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Table of Contents

Table of Contents. Chapter Preview 5.1 Atoms, Bonding, and the Periodic Table 5.2 Ionic Bonds 5.3 Covalent Bonds 5.4 Bonding in Metals. Chapter Preview Questions. 1. The atom is made of protons, electrons, and a. valence electrons. b. neutrons. c. molecules. d. ions.

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Table of Contents

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  1. Table of Contents • Chapter Preview • 5.1 Atoms, Bonding, and the Periodic Table • 5.2 Ionic Bonds • 5.3 Covalent Bonds • 5.4 Bonding in Metals

  2. Chapter Preview Questions • 1. The atom is made of protons, electrons, and • a. valence electrons. • b. neutrons. • c. molecules. • d. ions.

  3. Chapter Preview Questions • 1. The atom is made of protons, electrons, and • a. valence electrons. • b. neutrons. • c. molecules. • d. ions.

  4. Chapter Preview Questions • 2. Reactant atoms and molecules interact to form products with • a. identical physical properties. • b. different physical properties. • c. identical chemical properties. • d. different chemical properties.

  5. Chapter Preview Questions • 2. Reactant atoms and molecules interact to form products with • a. identical physical properties. • b. different physical properties. • c. identical chemical properties. • d. different chemical properties.

  6. Chapter Preview Questions • 3. In chemical reactions, the number of atoms • a. varies according to the elements involved. • b. changes from one reactant to another. • c. stays the same. • d. depends on atom arrangement.

  7. Chapter Preview Questions • 3. In chemical reactions, the number of atoms • a. varies according to the elements involved. • b. changes from one reactant to another. • c. stays the same. • d. depends on atom arrangement.

  8. Chapter Preview Questions • 4. Compounds are formed by • a. combining two or more different elements. • b. bombarding atoms with high-speed particles. • c. combining two or more different nuclei. • d. dissolving a solid in a liquid.

  9. Chapter Preview Questions • 4. Compounds are formed by • a. combining two or more different elements. • b. bombarding atoms with high-speed particles. • c. combining two or more different nuclei. • d. dissolving a solid in a liquid.

  10. Water is a compound made from • the elements hydrogen and • oxygen. How do the properties • of water differ from those of the • elements that it is made up of? How do compounds form?

  11. High-Use Academic Words v. To allow something to travel along or through it Metal strips on a circuit board conduct electric current. conduct

  12. High-Use Academic Words adj. Not easily or quickly changed from one state to another Gold is a stable metal that does not rust or tarnish. stable

  13. High-Use Academic Words n. The way in which parts of something are put together. The outside structure of the building is made of brick and concrete. structure

  14. High-Use Academic Words n. A written sign that stands for something else. The symbol for the element oxygen is O. symbol

  15. Apply It! Choose the word that best completes the sentence. 1. “H” is the for hydrogen. symbol 2. The of an atom consists of a nucleus of protons and neutrons, surrounded by a cloud of moving electrons. structure 3. Platinum jewelry lasts a long time because the metal is very . stable

  16. End of Chapter Preview

  17. Section 1:Atoms, Bonding, and the Periodic Table • How is the reactivity of elements related to valence electrons in atoms? • What does the periodic table tell you about the atoms of elements?

  18. Valence Electrons and Bonding • The number of valence electrons in an atom of an element determines many properties of that element, including the ways in which the atom can bond with other atoms.

  19. How the Periodic Table Works • The periodic table reveals the underlying atomic structure of atoms, including the arrangement of the electrons.

  20. Periodic Table Activity • Click the Active Art button to open a browser window and access Active Art about the periodic table.

  21. The Periodic Table • As the atomic number increases, the number of electrons also increases. As a result, the properties of the elements change in a regular way across a period.

  22. End of Section:Atoms, Bonding, and the Periodic Table

  23. Section 2:Ionic Bonds • How do ions form bonds? • How are the formulas and names of ionic compounds written? • What are the properties of ionic compounds?

  24. Ions and Ionic Bonds • You and a friend walk past a market that sells apples for 40 cents each and pears for 50 cents each. You have 45 cents and want an apple. Your friend also has 45 cents but wants a pear.

  25. Ions and Ionic Bonds • When an atom loses one of its electrons, it becomes a positively charged ion. The atom that gains the electron becomes a negatively charged ion.

  26. Ions and Ionic Bonds • Ions are atoms or groups of atoms that have lost or gained electrons.

  27. Ions and Ionic Bonds • Ionic bonds form as a result of the attraction between positive and negative ions.

  28. Properties of Ionic Compounds • In general, ionic compounds are hard, brittle solids with high melting points. When melted or dissolved in water, they conduct electric current.

  29. Links on Ionic Compounds • Click the SciLinks button for links on ionic compounds.

  30. Salt • Click the Video button to watch a movie about salt.

  31. End of Section:Ionic Bonds

  32. Section 3:Covalent Bonds • What holds covalently bonded atoms together? • What are the properties of molecular compounds? • How does unequal sharing of electrons affect molecules?

  33. How Covalent Bonds Form • The force that holds atoms together in a covalent bond is the attraction of each atom’s nucleus for the shared pair of electrons.

  34. How Covalent Bonds Form • The oxygen atom in water and the nitrogen atom in ammonia each have eight valence electrons as a result of forming covalent bonds with hydrogen atoms.

  35. How Covalent Bonds Form • Double and triple bonds can form when atoms share more than one pair of electrons.

  36. Comparing Molecular and Ionic Compounds • The table compares the melting points and boiling points of a few molecular compounds and ionic compounds. Use the table to answer the following questions.

  37. Check that the graphs are correctly set up and labeled before students plot the data. Graphing: Create a bar graph of just the melting points of these compounds. Arrange the bars in order of increasing melting point. The y-axis should start at –200ºC and go to 900ºC. Comparing Molecular and Ionic Compounds

  38. Melting points of molecular compounds are lower than those of ionic compounds. Interpreting Data: Describe what your graph reveals about the melting points of molecular compounds compared to those of ionic compounds. Comparing Molecular and Ionic Compounds

  39. Molecular compounds have weak attractive force between molecules compared to those between ions, so less energy is needed to melt molecular compounds. Inferring: How can you account for the differences in melting points between molecular compounds and ionic compounds? Comparing Molecular and Ionic Compounds

  40. Boiling points of molecular compounds are lower than those of ionic compounds. Interpreting Data: How do the boiling points of the molecular and ionic compounds compare? Comparing Molecular and Ionic Compounds

  41. Students may predict that ammonia is a molecular compound because it has relatively low melting and boiling points. Predicting: Ammonia’s melting point is –78ºC and its boiling point is –34ºC. Is ammonia a molecular compound or an ionic compound? Explain. Comparing Molecular and Ionic Compounds

  42. Unequal Sharing of Electrons • Fluorine forms a nonpolar bond with another fluorine atom. In hydrogen fluoride, fluorine attracts electrons more strongly than hydrogen does, so the bond formed is polar.

  43. Unequal Sharing of Electrons • A carbon dioxide molecule is a nonpolar molecule because of its straight-line shape. In contrast, a water molecule is a polar molecule because of its bent shape.

  44. Links on Molecular Compounds • Click the SciLinks button for links on molecular compounds.

  45. End of Section:Covalent Bonds

  46. Section 4:Bonding in Metals • How do the properties of metals and alloys compare? • How do metal atoms combine? • How does metallic bonding result in useful properties of metals?

  47. Metallic Bonding • Metal atoms combine in regular patterns in which the valence electrons are free to move from atom to atom.

  48. Metallic Properties • The “sea of electrons” model of solid metals explains their ability to conduct heat and electricity, the ease with which they can be made to change shape, and their luster.

  49. Links on Metallic Bonding • Click the SciLinks button for links on metallic bonding.

  50. End of Section:Bonding in Metals

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