Displacement Reactions Video Lecture | Chemistry Class 11 - NEET

welcome to electron line and here we're
going to talk about our third oxidation
reduction reaction which is called the
displacement reaction where one element
is displacing another element in a
reaction and typically the reason why
that happens is either because the
element is more or less electronegative
if it's more electronegative it's more
likely to grab electrons if it's less
electronegative it's more likely to
donate electrons and so there's going to
be switching taking place in which
element the molecule takes up so that
let's take a look at these examples here
here we have solid zinc and copper
sulfate now it turns out that copper is
more electronegative than zinc and so
therefore it's more likely to grab the
electrons from zinc turn that way this
will be oxidized this will be reduced
they'll switch around places and zinc
will now combine with sulphur dye with
the sulfate ion and copper will then
come out as a solid in the precipitate
on the next example right here we have
chlorine gas we have potassium bromine
notice that chlorine is more
electronegative than bromine so it's
more likely to grab electrons so it's
going to take the electron away from
bromine that then becomes
electronegative so you can see minus 1
it will then combine with potassium
which is positive and therefore we have
bromine coming out as a liquid that is
now has an oxidation number of 0 here we
have sodium and water sodium is very
easily oxidized and so the hydroxide ion
from water will oxidize sodium they will
then form sodium hydroxide and hydrogen
gas will then come out here we have
magnesium and hydrochloric acid notice
magnesium is very easily oxidized as
well very easily gives an electron away
chlorine is very electronegative it will
grab the electron turn magnesium into a
positive ion oxidation number plus to
combine with the chlorine and hydrogen
gas will then escape and here we have
aluminum and iron oxide or that's also
called ferric oxide because it's
oxidized to the +3 State notice that
iron is more electronegative than
aluminum so it's more likely to grab
electrons aluminum will be more likely
to give up those electrons
exactly what happens iron comes in grabs
electrons some aluminum turns aluminum
into an oxidation state of +3 iron will
then go to neutral state come out as a
liquid why does iron come out as liquid
because it's done under very high
temperatures and matter of fact this is
how we actually get iron ore out of the
other defero oxide state by heating up
to very high temperatures we can then do
the displacement and combine it with
aluminum here and feed the iron I don't
know if that's the economical way to do
that but that definitely that reaction
works again for the reason iron is more
electronegative than aluminum more
likely to graft electrons so a lot of
the displacement reactions all have to
do with one element being either more
electronegative or an electro positive
and therefore or less electronegative I
should say it's not electro positive and
it's so high or low electronegativity
which then causes the element to be
replaced or displaced in the solution
and that's a good example of oxidation
reaction reactions