Which statement correctly explains why H2S is a stronger acid than water?(1 point)
Responses
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 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 HS– is a more stable, weaker base than OH–.
Sulfur (S) has a larger atomic size than oxygen (O), so H2S is a more stable, stronger acid than H2O.
You know that water can act as an acid to form OH−. H2S is also an acid that can lose an H+ to form the conjugate base HS−. To determine which is the stronger acid, you need to look at the strength of the conjugate bases. Sulfur (S) and oxygen (O) are in the same group, but sulfur has a larger atomic size. Therefore, HS− is a more stable, weaker base than OH−. Since strong acids form weaker conjugate bases, H2S is a stronger acid than water.
Sulfur (S) has a larger atomic size than oxygen (O), so HS− is a more stable, weaker base than OH−.
To determine why H2S is a stronger acid than water, we need to compare the properties of sulfur (S) and oxygen (O). The statement that correctly explains this is: "Sulfur (S) has a larger atomic size than oxygen (O), so H2S is a more stable, stronger acid than H2O."
Explanation: In general, acid strength is determined by the stability of the conjugate base. A stronger acid has a more stable conjugate base. In this case, comparing H2S (hydrogen sulfide) with H2O (water), the difference lies in the central atom - sulfur versus oxygen.
Sulfur is located below oxygen in the periodic table, and it has a larger atomic size. Since sulfur has more electron shells, the electrons around the sulfur atom are further away from the nucleus compared to oxygen. As a result, the electron density in the sulfur is more spread out, making it easier to release an H+ ion (proton). This greater ability to donate a proton makes H2S a stronger acid than H2O.
Therefore, the correct statement is: "Sulfur (S) has a larger atomic size than oxygen (O), so H2S is a more stable, stronger acid than H2O."