Question

Que give reasons:
@ Plumpous compounels are more stable than plumbic
b)Steaaic aremore stable than stenace,
© Pbcl4 is a good enidizing agent.
d)Sncl2 is a good reducing agent.
​

Answer 1

ANSWER

Assertion: PbCl  

2

​  

 is more stable than PbCl  

4

​  

 

The inert pair effect is the tendency of the two electrons in the outermost atomic s orbital to remain unionized or unshared in compounds of post-transition metals., out of which (Pb) lead is one. The term inert pair effect is often used in relation to the increasing stability of oxidation states, that are two less than the group valency for the heavier elements of groups 13, 14, 15 and 16.

The s electrons are more tightly bound to the nucleus and therefore more difficult to ionize.

Due to inert pair effect, the higher oxidation state of an element is not stable as we move down the group.

In other words, Pb  

+4

 is less stable than Pb  

+2

, hence PbCl  

4

​  

 is also less stable.

Reason: PbCl  

4

​  

 is a powerful oxidizing agent.

As we go down in a group 14 elements of periodic table, we observe that +4 oxidation state decreases while that of +2 oxidation state increases due to inert pair effect. So, the outermost s-orbital electrons show reluctance to take part in the reaction. This leads to greater stability of +2 oxidation state in group 14 elements.

Instead of losing 4 electrons[2 electrons from S and 2 from P orbitals}, they tend to lose the p orbitals electrons, hence Pb  

+4

 can easily gain 2 electrons to form more stable Pb  

+2

 ions.

Pb(lead) show +2 oxidation state and easily gets reduced and therefore oxides others

Hence PbCl  

4

​  

 is the stronger oxidizing agent.

mark as brainly please

Answer 2

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Answer a)

In pbx2 , oxidation state of pb =+2 and pbx4 , oxidation state of pb =+4 we know ,oxidation state of +2 is more stable than +4 . due to inert pair effect . this is due to poor screening effect of d and f electrons that restrict ns electron to take part in the bond formation .so, PbX2 is more stable than PbX4

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Answer b) - Trans isomers are more stable. In trans isomers same group or atom on two different carbon atoms are located on the opposite sides of the carbon- carbon double bond and hence the trans molecule is non polar. The polarity on both the sides cancel out. And hence trans isomer is stable than cis isomer.

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Answer c) - Sn4+ is more stable than Sn2+. SnCl2 readily reacts with other compounds & get converted to stable SnCl4. During the reaction, SnCl2 gets oxidised while other compound is reduced. Thus, SnCl2 is a good reducing agent.

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