Chapter 9 The Chemical Bond and Intermolecular Forces Section Review 9.1
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1 Name Date Chemistry Precision and Design Concept Review Chapter 9 The Chemical Bond and Intermolecular Forces Section Review Give three properties of ionic compounds and three properties of molecular compounds. Ionic compounds a. b. c. Molecular compounds a. b. c. 2. What is the octet rule? Why might this principle be considered the driving force that causes elements to react to form chemical bonds? 3. Define ionic bond. Chapter 9 The Chemical Bond and Intermolecular Forces 1
2 4. Define covalent bond. 5. Give two examples of covalent networks. a. b. 6. What is a metallic bond? Application 1. a. Write Lewis structures of calcium and fluorine atoms. b. If Ca and F are allowed to react, what will be the Lewis structures of the resultant ions? c. Show the reaction between Ca and F atoms by using Lewis structures. 2. Which of the following compounds would you expect to contain ionic bonds? Which one of these compounds would you expect to have the most ionic character? SrI 2 SO 2 Li 2 O BrCl CsF CaCl 2 Chapter 9 The Chemical Bond and Intermolecular Forces 2
3 3. Draw Lewis structures for each of the following. a. an iodine atom b. an iodine molecule c. an HI molecule 4. Predict what type of bonding predominates in each of the following. Bonding a. AsCl 2 g. MnF 2 Bonding b. LiBr h. HCN c. CuNi i. Al 2 O 3 d. SO 2 j. KCl e. XeF 6 k. O 2 f. Fe l. Cr 5. Indicate whether the bonds between the following atoms are polar or nonpolar bonds. Polar Nonpolar a. Si-Si e. Cl-F Polar - Nonpolar b. H-O f. Cl-Cl c. C-H g. N-H d. C-O j. O-O Chapter 9 The Chemical Bond and Intermolecular Forces 3
4 Name Date Chemistry Precision and Design Concept Review 1. What are delocalized electrons? Section Review What term refers to a situation in which electrons are shared by more than two atoms? 3. What is meant when a molecule is described as being polar? Application 1. What shape would you expect a molecule based on an atom with only two bonding pairs of electrons to have? Three bonding pairs? Four? 2. What conditions must exist for a polyatomic molecule to be nonpolar? Chapter 9 The Chemical Bond and Intermolecular Forces 4
5 tetrahedral 3. Based on the Lewis structures you have already studied and the group similarities of the elements, give the Lewis structure and shape of each of the following molecules: Lewis Structure Shape Lewis Structure Shape SiH 4 SeCl 2 AlF 3 O 3 H 2 S PI 3 HBr CCl 4 Chapter 9 The Chemical Bond and Intermolecular Forces 5
6 Name Date Chemistry Precision and Design Section Review 9.3 Concept Review 1. How are intermolecular forces different from chemical bonds? 2. Explain the dipole-dipole force. 3. What causes London forces? 4. Explain the difference between hydrogen bonds and dipole-dipole forces. Application Tell which intermolecular force(s) would exist between molecules of the following substances. a. H 2 S (polar) b. H 2 O c. O 2 d. SiH 4 (nonpolar) e. HCl f. CH 3 Cl (polar) g. CO 2 (nonpolar) h. NH 3 Chapter 9 The Chemical Bond and Intermolecular Forces 6
7 Name Date Chemistry Precision and Design Section Review Distinguish between amorphous and crystalline solids and give an example of each. 2. What is a unit cell? 3. What types of close-packed unit cells do most metals assume? 4. In what ways does a liquid crystal have characteristics of both liquids and solids? Chapter 9 The Chemical Bond and Intermolecular Forces 7
8 Name Date Chemistry Precision and Design Questions 1. What is a chemical bond? Chapter Review 2. State the octet rule. 3. How do ionic and covalent bonds differ in the electron rearrangements involved? 4. What is the difference between single, double, and triple covalent bonds? 5. Why do covalent networks such as diamond and silicon carbide tend to be very hard? 6. What is the primary difference between covalent and metallic bonding? 7. What type of covalent bond forms a dipole? 8. What are delocalized electrons? Chapter 9 The Chemical Bond and Intermolecular Forces 8
9 9. How is resonance indicated when drawing Lewis structures? 10. How does an intermolecular force differ from a chemical bond? 11. Which type of intermolecular force is the strongest? Which type is the weakest? 12. Name the only intermolecular force that affected nonpolar molecules. 13. What is the difference between crystalline and amorphous solids at the molecular level? How does this affect the properties of the substances? 14. What are the three main types of cubic unit cells? Which one is also called cubic close package? a. b. c. Chapter 9 The Chemical Bond and Intermolecular Forces 9
10 Problems 1. Predict what type of bonding predominates in each of the following substances. a. I 2 b. V c. CsI d. NaF e. CO 2 f. Fe 3 Al 2. Draw the Lewis structure and predict the shape of antimony trichloride, (SbCl 3 ). 3. Which types of intermolecular forces exist in a liquid made up of each of the following molecules? a. H H Ge H H b. F O H c. Cl O Cl Chapter 9 The Chemical Bond and Intermolecular Forces 10
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