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Ionic and Metallic Bonding

Ionic and Metallic Bonding. Chapter 7 Concepts and Applications. Valence Electrons. Electrons in the highest occupied energy level Determines the properties of an element Inner electrons are called kernel electrons.

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Ionic and Metallic Bonding

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  1. Ionic and Metallic Bonding Chapter 7 Concepts and Applications

  2. Valence Electrons • Electrons in the highest occupied energy level • Determines the properties of an element • Inner electrons are called kernel electrons

  3. The number of valence electrons are determined by the electron configuration of an atom.

  4. The number of valence electrons are determined by the electron configuration of an atom. • 1s1 • 1s2 • 1s22s1 • 1s22s2 • 1s22s22p1 • 1s22s22p2 • 1s22s22p3 • 1s22s22p4 • 1s22s22p5 • 1s22s22p6 • 1s22s22p63s1 • 1s22s22p63s23p6 • 1s22s22p63s23p64s23d7 • 1s22s22p63s23p64s23d104p3 • 1s22s22p63s23p64s23d104p65s24d9

  5. 1s22s22p63s23p64s23d104p65s24d105p66s24f14 • 1s22s22p63s23p64s23d104p65s24d105p66s24f14 5d8 • 1s22s22p63s23p64s23d104p65s24d105p66s24f14 5d106p1 • [Ne]3s23p2 • [Ar]4s23d104p1 • [Kr]5s24d3 • [Xe]6s24f145d10 • [Rn] 7s1

  6. Lewis Dot Diagrams

  7. The Octet Rule • When forming compounds, atoms achieve the electron configuration of a noble gas (ns2np6) • Metal atoms lose electrons producing cations (positive) • Nonmetal atoms gain electrons producing anions (negative)

  8. Formation of the Sodium Cation Na1+ • Sodium has 3 energy levels. 1s22s22p63s1 • The third energy level has 1 valence electron. • To be stable (have 8 valence electrons )it can • give away the only electron it has in the third energy level OR • receive 7 more electrons from other atoms • Giving away 1 electron is more favorable than receiving 7 more—Why? • Sodium will lose 1 electron • 10 electrons and 11 protons. • Na 1+ • Na - 1e --> Na1+

  9. Other Cations • Calcium • Cobalt • Aluminum

  10. Cation Generalizations • Alkali Metals (Column 1) 1+ • Alkaline Earth Metal (Column 2) 2+ • Transition Metals 1+, 2+, 3+, 4+ • Rare Earth Metals 1+, 2+, 3+, 4+ • The name of the cation is the same as the name of the neutral atom

  11. Oxygen has 2 energy levels 1s22s22p4.  The 2rd energy level has 6 valence electrons. To be stable it can give away all the 6 electrons on the second orbit OR receive 2 more electrons from another atom. Gaining 2 electrons is more favorable than giving away 6—Why? This makes oxygen to have a negative charge. O + 2e --> O 2- Formation of the Oxygen Anion O2-

  12. Other Anions • Chlorine • Nirogen

  13. Anion Generalizations • Nitrogen Group (Column 15) 3- • Alkaline Earth Metal (Column 16) 2- • Halogens (Column 17) 1- • The name of the anion you change the ending of the atom’s name to –ide • Chloride • Fluoride • Oxide

  14. Complete the following table

  15. Complete the following table

  16. Formation of Ionic Compounds • Cation + Anion • Metal + Nonmetal • Rule: net charge of the compound is zero! - +

  17. Example: Na gives Cl one electron and now both atoms are stable Na 1+ Cl1-

  18. Mg and N? • Mg3N2 • magnesium nitride

  19. Naming Simple Ionic Compounds • Rules • Cation always comes first, name does not change • Anion is second, end of name becomes –ide • Net Charge of compound is zero • Practice—Write formulas and names • Al and Cl • Mg and S • K and O • Li and P

  20. Ionic Compounds • Usually composed of metallic cations and nonmetallic anions • Electrons are “transferred” from one element to another • Are electrically neutral Na 1+ + Cl 1- NaCl Ca 2+ + 2(Cl 1-)  CaCl2 Al 3+ + 3(O 2-)  Al2O3

  21. Formation of Ionic Compounds http://dl.clackamas.cc.or.us/ch104-07/images/8ionform.JPG

  22. Formation of Ionic Compounds Na 1+ + F 1- NaF

  23. Properties of Ionic Compounds • Form crystal lattices • Repeating three dimensional patterns • Vast array of ions in a simple whole number ratio • Relatively stable structures • High melting points • Can conduct electric currents when melted or dissolved in water • Will shatter if impacted or crushed

  24. Crystalline Shapes http://www.seas.upenn.edu/~chem101/sschem/bravais.gif

  25. Crystals Found in Nature http://www.tufts.edu/as/engdept/resources/Prof_Pages/images/crystals.jpg

  26. Crystals Found in Nature http://www.xtal.tsinghua.edu.cn/research/crystals.jpg

  27. Most Abundant Ions in the Oceans http://research.haifa.ac.il/~maritime/departm/lessons/ocean/wwr151.gif

  28. Polyatomic Ions • Two or more atoms covalently bonded together that will gain or lose electrons to become stable.

  29. http://www.iun.edu/~cpanhd/C101webnotes/chemical-nomenclature/images/polyions.jpghttp://www.iun.edu/~cpanhd/C101webnotes/chemical-nomenclature/images/polyions.jpg

  30. Metallic Bonds and Properties • Valence electrons are like a “sea of electrons” -mobile -can drift freely between metallic atoms • Bonds formed hold metals together • Therefore metals have the following characteristics….

  31. Structure of Metallic Crystals http://www.ndt-ed.org/EducationResources/CommunityCollege/Materials/Graphics/MetallicBonding/Metalbond5.gif

  32. Crystalline Structure of Metals http://images.google.com/imgres?imgurl=http://www.mandarava.com/a1grph/Mgph/M_graphics/MSPC3038.jpg&imgrefurl=http://www.mandarava.com/Retail/Metallic_crystal_specimens.htm&h=162&w=159&sz=7&tbnid=_8NTUzweSjwJ:&tbnh=92&tbnw=90&hl=en&start=3&prev=/images%3Fq%3Dmetallic%2Bcrystals%26svnum%3D10%26hl%3Den%26lr%3D%26sa%3DN

  33. Structure of Metallic Crystals http://www.ndt-ed.org/EducationResources/CommunityCollege/Materials/Graphics/MetallicBonding/Metalbond5.gif

  34. Ductility http://images.google.com/imgres?imgurl=http://www.mykonosbeads.com/images/nickel_findings.jpg&imgrefurl=http://www.mykonosbeads.com/docs/metal.htm&h=375&w=342&sz=26&tbnid=Dql2VD8x0vgJ:&tbnh=118&tbnw=107&hl=en&start=21&prev=/images%3Fq%3Dmetal%2Bjewelry%26start%3D20%26svnum%3D10%26hl%3Den%26lr%3D%26sa%3DN

  35. Malleability http://www.hearthsong.com/assets/images/hearthsong/images/shop/catalog/724137.jpg

  36. Conductivity http://lib1.store.vip.sc5.yahoo.com/lib/bettercablesdotcom/conductivity.jpg

  37. Luster http://www.petcremationnevada.com/images/glassceramicImpression.jpg

  38. Alloys • Mixtures composed of two or more elements (at least one metal) • Properties superior to those of their component elements -stronger / harder -more lustrous -more conductive -more resistant to corrosion

  39. Sterling Silver Cast Iron Stainless Steel Bronze Ag (92.5%) Cu (7.5 %) Fe (96%) and C (4%) Fe (80.6 %), Cr (18%), C (0.4%), Ni (1%) Cu (86%) and Sn (14%) Common Alloys

  40. Common Alloys http://www.pacificsintered.com/pacific/castinvest.gif

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