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Out of Be AND B, WHICH HAS MORE IONIZATION ENTHHALPY AND WHY ?

Asked by निकोदिमुस 4th October 2017, 6:07 PM
Answered by Expert
Answer:
Be has more ionisation enthalpy B. 
Because,
Beryllium's configuration is 1s2, 2s2  and Boron's is Boron (1s2, 2s2, 2p1) 
 
Be has stable configuration as the orbitals are completely filled up whereas for boron's electronic configuration isn’t  stable.

Ionisation enthalpy means energy required to loose/take out electrons. It is higher for Be because it is more stable and has more nuclear charge due to which electrons are closely and strongly attached than in Boron that is more energy will be required to pull out electrons from Be, so its ionisation energy is more.

Answered by Expert 5th October 2017, 10:50 AM
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