Question

A)
Oxygen and sulfur are in the same group in the periodic table. Sulfur is in the row below oxygen. Thebond energy of an O=O bond is 494 kJ/mol. Which statement about the bond energy of the S=S bond ismost reasonable?
(1 point)
The bond energy of S=S is greater than 494 kJ/mol because the atoms are closer together than the oxygenatoms.
The bond energy of S=S is greater than 494 kJ/mol because sulfur has more electron shells than oxygen.
The bond energy of S=S is less than 494 kJ/mol because the atoms are closer together than the oxygenatoms.
The bond energy of S=S is less than 494 kJ/mol because sulfur has more electron shells than oxygen

Answer 1

"The bond energy of S=S is less than 494 kJ/mol because sulfur has more electron shells than oxygen."

Reason: sulfur atoms are larger with more electron shells, so their valence orbitals are more diffuse and overlap less effectively than oxygen's, giving a longer, weaker S=S bond.