**Understanding Melting Points of Iodine and Silicon Dioxide**Iodine (I₂) exists as molecules of I₂, whereas silicon dioxide (SiO₂) exists as an extended network of silicon-oxygen bonds (similar to diamond). Both iodine and silicon dioxide are solids at room temperature. This raises an important question regarding their melting points.**Question:**Which of the two substances has a higher melting point and why?**Options:**1. **I₂ because it is heavier and therefore has the largest London Dispersion Forces (LDFs).**2. **I₂ because it is an element.**3. **Silicon dioxide because to melt it you would have to break covalent bonds.**4. **Silicon dioxide because it is a compound and has stronger intermolecular forces than iodine molecules.****Answer:**Option **3**: **Silicon dioxide because to melt it you would have to break covalent bonds.****Explanation:**- **Option 1:** While I₂ molecules are heavier and have significant London Dispersion Forces (LDFs), these forces are relatively weaker when compared to covalent bonds.- **Option 2:** Being an element does not inherently determine the melting point; it depends on the bonding between atoms or molecules.- **Option 3:** Silicon dioxide has a giant covalent structure, meaning its atoms are bonded by strong covalent bonds in a continuous network. Breaking these covalent bonds requires a substantial amount of energy, resulting in a higher melting point.- **Option 4:** While it's true that silicon dioxide is a compound and has strong intermolecular forces, the primary reason for its high melting point is the strong covalent bonds within its structure.This fundamental concept in chemistry illustrates the relationship between the type of atomic or molecular bonding and a substance's physical properties, such as melting point.

lodine exists as molecules of 12, and silicon dioxide exists as an extended network of silicon-oxygen bonds (similar to diamond). They both are solids at room temperature, but which do you think has the higher melting point and why? 1. 12 because it is heavier and therefore has the largest LDFs. 2. 12 because it an element. 3. Silicon dioxide because to melt it you would have to break covalent bonds. 4. Silicon dioxide, because it is a compound and has stronger intermolecular forces than iodine molecules.

lodine exists as molecules of 12, and silicon dioxide exists as an extended network of silicon-oxygen bonds (similar to diamond). They both are solids at room temperature, but which do you think has the higher melting point and why? 1. 12 because it is heavier and therefore has the largest LDFs. 2. 12 because it an element. 3. Silicon dioxide because to melt it you would have to break covalent bonds. 4. Silicon dioxide, because it is a compound and has stronger intermolecular forces than iodine molecules.

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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