Question

Explain the reactivity of hydrides, oxides, and halides of 16th group elements.​

Answer 1

Answer:

Electronic Configuration of Group 16 Elements

Group 16 elements have 6 electrons in their valence shell and their general electronic configuration is ns2np4.

Element

Electronic Configuration

Oxygen [He] 2s2 2p4

Sulphur [Ne] 3s2 3p4

Selenium [Ar] 3d10 4s2 4p4

Tellurium [Kr] 4d10 5s2 5p4

Polonium [Xe] 4f14 5d10 6s2 6p4

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Answer 2

Hi,

Here is your answer

Reactivity with hydrogen:

• Elements of group 16 react with hydrogen to form hydrides(H2E)where E=O,S,Se,Te,Po
• Their acidic character increases from H2O to H2Te
• The thermal stability of hydrides decrease down the group
• All the hydrides except H2O possess reducing property and this character decreases down the group.

Reactivity with oxygen:

• Elements of group 16 react with oxygen to form oxides of the type EO2 and EO3 where both types of oxides are acidic.
• The reducing property of dioxide decreases down the group.

Reactivity towards halogens:

• Elements of group 16 reacts with halogens to form halides of the form EX6, EX4 and EX2 where X is a halogen.
• The stability of halides decrease in the order F->Cl->Br->I-
• All elements except oxygen form dichlorides annd dibromides which has sp³hybridisation and tetrahedral structure.

Notes:

1. Increase in the acidic character is due to decrease in bond enthalpy for the dissociation of H-E bond down the group.

2. SO2 is a reducing agent while TeO2 is an oxidising agent.

3. Amongst hexahalides, hexafluorides are the only stable halides and they have octahedral structure.

Hope this helps you.