Question

Kindly explain:
Thr correct order of 2nd ionization enthalpy is

Answer 1

Be have low ionisation enthalpy because it belong 2nd group and 2?nd period and the cell size is large and nuclear force is small on outermost cell of electron so electron on outermost cell easily released so ionisation potential is low .The size of cell Decrease from left to right in period except inert gas .so ionisation potential also decreases from left to right .

so

N>C>B>Be is right one

Answer 2

Answer:

Explanation:

among  nitrogen boron carbon and beryllium if we observe they belong to same period so along a period there will be no gradual increase or decrease of ionization energies so if we observe this order

if we take the electronic configurations of these elements

Be - 1s2 2s2       / I.P 2  1S2 2S1

B - 1s2 2s2 2p1   /I.P 2   1S2 2S2

C - 1s2 2s2 2p2  /I.P 2   1S2 2S2 2P1

N - 1s2 2s2 2p3   /I.P 2  1S2 2S2 2P2

IF WE OBSERVE nitrogen requires more energy because 2 electrons are present in p orbital and next boron requires energy because it is completely filled orbital and is more stable and carbon has 1 electron in its p orbital and next it is easier to remove electron from beryllium as it has only one electron and in s orbital

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