H2S is better reducing agent than water or H2S is thermally less stable than H2O. Explain.
On going down the group, the size of the central atom increases, and therefore, its tendency to form a stable covalent bond with hydrogen decreases. As a result, the M-H bond strength decreases, and therefore, thermal stability decreases.
All the hydrides except water are reducing agents. The reducing power of these hydrides increases from H2O to H2Te.
This is due to the decrease in the thermal stability of the hydrides. Greater the instability of hydride, the greater is its reducing character.
This behavior could be explained on the basis of the electronegativity of the central atom. As we move from O to S in the group VI of the periodic table, the atomic size increases gradually and thus the length of the H−X bond increases as we move down the group. consequently, hydrides dissociate to releaseH+ increases as we go from H2O to H2S. Thus, H2S is reducing agent.
On going down the group, the size of the central atom increases, and therefore, its tendency to form a stable covalent bond with hydrogen decreases. As a result, the M-H bond strength decreases, and therefore, thermal stability decreases.
All the hydrides except water are reducing agents. The reducing power of these hydrides increases from H2O to H2Te.
This is due to the decrease in the thermal stability of the hydrides. Greater the instability of hydride, the greater is its reducing character.
This behavior could be explained on the basis of the electronegativity of the central atom. As we move from O to S in the group VI of the periodic table, the atomic size increases gradually and thus the length of the H−X bond increases as we move down the group. consequently, hydrides dissociate to releaseH+ increases as we go from H2O to H2S. Thus, H2S is reducing agent.
