Oxygen and sulfur are in the same group in the periodic table. Sulfur is in the row below oxygen. The bond energy of an O=O bond is

Question

494 kJ/mol. Which statement about the bond energy of the S=S bond is most reasonable? (1 point)
The bond energy of S=S is less than 494 kJ/mol because the atoms are closer together than
the oxygen atoms.
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 sulfur has more electron shells than
oxygen.
The bond energy of S=S is greater than 494 kJ/mol because the atoms are closer together
than the oxygen atoms.

Answer 1

The most reasonable statement regarding the bond energy of the S=S bond, compared to the O=O bond energy of 494 kJ/mol, is:

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

This statement makes sense because as you move down a group in the periodic table, the atoms have more electron shells, which increases electron-electron repulsion and can lead to weaker bonds. The S=S bond has a lower bond energy than the O=O bond primarily due to the larger atomic size and increased shielding effect in sulfur, which typically results in weaker bonding interactions compared to the smaller oxygen atoms.