Why SnCl2 is more stable than SnCl4?

Why SnCl2 is more stable than SnCl4?

Sncl2 is more stable than sncl4. According, to the rule more charge has higher tendency to polarise the surrounding atom which tends to introduce a covalent character in molecule. sncl4 tends to have higher positive charge and its size is smaller. Hence, sncl4 is covelant and sncl2 is iocnic and stable.

Why SnCl4 is more stable than Pbcl4?

As we move down the group from C to Pb, the stability of +4 oxidation state decreases while that of +2 oxidation state increases due to the same inert pair effect. Therefore, for Pb +2 oxidation state becomes more stable than +4 oxidation state and vice-versa for Sn.

Why SnCl2 is less stable than pbcl2?

Since Pb is more down the group than Sn, it’s stable with +2 oxidation state where Sn can exhibit both +2&+4 but +4 is more stable due to which SnCl2 is a strong reducing agent.

Why Pbcl4 is less stable than SnCl4 but pbcl2 is more stable then SnCl2?

Pbcl4 is less stable than sncl4 but pbcl2 is more stable than sncl2 because pb has +4 oxidation state in pbcl4 while has +2 oxidation state in pbcl2. The +2 oxidation state of pb is much more stable than +4.

What is the difference between SnCl2 and SnCl4?

In SnCl2, Sn has +2 oxidation state. Whereas in SnCl4, Sn has +4 oxidation state. According to Fajan’s rule, the central metal with more oxidation number will be considered to be more covalent. Therefore, SnCl4 is more covalent than SnCl2.

Why SnCl2 is a strong reducing agent?

● SnCl2 acts as reducing agent because – -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.

Why is PbCl4 less stable?

Pb has electronic configuration [Xe] 4f14 5d10 6s2 6p2. Due to poor shielding of 6s2 electrons by inner d and f electrons, it is difficult to remove 6s2 electrons (inert pair). Thus, due to inert pair effect, the +2 oxidation state is more stable than +4 oxidation state. Hence, PbCl4 is less stable than PbCl2.

Which of the following compounds is the least stable a PbCl2 B SnCl2 C gecl2 D sicl2?

Due to inert pair effect +2 oxidation state of Pb is more stable than +4 . But in case of Sn it’s +4 oxidation state is more stable than +2 oxidation state. Thus, PbCl4 is less stable than SnCl4, while PbCl2 is more stable than SnCl2.

What is inert pair effect out of PbCl4 and SnCl4 which one shows higher oxidising nature?

Inert pair effect: Reluctance of outermost s-orbital electrons to take part in the reaction. Thus, lead show stable +2 oxidation state while tin shows stable +4 oxidation state. So PbCl4 tends to get reduced easily and therefore oxidise others. Hence, PbCl4 is stronger oxidising agent than SnCl4​.

Which one has higher melting point SnCl2 or SnCl4?

SnCl2 has high melting point (is solid) while SnCl4 has low melting point (is a liquid).

Which is the strongest reducing agent in electrochemical series?

At top end of electrochemical series there is lithium which is the strongest reducing agent and at the bottom end of electrochemical series there is fluorine which is the weakest reducing agent or the strongest oxidizing agent.

Is SnCl4 reducing agent?

SnCl 4 is a reducing agent, SnCl 4 is an oxidizing agent. ; Gray to almost silver-white, ductile, malleable, lustrous solid.

Why is the covalent nature of SnCl4 higher than SnCl2?

According to Fazan’s rule,smaller the size of an atom higher will be its polarising capacity. As we can see, in SnCl4 and SnCl2, the oxidation states of Sn are +4 and +2 respectively(this shows Sn in SnCl4 is smaller than Sn in SnCl2). That’s the reason behind the higher covalent nature of SnCl4. Happy reading ^_^.

Why is SnCl2 a good conductor of electricity in water?

SnCl2 is soluble in water and good conductor in aqueous solutions. This is because of ionic character of SnCl2, which produces ions in aqueous soution. Look the best way to understand this is that as we move down the group the stability of +2 oxidation state increases where as for +4 decreases due to inert pair effect.

Why is the ionic radius of Sn4+ smaller than SN2+?

As Sn4+ has less electrons, it’s electrons get more attracted by the protons so it’s ionic radius is smaller than Sn2+’s. According to fajan’s rule ,a small cation with high positive charge and a large anion react they share covalent bond because the anion bends towards the cation and ultimately they overlap.