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Chemical Bonds

Chemical Bonds. Ionic Bonds. Form between a metal (electron donor) and a non-metal (electron receiver). Ionic Bond. A positive ion ( cation ) is attracted to a negative ion (anion ) The positive ion gives electron(s) to the negative ion forming an ionic bond. Ionic Bond.

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Chemical Bonds

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  1. Chemical Bonds

  2. Ionic Bonds Form between a metal (electron donor) and a non-metal (electron receiver)

  3. Ionic Bond • A positive ion (cation) is attracted to a negative ion (anion) • The positive ion gives electron(s) to the negative ion forming an ionic bond

  4. Ionic Bond • The compound and/or molecule formed is neutral. • Follows the Octet Rule (rule of 8): atoms react so that they have a full outer shell (Hydrogen and Helium 2/0 electrons, the rest 8/0 electrons)

  5. Ionic Bond Na + Cl NaCl Na 1+ + Cl1-  NaCl Na + Cl  Na Cl

  6. Ionic Bond 2Li + O  Li2O 2Li 1+ + O 2-  Li2O Li + O + Li  Li O Li

  7. Covalent Bond Formed between a non-metal and another non-metal. The atoms share their valence electrons to fill their outer energy shell with a complete set of 8 (2 for H and He)

  8. Covalent Bond C 4+ + 2O 2- CO2 O C O O C O

  9. Covalent Bond C 4+ + H 1- CH4 H H C H H H H C H H

  10. http://www.youtube.com/watch?v=QqjcCvzWwww&feature=player_embedded#!http://www.youtube.com/watch?v=QqjcCvzWwww&feature=player_embedded#! http://www.youtube.com/watch?v=yjge1WdCFPs&feature=player_embedded

  11. Role of Polyatomic Ions Polyatomic Ions allow for the formation of compounds/molecule having both ionic and covalent bonds.

  12. Polyatomic Ions NH41+ + Cl1- NH4Cl H Cl H Cl H N H  H N H H H

  13. Polyatomic Ions 2Na 1+ + CO32- Na2CO3 O O Na O C  Na O C Na O Na O

  14. Periodic Table with Electronegativities

  15. Bonds by Electronegativity • If the electronegativity difference (ΔEN)< 0.5, the bond is non-polar covalent. • If the ΔEN = 0.5 to 1.6, the bond is polar covalent • If the ΔEN >2.0, then the bond is ionic. • If the ΔEN = 1.6 to 2.0 and a metal is involved, then the bond is ionic. If only nonmetals are involved, the bond is polar covalent.

  16. Polar Bonds a covalent bond in which the atom with more protons “hogs” the electrons becoming slightly negative while the other atom(s) become slightly positive. This is NOT a polyatomic ion because there is no left over protons or electrons.

  17. Polar Bonds Because it is a polar covalent bond, the electrons shared by the atoms spend a greater amount of time closer to the Oxygen nucleus than the Hydrogen nucleus. This is because of the great electronegativity difference between the Hydrogen atom and the Oxygen atom. Oxygen, has a partial negative charge and the Hydrogen’s have a partial positive charge. This molecule is not an ion because there are no extra protons or electrons

  18. Polar Bond - Water

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