Which of the following halides are least stable and whose existence is suspicious Options are 1-Cl4 2-GeI4 3-Snl4 4-Pbl4 Correct answer is Pbl4 .can you plz explain the reason .?

Question

Answer

As we go down the group stability of halides will decrease due to increase in size of halogen atom hence it easily dissociate from the compound
Lead iodide is least stable among the halides.

Answer

Deu to inert pair effects we know that oxidation state becomes decreases down the group , thus Pb can not show +4 oxidation state , it shows +2 oxidation state . So it can not form PbI4.

Answer

Due to inert pair effect

Answer

Introduction:
Among the given halides (Cl4, GeI4, Snl4, Pbl4), Pbl4 is the least stable and its existence is suspicious. This can be explained by considering the electronic configurations and size of the elements involved.

Explanation:
1. Electronic Configuration:
The stability of a compound is influenced by the electronic configuration of the central atom. In the case of Pbl4, lead (Pb) belongs to the 6th period of the periodic table and has the electronic configuration [Xe] 4f14 5d10 6s2 6p2. The valence shell of Pb has two electrons in the 6s orbital and two electrons in the 6p orbital.

2. Size of the Central Atom:
The size of the central atom also plays a crucial role in determining the stability of a compound. In this case, lead (Pb) is a larger atom compared to chlorine (Cl), germanium (Ge), and tin (Sn). The larger size of Pb makes it difficult to accommodate four chlorine atoms around it due to increased repulsion between the negatively charged electrons.

3. Lone Pair Repulsion:
In Pbl4, the lead atom tries to accommodate four chlorine atoms around it. However, the presence of lone pairs on the lead atom creates significant repulsion between the lone pair electrons and the chlorine atoms. This repulsion destabilizes the compound, making it less stable.

4. Oxidation State of Lead:
Lead has a maximum oxidation state of +4. In order to form Pbl4, lead needs to have a +4 oxidation state. However, the electronegativity of chlorine is higher than that of lead, making it difficult for lead to maintain a +4 oxidation state in the presence of four chlorine atoms. This further contributes to the instability of Pbl4.

Conclusion:
Based on the electronic configuration, size of the central atom, lone pair repulsion, and oxidation state considerations, Pbl4 is the least stable and its existence is suspicious. The inability of lead to accommodate four chlorine atoms and maintain a +4 oxidation state, along with the repulsion between lone pairs and chlorine atoms, leads to the instability of Pbl4.

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