Question #fbdfe

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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.

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