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Assertion: The first ionisation energy o...

Assertion: The first ionisation energy of `Be` is greater than that of `B`.
Reason: 2p-orbital is lower in energy than 2s-orbital.

A

Statement-I is true, Statement-II is true ,Statement -II is the correct explanation for Statement-I

B

Statement-I is true ,Statement -II is true, Statement -II is not the correct explanation for statement -II

C

Statement-I is true. Statement -II is false.

D

Statement-I is false. Statement -II is true.

Text Solution

Verified by Experts

The correct Answer is:
C
Statement II is incorrect. The first ionisation energy of Be is greater than that of B because of its relatively stable electronic configuration.
`Be=2s^(2), B=2s^(2) 2p^(2)`
It is easier to remove electron from `2p` orbitals than `2s` orbitals since `2s` is much more penetrated towards nucleus.
Hence `IE_(1)` of `Be gt IE_(1)` of B.
Therefore, `2p`-orbital has rather higher energy than `2s`.
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