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

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Explanation:

Using Slater's rule;

the shielding experienced by an electron in an s- or p- orbital such as in Boron or oxygen is calculated based on the the fact that; electrons within same group shield 0.35, except the 1s which shield 0.30

Hence, for oxygen;

1s2 2s2 2p4

Zeff = (2× 0.3) + (5 × 0.35) = 2.35

For Boron

1s2 2s2 2p1

Zeff= (2 ×0.3) + {2 × 0.35) = 1.3

Hence the effective nuclear charge on a valence electron in boron is less than the effective nuclear charge on a valence electron in oxygen. Hence boron is larger than oxygen.