Trends in Ionization Enthalpy of Transition Elements Video Lecture | Chemistry for JEE Main & Advanced

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now we'll talk about the trends in the
ionization enthalpy what is I nation
helping ionization helping nothing but
the minimum energy required to remove
one electron to infinite distance from
the atom all nucleus in the gaseous
state so you have something in the
gaseous state please note it has to be
in the gaseous state and from there you
make it Fe plus and vector minus so if
you say Fe solid from there if you are
making Fe plus electro - this is not my
an agenda this is ionized enthalpy
actually from every solid you have to
apply some heat to make it Fe gas and
then from the gas you can actually pull
out from the top so this part is ionized
enthalpy ie
in this part is atomization okay should
we talk about MF ionization energy it
refers to the minimum amount of energy
required to remove electron from the
species which already has n minus 1
charge for example if you talk about
second ie then from this Fe you make Fe
2 plus this is second I second energy
and this is first I a message talk about
third reaction energy from this you take
one electron out and you make Fe 3 plus
so this will be third ionization energy
okay and typically ionization energy
increased from left to right if you see
the ionization energy is increasing from
left to right little bit decrease but
overall is increasing but there is some
variation you can see example from here
later copper has lower value zinc has
higher value the answer lies in the
electronic configuration if you see
chromia
also has low value only let's talk about
the copper copper is 3d10 for s1 it lose
my electron energy come 3d10 this is
more stable
little stable talk about zinc zinc has a
higher value of minus energy
zinc electronic configuration was my
argon and then 3d10 for s2 this is
already stable if it lose one electron
at this accounts 3d10 for s1 buzzer
electron will be lost from the S orbital
not this is not that say well this is
more stable so zinc will not like to
lose electron so it will have a higher
value of ionization okay if you talk
about the chromium also the value is
little less only why if you talk about
chromium the electronic contingent is
argon and then 3d5
for this one now if you see if you lose
one electron this becomes 3 D 5 this is
more stable and those it has lower value
of ionization al but if you see the
second ionization in 30 or from is very
high C is very high compared to this
values the very high by because the
second ionization thought me I am
talking about this guy now now removing
one electron from this you get
argon 3d for this is not very stable
this is at least has some stability
because of efendi orbital so this value
is very high okay
similarly for zinc I mean this all
actually you know you can for even thing
ever reason you understand these stuffs
you see that the electronic
configuration will actually tell you why
the values are less and by the values
are let's talk about the trend in the
ionization enthalpy see ionized enthalpy
actually typically depends on that of
excites so it is inversely proportional
to atomic size smaller is the size
higher is the I enthalpy because smaller
is the size it is difficult
to pluck electron but actually this is
not the atomic size which actually
governs ionization energy ionization
energy is actually governed by effective
nuclear charge it so higher is the
effective nuclear charge more is the
ionization energy that means if the
effective nuclear charge on this
electron is more it is held by this
nucleus more and more energy will be
required to pull this electron if you
see here chromium and manganese these
two have same atomic radius but actually
if you see there is a difference in
their financial enthalpy so we can say
that ionization in help it does not
depend only on the size the main driving
force for the ionization enthalpy is the
effective nuclear charge higher is the
effective nuclear charge on the electron
more difficult it is to plug that
electron out and higher is ionization in
that way thank you
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