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H(2)S is less acidic than H(2)Te. Why?...

`H_(2)S `is less acidic than `H_(2)Te`. Why?

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Due to extra stable half-filled p orbitals of group-15 larger amount of energy is required to remove electron as compared to group 16.
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(a) Elements of group 16 generally show lower value of first ionisation enthalpy as compared to the corresponding periods of group 15 . Why ? (b) H_2 S is less than acidic than H_2 Te . Why ?

(a) Elements of group 16 generally show lower value of first ionisation enthalpy as compared to the corresponding periods of group 15 . Why ? (b) H_2 S is less than acidic than H_2 Te . Why ?

Why is H_(2)S less acidic than H_(2)Te ?

Why is H_(2)S less acidic than H_(2)Te ?

(a) Write the balanced chemical equations for obtaining XeO_(3) " and " XeOF_(4) "from "XeF_(6). (b) Account for the followingk : (i) H_(2)S is less acidic then H_(2) Te. (ii) H_(3)PO_(2) has reducing nature. (iii) SO_(2) is an air pollutant.

Assertion : H_(2)Se is less acidic than H_(2)S. Reason : S is less electronegative than Se.

State true or Fasle: H_(2)S is acidic than H_(2)O .

Draw the structure of : {:((i)BrF_(3),(ii)XeOF_(4)):} (b) Explain giving reason in each case : (i) Why H_(2) Te is more acidic than H_(2)S ? (ii) Why are halogens strong oxidising agents ? (iii) Why does nitrogen show catenation tendentcy less than phosphorus ?

A : H_(3) PO_4 is less acidic than H_(3) PO_(3) . R : Oxidation state of phosphorus in H_(3) PO_(4) lt H_(3) PO_(3) .

H_2S is more acidic than H_2O . The reason is