Question

answer the following questions
1) discuss the variation of oxidation state in the group 14 elements.
2) why SiO2 does dissolve in water.​

Answer 1

Answer:

The element of group 14 has 4 valence electrons. Therefore, the oxidation state of the group is +4. However, as a result of the inert pair effect, the lower oxidation state becomes more stable and the higher oxidation state becomes less stable. Therefore, this group exhibits +4 and +2 oxidation states.

Silicon dioxide does not consist of separate molecules that can dissolve individually into water. The SiO units are covalently bound in the solid. They are too strongly connected for water to be able to break them apart.

Answer 2

1st answer

• The common oxidation states exhibited by group-14 elements are +4 and +2.
• Carbon exhibits negative oxidation states.
• Heavier elements exhibits +2 oxidation state.
• The tendency to show +2 oxidation state increases in the order Ge < Sn < pb.
• pb exhibits +2 oxidation state as stable state because of inert pair effect.

2nd answer

• Silica is a non reactive compound in its normal state.
• In silica each silicon atom is convalently bonded in a tetrahedral manner to four oxygen atoms.
• This non reactivity is due to very high Si - O bond enthalpy.
• Silica is a giant molecule with 3 - dimensional structure.
• Thus, it is insoluble in water.

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