Question #fbdfe

1 Answer
Stefan V.
Dec 29, 2014

The difference in ionization energy between #B# and #Be# can be explained by detailing their respective electron configurations:

#Be#: #1s^(2)2s^2#
#B#: #1s^(2)2s^(2)2p^(1)#

Notice that #Be# has a stable electron configuration, which means that more energy is required to remove an electron from it. On the other hand, #B#'s ionization energy is smaller because of the electron present in its p-orbital.

Since p-orbitals are higher in energy than s-orbital, therefore less stable, it is easier for an electron to be removed from a p-orbital. Electrons located in p-orbitals are further away from the nucleus, which means that they can withstand its effective nuclear charge better #<=># more easy to remove from the atom.

Losing an electron from its outermost shell will make #B# more stable, since it will be lower in energy.

Related questions
See all questions in Periodic Trends in Ionization Energy
Impact of this question
10120 views around the world
You can reuse this answer
Creative Commons License