Chapter Six Chemical Names and Formulas WS C U1C6 Name Period Section 6.1 Part I: Matching. Match the definition with the term that best correlates to it. No definition will be used more than once. 1. Anion 2. Cation 3. Ion 4. Ionic compound 5. Molecular compound 6. Molecule A) Neutral atom that loses or gains electrons B) Smallest electrically neutral unit of a substance that maintains all the properties of the substance C) Compound composed of molecules D) Positively charged ion E) Negatively charged ion F) Compound composed of ions Part II: Short Answer. Answer the following questions. Give the name and symbol of the ion formed when the following neutral atom experiences the stated behavior. 7. a chlorine atom gains one electron Name: Symbol: 8. a potassium atom loses one electron Name: Symbol: 9. an aluminum atom loses three electrons Name: Symbol: 10. an oxygen atom gains two electrons Name: Symbol: page 1 WS C U1C6
Complete the following table. Name of ion/atom Chloride ion Sulfide ion Classification (check the correct one) 11. Cation 16. Cation 21. Cation Neutral Atom Water 25. Cation 26. 27. Cation 31. 32. Cation Oxide ion 36. Cation Number of electrons gained (if Overall charge (including + or Number of Symbol/ formula electrons lost (if any) any) sign) 12. 13. 14. 15. 17. 18. 19. 20. Ca 22. 23. 24. H 2 O 0 0 0 Sr 2+ Na + O 2 28. 29. 30. 33. 34. 35. 37. 38. 39. 40. What types of elements tend to form molecular compounds? page 2 WS C U1C6
Section 6.2 Part I: Matching. Match the definition with the term that best correlates to it. No definition will be used more than once. 1. Chemical formula 2. Formula unit 4. Law of Multiple Proportions 5. Molecular formula 3. Law of Definite Proportions A) Chemical formula for a molecular compound B) Chemical formula for an ionic compound C) In any sample of a compound, the masses of the elements are always in the same proportions D) Shows the kinds and numbers of atoms in the smallest representative unit of a substance E) Whenever 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 the ratio of small whole numbers. Part II: Short Answer. Answer the following questions. Classify each of the following chemical formulas as a molecular formula or a formula unit by circling the choice that best describes it. 6. NaBr: molecular formula formula unit 7. CaCl 2 : molecular formula formula unit 8. C 2 H 6 : molecular formula formula unit 9. CCl 4 : molecular formula formula unit 10. H 2 O: molecular formula formula unit Identify the number and kinds of atoms present in a molecule of each compound. 11. Citric acid (C 6 H 8 O 7 ): 12. Chloroform (CHCl 3 ): page 3 WS C U1C6
13. Glycine (C 2 H 5 NO 2 ): 14. Mr. Geist s breath (CH 4 ): 15. Jolly Rancher s candy main component (C 12 H 22 O 11 ): Section 6.3 Short Answer. Answer the following questions. Using only the periodic table, name and write the formula for the typical ion of each of the following representative elements. 1. Potassium: 7. Oxygen: 2. Sulfur: 8. Nitrogen: 3. Bromine: 9. Beryllium: 4. Barium: 10. Fluorine: 5. Aluminum: 11. Sodium: 6. Strontium: 12. Magnesium: page 4 WS C U1C6
Write the formula (including charge) for each ion. 13. Nitrite: 16. Permanganate: 14. Sulfite: 17. Cyanide: 15. Acetate: 18. Chromate: 19. Explain what is meant by a polyatomic ion. Section 6.4 Short Answer. Answer the following questions. Name the following compounds. 1. MgSO 4 2. FeBr 3 3. Na 2 Cr 2 O 7 4. Mg 3 (PO 4 ) 2 5. KClO 6. Al(OH) 3 page 5 WS C U1C6
7. NH 4 Cl 8. Fe(OH) 3 9. Cr(SO 4 ) 3 10. NaF Write the formula of the compound. 11. Chromium (III) nitrite 12. Sodium perchlorate 13. Magnesium hydrogen carbonate 14. Lithium phosphate 15. Barium nitrate 16. Magnesium hydroxide 17. Copper (III) carbonate page 6 WS C U1C6
18. Copper (II) phosphate 19. Iron (III) carbonate 20. Sodium oxide 21. When are parentheses used in writing a chemical formula? Section 6.5 Short Answer. Answer the following questions. Name the following compounds. 1. PCl 3 2. SO 2 3. P 4 S 10 4. NO 2 5. HBr (acid) page 7 WS C U1C6
6. CCl 4 7. XeF 2 8. N 2 F 2 9. Cl 2 O 7 10. CO Write the formula of the compound. 11. Nitrogen tribromide 12. Dichlorine monoxide 13. Sulfur dioxide 14. Dinitrogen tetrafluoride 15. Hydrofluoric acid 16. Nitric acid 17. Sulfuric acid page 8 WS C U1C6
18. Carbon tetrabromide 19. Dinitrogen tetroxide 20. Carbon dioxide Section 6.6 Part I: Short Answer. Answer the following questions. Name the following compounds. 1. CuCl 2 2. MnO 2 3. Li 3 N 4. SrBr 2 5. SnCl 2 6. K 2 S 7. NBr 3 page 9 WS C U1C6
8. (NH 4 ) 2 SO 4 9. MgSO 4 10. KNO 3 Write the formula of the compound. 11. Potassium sulfide 12. Sulfur hexafluoride 13. Tin (IV) chloride 14. Aluminum fluoride 15. Magnesium chloride 16. Dihydrogen sulfide 17. Iron (III) carbonate 18. Barium phosphate 19. Calcium oxide page 10 WS C U1C6
20. Chromium (III) sulfate 21. Potassium iodide 22. Ammonium sulfate Part II: Table Completion. OH (23) Complete the following table by writing in the chemical formulas next to and names for the compounds formed by combining the indicated positive and negative ions next to. Ca 2+ Al 3+ Na + Pb 4+ (27) (31) (35) (24) (28) (32) (36) PO 4 3 (25) (29) (33) (37) (26) (30) (34) (38) page 11 WS C U1C6