Why is the first ionization energy of boron lower than beryllium?

Answer 1

The rise in ionisation energy is not regular. To explain this we must remember that the second shell of electrons is actually subdivided into 2s and 2p. The most easily removed electron in Boron is that in the 2p orbital, higher in energy than the 2s electrons in Beryllium. It therefore needs less energy for total removal than does the 2s electron of Boron. This outweighs the effect of the increased nuclear charge of Boron, which tends to make its outer electron harder to remove.

Answer 2

1. Because in boron the outer electron is in the 2p shell therefore it is further away from the nucleus as compared to the outer electron of beryllium ,which is in 2s.

2. Also because the 2s shell electrons of boron shield the electrons of the 2p shell.

Hope this helps!!!!!!!!!!!!!!!!! :)

Answer 3

The p orbital is slightly higher in energy than the s orbital. That why, it's easier to remove the 2p1 elecrtron from B, therefore the 1st ionisation energy in B will be lower

Answer 4

yes does because the ionization level decreases as it goes across in each period level.