Chemical bonding involves atoms forming stable electronic configurations through gaining, losing or sharing electrons. Ionic bonds form between metals and nonmetals when electrons are transferred, while covalent bonds involve sharing electron pairs between nonmetals to achieve stable octets. Different bond types including ionic, covalent and metallic bonding can be identified based on the participating elements and electron configurations involved.

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