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Which of the following oxidation states are the most characteristic for lead and tin respectively?
- a)+ 2, + 4
- b)+ 4, + 4 [2007]
- c)+ 2, + 2
- d)+ 4, + 2
Correct answer is option 'A'. Can you explain this answer?
Verified Answer
Which of the following oxidation states are the most characteristic fo...
All the group IV elements show tetravalency which can be explained on the basis of shifting of one e– of ns to the vacant np orbital.These four orbitals give rise to four sp3 hybrid orbitals.
When ns2 electrons of the outermost shell do not participate in bonding it is called inert pair and the effect is called inert pair effect. The last three elements of group 4 i.e. Ge, Sn and Pb, have a tendency to form divalent as well as tetravalent ions. Since the inert pair effect increases from Ge to Pb, the stability of tetravalent ion decreases and that of divalent ion increases that is why Pb++ is more stable than Pb4+ and Sn4+ ions is more stable than Sn2+.
When ns2 electrons of the outermost shell do not participate in bonding it is called inert pair and the effect is called inert pair effect. The last three elements of group 4 i.e. Ge, Sn and Pb, have a tendency to form divalent as well as tetravalent ions. Since the inert pair effect increases from Ge to Pb, the stability of tetravalent ion decreases and that of divalent ion increases that is why Pb++ is more stable than Pb4+ and Sn4+ ions is more stable than Sn2+.
Most Upvoted Answer
Which of the following oxidation states are the most characteristic fo...
The oxidation states of lead and tin can vary depending on the compound they are present in. However, there are certain oxidation states that are more characteristic for these elements.
Lead:
- The most characteristic oxidation state for lead is +2. This means that lead can lose two electrons to form a 2+ cation. This oxidation state is commonly observed in lead compounds such as lead(II) oxide (PbO), lead(II) chloride (PbCl2), and lead(II) nitrate (Pb(NO3)2).
Tin:
- The most characteristic oxidation state for tin is +4. This means that tin can lose four electrons to form a 4+ cation. This oxidation state is commonly observed in tin compounds such as tin(IV) oxide (SnO2), tin(IV) chloride (SnCl4), and tin(IV) sulfate (Sn(SO4)2).
Explanation:
- The oxidation state of an element refers to the charge that element would have if all its bonds were ionic. It is a measure of the electron gain or loss of an atom in a compound.
- In the case of lead, it has a tendency to lose two electrons to achieve a stable configuration. This results in its most characteristic oxidation state of +2.
- Similarly, tin has a tendency to lose four electrons to achieve a stable configuration. This results in its most characteristic oxidation state of +4.
- It is important to note that lead and tin can also exhibit other oxidation states depending on the compound they are present in. For example, lead can also exist in the +4 oxidation state in compounds such as lead(IV) oxide (PbO2), while tin can also exist in the +2 oxidation state in compounds such as tin(II) chloride (SnCl2).
- However, the most characteristic oxidation states for lead and tin respectively are +2 and +4.
- Therefore, the correct answer is option A, which states that the most characteristic oxidation states for lead and tin are 2 and 4 respectively.
Lead:
- The most characteristic oxidation state for lead is +2. This means that lead can lose two electrons to form a 2+ cation. This oxidation state is commonly observed in lead compounds such as lead(II) oxide (PbO), lead(II) chloride (PbCl2), and lead(II) nitrate (Pb(NO3)2).
Tin:
- The most characteristic oxidation state for tin is +4. This means that tin can lose four electrons to form a 4+ cation. This oxidation state is commonly observed in tin compounds such as tin(IV) oxide (SnO2), tin(IV) chloride (SnCl4), and tin(IV) sulfate (Sn(SO4)2).
Explanation:
- The oxidation state of an element refers to the charge that element would have if all its bonds were ionic. It is a measure of the electron gain or loss of an atom in a compound.
- In the case of lead, it has a tendency to lose two electrons to achieve a stable configuration. This results in its most characteristic oxidation state of +2.
- Similarly, tin has a tendency to lose four electrons to achieve a stable configuration. This results in its most characteristic oxidation state of +4.
- It is important to note that lead and tin can also exhibit other oxidation states depending on the compound they are present in. For example, lead can also exist in the +4 oxidation state in compounds such as lead(IV) oxide (PbO2), while tin can also exist in the +2 oxidation state in compounds such as tin(II) chloride (SnCl2).
- However, the most characteristic oxidation states for lead and tin respectively are +2 and +4.
- Therefore, the correct answer is option A, which states that the most characteristic oxidation states for lead and tin are 2 and 4 respectively.
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Which of the following oxidation states are the most characteristic for lead and tin respectively?a)+ 2, + 4b)+ 4, + 4 [2007]c)+ 2, + 2d)+ 4, + 2Correct answer is option 'A'. Can you explain this answer? for Class 12 2025 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about Which of the following oxidation states are the most characteristic for lead and tin respectively?a)+ 2, + 4b)+ 4, + 4 [2007]c)+ 2, + 2d)+ 4, + 2Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for Class 12 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Which of the following oxidation states are the most characteristic for lead and tin respectively?a)+ 2, + 4b)+ 4, + 4 [2007]c)+ 2, + 2d)+ 4, + 2Correct answer is option 'A'. Can you explain this answer?.
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