Overview of Bonding
Atoms achieve low energy states through electrostatic attractions, resulting in:
Ionic Bonds: Formed by electron transfer between metals and nonmetals (e.g., NaCl); strength increases with smaller ion radius and higher charge.
Covalent Bonds: Atoms share electrons (e.g., H2O, SO2); types include single, double, and triple bonds. Polar bonds have unequal sharing (e.g., H2O); nonpolar bonds share equally (e.g., O2) based on electronegativity differences (<0.4 nonpolar; 0.4-1.8 polar).
Metallic Bonds: Involve delocalized electrons, providing conductivity and malleability.
Lewis Structures: 2D representations of molecules drawn by counting valence electrons; help visualize molecular shape and reactivity.
Understanding these bonding types and Lewis structures is essential for studying molecular interactions.
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