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Lewis Acids and Bases Video Lecture - JEE
FAQs on Lewis Acids and Bases Video Lecture - JEE
| 1. What are Lewis acids and bases? |  |
Ans. Lewis acids and bases are a concept in chemistry that describes the behavior of substances during chemical reactions. A Lewis acid is a substance that can accept a pair of electrons, while a Lewis base is a substance that can donate a pair of electrons. This concept was introduced by Gilbert N. Lewis in 1923 and expands upon the traditional Bronsted-Lowry acid-base theory.
| 2. How do Lewis acids and bases differ from Bronsted-Lowry acids and bases? | |
Ans. The main difference between Lewis acids and bases and Bronsted-Lowry acids and bases lies in their definition of acidity and basicity. In the Bronsted-Lowry theory, an acid is a substance that donates a proton, while a base is a substance that accepts a proton. On the other hand, in the Lewis theory, an acid is a substance that accepts an electron pair, and a base is a substance that donates an electron pair. Therefore, Lewis acids and bases have a broader definition and can include substances that do not necessarily involve protons.
| 3. Can you give examples of Lewis acids and bases? | |
Ans. Yes, examples of Lewis acids include metal cations such as aluminum(III) ion (Al3+), boron trifluoride (BF3), and hydrogen ion (H+). Examples of Lewis bases include ammonia (NH3), water (H2O), and hydroxide ion (OH-). It is important to note that a substance can act as a Lewis acid in one reaction and as a Lewis base in another, depending on the context.
| 4. What are some applications of Lewis acids and bases? | |
Ans. Lewis acids and bases have numerous applications in various fields of chemistry. In organic synthesis, Lewis acids are often used as catalysts to facilitate reactions that involve the formation of new chemical bonds. For example, boron trifluoride (BF3) can be used as a Lewis acid catalyst in the Friedel-Crafts reaction. In coordination chemistry, Lewis acids are essential for the formation of coordination compounds and complexes. Additionally, Lewis acids and bases play a crucial role in the design and development of new materials, such as metal-organic frameworks and catalysts.
| 5. How are Lewis acids and bases involved in Lewis acid-base reactions? | |
Ans. In a Lewis acid-base reaction, a Lewis acid accepts a pair of electrons from a Lewis base, forming a coordinate bond. The Lewis acid is referred to as the electron-pair acceptor, while the Lewis base is the electron-pair donor. This coordination bond allows the two substances to interact and undergo chemical reactions. The concept of Lewis acid-base reactions is particularly useful in understanding the behavior of metal ions and their interactions with ligands in coordination compounds.
Text Transcript from Video
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
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
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Nov 15, 2024 Last updated |
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