1. © Copyright Pearson Prentice Hall Slide 1 of 19 Metallic Bonding How do metals bond?

2. © Copyright Pearson Prentice Hall Bonding in Metals > Slide 2 of 19 By the end of this lesson the Student shall be able to 7.3.1Model the valence electrons of metal atoms. 7.3.2Describe the arrangement of atoms in a metal. 7.3.3Explain the importance of alloys

3. © Copyright Pearson Prentice Hall Bonding in Metals > Slide 3 of 19 SC1 Students will analyze the nature of matter and its classifications. b. Identify substances based on chemical and physical properties.

4. © Copyright Pearson Prentice Hall Bonding in Metals > Slide 4 of 19 SC3 Students will use the modern atomic theory to explain the characteristics of atoms. b. Use the orbital configuration of neutral atoms to explain its effect on the atom’s chemical properties.

5. © Copyright Pearson Prentice Hall Bonding in Metals > Slide 5 of 19 Alloys are a mixture of two or more elements, at least one of which is a metal. A great example: we take iron, add carbon to it to make steel. This is the Bessemer Process.

6. © Copyright Pearson Prentice Hall Bonding in Metals > Slide 6 of 19 metallic bonds are the attraction of free-floating valence electrons for positively charged metal ions

7. © Copyright Pearson Prentice Hall Bonding in Metals > Slide 7 of 19 Metallic Bonds and Metallic Properties How can you model the valence electrons of metal atoms? Pages 201-205 7.3

8. Slide 8 of 19 © Copyright Pearson Prentice Hall Bonding in Metals > Metallic Bonds and Metallic Properties The valence electrons of metal atoms can be modeled as a sea of electrons. The valence electrons are mobile and can drift freely from one part of the metal to another. Metallic bonds consist of the attraction of the free-floating valence electrons for the positively charged metal ions. 7.3

9. Slide 9 of 19 © Copyright Pearson Prentice Hall Bonding in Metals > Metallic Bonds and Metallic Properties Metals are ductile—that is, they can be drawn into wires. 7.3

10. Slide 10 of 19 © Copyright Pearson Prentice Hall Bonding in Metals > Metallic Bonds and Metallic Properties A force can change the shape of a metal. A force can shatter an ionic crystal. 7.3

11. © Copyright Pearson Prentice Hall Slide 11 of 19 Bonding in Metals > Animation 9 Animation 9 See how metallic bonding explains some physical properties of metals.

12. © Copyright Pearson Prentice Hall Bonding in Metals > Slide 12 of 19 Crystalline Structure of Metals How are metal atoms arranged? 7.3

13. Slide 13 of 19 © Copyright Pearson Prentice Hall Bonding in Metals > Crystalline Structure of Metals These tomatoes have a closed-packed arrangement. Similar arrangements can be found in the crystalline structure of metals. 7.3

14. Slide 14 of 19 © Copyright Pearson Prentice Hall Bonding in Metals > Crystalline Structure of Metals Metal atoms are arranged in very compact and orderly patterns. 7.3

15. © Copyright Pearson Prentice Hall Bonding in Metals > Slide 15 of 19 Alloys Why are alloys important? 7.3

16. Slide 16 of 19 © Copyright Pearson Prentice Hall Bonding in Metals > Alloys Alloys are mixtures composed of two or more elements, at least one of which is a metal. Alloys are important because their properties are often superior to those of their component elements. 7.3

17. Slide 17 of 19 © Copyright Pearson Prentice Hall Bonding in Metals > Alloys Bicycle frames are often made of titanium alloys that contain aluminum and vanadium. 7.3

18. Slide 18 of 19 © Copyright Pearson Prentice Hall Bonding in Metals > Alloys The most important alloys today are steels. Steels have a wide range of useful properties, such as corrosion resistance, ductility, hardness, and toughness. 7.3

19. © Copyright Pearson Prentice Hall Slide 19 of 19 Section Quiz -or- Continue to: Launch: Assess students’ understanding of the concepts in Section 7.3 Section Quiz. 7.3.

20. © Copyright Pearson Prentice Hall Slide 20 of 19 1.The valence electrons of metals can be modeled as a.a body-centered cube. b.octets of electrons. c.a rigid array of electrons. d.a sea of electrons. 7.3 Section Quiz.

21. © Copyright Pearson Prentice Hall Slide 21 of 19 2. In most metals, the atoms are a.free to move from one part of the metal to another. b.arranged in a compact and orderly pattern. c.placed at irregular locations. d.randomly distributed. 7.3 Section Quiz.

22. © Copyright Pearson Prentice Hall Slide 22 of 19 3. Alloys are important because they a.are pure substances. b.are the ores from which metals can be refined. c.can have properties superior to those of their components. d.are produced by the combustion of metals. 7.3 Section Quiz.

23. © Copyright Pearson Prentice Hall Slide 23 of 19 Bonding in Metals > Concept Map 7 Concept Map 7 Solve the Concept Map with the help of an interactive guided tutorial.

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