KEY-FinalExamStudyGuide_Fall2013

Recommendations

Info

Name ___________________________ Date ___________________ Class __________________ CHAPTER 7, Ionic and Metallic Bonding (continued) 4. Why do beryllium and fluorine combine in a 1 : 2 ratio? They combine in a 1 : 2 ratio because each beryllium atom gives up two electrons, but each fluorine atom only accepts one electron. Therefore, two fluorine atoms are needed to react with each beryllium atom. 5. A chemical formula shows the types and ______________________ numbers of atoms in the smallest representative unit of a substance. 6. List the numbers and types of atoms represented by these chemical formulas. a. Fe 2 O 3 _____________________________________________________________________ 2 atoms of iron, 3 atoms of oxygen b. KMnO 4 ___________________________________________________________________ 1 atom of potassium, 1 atom of manganese, 4 atoms of oxygen c. CH 3 ______________________________________________________________________ 1 atom of carbon, 4 atoms of hydrogen d. NH 4 NO 3 __________________________________________________________________ 2 atoms of nitrogen, 4 atoms of hydrogen, 3 atoms of oxygen 7. What is a formula unit? A formula unit is the lowest whole-number ratio of ions in an ionic compound. 8. Explain why the ratio of magnesium ions to chloride ions in MgCl 2 is 1 : 2. There must be twice as many chloride ions (Cl – ) to balance the magnesium ions (Mg 2+ ) to form an electrically neutral compound. 9. Describe the structure of ionic compounds. Ionic compounds exist as collections of positively and negatively charged ions arranged in repeating three-dimensional patterns. Properties of Ionic Compounds (pages 196–198) 10. Most ionic compounds are _____________________________ crystalline solids at room temperature. 11. Is the following sentence true or false? Ionic compounds generally have low melting points. _________________ false 12. What does a coordination number tell you? It is the number of ions of opposite charge that surround an ion in a crystal. 13. What is the coordination number of the ions in a crystal of NaCl? _________________ 6 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 62 Guided Reading and Study Workbook
Name ___________________________ Date ___________________ Class __________________ 14. Circle the letter of each statement that is true about ionic compounds. a. When dissolved in water, ionic compounds can conduct electricity. b. When melted, ionic compounds do not conduct electricity. c. Ionic compounds have very unstable structures. d. Ionic compounds are electrically neutral. Reading Skill Practice By looking carefully at photographs and drawings in textbooks, you can better understand what you have read. Look carefully at Figure 7.9 on page 197. What important idea does this drawing communicate? Do your work on a separate sheet of paper. The shape of a crystalline solid depends on the composition of the ionic compound that forms the crystal. Different combinations of ions produce different repeating three-dimensional patterns. SECTION 7.3 BONDING IN METALS (pages 201–203) This section uses the theory of metallic bonds to explain the physical properties of metals. It also describes the arrangements of atoms in some common metallic crystal structures. © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Metallic Bonds and Metallic Properties (pages 201–202) 1. Is the following sentence true or false? Metals are made up of cations, not neutral atoms. _________________ true 2. What are metallic bonds? Metallic bonds are the forces of attraction between free-floating valence electrons and positively charged metal ions. 3. Name three properties of metals that can be explained by metallic bonding. a. b. c. electrical conductivity ductility malleability 4. What happens to an ionic crystal when a force is applied to it? The force tends to push ions of like charge into contact. They repel each other and the crystal shatters. Crystalline Structure of Metals (page 202) 5. Metal atoms in crystals are arranged into very ____________________ compact and orderly patterns. Chapter 7 Ionic and Metallic Bonding 63
Page 1 and 2:
Leaming-Focused® Notebook ©2005 L
Page 3 and 4: Name ___________________________ Da
Page 5 and 6: Name ___________________________ Da
Page 7 and 8: Name ______________________________
Page 9 and 10: Name ___________________________ Da
Page 11 and 12: Name ___________________________ Da
Page 13 and 14: Name ___________________________ Da
Page 15 and 16: Name ___________________________ Da
Page 17 and 18: Name ___________________________ Da
Page 19 and 20: Name ___________________________ Da
Page 21 and 22: Name ___________________________ Da
Page 23 and 24: Leaming-Focused® Notebook ©2005 L
Page 25 and 26: Name ___________________________ Da
Page 27 and 28: Name ___________________________ Da
Page 29 and 30: Name ___________________________ Da
Page 31 and 32: Name ___________________________ Da
Page 33 and 34: Name ___________________________ Da
Page 35 and 36: Name ______________________________
Page 37 and 38: Name ___________________________ Da
Page 39 and 40: Name ___________________________ Da
Page 41 and 42: Name ___________________________ Da
Page 43 and 44: Name ___________________________ Da
Page 45 and 46: Name ___________________________ Da
Page 47 and 48: Name ___________________________ Da
Page 49 and 50: Name ___________________________ Da
Page 51 and 52: Name ___________________________ Da
Page 53: Name ___________________________ Da
Page 57 and 58: Name ___________________________ Da
Page 59 and 60: Name ___________________________ Da
Page 61 and 62: Name ___________________________ Da
Page 63 and 64: Name ___________________________ Da
Page 65 and 66: Name ___________________________ Da
Page 67 and 68: Name ___________________________ Da
Page 69 and 70: Name ___________________________ Da
Page 71 and 72: Name ___________________________ Da
Page 73 and 74: Name ___________________________ Da
Page 75 and 76: Name ___________________________ Da
show all

KEY-FinalExamStudyGuide_Fall2013

You also want an ePaper? Increase the reach of your titles

Delete template?

Save as template?