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35 Name Date Class 9 CHEMICAL NAMES AND FORMULAS SECTION 9.1 NAMING IONS (pages ) This section explains the use of the periodic table to determine the charge of an ion. It also defines polyatomic ion and gives the names and formulas for the most common polyatomic ions. Monatomic Ions (pages ) 1. What are monatomic ions? Monatomic ions are ions consisting of only one atom. 2. How is the ionic charge of a Group 1A, 2A, or 3A ion determined? The ionic charge is numerically equal to the group number. 3. How is the ionic charge of a Group 5A, 6A, or 7A ion determined? The charge of an ion in Groups 5A, 6A, or 7A is determined by subtracting 8 from the group number. 4. Circle the letter of the type of element that often has more than one common ionic charge. a. alkali metal Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. b. alkaline earth metal c. transition metal d. nonmetal 5. The Stock system of naming transition metal cations uses a Roman numeral in parentheses to indicate the numeric value of the ionic charge. 6. An older naming system uses the suffix -ous to name the cation with the lesser charge, and the suffix -ic to name the cation with the greater charge. 7. What is a major advantage of the Stock system over the old naming system? The Stock system gives the actual charge of the ion. Chapter 9 Chemical Names and Formulas 79

36 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Name Date Class CHAPTER 9, Chemical Names and Formulas (continued) 8. Use the periodic table to write the name and formula (including charge) for each ion in the table below. Element Name Formula Fluorine Calcium Oxygen fluoride ion calcium ion oxide ion F Ca 2+ O 2 Polyatomic Ions (pages ) 9. What is a polyatomic ion? A polyatomic ion is a tightly bound group of atoms that behaves as a unit and carries a charge. 10. Is the following sentence true or false? The names of polyatomic anions always end in -ide. false 11. What is the difference between the anions sulfite and sulfate? The sulfite ion has one less oxygen atom than the sulfate ion. 12. Look at Table 9.3 on page 257. Circle the letter of a polyatomic ion that is a cation. a. ammonium b. acetate c. oxalate d. phosphate 13. How many atoms make up the oxalate ion and what is its charge? It is made up of 6 atoms (2 carbon atoms and 4 oxygen atoms) and it has a charge of What three hydrogen-containing polyatomic anions are essential components of living systems? a. hydrogen carbonate ion b. hydrogen phosphate ion c. dihydrogen phosphate ion 80 Guided Reading and Study Workbook

37 Name Date Class 15. Look at Figure 9.5 on page 257. Identify each of the ions shown below. N 1 P 3 N 1 ammonium ion a. b. phosphate ion nitrate ion c. SECTION 9.2 NAMING AND WRITING FORMULAS FOR IONIC COMPOUNDS (pages ) This section explains the rules for naming and writing formulas for binary ionic compounds and compounds containing a polyatomic ion. Binary Ionic Compounds (pages ) 1. Traditionally, common names were based on some property of a compound or its source. 2. What is the general name for compounds composed of two elements? They are binary compounds. 3. When writing the formula for any ionic compound, the charges of the ions must balance. 4. What are two methods for writing a balanced formula? Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. a. finding the least common multiple of the charges b. using the crisscross method 5. What are the formulas for the compounds formed by the following pairs of ions? a. Fe 2, Cl FeCl 2 b. Cr 3, O 2 Cr 2 O 3 c. Na, S 2 Na 2 S 6. What are the formulas for these compounds? a. lithium bromide LiBr b. cupric nitride Cu 3 N 2 c. magnesium chloride MgCl 2 7. The name of a binary ionic compound is written with the name of the cation first followed by the name of the anion. Chapter 9 Chemical Names and Formulas 81

38 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Name Date Class CHAPTER 9, Chemical Names and Formulas (continued) 8. How can you tell that cobalt(ii) iodide is a binary ionic compound formed by a transition metal with more than one ionic charge? The name includes a Roman numeral representing the ionic charge of the transition metal cation. 9. Write the names for these binary ionic compounds. a. PbS lead(ii) sulfide b. MgCl 2 magnesium chloride c. Al 2 Se 3 aluminum selenide Compounds with Polyatomic Ions (pages ) 10. What is a polyatomic ion? A polyatomic ion contains more than one element. 11. How do you write the formula for a compound containing a polyatomic ion? Write the symbol for the cation followed by the formula for the polyatomic ion and balance the charges. 12. Why are parentheses used to write the formula Al(OH) 3? The parentheses indicate how many polyatomic ions are needed in the formula. 13. Complete the table for these ionic compounds containing polyatomic ions. Cation Anion Name Formula NH 4 + S 2 ammonium sulfide (NH 4 ) 2 S Fe 3+ CO 3 2 iron(iii) carbonate Fe 2 (CO 3 ) 3 Ag + NO 3 silver nitrate AgNO 3 K + CN potassium cyanide KCN 82 Guided Reading and Study Workbook

39 Name Date Class SECTION 9.3 NAMING AND WRITING FORMULAS FOR MOLECULAR COMPOUNDS (pages ) This section explains the rules for naming and writing formulas for binary molecular compounds. Naming Binary Molecular Compounds (pages ) 1. Circle the letter of the type(s) of elements that form binary molecular compounds. a. two nonmetallic elements b. a metal and a nonmetal c. two metals 2. Is the following sentence true or false? Two nonmetallic elements can combine in only one way. false 3. What method is used to distinguish between different molecular compounds that contain the same elements? Prefixes are used. Match the prefix with the number it indicates. c 4. octa- a. 4 a 5. tetra- b. 7 b 6. hepta- c. 8 d 7. nona- d. 9 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 8. What are the names of the following compounds? a. BF 3 boron trifluoride b. N 2 O 4 dinitrogen tetroxide c. P 4 S 7 tetraphosphorus heptasulfide Writing Formulas for Binary Molecular Compounds (page 270) 9. What are the formulas for the following compounds? a. carbon tetrabromide CBr 4 b. nitrogen triiodide NI 3 c. iodine monochloride ICl d. tetraiodine nonaoxide I 4 O 9 Chapter 9 Chemical Names and Formulas 83

40 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Name Date Class CHAPTER 9, Chemical Names and Formulas (continued) Reading Skill Practice Writing a summary can help you remember the information you have read. When you write a summary, include only the most important points. Write a summary of the information in Section 9.3 on pages Your summary should be shorter than the text on which it is based. Do your work on a separate sheet of paper. Students summaries should focus on the main points of each subsection and include the information given in Table 9.4. SECTION 9.4 NAMING AND WRITING FORMULAS FOR ACIDS AND BASES (pages ) This section explains the three rules for naming acids and shows how these rules can also be used to write the formulas for acids. Names and formulas for bases are also explained. Naming Common Acids (pages ) 1. Acids produce hydrogen ions when dissolved in water. 2. When naming acids, you can consider them to be combinations of anions connected to as many hydrogen ions as are necessary to create an electrically neutral compound. 3. What is the formula for hydrobromic acid? HBr 4. What are the components of phosphorous acid? What is its formula? hydrogen ion and phosphite ion; H 3 PO 3 Writing Formulas for Acids (page 272) 5. Use Table 9.5 on page 272 to help you complete the table about acids. Acid Name Formula Anion Name acetic acid carbonic acid hydrochloric acid nitric acid phosphoric acid sulfuric acid HC 2 H 3 O 2 H 2 CO 3 HCl HNO 3 H 3 PO 4 H 2 SO 4 acetate carbonate chloride nitrate phosphate sulfate 84 Guided Reading and Study Workbook

41 Name Date Class Names and Formulas for Bases (page 273) 6. A base is a compound that produces hydroxide ions when dissolved in water. 7. How are bases named? Name the cation first followed by the anion (hydroxide ion). SECTION 9.5 THE LAWS GOVERNING FORMULAS AND NAMES (pages ) This section uses data to demonstrate that a compound obeys the law of definite proportions. It also explains how to use flow charts to write the name and formula of a compound. The Laws of Definite and Multiple Proportions (pages ) 1. What is the law of definite proportions? In different samples of the same chemical compound, the masses of the elements are always present in the same proportions. 2. Circle the whole-number mass ratio of Li to Cl in LiCl. The atomic mass of Li is 6.9; the atomic mass of Cl is a. 42 : 1 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. b. 5 : 1 c. 1 : 5 3. Circle the whole-number mass ratio of carbon to hydrogen in C 2 H 4. The atomic mass of C is 12.0; the atomic mass of H is 1.0. a. 1 : 6 c. 1 : 12 b. 6 : 1 d. 12 : 1 4. In the compound sulfur dioxide, a food preservative, the mass ratio of sulfur to oxygen is 1 : 1. An 80-g sample of a compound composed of sulfur and oxygen contains 48 g of oxygen. Is the sample sulfur dioxide? Explain. No; If the sample contains 48 g of oxygen, it contains 32 g of sulfur. The ratio 32 : 48 is equivalent to 2 : 3, not 1 : What is the law of multiple proportions? When two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in a ratio of small whole numbers. Chapter 9 Chemical Names and Formulas 85

42 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Name Date Class CHAPTER 9, Chemical Names and Formulas (continued) 6. Complete the table using the law of multiple proportions. Mass of Cu Mass of Cl Mass Ratio Whole-number Cl : Cu Ratio of Cl Compound A 8.3 g 4.6 g Compound B 3.3 g 3.6 g Practicing Skills: Naming Chemical Compounds (pages ) 7. How can a flowchart help you to name chemical compounds? It gives step-by-step directions for naming a compound. 8. Use the flowchart in Figure 9.20 on page 277 to write the names of the following compounds: a. CsCl cesium chloride b. SnSe 2 tin(iv) selenide c. NH 4 OH ammonium hydroxide d. HF hydrofluoric acid e. Si 3 N 4 trisilicon tetranitride 9. Complete the following five rules for writing a chemical formula from a chemical name. a. In an ionic compound, the net ionic charge is zero. b. An -ide ending generally indicates a binary compound. c. An -ite or -ate ending means there is a polyatomic ion that includes oxygen in the formula. d. Prefixes in a name generally indicate that the compound is molecular and show the number of each kind of atom in the molecule. e. A Roman numeral after the name of a cation shows the ionic charge of the cation. 86 Guided Reading and Study Workbook

43 Name Date Class Practicing Skills: Writing Chemical Formulas (page 278) 10. Fill in the missing labels from Figure 9.22 on page 278. Name of Compound Contains prefixes? no Ionic compound yes Molecular compound Uses prefixes to write formula. Identify symbols Group A elements Use Table 9.1 for charges. Roman numerals Give charges for cations. Polyatomic ions Use Table 9.3 for charges. Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Balance charges Use crisscross method. Add parentheses for any multiple polyatomic ions. 11. Use the flowchart in Figure 9.22 to write the formulas of the following compounds: a. potassium silicate K 2 SiO 3 b. phosphorus pentachloride PCl 5 c. manganese(ii) chromate MnCrO 4 d. lithium hydride LiH e. diiodine pentoxide I 2 O 5 Chapter 9 Chemical Names and Formulas 87

44 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Name Date Class CHAPTER 9, Chemical Names and Formulas (continued) GUIDED PRACTICE PROBLEMS GUIDED PRACTICE PROBLEM 2 (page 256) 2. How many electrons were lost or gained to form these ions? a. Fe 3 b. O 2 c. Cu Step 1. Determine the number of electrons based on the size of the charge. Step 2. Determine whether the electrons were lost or gained based on the sign of the charge. a. Fe 3 lost 3 electrons. b. O 2 gained 2 electrons. c. Cu lost 1 electron. GUIDED PRACTICE PROBLEMS 10B AND 10C (page 263) 10. Write formulas for compounds formed from these pairs of ions. b. Li +, O 2 Analyze Step 1. Do the ions combine in a 1:1 ratio? No, the charges on the ions are not equal. Solve Step 2. Use the crisscross method to balance the formula. Write the formula. Li 2 0 Evaluate Li 2 O 2 1 Step 3. How do you know your formula is reasonable? The positive and negative charges are equal. 88 Guided Reading and Study Workbook

45 Name Date Class c. Ca 2, N 3 Analyze Step 1. Will the calcium (Ca 2+ ) and nitride (N 3 ) ions combine in a 1 : 1 ratio? How do you know? No, because then the total charge would be negative, instead of neutral. Solve Step 2. Use the crisscross method to balance the formula. Write the formula. Ca 3 N 2 Ca N Evaluate Step 3. How do you know this formula is reasonable? The positive and negative charges are equal. Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. GUIDED PRACTICE PROBLEM 13B (page 265) 13b. Write the formula for chromium(iii) nitrate. Is the compound ionic or molecular? Explain. It is ionic because it has no prefixes and it contains a metal. Use Table 9.3 on page 257 to write the formula for NO 3 the nitrate ion. Use the crisscross method to balance the formula. Write the formula. Cr(NO 3 ) 3 Cr 3 (NO 3 ) 1 3 Chapter 9 Chemical Names and Formulas 89

46 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Name Date Class CHAPTER 9, Chemical Names and Formulas (continued) GUIDED PRACTICE PROBLEM 34 (page 275) 34. Lead forms two compounds with oxygen. One compound contains 2.98 g of lead and g of oxygen. The other contains 9.89 g of lead and g of oxygen. For a given mass of oxygen, what is the lowest whole-number mass ratio of lead in the two compounds? Complete the following steps to solve the problem. Step 1. Write the ratio of lead to oxygen for each compound. First compound 2.98 g lead g oxygen Second compound 9.89 g lead g oxygen Step 2. Divide the numerator by the denominator in each ratio g lead g oxygen 13.0 g lead g oxygen Step 3. Write a ratio comparing the first compound to the second g lead/g oxygen 13.0 g lead/g oxygen Step 4. Simplify. Note that this ratio has no units roughly The mass ratio of lead per gram of oxygen in the two compounds is 1 : Guided Reading and Study Workbook

47 Name Date Class 9 CHEMICAL NAMES AND FORMULAS SECTION 9.1 NAMING IONS (pages ) This section explains the use of the periodic table to determine the charge of an ion. It also defines polyatomic ion and gives the names and formulas for the most common polyatomic ions. Monatomic Ions (pages ) 1. What are monatomic ions? Monatomic ions are ions consisting of only one atom. 2. How is the ionic charge of a Group 1A, 2A, or 3A ion determined? The ionic charge is numerically equal to the group number. 3. How is the ionic charge of a Group 5A, 6A, or 7A ion determined? The charge of an ion in Groups 5A, 6A, or 7A is determined by subtracting 8 from the group number. 4. Circle the letter of the type of element that often has more than one common ionic charge. a. alkali metal Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. b. alkaline earth metal c. transition metal d. nonmetal 5. The Stock system of naming transition metal cations uses a Roman numeral in parentheses to indicate the numeric value of the ionic charge. 6. An older naming system uses the suffix -ous to name the cation with the lesser charge, and the suffix -ic to name the cation with the greater charge. 7. What is a major advantage of the Stock system over the old naming system? The Stock system gives the actual charge of the ion. Chapter 9 Chemical Names and Formulas 79

48 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Name Date Class CHAPTER 9, Chemical Names and Formulas (continued) 8. Use the periodic table to write the name and formula (including charge) for each ion in the table below. Element Name Formula Fluorine Calcium Oxygen fluoride ion calcium ion oxide ion F Ca 2+ O 2 Polyatomic Ions (pages ) 9. What is a polyatomic ion? A polyatomic ion is a tightly bound group of atoms that behaves as a unit and carries a charge. 10. Is the following sentence true or false? The names of polyatomic anions always end in -ide. false 11. What is the difference between the anions sulfite and sulfate? The sulfite ion has one less oxygen atom than the sulfate ion. 12. Look at Table 9.3 on page 257. Circle the letter of a polyatomic ion that is a cation. a. ammonium b. acetate c. oxalate d. phosphate 13. How many atoms make up the oxalate ion and what is its charge? It is made up of 6 atoms (2 carbon atoms and 4 oxygen atoms) and it has a charge of What three hydrogen-containing polyatomic anions are essential components of living systems? a. hydrogen carbonate ion b. hydrogen phosphate ion c. dihydrogen phosphate ion 80 Guided Reading and Study Workbook

49 Name Date Class 15. Look at Figure 9.5 on page 257. Identify each of the ions shown below. N 1 P 3 N 1 ammonium ion a. b. phosphate ion nitrate ion c. SECTION 9.2 NAMING AND WRITING FORMULAS FOR IONIC COMPOUNDS (pages ) This section explains the rules for naming and writing formulas for binary ionic compounds and compounds containing a polyatomic ion. Binary Ionic Compounds (pages ) 1. Traditionally, common names were based on some property of a compound or its source. 2. What is the general name for compounds composed of two elements? They are binary compounds. 3. When writing the formula for any ionic compound, the charges of the ions must balance. 4. What are two methods for writing a balanced formula? Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. a. finding the least common multiple of the charges b. using the crisscross method 5. What are the formulas for the compounds formed by the following pairs of ions? a. Fe 2, Cl FeCl 2 b. Cr 3, O 2 Cr 2 O 3 c. Na, S 2 Na 2 S 6. What are the formulas for these compounds? a. lithium bromide LiBr b. cupric nitride Cu 3 N 2 c. magnesium chloride MgCl 2 7. The name of a binary ionic compound is written with the name of the cation first followed by the name of the anion. Chapter 9 Chemical Names and Formulas 81

50 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Name Date Class CHAPTER 9, Chemical Names and Formulas (continued) 8. How can you tell that cobalt(ii) iodide is a binary ionic compound formed by a transition metal with more than one ionic charge? The name includes a Roman numeral representing the ionic charge of the transition metal cation. 9. Write the names for these binary ionic compounds. a. PbS lead(ii) sulfide b. MgCl 2 magnesium chloride c. Al 2 Se 3 aluminum selenide Compounds with Polyatomic Ions (pages ) 10. What is a polyatomic ion? A polyatomic ion contains more than one element. 11. How do you write the formula for a compound containing a polyatomic ion? Write the symbol for the cation followed by the formula for the polyatomic ion and balance the charges. 12. Why are parentheses used to write the formula Al(OH) 3? The parentheses indicate how many polyatomic ions are needed in the formula. 13. Complete the table for these ionic compounds containing polyatomic ions. Cation Anion Name Formula NH 4 + S 2 ammonium sulfide (NH 4 ) 2 S Fe 3+ CO 3 2 iron(iii) carbonate Fe 2 (CO 3 ) 3 Ag + NO 3 silver nitrate AgNO 3 K + CN potassium cyanide KCN 82 Guided Reading and Study Workbook

51 Name Date Class SECTION 9.3 NAMING AND WRITING FORMULAS FOR MOLECULAR COMPOUNDS (pages ) This section explains the rules for naming and writing formulas for binary molecular compounds. Naming Binary Molecular Compounds (pages ) 1. Circle the letter of the type(s) of elements that form binary molecular compounds. a. two nonmetallic elements b. a metal and a nonmetal c. two metals 2. Is the following sentence true or false? Two nonmetallic elements can combine in only one way. false 3. What method is used to distinguish between different molecular compounds that contain the same elements? Prefixes are used. Match the prefix with the number it indicates. c 4. octa- a. 4 a 5. tetra- b. 7 b 6. hepta- c. 8 d 7. nona- d. 9 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 8. What are the names of the following compounds? a. BF 3 boron trifluoride b. N 2 O 4 dinitrogen tetroxide c. P 4 S 7 tetraphosphorus heptasulfide Writing Formulas for Binary Molecular Compounds (page 270) 9. What are the formulas for the following compounds? a. carbon tetrabromide CBr 4 b. nitrogen triiodide NI 3 c. iodine monochloride ICl d. tetraiodine nonaoxide I 4 O 9 Chapter 9 Chemical Names and Formulas 83

52 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Name Date Class CHAPTER 9, Chemical Names and Formulas (continued) Reading Skill Practice Writing a summary can help you remember the information you have read. When you write a summary, include only the most important points. Write a summary of the information in Section 9.3 on pages Your summary should be shorter than the text on which it is based. Do your work on a separate sheet of paper. Students summaries should focus on the main points of each subsection and include the information given in Table 9.4. SECTION 9.4 NAMING AND WRITING FORMULAS FOR ACIDS AND BASES (pages ) This section explains the three rules for naming acids and shows how these rules can also be used to write the formulas for acids. Names and formulas for bases are also explained. Naming Common Acids (pages ) 1. Acids produce hydrogen ions when dissolved in water. 2. When naming acids, you can consider them to be combinations of anions connected to as many hydrogen ions as are necessary to create an electrically neutral compound. 3. What is the formula for hydrobromic acid? HBr 4. What are the components of phosphorous acid? What is its formula? hydrogen ion and phosphite ion; H 3 PO 3 Writing Formulas for Acids (page 272) 5. Use Table 9.5 on page 272 to help you complete the table about acids. Acid Name Formula Anion Name acetic acid carbonic acid hydrochloric acid nitric acid phosphoric acid sulfuric acid HC 2 H 3 O 2 H 2 CO 3 HCl HNO 3 H 3 PO 4 H 2 SO 4 acetate carbonate chloride nitrate phosphate sulfate 84 Guided Reading and Study Workbook

53 Name Date Class Names and Formulas for Bases (page 273) 6. A base is a compound that produces hydroxide ions when dissolved in water. 7. How are bases named? Name the cation first followed by the anion (hydroxide ion). SECTION 9.5 THE LAWS GOVERNING FORMULAS AND NAMES (pages ) This section uses data to demonstrate that a compound obeys the law of definite proportions. It also explains how to use flow charts to write the name and formula of a compound. The Laws of Definite and Multiple Proportions (pages ) 1. What is the law of definite proportions? In different samples of the same chemical compound, the masses of the elements are always present in the same proportions. 2. Circle the whole-number mass ratio of Li to Cl in LiCl. The atomic mass of Li is 6.9; the atomic mass of Cl is a. 42 : 1 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. b. 5 : 1 c. 1 : 5 3. Circle the whole-number mass ratio of carbon to hydrogen in C 2 H 4. The atomic mass of C is 12.0; the atomic mass of H is 1.0. a. 1 : 6 c. 1 : 12 b. 6 : 1 d. 12 : 1 4. In the compound sulfur dioxide, a food preservative, the mass ratio of sulfur to oxygen is 1 : 1. An 80-g sample of a compound composed of sulfur and oxygen contains 48 g of oxygen. Is the sample sulfur dioxide? Explain. No; If the sample contains 48 g of oxygen, it contains 32 g of sulfur. The ratio 32 : 48 is equivalent to 2 : 3, not 1 : What is the law of multiple proportions? When two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in a ratio of small whole numbers. Chapter 9 Chemical Names and Formulas 85

54 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Name Date Class CHAPTER 9, Chemical Names and Formulas (continued) 6. Complete the table using the law of multiple proportions. Mass of Cu Mass of Cl Mass Ratio Whole-number Cl : Cu Ratio of Cl Compound A 8.3 g 4.6 g Compound B 3.3 g 3.6 g Practicing Skills: Naming Chemical Compounds (pages ) 7. How can a flowchart help you to name chemical compounds? It gives step-by-step directions for naming a compound. 8. Use the flowchart in Figure 9.20 on page 277 to write the names of the following compounds: a. CsCl cesium chloride b. SnSe 2 tin(iv) selenide c. NH 4 OH ammonium hydroxide d. HF hydrofluoric acid e. Si 3 N 4 trisilicon tetranitride 9. Complete the following five rules for writing a chemical formula from a chemical name. a. In an ionic compound, the net ionic charge is zero. b. An -ide ending generally indicates a binary compound. c. An -ite or -ate ending means there is a polyatomic ion that includes oxygen in the formula. d. Prefixes in a name generally indicate that the compound is molecular and show the number of each kind of atom in the molecule. e. A Roman numeral after the name of a cation shows the ionic charge of the cation. 86 Guided Reading and Study Workbook

55 Name Date Class Practicing Skills: Writing Chemical Formulas (page 278) 10. Fill in the missing labels from Figure 9.22 on page 278. Name of Compound Contains prefixes? no Ionic compound yes Molecular compound Uses prefixes to write formula. Identify symbols Group A elements Use Table 9.1 for charges. Roman numerals Give charges for cations. Polyatomic ions Use Table 9.3 for charges. Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Balance charges Use crisscross method. Add parentheses for any multiple polyatomic ions. 11. Use the flowchart in Figure 9.22 to write the formulas of the following compounds: a. potassium silicate K 2 SiO 3 b. phosphorus pentachloride PCl 5 c. manganese(ii) chromate MnCrO 4 d. lithium hydride LiH e. diiodine pentoxide I 2 O 5 Chapter 9 Chemical Names and Formulas 87

56 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Name Date Class CHAPTER 9, Chemical Names and Formulas (continued) GUIDED PRACTICE PROBLEMS GUIDED PRACTICE PROBLEM 2 (page 256) 2. How many electrons were lost or gained to form these ions? a. Fe 3 b. O 2 c. Cu Step 1. Determine the number of electrons based on the size of the charge. Step 2. Determine whether the electrons were lost or gained based on the sign of the charge. a. Fe 3 lost 3 electrons. b. O 2 gained 2 electrons. c. Cu lost 1 electron. GUIDED PRACTICE PROBLEMS 10B AND 10C (page 263) 10. Write formulas for compounds formed from these pairs of ions. b. Li +, O 2 Analyze Step 1. Do the ions combine in a 1:1 ratio? No, the charges on the ions are not equal. Solve Step 2. Use the crisscross method to balance the formula. Write the formula. Li 2 0 Evaluate Li 2 O 2 1 Step 3. How do you know your formula is reasonable? The positive and negative charges are equal. 88 Guided Reading and Study Workbook

57 Name Date Class c. Ca 2, N 3 Analyze Step 1. Will the calcium (Ca 2+ ) and nitride (N 3 ) ions combine in a 1 : 1 ratio? How do you know? No, because then the total charge would be negative, instead of neutral. Solve Step 2. Use the crisscross method to balance the formula. Write the formula. Ca 3 N 2 Ca N Evaluate Step 3. How do you know this formula is reasonable? The positive and negative charges are equal. Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. GUIDED PRACTICE PROBLEM 13B (page 265) 13b. Write the formula for chromium(iii) nitrate. Is the compound ionic or molecular? Explain. It is ionic because it has no prefixes and it contains a metal. Use Table 9.3 on page 257 to write the formula for NO 3 the nitrate ion. Use the crisscross method to balance the formula. Write the formula. Cr(NO 3 ) 3 Cr 3 (NO 3 ) 1 3 Chapter 9 Chemical Names and Formulas 89

58 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Name Date Class CHAPTER 9, Chemical Names and Formulas (continued) GUIDED PRACTICE PROBLEM 34 (page 275) 34. Lead forms two compounds with oxygen. One compound contains 2.98 g of lead and g of oxygen. The other contains 9.89 g of lead and g of oxygen. For a given mass of oxygen, what is the lowest whole-number mass ratio of lead in the two compounds? Complete the following steps to solve the problem. Step 1. Write the ratio of lead to oxygen for each compound. First compound 2.98 g lead g oxygen Second compound 9.89 g lead g oxygen Step 2. Divide the numerator by the denominator in each ratio g lead g oxygen 13.0 g lead g oxygen Step 3. Write a ratio comparing the first compound to the second g lead/g oxygen 13.0 g lead/g oxygen Step 4. Simplify. Note that this ratio has no units roughly The mass ratio of lead per gram of oxygen in the two compounds is 1 : Guided Reading and Study Workbook

59 Name Date Class 9 CHEMICAL NAMES AND FORMULAS Practice Problems In your notebook, solve the following problems. Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. SECTION 9.1 NAMING IONS 1. What is the charge on the ion typically formed by each element? a. oxygen c. sodium e. nickel, 2 electrons lost b. iodine d. aluminum f. magnesium 2. How many electrons does the neutral atom gain or lose when each ion forms? a. Cr 3 c. Li e. Cl b. P 3 d. Ca 2 f. O 2 3. Name each ion. Identify each as a cation or an anion. a. Sn 2 c. Br e. H b. Co 3 d. K f. Mn 2 4. Write the formula (including charge) for each ion. Use Table 9.3 if necessary. a. carbonate ion c. sulfate ion e. chromate ion b. nitrite ion d. hydroxide ion f. ammonium ion 5. Name the following ions. Identify each as a cation or an anion. a. CN 3 c. PO 4 e. Ca 2 b. HCO 3 d. Cl f. SO 3 2 SECTION 9.2 NAMING AND WRITING FORMULAS FOR IONIC COMPOUNDS 1. Write the formulas for these binary ionic compounds. a. magnesium oxide c. potassium iodide e. sodium sulfide b. tin(ii) fluoride d. aluminum chloride f. ferric bromide 2. Write the formulas for the compounds formed from these pairs of ions. a. Ba 2, Cl c. Ca 2, S 2 e. Al 3, O 2 b. Ag, I d. K, Br f. Fe 2, O 2 3. Name the following binary ionic compounds. a. MnO 2 c. CaCl 2 e. NiCl 2 g. CuCl 2 b. Li 3 N d. SrBr 2 f. K 2 S h. SnCl 4 Chapter 9 Chemical Names and Formulas 221

60 Name Date Class 4. Write formulas for the following ionic compounds. a. sodium phosphate c. sodium hydroxide e. ammonium chloride b. magnesium sulfate d. potassium cyanide f. potassium dichromate 5. Write formulas for compounds formed from these pairs of ions. a. NH 2 4, SO 4 c. barium ion and hydroxide ion b. K, NO 3 d. lithium ion and carbonate ion 6. Name the following compounds. a. NaCN c. Na 2 SO 4 e. Cu(OH) 2 b. FeCl 3 d. K 2 CO 3 f. LiNO 3 7. Name and give the charge of the metal cation in each of the following ionic compounds. a. Na 3 PO 4 c. CaS e. FeCl 3 b. NiCl 2 d. K 2 S f. CuI SECTION 9.3 NAMING AND WRITING FORMULAS FOR MOLECULAR COMPOUNDS 1. Name the following molecular compounds. a. PCl 5 c. NO 2 e. P 4 O 6 g. SiO 2 b. CCl 4 d. N 2 F 2 f. XeF 2 h. Cl 2 O 7 2. Write the formulas for the following binary molecular compounds. a. nitrogen tribromide c. sulfur dioxide b. dichlorine monoxide d. dinitrogen tetrafluoride SECTION 9.4 NAMING AND WRITING FORMULAS FOR ACIDS AND BASES 1. Name the following compounds as acids. a. HNO 2 b. H 2 SO 4 c. HF d. H 2 CO 3 2. Write the formulas for the following bases. a. calcium hydroxide c. aluminum hydroxide b. ammonium hydroxide d. lithium hydroxide SECTION 9.5 THE LAWS GOVERNING FORMULAS AND NAMES 1. Write the formulas for these compounds. a. potassium sulfide e. hydrobromic acid i. sulfur hexafluoride b. tin(iv) chloride f. aluminum fluoride j. magnesium chloride c. hydrosulfuric acid g. dinitrogen pentoxide k. phosphoric acid d. calcium oxide h. iron(iii) carbonate l. nitric acid Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 222 Core Teaching Resources

61 Name Date Class 2. Complete this table by writing correct formulas for the compounds formed by combining positive and negative ions. SO 4 2 NO 3 OH PO 4 3 Ca 2 Al 3 Na Pb 4 3. Name the following compounds. a. K 3 PO 4 c. NaHSO 4 e. N 2 O 5 g. PI 3 b. Al(OH) 3 d. HgO f. NBr 3 h. (NH 4 ) 2 SO 4 4. Explain the difference between the law of definite proportions and the law of multiple proportions. Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Chapter 9 Chemical Names and Formulas 223

62 Name Date Class 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. Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 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

63 Name Date Class 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 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. b. S 2 d. Mn Core Teaching Resources

64 Name Date Class 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. Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 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

65 Name Date Class 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 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 214 Core Teaching Resources

66 Name Date Class 9.3 NAMING AND WRITING FORMULAS FOR MOLECULAR COMPOUNDS Section Review Objectives Interpret the prefixes in the names of molecular compounds in terms of their chemical formulas Apply the rules for naming and writing formulas for binary molecular compounds 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 molecular compounds are composed of two 1 1. elements. The name of this type of compound ends in Prefixes are used to show how many 3 of each element 3. are present in a molecule of the compound. For example, 4. Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. the name of As 2 S 5 is 4. Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 5. Binary molecular compounds contain carbon. 6. Charges must be balanced when writing formulas for molecular compounds. 7. CO 2 is named monocarbon dioxide. Chapter 9 Chemical Names and Formulas 215

67 Name Date Class Part C Matching Match each description in Column B to the correct term in Column A. Column A Column B 8. binary molecular compound a. used to indicate the relative number of atoms of an element in a molecular compound prefix mono- tetra- b. prefix indicating one atom of an element in a molecule c. prefix indicating four atoms of an element in a molecule d. nonionic compound containing atoms of two elements Part D Questions and Problems Answer the following in the space provided. 12. Name each of the following compounds. a. PCl 5 b. SO 2 c. P 4 S Write formulas for the following compounds. a. carbon tetrabromide b. dinitrogen tetroxide Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 216 Core Teaching Resources

68 Name Date Class 9.4 NAMING AND WRITING FORMULAS FOR ACIDS AND BASES Section Review Objectives Apply three rules for naming acids Apply the rules in reverse to write formulas of acids Apply the rules for naming bases Vocabulary acid base 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. An acid is a compound that contains one or more 1 1. Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. atoms and produces 2 when dissolved in water. There 2. are rules for naming acids. For example, HBr is called 3. 3 acid, whereas HNO 3 is called 4 acid. 4. A base is a(n) 5 compound that produces 6 when 5. dissolved in water. Ionic compounds that are bases are named 6. in the same way as other 7 compounds, that is, the name 7. of the 8 is followed by the name of the Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 10. A compound that contains hydrogen atoms will be an acid when dissolved in water. Chapter 9 Chemical Names and Formulas 217

69 Name Date Class 11. An acid contains one or more hydroxide ions. 12. Chemists have a special system for naming bases. Part C Matching Match each description in Column B to the correct term in Column A. Column A 13. acid 14. base 15. aqueous solution Column B a. a compound containing hydrogen that ionizes to yield hydrogen ions in solution b. a solution in which the solvent is water c. a compound that produces hydroxide ions in water Part D Questions and Problems Answer the following in the space provided. 16. Write the formula for each acid or base. a. magnesium hydroxide b. hydrofluoric acid c. phosphoric acid d. lithium hydroxide 17. Name each acid or base. a. KOH b. HI c. H 2 SO 4 Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 218 Core Teaching Resources

70 Name Date Class 9.5 THE LAWS GOVERNING FORMULAS AND NAMES Section Review Objectives Define the laws of definite proportions and multiple proportions Apply the rules for writing chemical formulas by using a flowchart Apply the rules for naming chemical compounds by using a flowchart Vocabulary law of definite proportions law of multiple proportions 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. [Use Figure 9.20 to complete this exercise.] The law of 1 states that in samples of any chemical 1. compound, the masses of the elements are always in the same 2. Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 2. The law of 3 states that whenever the same two 3. elements form more than one compound, the different masses 4. of one element that combine with the same mass of the other 5. element are in the ratio of 4 numbers. 6. H 3 PO 4 is a(n) 5. It is called CCl 4 is not a(n) 7. It contains two elements, so it is a 8. 8 compound. It does not contain a metal, so it is a binary 9. 9 compound. The compound is called Pb(C 2 H 3 O 2 ) 2 is not a(n) 11. It contains more than two C 2 H 3 O 2 is a polyatomic 13. Pb is a Group metal. The compound is called Chapter 9 Chemical Names and Formulas 219

71 Name Date Class Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 16. Roman numerals are used when naming Group B metal cations. 17. Names of compounds containing polyatomic anions end in -ide. 18. Prefixes are used when naming binary ionic compounds. 19. Compounds containing two elements are called binary compounds. Part C Questions and Problems Answer the following in the space provided. 20. Name the following compounds. a. Pb(C 2 H 3 O 2 ) 4 b. HF c. P 2 O 5 d. LiBr 21. Write formulas for the following compounds. a. phosphorus pentachloride b. iron(ii) oxide c. nitric acid d. potassium chloride e. calcium nitrate Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 220 Core Teaching Resources

72 Name Date Class 9 INTERPRETING GRAPHICS Use with Section 9.1 Group 1A 1 H Hydrogen 3 Li Lithium 2A 3A 4A 5A 6A 7A 4 Be Beryllium 5 B Boron 6 C Carbon 7 N Nitrogen 8 O Oxygen 9 F Fluorine 8A 2 He Helium 10 Ne Neon 11 Na Sodium 12 Mg Magnesium 13 Al Aluminum 14 Si Silicon 15 P Phosphorus 16 S Sulfur 17 Cl Hydrogen 18 Ar Argon 19 K Potassium 20 Ca Calcium Use the abbreviated periodic table above to answer the following questions. 1. Which group on the periodic table contains magnesium (Mg)? 2. How many electrons does a magnesium atom lose to form a magnesium cation? 3. How many electrons does a neutral magnesium atom contain? 4. How many electrons does a magnesium cation contain? 5. Which group on the periodic table contains fluorine (F)? 6. How many electrons does a fluorine atom gain to form a fluoride anion? 7. How many electrons does a neutral fluorine atom contain? Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 224 Core Teaching Resources

73 Name Date Class 8. How many electrons does a fluoride anion contain? 9. How many electrons does a sodium cation contain? 10. How many electrons does an oxide anion contain? 11. How many electrons does each of the following ions contain? a. S 2 b. Ca 2 c. K d. Cl Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Chapter 9 Chemical Names and Formulas 225