s
has 2 electrons and in 2p there is one electron in x orbital and one electron in y orbital while
an excited state of carbon 1s has two electrons 2s has one electron and n2p there is one electron
in x orbital one electron in y orbital and one electron in z orbital now in the hybrid state
there are already two electrons present in the 1s orbital we know that in sp2 hybridization 1s
orbital and 2 p orbitals combined together so this 2s orbital x and y orbitals of 2p would combine
together to form 3 orbitals of sp2 hybridization thus i will put this unpaired electron in
these hybrid orbitals having same spin this is the first sp2 orbital this is the second
sp2 orbital and this is the third sp2 orbital lastly i write this z orbital of 2p
here this z orbital is unhybrid orbital it means that this c orbital do not combine
with 2s 2px and 2py also it has more energy than all these three hybrid orbitals now carbon has
this type of geometry and sp2 hybridization this is the first sp2 orbital this is the second
and third sp2 orbitals while this long orbital is the 2pz orbital which is unhybridized orbital
these all orbitals have one electron each remember that the bond angle in sp2 hybridization is 120
degree while the shape of carbon is trigonal also let me give you an example of sp2 hybridization
of carbon in a molecule like ethane let's consider sp2 hybridization in this carbon atom and
in this carbon atom firstly both the carbon atoms will form chemical bond by sharing the
unpaired electrons in these spsp orbitals secondly they both will share the unpaired
electrons and unhybrid orbitals to pz then hydrogen will share its one electron with
this sp2 orbital and with this sp2 orbital also hydrogen will share its electron with
this sp2 orbital and with this sp2 orbital note it down that unhybrid orbitals always
form pi bond for example this 2pz form pi bond while hybrid orbitals always form sigma bond
for example these sp2 orbitals form sigma bond thus in ethane there is one pi bond and one sigma
bond between carbon-carbon atoms hence this is the shape and geometry of a molecule in which carbon
has sp2 hybridization so noted down this example finally let me teach you sp hybridization sp
hybridization means that in this mixture of atomic orbitals there is one orbital of s and one
orbital of b present in it so there are total two orbitals present in sp hybridization there
is 50 percent s character and 50 percent p character in it know how one is orbital and one p
orbital combine together to form sp hybridization well again consider carbon in ground
state and an excited state we know that in sp hybridization only 1s and 1p orbitals mix
are combined together to form sp hybridization hence in the excited state 2s orbital
and only x orbital of 2p combine together to form two sp hybrid orbitals this is the first
sp orbital and this is the second sp orbital the y and z orbitals of 2p do not take part in
sp hybridization of carbon so they both are unhybrid orbitals thus we have two hybrid orbitals
and sp hybridization each having unpaired electron now carbon has this type of geometry and sp
hybridization this is the first sp orbital and this is the second sp orbital while this long
orbital is 2py and this long orbital is too pc they both are unhybrid orbitals the bond
angle of sp hybridization is 180 degree and its ship is linear also let me give you
an example of sp hybridization of carbon and a molecule like ethane let's consider sp
hybridization in this carbon and in this carbon firstly both the carbon atoms will shear the
unpaired electrons in spsp orbitals to form a chemical bond secondly they both will share the
unpaired electrons in unhybrid orbitals like 2py and 2pz to form a chemical bond then hydrogen
will share its one electron with this sp orbital and with this sp orbital there are two unhybrid
orbitals like 2py and 2pz joined between carbon atoms so there are two pi bonds present in
ethyne while there is one hybrid orbital joined between carbon atoms so there is only one
sigma bond present in ethane hence this is the shape and geometry of a molecule and which carbon
has sp hybridization just noted down this example