Nature of Bond in Haloalkanes and Haloarenes Video Lecture - Class 12

hello friends this video on haloalkanes
in hello arenas part 7 is brought to you
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so now let's talk about the polar nature
and Burnley
so if you see this my fluorine since
chlorine
this is bromine and this ivory okay this
is my fluorine chlorine bromine ID and
if you see the size increase as we go
down the group so this is my fluorine
has this must sign then my fluorine will
have this much size and bromine will
have bigger size and then iodine will
have all the more because things right
this is how it is as you go down the
group and if you don't put the
electronegativity let me write this let
me write here en but fluorine eliminated
is 4 for chlorine in this 3 domain it is
2.8 and iodine this 2.5 and for carbon
we know that it is 2.5 so if you see as
we go down the groups so if you see this
carbon and halogen this halogen has
tendency to attract electrons towards
itself right this is more
electronegative so this halogen will get
partial negative charge all right
hello this will get partial negative
charge and carbon since halogen has got
partial negative charge Carbon will get
slightly position and that's why my CX
bond is slightly polar in nature why
because the halogen has tendency to
attract electron it has higher
electronegativity as I've seen fluorine
has a electronegativity of 4h of it is C
a bond so fluorine will try to hog
electron and so carbon again slightly
positive Church and this does we see
that hello alkenes have are polar in
nature correct so if you talk about the
bond length if you go down the bond
length increase why because the sizing
is including have a smaller size
chlorine bigger i improving all the more
big adding all the more big since the
size is increasing this length is
increasing this is the morning
correct hope you understood why the
bondage is easy right
so ch3 F has bond lengths of CF as the
model in the 139 picometer and CI a has
the monocoque 240 since bond length is
more it is easy to break is though the
energy required is less it is less tip
you can say this is mostly right this
thing we have done learned in the class
lemon chapter where we see that the mod
length is more easy to bring less stable
bond length is less difficult to break
more stable
correct and if you see if you talk about
the pole of nature now see f3 is maximum
per Y because the Delta of
electronegativity between carbon and
chlorine is what 0.5 minus 4 take the
absolute value there's nothing but 1.5
so this is very polar if you talk about
CI bond it is 2.5 minus 2.5 almost zero
right we talked about CBR bond then it
is 2.5 minus 2.8 is 0.3 talk about CCL
it is three minus 2.5 that is 0.5 so
this is maximum polar this is max fuller
I will write here max power and this is
minimum Pole all right this is max
fuller and this is mean this is less
stable this is most stable hope you
understand see if we talk about its
stability usually talk about the bond
length and that depends on the size so
CI is CI bond is very unstable because
this just the length is more and we talk
about the full of nature you talk about
a difference in electronegativity in
that case you see that CF bond is more
electronegative because the difference
between
a duty of carbon and fluorine is maximum
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