Question

Explain the variation in ionization energy across the elements of period 2 in the periodic
table

Answer 1

In general, ionization energy increases along the period due to increase in nuclear charge...... But there are many other factors which affect the ionization energy .

For eg. In 2nd period the 1st ionization energy of beryllium is more than boron because of the electonic configuration..., Be 1s2 2s2 and B 1s2 2s2 2p1 since we can see that Be has full filled electronic configuration so it is more stable and thus the ionization energy of beryllium is more than boron

Answer 2

Explanation:

• The “amount of energy” required to removal of an electron from a gaseous atom which is isolated, is called “ionization energy”.

• As we move from ‘left to right’ over the second period, the first ionization power generally rises.
• If we can observe the following graph it have two drops one is Be $\left(1 s^{2} 2 s^{2}\right) to B \left(1 s^{2} 2 s^{2} 2 p^{1}\right)$ because screening effect of the p electrons and another one is  $N \left(1 \mathrm{s}^{2} 2 \mathrm{s}^{2} 2 \mathrm{p}^{3}\right) to O \left(1 s^{2} 2 s^{2} 2 p^{4}\right),$ due to the increases distance form outermost electrons to nucleus.

The Graph attachment is attached below: