Chemical Names and Formulas
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1 Name Class Date Chemical Names and Formulas ELECTRONS AND THE STRUCTURE OF ATOMS BONDING AND INTERACTIONS 9.1 Naming Ions Essential Understanding certain rules. Ions are named by determining their charges and applying Reading Strategy As you read Lesson 9.1, use the concept map below. Fill in this concept map to show how to identify and name different types of ions. Ions Made of a single atom: Made of more than one atom: Positively charged ion: Negatively charged ion: The only common positive ion of this type: The names of most common negative ions of this type end in: Named by: Named by: 110
2 Name Class Date Lesson Summary Monatomic Ions A one-atom ion is called a monatomic ion. A monatomic ion s charge depends on its place in the periodic table. Atoms that lose electrons become positively charged ions, or cations. Atoms that gain electrons become negatively charged ions, or anions. Polyatomic Ions Polyatomic ions contain more than one atom and behave as a unit. Negatively charged polyatomic ions are named using a root word and an -ate or ite suffix. After reading Lesson 9.1, answer the following questions. Monatomic Ions 1. What are monatomic ions? 2. How is the ionic charge of a Group 1A, 2A, or 3A ion determined? 3. How is the ionic charge of a Group 5A, 6A, or 7A ion determined? 4. Circle the letter of the type of element that often has more than one common ionic charge. a. alkali metal b. alkaline earth metal c. transition metal d. nonmetal 5. The 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 charge, and the suffix -ic to name the cation with the charge. 7. What is a major advantage of the Stock system over the old naming system? 111
3 0 Name Class Date 8. Use the periodic table to write the name and formula (including charge) for the ion formed from each element in the table below. Element Name Formula Fluorine Calcium Oxygen Polyatomic Ions 9. What is a polyatomic ion? 10. Is the following sentence true or false? The names of polyatomic anions always end in -ide. 11. What is the difference between the sulfite and sulfate anions? 12. Look at Table 9.3. 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? 14. What three hydrogen-containing polyatomic anions are essential components of living systems? a. b. c. 15. Look at Figure 9.5. Identify each of the ions shown below. a. b. c. 112
4 9.2 Naming and Writing Formulas for Ionic Compounds Essential Understanding In writing names and formulas for ionic compounds, the cation is listed first, followed by the anion. Lesson Summary Binary Ionic Compounds Binary ionic compounds are composed of two elements, one with a positive charge and one with a negative charge. The chemical formula of a binary ionic compound includes the cation s symbol, followed by the anion s symbol, with subscripts that balance positive and negative charges. Compounds With Polyatomic Ions Ionic compounds are named by joining the cation and anion names. To indicate more than one polyatomic ion in a chemical formula, place parentheses around the polyatomic ion and use a subscript. Roman numerals indicate the oxidation number of cations having multiple possible oxidation states. After reading Lesson 9.2, answer the following questions. Binary Ionic Compounds 1. Traditionally, common names were based on some of a compound or its. 2. What is the general name for compounds composed of two elements? They are. 3. When writing the formula for any ionic compound, the charges of the ions must. 4. What are two methods for writing a balanced formula? a. b. 5. What are the formulas for the compounds formed by the following pairs of ions? a. Fe 2+, Cl b. Cr 3+, O 2 c. Na +, S 2 6. What are the formulas for these compounds? a. lithium bromide b. cupric nitride c. magnesium chloride 11
5 7. The name of a binary ionic compound is written with the name of the first, followed by the name of the. 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? 9. Write the names for these binary ionic compounds. a. PbS b. MgCl 2 c. Al 2 Se 3 Compounds With Polyatomic Ions 10. What is a polyatomic ion? 11. How do you write the formula for a compound containing a polyatomic ion? 12. Why are parentheses used to write the formula Al(OH) 3? 13. Complete the table for these ionic compounds containing polyatomic ions. Cation Anion Name Formula NH 4 + S 2 Fe 3+ iron(iii) carbonate NO 3 AgNO 3 potassium cyanide KCN 9.3 Naming and Writing Formulas for Molecular Compounds Essential Understanding is an ion, bonded together. Molecular compounds consist of nonmetal atoms, none of which Lesson Summary Binary Molecular Compounds Binary molecular compounds consist of two nonmetals. The prefixes in the name of a binary molecular compound show the number of atoms of each element in a molecule of the compound.
6 The numbers related to the prefixes are used as subscripts when writing formulas of binary molecular compounds. When naming binary molecular compounds from their formulas, the subscripts in the formulas show what prefixes to use for each nonmetal in the compound. After reading Lesson 9.3, answer the following questions. Binary Molecular Compounds 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. 3. What method is used to distinguish between different molecular compounds that contain the same elements? 4. What are the names of the following compounds? a. BF 3 b. N 2 O 4 c. P 4 S 7 5. What are the formulas for the following compounds? a. carbon tetrabromide b. nitrogen triiodide c. iodine monochloride d. tetraiodine nonaoxide Match the prefix with the number it indicates. 6. octa- 7. tetra- 8. hepta- 9. nona- a. 4 b. 7 c. 8 d. 9
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