University:
East Georgia State College
Course:
CHEM 1211 | Principles of Chemistry I
Academic year:

2023
Views:

422

Pages:

2
Author:

5CelestialChronicle

Solids questions 1. Identify the attractive force (IMF or chemical bond) that holds the following solid types together a. Molecular solids d. Metallic solids b. Covalent network e. Amorphous solids c. Ionic solids 2. Sketch a diagram depicting the bonding found in the solid a. NaF b. Mg 3. Using the diagrams above, answer the following questions a. Why are ionic solids brittle b. Why are ionic solids hard c. Why are metallic solids malleable d. Why are metals generally good conductors e. Why are ionic solids insulators f. Why do ionic solids conduct electricity when dissolved in solution 4. Why is I2 a solid at room temperature, Br2 a liquid, and Cl2 and F2 are gases? 5. Identify the specific type of attractive force (IMF or bond) that must be overcome to do the following: a. Metal ammonia, NH3 ________ c. Melt copper _________ b. Melt calcium carbonate, CaCO3 d. Melt wax ___________ 6. Which of the following would you expect to dissolve in water the easiest: C8H18, Cr, CaCl2. Why? 7. What is the primary difference between an amorphous solid and a crystalline solid? 8. List the four types of crystalline solids 9. Describe how you would determine the attractive force within a solid 10. Rank the following substances in order of decreasing melting points: PbF2, TlF3, TlF, PbF4, TlF5 11. State the general rule for predicting the solubility of a solid in a liquid solvent. Give an example. 12. Rank the following substances in order of increasing melting points: CsF, NaF, LiF, KF, RbF 13. Specifically, why does CaCl2 have a higher melting point than BaCl2? 14. Identify the attractive force (IMF or bond) needed to overcome to do the following: a. Melt wax ________________ e. Melt ice ________________ b. Melt CH2F2 ________________ f. c. Melt a coin ________________ g. Melt table salt ________________ d. Melt a rock ________________ h. Melt steel ________________ Melt a diamond ________________ 15. What is the difference between the covalent bonding found in a molecular solid and the covalent bonding found in a network covalent solid? 16. Why do some ionic solids dissolve in water while others do not?

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