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Starter. What ions do Chlorine form? Imagine you have 2 chlorine ions – how could they help EACH OTHER to reach a stable state? It might help if you draw out the Lewis structures for 2 chlorine ions!. LET’S FIRST REVIEW IONIC BONDING. K. F. In an IONIC bond,

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  1. Starter • What ions do Chlorine form? • Imagine you have 2 chlorine ions – how could they help EACH OTHER to reach a stable state? • It might help if you draw out the Lewis structures for 2 chlorine ions!

  2. LET’S FIRST REVIEW IONIC BONDING

  3. K F In an IONIC bond, electrons are lost or gained, resulting in the formation of IONS in ionic compounds.

  4. K F

  5. K F

  6. K F

  7. K F

  8. K F

  9. K F

  10. _ + K F

  11. _ + K F The compound potassium fluoride consists of potassium (K+) ions and fluoride (F-) ions

  12. _ + K F The ionic bond is the attraction between the positive K+ ion and the negative F- ion

  13. So what are covalent bonds?

  14. In covalent bonding, atoms still want to achieve a noble gas configuration (8 valence electrons).

  15. In covalent bonding, atoms still want to achieve a noble gas configuration. But rather than losing or gaining electrons, atoms now share an electron pair.

  16. In covalent bonding, atoms still want to achieve a noble gas configuration (the octet rule). But rather than losing or gaining electrons, atoms now share an electron pair. The shared electron pair is called a bonding pair

  17. Fluorine forms a covalent bond with itself F2

  18. How will two fluorine atoms react? F F

  19. F F Each fluorine atom wants to gain one electron to have 8 valence electrons.

  20. F F Neither atom will give up an electron What’s the solution –what can they do to achieve 8 valence electrons?

  21. F F

  22. F F

  23. F F

  24. F F

  25. F F 8 valence electrons

  26. F F 8 valence electrons circle the electrons for each atom that completes their octets

  27. F F Bysharing the electron pair in the middle, each fluorine atom feels like it has 8 valence electrons circle the electrons for each atom that completes their octets

  28. F F The electron pair in the middle (the circled one) is shared by the two atoms of fluorine. circle the electrons for each atom that completes their octets

  29. F F This is called the bonding pair circle the electrons for each atom that completes their octets

  30. F F It is a single bonding pair circle the electrons for each atom that completes their octets

  31. F F It is called aSINGLE BOND circle the electrons for each atom that completes their octets

  32. F F Single bonds are shown with with a dash circle the electrons for each atom that completes their octets

  33. F F This is the fluorine molecule, F2 circle the electrons for each atom that completes their octets

  34. O2 How will this molecule form?

  35. O O

  36. O O Each atom has two unpaired electrons

  37. O O

  38. O O

  39. O O

  40. O O

  41. O O

  42. O O

  43. O O Both atoms want to gain two electrons.

  44. O O Oxygen atoms are highly electronegative. So both atoms want to gain two electrons.

  45. O O

  46. O O

  47. O O

  48. O O

  49. O O Both electron pairs are shared.

  50. O O 6 valence electrons plus 2 shared electrons = 8 valence electrons 

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