Compare IE1 ,IE2,IE3 of Cr and Mn
Answers
The value is second IE generally increases towards the right in period, however Cr
+
has 3d
5
configuration which is extra-stable.
Hence 2
nd
IE of Cr is more than that of Mn. Thus correct order of 2
nd
IE is Cr>Mn>V>Ti
Answer:
IE1 and IE3 of Mn are greater than Cr and IE2 of Cr is greater than Mn.
Explanation:
The first ionisation enthalpy is the energy required to remove the most loosely bound electron.
Similarly, the energy required to remove the second electron from the positive ion is called second ionisation energy and so on.
On moving from left to right along a period, there is an increase in ionisation energy. The first ionisation energy of Mn is greater than Cr.
Cr has greater second ionisation energy than Mn. This is because Cr⁺ has a stable half-filled configuration.
The stable configuration of the Mn²⁺ ion makes the third ionisation energy of Mn greater than that of Cr.
#SPJ3