Question

H2S is less acidic than H2Te. why?

Answer 1

because Te is present at 5th period while S ispresent at 3rd period while going down the group the bond dissociation enthalpy decreased so therfore acidic character increases.
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Answer 2

In the case of $H_{2} Te$, removing a hydrogen ion from the molecule is simple, resulting in more acidity, but in the case of $H_{2} S$, bond dissociation is less, resulting in lesser acidity.

Acidic character in the periodic table

• The ability or inclination to lose a proton is referred to as an acidic character.
• We know that the atomic size of the elements diminishes as we travel from left to right in a period.
• As a result of the smaller size, the electronegativity of an element, or its capacity to give electrons, rises.
• As we all know, electronegativity is an element's ability to attract electron pairs.
• As a result, because the electronegativity lowers down the group, the acidic character of the oxides "decreases down the group."
• Similarly, more electropositive metals have more basic oxide in their natural state.
• Because the bond strength reduces as the group progresses, the acidic strength increases.

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