Types of Redox Reactions Video Lecture - Chemistry Class 11 - NEET

welcome to electron line and in order to
understand oxidation reduction reactions
a little bit better let's talk about
what type of oxidation reduction
reactions we have or better yet what
type of reactions are oxidation
reduction reactions and so what I've
listed here is five typical reactions
five very common reactions they are
combination reactions decomposition
reactions displacement reactions
metathesis reactions and acid-base
neutralization reactions myth that
theses reactions are the ones where you
have double this license where compared
to what we call displacement reaction
here where only one element is being the
place here two elements are being the
place that's called a double
displacement reaction then there's a
couple more called disproportionate
reaction and miscellaneous reactions
that of course don't meet any other of
the other criteria now it turns out of
those seven five are what we call
oxidation reduction reactions sometimes
you also say redox reaction to mean
oxidation reduction reaction two of the
five to the seven however are not
oxidation reduction reactions so that
means is that the oxidation numbers do
not change for any of the elements
throughout the reaction so I meant ahead
and put some examples down for that so
here we have a method thesis reaction
and here we have an acid-base reaction
we'll take a look at those in just a
moment
so in all case of the other five the
oxidation numbers are one or more the
elements will change in one form or
another but for these two it does now so
let's take a look at it double
displacement reaction so we have sodium
iodide and let nitrate both in an
aqueous solution
notice that the oxidation number for
sodium of course is gonna be plus one
and for iodine is gonna be minus one for
lead plus two and for the nitrate ion
minus one that's why you need two of
them to balance out the lead now there
in the reaction what will happen is the
sodium will combine with the nitrate and
the lead will combine with the iodine so
there we go and that's what we call
double displacement so two elements are
being switched around and because
that the oxidation numbers do not have
to change so what you see here is that
sodium still is plus one and the nitrate
ion is still minus one here the lead ion
is still plus two in iodine iron is
still minus one of course that's why you
need two of them but notice that nothing
has changed as far as the oxidation
number is concerned so therefore that's
not a redox reaction not a oxidation
reduction reaction the other one is an
acid-base neutralization reaction so
that's where we put an acid and a base
together in sufficient quantities to
neutralize one another and so here we
have hydrochloric acid and sodium
hydroxide
notice that the sodium and the chlorine
will then join together in the aqueous
solution of course in aqueous solution
they'll still be separated with ions but
notice that the sodium has not changed
the oxidation number and the chlorine
also has not changed its oxidation
number now as far as the water that's
being produced that is a combination of
the hydrogen ion right here which has a
plus one and the hydroxide I'm here with
has a minus one but remember with a
hydroxide ion the oxygen is minus two in
the hydrogen is plus one so I put that
bomb below to show you that those add up
to a total of a minus one oxidation
number and then notice that when you
look at water water the oxygen is minus
two and the hydrogen is plus one which
is exactly the same as what we have on
the left side of the reaction so again
no changes in the oxidation number so
therefore this is not called a redox
reaction or an oxidation reduction
reaction so those two are not in that
category the other five are so what
we're going to do now over the next five
videos we're going to take a look at
each one of these five types of
reactions that are oxidation reduction
reactions and show you why they are and
then we'll show you how to find the
balancing of equations using the using
the oxidation numbers in some examples
that are coming up as well there you go
there gives you a nice little overview
of the top reactions that are and top
reactions are not redox reactions