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1 Section 6.4 Metallic BondingPre-AP Chemistry 2 Chapter 6 Objectives Section 4 Metallic BondingDescribe the electron-sea model of metallic bonding, and explain why metals are good electrical conductors. Explain why metal surfaces are shiny. Explain why metals are malleable and ductile but ionic-crystalline compound are not. 3 Sec 6.4 Vocabulary metallic bonding malleability ductility 4 Properties of Substances with Metallic, Ionic, and Covalent BondsChapter 6 Section 4 Metallic Bonding Properties of Substances with Metallic, Ionic, and Covalent Bonds 5 Metallic Bonds are… How metal atoms are held together in the solid.Metals hold on to their valence electrons very weakly. Think of them as positive ions (cations) floating in a sea of electrons 6 Sea of Electrons + Electrons are free to move through the solid.Metals conduct electricity. + 7 Chapter 6 Section 4 Metallic Bonding Metallic BondingChemical bonding is different in metals than it is in ionic, molecular, or covalent-network compounds. The unique characteristics of metallic bonding gives metals their characteristic properties, listed below. electrical conductivity thermal conductivity malleability ductility shiny appearance (luster) 8 Why metals are Shiny metals are strong absorbers and reflectors of light absorption of light excites metals electrons to higher energy levels electrons immediately fall emitting energy at same frequency as absorbed (reflection of light) 9 Chapter 6 Section 4 Metallic Bonding Metallic Bonding, continued Malleability is the ability of a substance to be hammered or beaten into thin sheets. Ductility is the ability of a substance to be drawn, pulled, or extruded through a small opening to produce a wire. 10 Metals are Malleable Hammered into shape (bend). Also ductile - drawn into wires. Both malleability and ductility explained in terms of the mobility of the valence electrons (sea of electrons) 11 Due to the mobility of the valence electrons, metals have:Notice that the ionic crystal breaks due to ion repulsion! 1) Ductility 2) Malleability and 12 Malleable + Force 13 Malleable + + + + Force + + + + + + + +Mobile electrons allow atoms to slide by, sort of like ball bearings in oil. + + + + Force + + + + + + + + 14 Metallic properties.. The valence electrons of metal atoms can be modeled as a sea of electrons. metals are.. a) good conductors of electric current b) ductile and malleable which explains the mobility of valence e- 15 Ionic solids are brittleForce + - 16 Ionic solids are brittleStrong Repulsion breaks a crystal apart, due to similar ions being next to each other. + - Force + - + - + - 17 Chapter 6 Section 4 Metallic Bonding The Metallic-Bond ModelIn a metal, the vacant orbitals in the atoms outer energy levels overlap. This overlapping of orbitals allows the outer electrons of the atoms to roam freely throughout the entire metal. The electrons are delocalized, which means that they do not belong to any one atom but move freely about the metals network of empty atomic orbitals. These mobile electrons form a sea of electrons around the metal atoms, which are packed together in a crystal lattice. 18 Chapter 6 The Metallic-Bond Model, continuedSection 4 Metallic Bonding The Metallic-Bond Model, continued The chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons is called metallic bonding. 19 20 Chapter 6 Objectives Section 4 Metallic BondingDescribe the electron-sea model of metallic bonding, and explain why metals are good electrical conductors. Explain why metal surfaces are shiny. Explain why metals are malleable and ductile but ionic-crystalline compound are not. 21 End of Sec 6.4 Name ___________________________ Class ___________________ Date_____________Chapter 6 Chemical BondsPearson Education, Inc.,publishingas PearsonPrentice Hall. All rights reserved.Physical Science Reading and Study Workbook Level B Chapter 665IPLSName ___________________________ Class ___________________ Date_____________Chapter 6 Chemical BondsPearson Education, Inc.,publishingas PearsonPrentice Hall. All rights reserved.Section 6.4 The Structure of Metals(pages 176181)This section discusses metallic bonds and the properties ofmetals. It also explainshow the properties of an alloy arecontrolled.Reading Strategy (page 176)Relating Cause and Effect As youread, complete the concept map to relatethe structure of metals totheir properties. For more information on thisReading Strategy, seethe Reading and Study Skills in the Skills andReference Handbook atthe end of your textbook.Metallic Bonds (pages 176177)1. Circle the letter of the metalwith the highest melting point.a. goldb. titaniumc. tungsten2. Is the following sentence true or false? The properties of ametal arerelated to bonds within the metal.3. Define a metallic bond.4. Use the words in the box below to fill in the blanks.anions orbitalscations valence electronsThe cations in a metal form a lattice. The lattice is held inplace by strongmetallic bonds between the and the surrounding them.5. Is the following sentence true or false? The more valenceelectrons ametal has, the stronger its metallic bonds will be.Mobileelectrons produce0055_hsps09_GRSW_Ch06.qxd 72707 3:24 PM Page 65Name ___________________________ Class ___________________ Date_____________Chapter 6 Chemical BondsPearson Education, Inc., publishing as Pearson Prentice Hall.All rights reserved.66 Physical Science Reading and Study Workbook Level B Chapter6IPLSName ___________________________ Class ___________________ Date_____________Chapter 6 Chemical BondsPearson Education, Inc., publishing as Pearson Prentice Hall.All rights reserved.Explaining Properties of Metals (page 177)6. Some of theproperties of metals can be explained by theof the electrons within a metal lattice. Circle the correctanswer.mobility malleability conductivity7. Circle important properties of metals that can be explainedby metallicbonding.a. ability to conduct electric currentb. malleabilityc.ductilityAlloys (pages 178181)8. Define an alloy.9. Circle the letter of the sentences that correctly compare thehardness andstrength of bronze to the hardness and strength ofcopper alone and tinalone.a. Copper is stronger than bronze.b. Tin is stronger thanbronze.c. Bronze is stronger than copper.10. Circle the factor(s) that scientists can vary to designalloys with specificproperties.a. the types of elements in the alloyb. the amounts of elementsin the alloyc. the temperature of elements in the alloy11. When carbon is added to iron, the lattice becomes andthan a lattice that contains only iron.12. Circle the letters ofthe elements that all types of steel contain.a. carbon b. chromium c. iron13. Circle the letter(s) of each correct description ofstainless steel.a. Stainless steel contains more carbon than chromium.b.Chromium forms an oxide that protects stainless steel fromrusting.c. Stainless steel is more brittle than steels that containmore carbon.0055_hsps09_GRSW_Ch06.qxd 72707 3:24 PM Page 66
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