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Why is this 5. Explain how the melting point of compounds relates to the attractions found in the molecules.

Why is this 5. Explain how the melting point of compounds relates to the attractions found in the molecules.

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter3: Atomic Shells And Classical Models Of Chemical Bonding
Section: Chapter Questions
Problem 86AP
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Please just answer question 5
Part B: Properties such as melting point, boiling point, solubility, electrical conductivity, and colour, can help you distinguish ionic from covalent compounds. As in many areas of chemistry, the distinctions are not always clear, nor do the distinctions apply to all compounds. The salt and sugar on your kitchen table both dissolve easily in water, but the solutions they form have an important difference. One of those kinds of white crystals is an ionic compound, and when it dissolves, it dissociates, or breaks up into ions. The ions are free to move in the solution, and that solution, therefore, conducts electricity. The more ions in solution, the better it conducts electricity. The other kind of crystal, however, is a molecular compound, and its molecules remain whole when they dissolve. With no ions, that solution does not conduct electricity. Use your knowledge of compounds to answer the following questions. 1. What kinds of elements generally form ionic compounds? How about covalent compounds? 2. How do aqueous solutions of ionic and molecular compounds differ? 3. When some ionic compounds dissolve, not all of their bonds dissociate. What kind of conductivity would you expect such a solution to have? 4. The phrase "like dissolves like" means that compounds will dissolve other compounds with similar bond types. Water, a polar molecule, will dissolve both ionic compounds and polar compounds. Why is this the case? 5. Explain how the melting point of compounds relates to the attractions found in the molecules.
Transcribed Image Text:Part B: Properties such as melting point, boiling point, solubility, electrical conductivity, and colour, can help you distinguish ionic from covalent compounds. As in many areas of chemistry, the distinctions are not always clear, nor do the distinctions apply to all compounds. The salt and sugar on your kitchen table both dissolve easily in water, but the solutions they form have an important difference. One of those kinds of white crystals is an ionic compound, and when it dissolves, it dissociates, or breaks up into ions. The ions are free to move in the solution, and that solution, therefore, conducts electricity. The more ions in solution, the better it conducts electricity. The other kind of crystal, however, is a molecular compound, and its molecules remain whole when they dissolve. With no ions, that solution does not conduct electricity. Use your knowledge of compounds to answer the following questions. 1. What kinds of elements generally form ionic compounds? How about covalent compounds? 2. How do aqueous solutions of ionic and molecular compounds differ? 3. When some ionic compounds dissolve, not all of their bonds dissociate. What kind of conductivity would you expect such a solution to have? 4. The phrase "like dissolves like" means that compounds will dissolve other compounds with similar bond types. Water, a polar molecule, will dissolve both ionic compounds and polar compounds. Why is this the case? 5. Explain how the melting point of compounds relates to the attractions found in the molecules.
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