Chemistry I: Bonding Unit Worksheet. Period Date Chemical Bonding
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1 Name Chemistry I: Bonding Unit Worksheet Period Date Chemical Bonding IONIC AND METALLIC BONDING SECTION 7.1 IONS (pages ) This section explains how to use the periodic table to infer the number of valence electrons in an atom and draw its electron dot structure. It also describes the formation of cations from metals and anions from nonmetals. Valence Electrons (pages ) 1. What are valence electrons? 2. The valence electrons largely determine the of an element and are usually the only electrons used in. 3. true or false? The group number of an element in the periodic table is related to the number of valence electrons it has. 4. What is an electron dot structure? The Octet Rule (page 188) 5. What is the octet rule? 6. Metallic atoms tend to lose their valence electrons to produce a(n) or a positively charged ion. Most nonmetallic atoms achieve a complete octet by gaining or electrons. Chemistry I: Bonding TEXT 2012 WS 1 October 12
2 Formation of Cations (pages ) 7. Write the electron configurations for these metals and circle the electrons lost when each metal forms a cation. a. Mg b. Al c. K Match the noble gas with its electron configuration. 8. argon a. 1s 2 9. helium b. 1s 2 2s 2 2p neon c. 1s 2 2s 2 2p 6 3s 2 3p krypton d. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p What is the electron configuration called that has 18 electrons in the outer energy level and all of the orbitals filled? Formation of Anions (pages ) 13. Atoms of most nonmetallic elements achieve noble-gas electron configurations by gaining electrons to become, or negatively charged ions. 14. What property of nonmetallic elements makes them more likely to gain electrons than lose electrons? 1s22s22p6 2s2 15. True or false? Elements of the halogen family lose one electron to become halide ions. Chemistry I: Bonding TEXT 2012 WS 2 October 12
3 16. How many electrons will each element gain in forming an ion? a. nitrogen b. oxygen c. sulfur d. bromine 17. Write the symbol and electron configuration for each ion from Question 19, and name the noble gas with the same configuration. a. nitride b. oxide c. sulfide d. bromide SECTION 7.2 IONIC BONDS AND IONIC COMPOUNDS (pages ) This section lists the characteristics of an ionic bond. It also describes the use of these characteristics to explain the electrical conductivity of ionic compounds when melted and when in aqueous solutions. Formation of Ionic Compounds (pages ) 18. What is an ionic bond? 19. In an ionic compound, the charges of the and must balance to produce an electrically substance.; argon 20. A chemical formula shows the types and of atoms in the smallest representative unit of a substance. 21. List the numbers and types of atoms represented by these chemical formulas. a. Fe 2 O 3 b. KMnO 4 c. CH 4 d. NH 4 NO 3 Chemistry I: Bonding TEXT 2012 WS 3 October 12
4 22. What is a formula unit? 23. Explain why the ratio of magnesium ions to chloride ions in MgCl 2 is 1: Describe the structure of ionic compounds. Properties of Ionic Compounds (pages ) 25. Most ionic compounds are at room temperature. 26. True or false? Ionic compounds generally have low melting points. 27. 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. SECTION 7.3 BONDING IN METALS (pages ) 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. Metallic Bonds and Metallic Properties (pages ) 28. True or false? Metals are made up of cations, not neutral atoms. 29. What are metallic bonds? Chemistry I: Bonding TEXT 2012 WS 4 October 12
5 30. Name three properties of metals that can be explained by metallic bonding. a. b. c. 31. What happens to an ionic crystal when a force is applied to it? Crystalline Structure of Metals (page 202) 32. Metal atoms in crystals are arranged into very and orderly pattern. COVALENT BONDING SECTION 8.1 MOLECULAR COMPOUNDS (pages ) This section explains how to distinguish between ionic and molecular compounds. Molecules and Molecular Compounds (pages ) 33. What is a covalent bond? 34. Most elements found in nature, with the exception of the exist as molecules. 3. What is a molecule? 35. Compounds that are formed when two or more atoms combine to form molecules are called. Chemistry I: Bonding TEXT 2012 WS 5 October 12
6 36. Circle the letter of the substances that do NOT exist as molecules in nature. a. oxygen b. water c. neon d. ozone e. helium 37. List two properties of molecular compounds. a. b. A covalent bond is a bond formed when two atoms share electrons. Molecular Formulas (pages ) 38. What is a molecular formula? Match each compound with its molecular formula. 39. carbon dioxide a. C 2 H ethane b. CO ammonia c. NH True or false? A molecular formula shows the arrangement of the atoms in a molecule. Chemistry I: Bonding TEXT 2012 WS 6 October 12
7 43. In the diagram, match the type of model or formula with its representation. a. ball-and-stick model b. molecular formula c. perspective drawing d. space-filling molecular NN e. structural formula SECTION 8.2 THE NATURE OF COVALENT BONDING (pages ) This section uses electron dot structures to show the formation of single, double, and triple covalent bonds. It also describes and gives examples of coordinate covalent bonding, resonance structures, and exceptions to the octet rule. The Octet Rule in Covalent Bonding (page 217) 48. How does electron sharing occur in forming covalent bonds? Single Covalent Bonds (pages ) 49. True or false? A shared pair of electrons is represented by a double dash. 50. Structural formulas show the arrangement of in molecules. 51. Use the electron dot diagram below. Circle each unshared pair of electrons in a water molecule. Double and Triple Covalent Bonds (pages ) 52. A chemical bond formed when atoms share two pairs of electrons is called a (n) Chemistry I: Bonding TEXT 2012 WS 7 October 12
8 53. How many covalent bonds are in the nitrogen molecule? 54. True or false? All diatomic molecules contain double bonds. Coordinate Covalent Bonds (pages ) 55. What is a coordinate covalent bond? 56. Look at Table 8.2 on page 224. Which two nitrogen compounds contain coordinate covalent bonds? Bond Dissociation Energies (page 226) 57. What is bond dissociation energy? Resonance (pages ) 58. The actual bonding in ozone is a of the extremes represented by its. 59. What are resonance structures? Exceptions to the Octet Rule (pages ) 60. Why does NO 2 not follow the octet rule? SECTION 8.3 BONDING THEORIES (pages ) This section describes the molecular orbital theory of covalent bonding, including orbital hybridization. It also explains the use of VSEPR theory to predict the shapes of some molecules. Molecular Orbitals (pages ) 61. What is a molecular orbital? Chemistry I: Bonding TEXT 2012 WS 8 October 12
9 VSEPR Theory (pages ) 62. What is VSEPR theory? 63. When the central atom of a molecule has unshared electrons, the bond angles will be than when all the central atom s electrons are shared. 64. What is the bond angle in carbon dioxide? Why? 65. What are the names of these common molecular shapes? Hybrid Orbitals (pages ) 66. True or false? Orbital hybridization theory can describe both the shape and bonding of molecules. 67. What is orbital hybridization? Match the hybrid orbitals formed by carbon with the carbon compound in which they are found. 68. sp 3 a. ethyne 69. sp 2 b. ethene 70. sp c. methane a Chemistry I: Bonding TEXT 2012 WS 9 October 12
10 SECTION 8.4 POLAR BONDS AND MOLECULES (pages ) This section explains the use of electronegativity values to classify a bond as nonpolar covalent, polar covalent, or ionic. It also names and describes the weak attractive forces that hold groups of molecules together. Bond Polarity (pages ) 71. True or false? Covalent bonds differ in the way electrons are shared by the bonded atoms, depending on the kind and number of atoms joined together. 72. Describe how electrons are shared in each type of bond. Write equally or unequally. a. Nonpolar bond b. Polar bond 73. Why does the chlorine atom in hydrogen chloride acquire a slightly negative charge? 74. What symbols are used to represent the charges on atoms in a polar covalent bond? The polarity of the bond? Match the electronegativity difference range with the most probable type of bond that will form a. ionic b. nonpolar covalent c. very polar covalent 78. >2.0 d. moderately polar covalent. Chemistry I: Bonding TEXT 2012 WS 10 October 12
11 Reading Skill Practice Students tables should include the basic information about the three types of hybrid You can increase your understanding of what you have read by making comparisons. orbitals A compare/contrast table can help you do this. On a separate sheet of paper, draw a table to compare the three types of hybrid orbitals as explained on pages 235 and 236. The three heads for the rows should be sp, sp 2, and sp 3. Then list the characteristics that will form the basis of your comparison above each column. The column heads should be Number of Hybrid Orbitals, Component Orbitals, Number of Bonds, and Bond Angle. 10 EC PTS Polar Molecules (pages ) 79. Circle the letter of each sentence that is true about polar molecules. a. Some regions of a polar molecule are slightly negative and some are slightly positive. b. A molecule containing a polar bond is always polar. c. A molecule that has two poles is called a dipolar molecule. d. When polar molecules are placed in an electric field, they all line up with the same orientation in relation to the charged plates. 80. Are the following molecules polar or nonpolar? a. H 2 O c. NH 3 b. CO 2 d. HCl A t t ract ions bet ween M olecules (pages ) 81. What causes dispersion? 82. Is the following sentence true or false? Dispersion forces generally increase in strength as the number of electrons in a molecule increases. Chemistry I: Bonding TEXT 2012 WS 11 October 12
12 83. The strongest of the intermolecular forces are. Intermolecular Attractions and Molecular Properties (pages ) 84. What determines the physical properties of a compound? 85. Use Table 8.4 on page 244. Complete the following table comparing ionic and covalent compounds. forces a Charact erist ic Ionic Compound Covalent Compound Representative unit Physical state Melting point Solubility in water Chemistry I: Bonding TEXT 2012 WS 12 October 12
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