Ionic, Covalent and metallic bonds

1. Chemical Bonding. Unions that build

6. Element Group Valence e - Electrons to form Ion Ion Formed Lost Gained Sodium IA Na + Magnesium IIA Mg 2+ Calcium IIA Ca 2+ Aluminum IIIA Al 3+ Sulfur VIA S 2- Oxygen VIA O 2- Chlorine VIIA Cl - Bromine VIIA Br -

9. However, because of the high charge that would result, either C 4+ or C 4- for carbon and Si 4+ or Si 4- for silicon

11. Symbol Atomic Electronic configuration Lewis atom structure Formed ion Ionic Electronic configuration Lewis ionic structure Li 1s 2 2s 1 Li  Li + 1s 2 Li + Be B C N O F Ne

14. For example, common salt is sodium chloride. When sodium (Na) and chlorine (Cl) are combined, the sodium atoms each lose an electron forming a cation (Na + ), and the chlorine atom gain an electron to form an anion (Cl − ). Na + Cl  Na + + Cl -

19. The pair of shared electrons can be drawn with lines Chlorine molecule Cl 2 Cl = 7 e pair of shared electrons in red, each chlorine atom has 8 e or     Cl        Cl   

25. Compound Electronegativity value of each atom Electronegativity difference Type of bond F 2 F: 4.0 F: 4.0 4.0 – 4.0 = 0 Covalent Non-polar H 2 S NaF RbBr NH 3 HF MgO KCl N 2 CH 4