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Solve for question 17 please and use question 3 to solve for question 17, short answer please, thanks

Solve for question 17 please and use question 3 to solve for question 17, short answer please, thanks

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Solve for question 17 please and use question 3 to solve for question 17, short answer please, thanks
sharing of electrons. Bonding in water is different from the bonding in salts because salt is the formation of ionic bond while in water there is covalent bond. 2. What do wve call this type of bonding? Covalent Bonding INITIAL IDEAS Water molecules aren't made of ions. But we did see in Lesson 3 that water molecules stick to each other much better than acetone molecules or mineral oil molecules. 3. What does that tell us about the strength of attractions between water molecules compared to the attractions between acetone molecules or mineral oil molecules? Water molecules stick to each other much better than acetone molecules or mineral oil molecules because in water hydrogen bonding takes place while acetone is a dipolar molecule so it contains dipole attraction between the molecules. Hydrogen bonding is more stronger than dipole attraction 4. What ideas do we have about why water is better at dissolving salts than mineral oil? Because water can become so heavily attracted to a different molecule, like salt (NaCI), that it can disrupt the attractive forces that hold the sodium and chloride in the salt molecule together and, thus, dissolve it. 5. What does your group think about the idea that there is some type of charge in between ionic and covalent bonds? Between ionic and bonds there is a metal and nonmetal.
Transcribed Image Text:sharing of electrons. Bonding in water is different from the bonding in salts because salt is the formation of ionic bond while in water there is covalent bond. 2. What do wve call this type of bonding? Covalent Bonding INITIAL IDEAS Water molecules aren't made of ions. But we did see in Lesson 3 that water molecules stick to each other much better than acetone molecules or mineral oil molecules. 3. What does that tell us about the strength of attractions between water molecules compared to the attractions between acetone molecules or mineral oil molecules? Water molecules stick to each other much better than acetone molecules or mineral oil molecules because in water hydrogen bonding takes place while acetone is a dipolar molecule so it contains dipole attraction between the molecules. Hydrogen bonding is more stronger than dipole attraction 4. What ideas do we have about why water is better at dissolving salts than mineral oil? Because water can become so heavily attracted to a different molecule, like salt (NaCI), that it can disrupt the attractive forces that hold the sodium and chloride in the salt molecule together and, thus, dissolve it. 5. What does your group think about the idea that there is some type of charge in between ionic and covalent bonds? Between ionic and bonds there is a metal and nonmetal.
d dotted line. BACK TO THE SIMULATION (Check out mineral oil, again in "opaque" surface view.) 16. Is mineral oil a symmetrical molecule? Does it have partial charges? No mineral oil is not a symmetrical molecule because much of the barbon is in sp3 hydration. Yes it has partial change due to presence of hydroxyl (-oH) group. 17. Think back to lesson 3 and when we put drops of liquids on pennies. Could we get many drops of oil to stick on a penny? What can we infer about attractions between mineral oil molecules? Do we think it is a polar molecule? Electronegativity and Polarity (Here's a link to an Electronegativity Chart) 18. What is electronegativity, and might differences in electronegativity help us determine if a bond is polar or nonpolar (or ionic)? The difference in electronegativity aen between two atoms in a bond can determine whether the bond is polar or nonpolar The general rule is aen > 2 bond is ionic 0.5< aen < bond is polar covalent Aen <0.5 bond is covalent non polar. 19. The data table below shows molecular weight, melting point, and boiling point for several covalent comnpounds. Complete the table by filling in the last three columns. Use the melting and boiling points to determine what state of matter each substance will be at room temperature, Use the diagram of the compounds to determine symmetry. As for the last
Transcribed Image Text:d dotted line. BACK TO THE SIMULATION (Check out mineral oil, again in "opaque" surface view.) 16. Is mineral oil a symmetrical molecule? Does it have partial charges? No mineral oil is not a symmetrical molecule because much of the barbon is in sp3 hydration. Yes it has partial change due to presence of hydroxyl (-oH) group. 17. Think back to lesson 3 and when we put drops of liquids on pennies. Could we get many drops of oil to stick on a penny? What can we infer about attractions between mineral oil molecules? Do we think it is a polar molecule? Electronegativity and Polarity (Here's a link to an Electronegativity Chart) 18. What is electronegativity, and might differences in electronegativity help us determine if a bond is polar or nonpolar (or ionic)? The difference in electronegativity aen between two atoms in a bond can determine whether the bond is polar or nonpolar The general rule is aen > 2 bond is ionic 0.5< aen < bond is polar covalent Aen <0.5 bond is covalent non polar. 19. The data table below shows molecular weight, melting point, and boiling point for several covalent comnpounds. Complete the table by filling in the last three columns. Use the melting and boiling points to determine what state of matter each substance will be at room temperature, Use the diagram of the compounds to determine symmetry. As for the last
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