Assuming sulfur has an electron configuration of 1s2,2s2,2p6,3s2,3p3 and a Zeff

Question

Assuming sulfur has an electron configuration of 1s2,2s2,2p6,3s2,3p3 and a Zeff of 5, and phosphorus has an electron configuration of 1s2,2s2,2p6,3s2,3p4 and a Zeff of 6; which atom would you predict to have a larger atomic radius based on their electron configuration and Zeff? Assuming sulfur has an electron configuration of 1s2,2s2,2p6,3s2,3p3 and a Zeff of 5, and phosphorus has an electron configuration of 1s2,2s2,2p6,3s2,3p4 and a Zeff of 6; which atom would you predict to have a larger atomic radius based on their electron configuration and Zeff?

Explanation / Answer

Assuming sulfur has an electron configuration of 1s2,2s2,2p6,3s2,3p3 and a Zeff of 5, and phosphorus has an electron configuration of 1s2,2s2,2p6,3s2,3p4 and a Zeff of 6;

Sulfur will have more atomic radius, because with that electronic configuration the total no of protons for sulfur= 15 and that of phosphorus=16. Thus, as both have no of shells equal, higher proton of phosphorus will hold electrons more tight to nucleus, hence will have lesser atomic radius.

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