Question

explain the property of hydrides of group 16 elements H2O H2S H2S ch2 Te boiling point thermal stability reducing power acidic nature​

Answer 1

Answer:

Explanation:

The thermal stability of the hydrides of group 16 elements decreases down the group, i.e., H2O > H2S > H2Se > H2Te > H2Po. This is because M-H bond dissociation energy decreases down the group with the increase in the size of central atom.

Answer 2

Properties of Hydrides of group 16

Explanation:

The group 16 members with general electronic configuration are :

General configuration  : ns² np⁴

Oxygen (O)          

Sulphur (S)        

Selenium (Se)    

Tellurium(Te)      

Polonium (Po)      

Their hydrides are :

When group 16 elements combine with hydrogen they form hydrides with general formula H₂E that is :

H₂O

H₂S

H₂Se

H₂Te

All of them have bent geometry with sp3 hybridization

Boiling point

The boiling point depends upon Vander wall force and this Vander wall force increases with increase in size .

The order of their boiling points for 15 group hydrides is :

 H₂O >H₂S<H₂Se<H₂Te

In case of H₂O and H₂S, water has higher boiling point than hydrogen sulphide because of hydrogen bonding .

 Thermal Stability

The stability of hydrides depends upon the comparability of size . The order of stability of hydrides is :

   H₂O >H₂S>H₂Se>H₂Te

Due to increase in size, bond length increase due to which bond dissociation energy decrease therefore stability decrease. .

Reducing nature

The order of reducing character of hydrides are :

 H₂O <H₂S<H₂Se<H₂Te

Out of them in case of  H₂Te the bond strength is low therefore reducing character is highest  .

Acidic nature

The order of acidic nature  of hydrides are :

 H₂O <H₂S<H₂Se<H₂Te

Out of them in case of  H₂Te the bond strength is low therefore it can easily release hydrogen ion therefore acidic  character is highest  .