Chapter 6 Assessment. Name: Class: Date: ID: A. Multiple Choice Identify the choice that best completes the statement or answers the question.

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1 Name: Class: Date: ID: A Chapter 6 Assessment Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When an atom loses an electron, it forms a(n) a. anion. c. polyatomic ion. b. cation.. d. neutral ion. 2. The charge on a chloride ion in is a. 1+. c. 1-. b. 3+. d Which pair has the same electron configuration? a. CI- and Ar c. CI and Ar b. CI- and Ar- d. CI+ and Ar 4. A chemical bond that forms when atoms share electrons is always a(n) a. polar bond. c. metallic bond. b. ionic bond. d. covalent bond. 5. When two fluorine atoms share a pair of electrons, the bond that forms is a(n) a. polar covalent bond. c. nonpolar covalent bond. b. ionic bond. d. double bond. 6. The chemical formula for magnesium bromide is a. MgBr. c. Mg(II)Br. b. MgBr d. Mg Br. 7. The compound with the formula is a. silicon chloride. c. silicon (I) chloride. b. silicon chlorine. d. silicon tetrachloride. 8. The attraction among water molecules is stronger than the attraction among a. sodium and chloride ions. c. the atoms in a polyatomic ion. b. carbon dioxide molecules. d. atoms in a diatomic molecule. 9. Which type of solid likely to be the best conductor of electric current? a. ionic compound c. metal element b. covalent compound d. nonmetal element 10. An alloy contains a. at least one metallic element. c. only metallic elements. b. at least one nonmetallic element. d. only nonmetallic elements. Short Answer 11. What is a stable electron configuration? 1

2 Name: ID: A 12. What does each dot in an electron dot diagram represent? 13. What process changes atoms into ions? 14. What keeps the ions in their fixed positions within a crystal lattice? 15. What are subscripts used for in chemical formulas? 16. Explain why a melted ionic compound is a good conductor of electric current, but a solid ionic compound is a poor conductor of electric current. 17. What distinguishes single, double, and triple covalent bonds? 18. Explain why the covalent bonds in molecules of elements are always nonpolar. 19. Explain why, in a covalent bond between oxygen and hydrogen, the hydrogen atom has a partial positive change and the oxygen atom has a partial negative charge. 20. What is the name of the binary compound formed from potassium and iodine? 21. Write the formulas for the compounds called copper(i) chloride and copper(ii) chloride. 22. Name the compounds represented by the space-filling models labeled A,B, and C. 23. In general, what determines the strength of metallic bonds? 24. What properties of copper and tin change when these metals are mixed together to form bronze? 25. What advantage of magnesium is retained in magnesium alloys? What disadvantage is reduced? Problem 26. What does a fluoride ion have in common with a neon atom and a sodium ion? 27. How are molecules and polyatomic ions similar? 28. Classify the bonds in each of these compounds as ionic, polar covalent, or nonpolar covalent: 2

3 Name: ID: A 29. Write the names for the compounds with these chemical formulas: 30. Which of the three elements are metals and which are nonmetals? 31. Element Q forms compounds with element X and with element Z. Write the formulas for these two compounds. 32. What would the formula be for a compound containing chromium(iii) ions and ions of element Z? 33. Draw an electron dot structure for a compound of fluorine and Z. 34. If an atom of X reacts with an atom of X, what kind of bond forms? 3

4 ID: A Chapter 6 Assessment Answer Section MULTIPLE CHOICE 1. ANS: B 2. ANS: C 3. ANS: A 4. ANS: D 5. ANS: C 6. ANS: B 7. ANS: D 8. ANS: B 9. ANS: C 10. ANS: A SHORT ANSWER 11. ANS: In a stable electron configuration, the highest occupied energy level is filled with electrons. 12. ANS: Each dot represents a valence electron. 13. ANS: The transfer of electrons. 14. ANS: Attractions between neighboring cations and anions keep the ions in fixed positions within the lattice. 15. ANS: A subscript is used to show the number of atoms of an element in a molecule or the ratio of ions in a crystal lattice. 16. ANS: When an ionic compound melts, ions can move away from their fixed locations in the crystal lattice. 1

5 ID: A 17. ANS: Two atoms share two electrons in a single bond, four in a double bond, and six in a triple bond. 18. ANS: The covalent bonds in molecules of elements are always nonpolar because the atoms have the same attraction for electrons. 19. ANS: The oxygen atom has a greater attraction for electrons than the hydrogen atom does. 20. ANS: Potassium iodide 21. ANS: CuCU and CuCI2 22. ANS: A is sulfur trioxide, B is carbon monoxide, and C is nitrogen dioxide. 23. ANS: In general, the more valence electrons a metal has, the stronger the metal bonds are. 24. ANS: A mixture of copper and tin is harder and stronger than either metal in its pure form. 25. ANS: The advantage that is retained is that magnesium is a lightweight metal. The disadvantage that is reduced is that magnesium is a soft metal. PROBLEM 26. ANS: All three have the same electron configuration. 2

6 ID: A 27. ANS: Molecules and polyatomic ions both contain covalent bonds. 28. ANS: Sulfur trioxide: polar covalent bonds; calcium oxide; ionic bonds; iodine: nonpolar covalent bonds. 29. ANS: Sulfur dichloride, silver(i) sulfate, lithium fluoride, carbon disulfide, calcium hydroxide. 30. ANS: Q is a metal. X and Z are nonmetals. 31. ANS: QX and Q2Z 32. ANS: Cr2Z3 33. ANS: F Z F 34. ANS: Nonpolar covalent bond 3

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