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Ionic Bonding

Ionic Bonding

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Ionic Bonding

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  1. Ionic Bonding …electrons are transferred

  2. Guiding Questions? What is that? How do we figure out what the chemical formula is? What does it mean to be "free of chemicals"?

  3. Keeping Track of Electrons • The electrons responsible for the chemical properties of atoms are those in the outer energy level. • Valence electrons - The s and p electrons in the outer energy level. • Core electrons -those in the energy levels below.

  4. Keeping Track of Electrons • Atoms in the same column • Have the same outer electron configuration. • Have the same valence electrons. • Easily found by looking up the group number on the periodic table. • Group 2A - Be, Mg, Ca, etc.- • 2 valence electrons

  5. 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

  6. 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.

  7. Write the electron dot diagram for • Na • Mg • C • O • F • Ne • He Na 1s22s22p63s1 Mg 1s22s22p63s2 C 1s22s22p2 O 1s22s22p4 F 1s22s22p5 Ne 1s22s22p6 He 1s2

  8. Electron Configurations for Cations • Metals lose electrons to attain noble gas configuration. • They make positive ions. • If we look at electron configuration it makes sense. • Na 1s22s22p63s1 - 1 valence electron • Na+ 1s22s22p6 -noble gas configuration

  9. 20 Ca 40.078 Electron Dots For Cations • Metals will have few valence electrons • These will come off • Forming positive ions 1s22s22p63s2 Ca +2

  10. Electron Configurations for Anions • Nonmetals gain electrons to attain noble gas configuration. • They make negative ions. • If we look at electron configuration it makes sense. • S 1s22s22p63s23p4 - 6 valence electrons • S-2 1s22s22p63s23p6 -noble gas configuration. (anions)

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

  12. Stable Electron Configurations • All atoms react to achieve noble gas configuration. • Noble gases have two s and six p electrons. • Eight valence electrons . • Also called the octet rule. Ar

  13. Ionic Bonding • Anions and cations are held together by opposite charges. • Ionic compounds are called salts. • Simplest ratio is called the formula unit. • The bond is formed through the transfer of electrons. • Electrons are transferred to achieve noble gas configuration.

  14. - + Ionic Bonding transfer of electron Na Cl NaCl

  15. Ionic Bonding Ca +2 Ca P -3 +2 Ca P -3 +2 • All the electrons must be accounted for!

  16. P3- P 3- Ca2+ Ca2+ Ca2+ Ionic Bonding Ca2+ Ca3P2 Ca2+ P3- Ca2+ Formula Unit P3-

  17. 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.

  18. Crystalline structure

  19. 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.

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

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

  22. + + + + + + + + + + + + Metals are Malleable • Hammered into shape (bend). • Ductile - drawn into wires. • Electrons allow atoms to slide by.

  23. - + - + + - + - - + - + + - + - - + - + Ionic solids are brittle Strong repulsion breaks crystal apart. Force