Lewis Acids and Bases Video Lecture - JEE

boid Pete and I'm back after a long
period off of YouTube and a three
Academy is back I am pretty excited so
today we're going to be looking at the
Lewis model of acids and bases so I hope
you guys are excited this is going to be
a fun one so let's dive right in so
before we look at the Lewis model of
acids and bases we need to look at first
two other models that were come up with
by other people so first we have the
Arrhenius definition and then after that
we came the brown step lowry definition
and then finally we have the Lewis
definition so if we look at this each
one encompasses the other so granier's
chem came up with a very specific
definition for acids and bases and then
bronsted-lowry expanded on that and then
Lewis came up with even a more
generalized definition encompassing more
than anything that either the two had
come up with before
so one encompasses the other now when we
normally refer to acids and bases we
know when we tend to look at the
bronsted-lowry acids and bases but some
compounds are Lewis acids that are not
bronsted-lowry acids so we're going to
take a look at that shortly an acid is
defined as an electron pair acceptor in
the Lewis model and the base likewise is
defined as an electron pair donor okay
so let's just take it a look at an
example to see what this all means
so we have our hydroxide ion on the
right and we have our H+ ion on the left
okay and in this reaction we see that
the hydroxide ion donates one of one of
its lone pair of electrons to the H+ ion
and now they're bonded is one water
molecule so what happened here was the
H+ accepted the electron pair making it
the Lewis acid well the oxygen or rather
the hydroxide donated its electron pair
making it the lowest base H+ had an
empty orbital to fill so here's another
reaction this is a classic reaction
between ammonia boron trifluoride so
this is a good example of where point
florette is not a bronsted-lowry acid or
an acid but rather when we look at the
Lewis definition we can see that it is a
clear acid so here ammonia is donating
its electron pair to boron trifluoride
and boron boron trifluoride is happily
taking that electron pair making it the
acid in this case so again
ammonia donates its electron pair making
it the lewis base and boron trifluoride
accepts the electron pair making it the
lewis acid so yeah so boron trifluoride
if you guys know is sp2 hybridized and
it has an empty 2p orbital to fill and
it does that by taking that electron
pair from ammonia being a Lewis acid so
that is all for this video guys I hope
you guys enjoyed that short overview of
the Lewis model of acids and bases and I
also wanted to thank you guys because a
t3 Academy just hit 500 subscribers on
YouTube we're pretty excited and we hope
to create more videos for you in the
coming days and not and be more active
in the future and as always guys the
more you know the better you are peace
yeah