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Ionic bonding: Li + O

8p +. 8p +. 8e - 2e -. 6e - 2e -. 8n 0. 8n 0. 1e -. 3p +. 3p +. 3p +. 3p +. 2e -. 2e -. 2e - 1e -. 2e - 1e -. 4n 0. 4n 0. 4n 0. 4n 0. 1e -. O. [Li] 2 +. [ O ] 2–. Li. Li. Ionic bonding: Li + O. 2Li + O  [Li] 2 + [O] 2– or 4Li + O 2  2[Li] 2 + [ O] 2–.

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Ionic bonding: Li + O

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  1. 8p+ 8p+ 8e- 2e- 6e- 2e- 8n0 8n0 1e- 3p+ 3p+ 3p+ 3p+ 2e- 2e- 2e-1e- 2e-1e- 4n0 4n0 4n0 4n0 1e- O [Li]2+ [ O ]2– Li Li Ionic bonding: Li + O 2Li + O [Li]2+[O]2–or 4Li + O2 2[Li]2+[ O]2–

  2. 17p+ 7e- 8e- 2e- 18n0 1e- 17p+ 13p+ 17p+ 17p+ 2e- 8e-3e- 8e- 8e- 2e- 8e- 8e- 2e- 8e- 8e- 2e- 14n0 18n0 18n0 18n0 1e- 17p+ 13p+ 7e- 8e- 2e- 2e- 8e- 18n0 14n0 1e- 17p+ 7e- 8e- 2e- 18n0 Ionic bonding: Al + Cl

  3. Al [Al]3+ [ Cl ]3– Cl Cl Cl Ionic bonding: Al + Cl Al + 3Cl [Al]3+[Cl]3–

  4. Covalent bonding • Thus far we have looked at when atoms bond due to the transfer of electrons • An ionic bond forms when an atom has a greater attraction for e–s than a second atom • However, if two atoms have approximately the same pull on electrons, they share the electrons (forming a “covalent” bond) • Read “Covalent bonding” and “Covalent bonding continued”. Do Q7.

  5. Cl Cl C Cl Cl H H H H H H H Cl N H O [Mg]2+ [Na] + [ F ]2– [ Cl ]– H O Covalent bonding CCl4 - Covalent HCl - Covalent MgF2 - Ionic Q7 NH3 - Covalent NaCl - Ionic H2O - Covalent H2 - Covalent OH– - Covalent For more lessons, visit www.chalkbored.com

  6. Cl H O O I Cl H H H H H I N O C O I I O O H H C H H N H H [Al]23+ [Na]2+ [ O ]2– [ O ]32– O O O O O C C H H H O O O H Multiple bonds CO2 - Covalent Na2O - Ionic HCl - Covalent Do Q. 8. Build models of molecules, O3 as challenge (can’t build it or ionic) NH3 - Covalent I2 - Covalent O2 - Covalent O3 - Covalent Al2O3 - Ionic

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