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Ionic Bonding

Learn about valence electrons, electron dot diagrams, and stable outer shells in Ionic Bonding. Explore how cations and anions are formed, the significance of formula units, and properties of ionic compounds. Understand metallic bonds and their characteristics, conductivity, and malleability in metals.

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Ionic Bonding

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  1. Ionic Bonding

  2. Keeping Track of Electrons • The electrons that are responsible for the chemical properties of atoms are those in the outer energy level. • Valence electrons - The outer electrons. • Core electrons -those in the inside.

  3. Keeping Track of Electrons • Same column = same valence electrons. • Easily found by looking up the group number on the periodic table. • Group 2A - Be, Mg, Ca, etc.- • 2 valence electrons

  4. Electron Dot diagrams • A way of keeping track of valence electrons. • How to write them • Write the symbol. • Put one dot for each valence electron • Don’t pair up until they have to X

  5. The Electron Dot diagram for Nitrogen • Nitrogen has 5 valence electrons. • First we write the symbol. N • Then add 1 electron at a time to each side. • Until they are forced to pair up.

  6. Write the electron dot diagram for • Na • Mg • C • O • F • Ne • He

  7. Electron Configurations for Cations • Metals lose electrons to attain noble gas configuration. • They make positive ions.

  8. Electron Dots For Cations • Metals lose electrons to look like noble gases. • They make positive ions. • Metals will have few valence electrons Ca

  9. Electron Dots For Cations • Metals will have few valence electrons • These will come off Ca

  10. Electron Dots For Cations • Metals will have few valence electrons • These will come off • Forming positive ions Ca+2

  11. Electron Configurations for Anions • Nonmetals gain electrons to look like noble gases. • They make negative ions.

  12. Electron Dots For Anions • Nonmetals will have many valence electrons. • They will gain electrons to fill outer shell. P P-3

  13. Stable Outer Shells • All atoms react to look like noble gases. • 8 valence electrons . • Also called the octet rule. Ar

  14. Ionic Bonding • Anions and cations are held together by the attraction between opposite charges. • Ionic compounds are called “salts”. • The simplest ratio is called the formula unit. • The bond is formed through the transfer of electrons.

  15. Ionic Bonding Na Cl

  16. Ionic Bonding Na+ Cl-

  17. Ionic Bonding • All the electrons must be accounted for! Ca P

  18. Ionic Bonding Ca P

  19. Ionic Bonding Ca+2 P

  20. Ionic Bonding Ca+2 P Ca

  21. Ionic Bonding Ca+2 P-3 Ca

  22. Ionic Bonding Ca+2 P-3 Ca P

  23. Ionic Bonding Ca+2 P-3 Ca+2 P

  24. Ionic Bonding Ca Ca+2 P-3 Ca+2 P

  25. Ionic Bonding Ca Ca+2 P-3 Ca+2 P

  26. Ionic Bonding Ca+2 Ca+2 P-3 Ca+2 P-3

  27. Ionic Bonding Ca3P2 Formula Unit

  28. Properties of Ionic Compounds • Crystalline structure. • A regular repeating arrangement of ions in the solid. • Ions are strongly bonded. • Structure is rigid. • High melting points- because of strong forces between ions.

  29. Crystalline structure

  30. Do they Conduct? • Conducting electricity is allowing charges to move. • In a solid, the ions are locked in place. • Ionic solids are insulators. • When melted, the ions can move around. • Melted ionic compounds conduct. • First get them to 800ºC. • Dissolved in water they conduct.

  31. Metallic Bonds • How atoms are held together in the solid. • Metals hold onto their valence electrons very weakly. • Think of them as positive ions floating in a sea of electrons.

  32. + + + + + + + + + + + + Sea of Electrons • Electrons are free to move through the solid. • Metals conduct electricity.

  33. Metals are Malleable • Hammered into shape (bend). • Ductile - drawn into wires.

  34. + + + + + + + + + + + + Malleable

  35. + + + + + + + + + + + + Malleable • Electrons allow atoms to slide by.

  36. + - + - - + - + + - + - - + - + Ionic solids are brittle

  37. - + - + - + - + + - + - - + - + Ionic solids are brittle • Strong Repulsion breaks crystal apart.

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