Question

The shielding of electrons gives rise to an effective nuclear charge, Zeff, which explains why boron is larger than oxygen. Estimate the approximate Zeff felt by a valence electron of boron and oxygen, respectively? View Available Hint(s) The shielding of electrons gives rise to an effective nuclear charge, , which explains why boron is larger than oxygen. Estimate the approximate felt by a valence electron of boron and oxygen, respectively? +5 and +8 +3 and +6 +5 and +6 +3 and +8 +1 and +4

Answer 1

Zeff = Z - S

Here, Z is the number of protons in the nucleus, that is, atomic number, and S is the number of nonvalence electrons.

For boron, the electronic configuration is 1s₂ 2s₂ 2p₄

Z = 5, S = 2

Zeff = 5-2 = +3

For O, electronic configuration is 1s₂ 2s₂ 2p₄

Z = 8, S = 2

Zeff = 8-2 = +6

Hence, the correct answer is second option, that is, +3 and +6, the Zeff of boron is smaller in comparison to O, thus, boron exhibits a bigger size than O.