Given below are two statements :
Statement I: The first ionization enthalpy of Cr is lower than that of Mn .
Statement II: The second and third ionization enthalpies of Cr are higher than those of Mn .
In the light of the above statements, choose the correct answer from the options given below:
Text Solution
Verified by ExpertsD
Statement I:
The electronic configuration of 
is 
and 
is 
.
For 
, the first electron is removed from 
, while for 
, it is removed from a stable fully filled 
subshell. Additionally, 
has a higher nuclear charge.
Thus, the first ionization enthalpy ( 
) of 
is lower than that of 
.
Statement I is true.
Statement II:
For the second ionization enthalpy ( 
), 
has configuration 
(stable half-filled) and 
has 
.
Removing an electron from the stable 
configuration of 
requires more energy than removing it from the 
of 
.
Thus, 
of 
is higher than 
.
For the third ionization enthalpy 
is 
and 
is 
.
Removing an electron from the stable half-filled 
configuration of 
requires significantly more energy than from the 
of 
.
Thus, 
of 
is higher than 
.
Since 
of 
is lower than 
, Statement II is false.
Prepare Smarter with CGP Edu
Get practice questions, solutions, and test series in one place.
Write a Review
Share your experience with this question and solution.
Commentary
Send your comment, doubt, correction, or feedback to admin.
Similar Questions
Explore conceptually related problems