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Ionic Bonding

Ionic Bonding

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Ionic Bonding

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  1. Ionic Bonding Mr. Thomson Experience Academy

  2. Classifying Pure Substances

  3. Comparison – Bond Types

  4. Ionic Bonding • Ionic Bond: Attraction between positive and negative ions that holds atoms in place in an ionic compound (usually a crystal). • Ionic compounds usually form when a metal positive ion (cation) bonds with a non-metal negative ion (anion). • Ionic compounds involve the transfer of electrons. (Unlike covalent bonding, where electrons are shared.)

  5. Crystal Structure of Ionic Compounds • Ionic compounds do not form molecules. Instead, ionic compounds form an organized three-dimensional structure of alternating positive and negative ions.

  6. Comparison: Molecules and Ionic Compounds Water, a molecular compound, is made of billions and billions of INDIVIDUAL water molecules. Salt, an ionic compound, is made of billions and billions of ions, all together in a crystal lattice. There are NO individual molecules of NaCl.

  7. How are ions formed? • When atoms form ions, they lose or gain electrons in order to have eight valence electrons.

  8. How is sodium chloride formed? Animation(Source:

  9. Na Cl Na 1s22s22p63s1 Remember the “rule of eight.” Sodium wants a full outer (valence) shell. So sodium can either gain seven electrons to fill the third shell, or get rid of the 3s1 electron. Then the outer shell (second) will be full. The new electron configuration will be: Na+ 1s22s22p6

  10. Na Cl Na+ 1s22s22p6 Why is sodium +1 when it loses an electron? Na Na+ p+ = 11 p+ = 11 e- = 11 e- = 10 Zero charge +1 charge

  11. Na Cl Cl 1s22s22p63s23p5 Remember the “rule of eight” again. Chlorine wants a full shell also. So it can either lose seven electrons, or gain one electron. The new electron configuration will be: Cl - 1s22s22p63s23p6

  12. Na Cl Cl - 1s22s22p63s23p6 So why is chlorine -1 when it gains an electron? Cl Cl - p+ = 17 p+ = 17 e- = 17 e- = 18 Zero charge -1 charge

  13. Sodium Chloride Na Cl -1 +1 Na Cl

  14. Crystal Structure of Sodium Chloride Source:

  15. Another Look at Sodium Chloride Crystal

  16. Na Cl In all ionic compounds, the charges cancel, so the overall charge for the compound is zero.

  17. Predicting Formulas for Ionic Compounds:

  18. Magnesium sulfide Mg S [Ne]3s2 [Ne]3s23p4 Mg S

  19. Magnesium sulfide Mg S [Ne]3s2 [Ne]3s23p4 Mg S

  20. Magnesium sulfide Mg S [Ne]3s2 [Ne]3s23p4 -2 +2 Mg S Extra Electrons from Magnesium Mg +2 S -2 [Ne] [Ne]3s23p6

  21. Magnesium sulfide Mg +2 S -2 [Ne] [Ne]3s23p6 MgS

  22. Calcium chloride Ca +2 Cl -1 CaCl2 When the charges don’t cancel…cross the charges to write the correct formula.

  23. Aluminum Oxide Al +3 O -2 Al2O3 When the charges don’t cancel…cross the charges to write the correct formula.

  24. Polyatomic Ions Polyatomic ions: a charged group of covalently bonded atoms. The charge comes from gaining or losing electrons as a group. (See back of your periodic table.) • Examples: • Ammonium: NH4+ • Nitrate: NO3-

  25. Sodium nitrate Na +1 NO3-1 Do the charges cancel? Yes…so just write the formula. NaNO3

  26. Potassium carbonate K +1 CO3-2 Do the charges cancel? No…so cross the charges. Answer: K2CO3

  27. Ammonium sulfate NH4+1 SO4-2 Charges cancel? No…so cross the charges. (NH4)2SO4

  28. Calcium Phosphate Ca +2 PO4-3 Charges cancel? No…so cross the charges. Ca3(PO4)2

  29. Classwork Homework: Naming Ionic Compounds WS 1 Ionic Bonding Classwork Both Stamped Tomorrow Many of you still need to finish the Molecule Building Activity…this will need to be completed on your own time… Many of you also still need to turn in your Online Bonding Activity.