Responses
Sulfur (S) has a larger atomic size than oxygen (O), so H2S is a more stable, weaker base than H2O.
Sulfur (S) has a larger atomic size than oxygen (O), so H 2 S is a more stable, weaker base than H 2 O.
Sulfur (S) has a larger atomic size than oxygen (O), so HS– is a more stable, stronger acid than OH–.
Sulfur (S) has a larger atomic size than oxygen (O), so HS – is a more stable, stronger acid than OH – .
Sulfur (S) has a larger atomic size than oxygen (O), so H2S is a more stable, stronger acid than H2O.
Sulfur (S) has a larger atomic size than oxygen (O), so H 2 S is a more stable, stronger acid than H 2 O.
Sulfur (S) has a larger atomic size than oxygen (O), so HS– is a more stable, weaker base than OH–.
1 answer
The correct statement is:
Sulfur (S) has a larger atomic size than oxygen (O), so HS⁻ is a more stable, stronger acid than OH⁻.
This is because the larger atomic size of sulfur relative to oxygen means that the H–S bond is weaker than the H–O bond. Therefore, it is easier for H₂S to donate a proton (H⁺) compared to water, making H₂S a stronger acid. Additionally, the anion HS⁻ is more stable than OH⁻, contributing to the stronger acidic character of H₂S compared to water.
