Question

10. Arrange the following in increasing order of the property indicated :

(a) SiCl2, GeCl2, SnCl2 and PbCl2 (stability)

(b) CO, SiO, SnO, GeO, PbO (basicity)

(c) SiF4, SiCl4, SiI4, SiBr4 (stability)

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Answer 1

(a) SiCl2 < GeCl2 < SnCl2 < PbCl2

(b) CO > SiO > SnO > GeO > PbO

(c) SiF4 > SiCl4 > SiI4 > SiBr4

Answer 2

Answer:

(A) SiCl₂<GeCl₂<SnCl₂<PbCl₂

(B)CO < SiO < GeO < SnO < PbO

(C)SiI₄ < SiBr₄ < SiCl₄ < SiF₄

Explanation:

The given elements are of group 14 of the periodic table.

(A)

$SiCl_2 < GeCl_2 < SnCl_2 < PbCl_2$

In heavier elements the tendency to show +2 oxidation state increases. It is due to the inability of the ns² valence shell to participate in bonding.

(B)

$CO < SiO < GeO < SnO < PbO$

The basicity of the oxides increases down the group as the metallic character increases down the group.

(C)

$SiI_4 < SiBr_4 < SiCl_4 < SiF_4$

As the smaller ions stabilize with the smaller atom.