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The melting point of lithium metal is 454 K, and that of sodium is 371 K. Which is the following statements can explain this difference in their melt ing points:
(I) Metallic bonding in lithium is stronger than metallic bonding in sodium.
(II) The delocalized electrons are more strongly attracted to the metal cation of lithium.
(III) The lithium cations have a greater charge density than sodium cation.
(IV) Li+ cations are smaller than Na+ cations.
(II) The delocalized electrons are more strongly attracted to the metal cation of lithium.
(III) The lithium cations have a greater charge density than sodium cation.
(IV) Li+ cations are smaller than Na+ cations.
- a)Only I and II
- b)Only II and III
- c)Only IV
- d)I, II, III, IV
Correct answer is option 'D'. Can you explain this answer?
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Most Upvoted Answer
The melting point of lithium metal is 454 K, and that of sodium is 371...
Explanation:
The difference in melting points between lithium and sodium can be explained by the following factors:
I. Strength of metallic bonding:
- Lithium cations have a higher charge density than sodium cations due to their smaller size.
- The smaller size results in a stronger attraction between the positively charged cation and negatively charged delocalized electrons, leading to stronger metallic bonding.
- Thus, metallic bonding in lithium is stronger than in sodium.
II. Attraction of delocalized electrons:
- Delocalized electrons are more strongly attracted to the smaller lithium cation than to the larger sodium cation due to the higher charge density.
- This results in a stronger metallic bond in lithium as compared to sodium.
III. Charge density of cations:
- Lithium cations have a higher charge density than sodium cations due to their smaller size.
- The higher charge density results in a stronger attraction between the cation and surrounding electrons, leading to stronger metallic bonding in lithium.
IV. Size of cations:
- Lithium cations are smaller than sodium cations, resulting in a stronger attraction between the cation and surrounding electrons.
- This leads to stronger metallic bonding in lithium as compared to sodium.
Therefore, all the given statements (I-IV) contribute to the difference in melting points between lithium and sodium, making option 'D' the correct answer.
The difference in melting points between lithium and sodium can be explained by the following factors:
I. Strength of metallic bonding:
- Lithium cations have a higher charge density than sodium cations due to their smaller size.
- The smaller size results in a stronger attraction between the positively charged cation and negatively charged delocalized electrons, leading to stronger metallic bonding.
- Thus, metallic bonding in lithium is stronger than in sodium.
II. Attraction of delocalized electrons:
- Delocalized electrons are more strongly attracted to the smaller lithium cation than to the larger sodium cation due to the higher charge density.
- This results in a stronger metallic bond in lithium as compared to sodium.
III. Charge density of cations:
- Lithium cations have a higher charge density than sodium cations due to their smaller size.
- The higher charge density results in a stronger attraction between the cation and surrounding electrons, leading to stronger metallic bonding in lithium.
IV. Size of cations:
- Lithium cations are smaller than sodium cations, resulting in a stronger attraction between the cation and surrounding electrons.
- This leads to stronger metallic bonding in lithium as compared to sodium.
Therefore, all the given statements (I-IV) contribute to the difference in melting points between lithium and sodium, making option 'D' the correct answer.
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The melting point of lithium metal is 454 K, and that of sodium is 371 K. Which is the following statements can explain this difference in their melt ing points:(I) Metallic bonding in lithium is stronger than metallic bonding in sodium.(II) The delocalized electrons are more strongly attracted to the metal cation of lithium.(III) The lithium cations have a greater charge density than sodium cation.(IV) Li+ cations are smaller than Na+ cations.a)Only I and IIb)Only II and IIIc)Only IVd)I, II, III, IVCorrect answer is option 'D'. Can you explain this answer?
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The melting point of lithium metal is 454 K, and that of sodium is 371 K. Which is the following statements can explain this difference in their melt ing points:(I) Metallic bonding in lithium is stronger than metallic bonding in sodium.(II) The delocalized electrons are more strongly attracted to the metal cation of lithium.(III) The lithium cations have a greater charge density than sodium cation.(IV) Li+ cations are smaller than Na+ cations.a)Only I and IIb)Only II and IIIc)Only IVd)I, II, III, IVCorrect answer is option 'D'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about The melting point of lithium metal is 454 K, and that of sodium is 371 K. Which is the following statements can explain this difference in their melt ing points:(I) Metallic bonding in lithium is stronger than metallic bonding in sodium.(II) The delocalized electrons are more strongly attracted to the metal cation of lithium.(III) The lithium cations have a greater charge density than sodium cation.(IV) Li+ cations are smaller than Na+ cations.a)Only I and IIb)Only II and IIIc)Only IVd)I, II, III, IVCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The melting point of lithium metal is 454 K, and that of sodium is 371 K. Which is the following statements can explain this difference in their melt ing points:(I) Metallic bonding in lithium is stronger than metallic bonding in sodium.(II) The delocalized electrons are more strongly attracted to the metal cation of lithium.(III) The lithium cations have a greater charge density than sodium cation.(IV) Li+ cations are smaller than Na+ cations.a)Only I and IIb)Only II and IIIc)Only IVd)I, II, III, IVCorrect answer is option 'D'. Can you explain this answer?.
The melting point of lithium metal is 454 K, and that of sodium is 371 K. Which is the following statements can explain this difference in their melt ing points:(I) Metallic bonding in lithium is stronger than metallic bonding in sodium.(II) The delocalized electrons are more strongly attracted to the metal cation of lithium.(III) The lithium cations have a greater charge density than sodium cation.(IV) Li+ cations are smaller than Na+ cations.a)Only I and IIb)Only II and IIIc)Only IVd)I, II, III, IVCorrect answer is option 'D'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about The melting point of lithium metal is 454 K, and that of sodium is 371 K. Which is the following statements can explain this difference in their melt ing points:(I) Metallic bonding in lithium is stronger than metallic bonding in sodium.(II) The delocalized electrons are more strongly attracted to the metal cation of lithium.(III) The lithium cations have a greater charge density than sodium cation.(IV) Li+ cations are smaller than Na+ cations.a)Only I and IIb)Only II and IIIc)Only IVd)I, II, III, IVCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The melting point of lithium metal is 454 K, and that of sodium is 371 K. Which is the following statements can explain this difference in their melt ing points:(I) Metallic bonding in lithium is stronger than metallic bonding in sodium.(II) The delocalized electrons are more strongly attracted to the metal cation of lithium.(III) The lithium cations have a greater charge density than sodium cation.(IV) Li+ cations are smaller than Na+ cations.a)Only I and IIb)Only II and IIIc)Only IVd)I, II, III, IVCorrect answer is option 'D'. Can you explain this answer?.
Solutions for The melting point of lithium metal is 454 K, and that of sodium is 371 K. Which is the following statements can explain this difference in their melt ing points:(I) Metallic bonding in lithium is stronger than metallic bonding in sodium.(II) The delocalized electrons are more strongly attracted to the metal cation of lithium.(III) The lithium cations have a greater charge density than sodium cation.(IV) Li+ cations are smaller than Na+ cations.a)Only I and IIb)Only II and IIIc)Only IVd)I, II, III, IVCorrect answer is option 'D'. Can you explain this answer? in English & in Hindi are available as part of our courses for Chemistry.
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