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Chapter 3

Chapter 3. Bonding. Bonding. The interaction of atoms with each other to form discrete groups. The Principles of Bonding. There is a force of attraction between (-) electrons and (+) nuclei. There is a force of repulsion between electrons.

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Chapter 3

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  1. Chapter 3 Bonding

  2. Bonding The interaction of atoms with each other to form discrete groups

  3. The Principles of Bonding • There is a force of attraction between (-) electrons and (+) nuclei. • There is a force of repulsion between electrons. • There is a force of repulsion between nuclei. • All chemical bonding reflects these interactions.

  4. The Trap of Stability • Noble gases have stable electron electron arrangements, so they don’t react to rearrange. • For many other elements, chemical reactions are often guided by the tendency to acquire a noble gas electron arrangement.

  5. Ionic Bonding – Electron Transfer

  6. Covalent Bonding-Electron Sharing water, H2O carbon dioxide, CO2

  7. Lewis Structures, H to He

  8. Some Lewis Structures, ball-and-stick, space-filling

  9. More Lewis Structures, ball-and-stick, space-filling

  10. Physical Properties • Melting point: the temperature at which the solid form of the compound becomes liquid. • Boiling point: the temperature at which the liquid boils and transforms into a gas.

  11. Electronegativity -electron-attracting ability

  12. Polar Covalent Bonds –water as a case-study Each H is d+ Each O is 2 d-

  13. Chemical Nomenclature:Binary Salts KBr = K+ and Br — ` potassium ion bromideion Potassium bromide FeBr3 = Fe3+ and 3 Br — ` iron(III) ion bromideion iron(III) bromide

  14. Chemical Nomenclature:Binary Covalent Compounds

  15. Binary Covalent Compounds PCl5 = phosphorus pentachloride N2O4 = dinitrogen tetroxide tetraphosphorus decoxide = P4O10

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