Name Date Class. octet rule halide ions
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1 7.1 IONS Section Review Objectives Determine the number of valence electrons in an atom of a representative element Explain the octet rule Describe how cations form Explain how anions form Vocabulary valence electrons electron dot structures octet rule halide ions Part A Completion Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. Elements within the same group of the periodic table behave 1. similarly because they have the same number of 1. The 2. 2 number of a representative element indicates how many 3. valence electrons that element has. Diagrams that show valence 4. electrons as dots are called 3. Gilbert Lewis s 4 states 5. that in forming compounds, atoms tend to achieve the electron 6. configuration of a noble gas. 7. The transfer of valence electrons produces positively charged 8. ions, or 5, and negatively charged ions called 6. The 9. cations of Group 1A elements always have a charge of are produced when atoms of the elements in Group 7A 9 an electron. For transition metals, the 10 of cations may vary. Chapter 7 Ionic and Metallic Bonding 155
2 Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 11. The chlorine atom gains seven electrons when it becomes an ion. 12. The chemical properties of an element are largely determined by the number of valence electrons the element has. 13. Atoms acquire the stable electron structure of a noble gas by losing electrons. 14. An atom of an element in Group 1A has seven valence electrons. 15. Among the Group 1A and 2A elements, the group number of each element is equal to the number of valence electrons in an atom of that element. 16. Sulfur and magnesium both have two valence electrons. Part C Matching Match each description in Column B to the correct term in Column A. Column A Column B 17. electron dot structure 18. valence electron a. ions that are produced when halogens gain electrons b. a depiction of valence electrons around the symbol of an element 19. octet rule 20. cations 21. anions 22. halide ions 23. chloride ion Part D Questions and Problems Answer the following in the space provided. 24. Write the electron dot structures for the following atoms. a. silicon b. rubidium c. has the electron configuration of argon d. an electron in the highest occupied energy level of an element s atom e. Atoms in compounds tend to have the electron configuration of a noble gas. f. atoms or groups of atoms with a negative charge g. atoms or groups of atoms with a positive charge c. barium 156 Core Teaching Resources
3 25. State the number of electrons lost or gained in forming each of these ions. Name the ions and tell whether it is an anion or a cation. a. Mg 2 c. Br b. Ca 2 d. Ag 26. Describe the formation of an ion from a metal and a nonmetal in terms of the octet rule. Chapter 7 Ionic and Metallic Bonding 157
4 9.1 NAMING IONS Section Review Objectives Determine the charges of monatomic ions by using the periodic table and write the names of the ions Define a polyatomic ion and write the names and formulas of the most common polyatomic ions Identify the two common endings for the names of most polyatomic ions. Vocabulary monatomic ions polyatomic ions Part A Completion Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. Ions that consist of a single atom are called 1 ions. 1. Metallic elements tend to 2 electrons. Group 1A ions have a 2. 3 charge, whereas Group 2A metals form ions with a 4 3. charge, and Group 3A metals form ions with a 5 charge. 4. The charge of a Group A nonmetal ion is determined by 5. subtracting 6 from the group number. For example, the 6. Group 7A elements form ions with a charge of Many of the 8 have more than one common ionic 8. charge. These ions are named using either the 9 system 9. or the 10 naming system. 10. Ions containing more than one atom are called 11 ions. 11. The names of most common polyatomic ions end in either or Chapter 9 Chemical Names and Formulas 211
5 Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 14. The names of polyatomic ions end in -ite or -ate. 15. In polyatomic ions for which there is an -ite/-ate pair, the -ite ending will always indicate one less oxygen atom than the -ate ending. 16. Polyatomic ions are anions. 17. The charge on Group A metal ions is determined by subtracting the group number from The Group 6A ions have a charge of 2. Part C Matching Match each description in Column B to the correct term in Column A. Column A Column B monatomic ions polyatomic ions cations anions a. negatively charged ions b. ions formed from single atoms c. a traditional way of naming transition metal cations d. positively charged ions 23. Part D Questions and Problems Answer the following in the space provided. 24. What is the charge on a typical ion for each of the following groups? a. 1A c. 7A b. 6A d. 2A 25. Write the name of each of the following polyatomic ions. a. HCO 3 b. NH 4 classical naming system c. MnO 4 d. OH 26. How many electrons does the neutral atom gain or lose to form each of the following ions? a. Ca 2 c. I e. ions formed from groups of atoms b. S 2 d. Mn Core Teaching Resources
6 7.2 IONIC BONDS AND IONIC COMPOUNDS Section Review Objectives Explain the electrical charge of an ionic compound Describe three properties of ionic compounds Vocabulary ionic compounds ionic bonds chemical formula formula unit coordination number Part A Completion Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. Anions and cations attract one another by means of The forces of attraction that hold 2 charged ions together in 2. ionic compounds are called 3. Although they are composed 3. of ions, ionic compounds are electrically 4. The lowest whole- 4. number ratio of ions in an ionic compound is called a Nearly all ionic compounds are solid 6 at room 6. temperature. Ionic compounds in general have very 7 7. melting temperatures. This is because the 8 attractive 8. forces between the ions result in a very 9 structure. 9. Ionic compounds conduct an electric current when in the state or dissolved in water. Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 11. During the formation of the compound NaCl, one electron is transferred from a sodium atom to a chlorine atom. 158 Core Teaching Resources
7 12. The coordination number of an ion is the number of ions of positive charge that surround the ion in a crystal. 13. The coordination number of the ion Na in NaCl is In forming an ionic compound, an atom of an element gains electrons. 15. Ionic compounds cannot conduct electricity if they are dissolved in water. Part C Matching Match each description in Column B to the correct term in Column A. Column A Column B 16. ionic compounds 17. ionic bonds 18. chemical formula 19. formula unit 20. coordination number a. the number of ions of opposite charge surrounding each ion in a crystal b. compounds composed of cations and anions c. shows the kinds and numbers of atoms in the smallest representative unit of a substance d. lowest whole-number ratio of ions in an ionic compound e. the electrostatic forces of attraction binding oppositely charged ions together Part D Questions and Problems Answer the following in the space provided. 21. List the characteristics of an ionic bond. 22. Explain the electrical conductivity of melted and of aqueous solutions of ionic compounds using the characteristics of ionic compounds. Chapter 7 Ionic and Metallic Bonding 159
8 9.2 NAMING AND WRITING FORMULAS FOR IONIC COMPOUNDS Section Review Objectives Apply the rules for naming and writing formulas for binary ionic compounds Apply the rules for naming and writing formulas for compounds with polyatomic ions Vocabulary binary compound Part A Completion Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. Binary ionic compounds are named by writing the name of 1. the 1 followed by the name of the 2. Names of 2. binary compounds end in 3. For example, NaI is When a cation has more than one ionic charge, a 5 4. is used in the name. 5. Compounds with polyatomic ions whose names end in -ite 6. or -ate contain a polyatomic 6 that includes In writing the formula of an ionic compound, the net ionic charge 8. must be 8. Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 9. The systematic name for baking soda (NaHCO 3 ) is sodium bicarbonate. 10. In writing a formula for an ionic compound, the net ionic charge of the formula must be zero. Chapter 9 Chemical Names and Formulas 213
9 11. Anions that contain oxygen end in -ite or -ate. 12. The cation name is placed first when naming ionic compounds. Part C Matching Match each description in Column B to the correct term in Column A. Column A Column B binary compounds monatomic ions polyatomic ions transition metals a. ions that consist of a single atom b. ionic compounds composed of two elements c. Group B metals, many of which have more than one common ionic charge d. ions that consist of more than one atom Part D Questions and Problems Answer the following in the space provided. 17. Name the following compounds and tell what type of compound they are (binary ionic or ionic with a polyatomic ion). a. FeBr 3 b. KOH c. Na 2 Cr 2 O Write the formulas for the following compounds. a. sodium chlorate b. lead(ii) phosphate c. magnesium hydrogen carbonate 214 Core Teaching Resources
10 7.3 BONDING IN METALS Section Review Objectives Model the valence electrons of metal ions Describe the arrangement of atoms in a metal Explain the importance of alloys Vocabulary metallic bonds alloys Part A Completion Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. Metals consist of closely packed 1 that are surrounded 1. by a sea of 2. This arrangement constitutes the 3 2. bond. The electron mobility accounts for the excellent 3. 4 conductivity of metals and helps explain why 4. metals are 5 and 6. Metal atoms are commonly 5. packed in a 7 cubic, a 8 cubic, or a 9 6. arrangement. When two or more elements, at least one of which 7. is a metal, are mixed together, the resulting mixture is called 8. an Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 11. In a body-centered cubic structure, each atom has 12 neighbors. 12. Metallic objects are formed from pure metals. 160 Core Teaching Resources
11 13. Metals that are good conductors of electricity are said to be ductile. 14. Drifting valence electrons insulate cations from one another and contribute to the malleability of a metal. 15. Metals are good conductors of electricity because electrons can flow freely in them. Part C Matching Match each description in Column B to the correct term in Column A. Column A Column B 16. ductile 17. metallic bonds 18. alloy 19. malleable 20. interstitial alloy a. an alloy whose component atoms are different sizes b. a mixture of two or more elements, at least one of which is a metal c. can be hammered or forced into shapes d. can be drawn into wires e. the attraction of valence electrons for positive metal ions Part D Questions and Problems Answer the following in the space provided. 21. Explain the physical properties of metals, using the theory of metallic bonding. 22. Explain why the properties of alloys are generally superior to their constituent components. Chapter 7 Ionic and Metallic Bonding 161
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