1. 1 Chapter 3 Bonding

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

3. 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. All chemical bonding reflects these interactions.

4. 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. 5 Ionic Bonding – Electron Transfer

6. 6 Covalent Bonding- Electron Sharing water, H 2 O carbon dioxide, CO 2

7. 7 Lewis Structures, H to He

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

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

10. 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. 11

12. 12 Electronegativity - electron-attracting ability

13. 13 Polar Covalent Bonds – water as a case-study Each H is  + Each O is 2 

14. 14 Chemical Nomenclature: Binary Salts KBr = K + and Br — ` potassium ion brom ide ion Potassium bromide FeBr 3 = Fe 3+ and 3 Br — ` iron(III) ion brom ide ion iron(III) bromide

15. 15 Chemical Nomenclature: Binary Covalent Compounds

16. 16 Binary Covalent Compounds PCl 5 = phosphorus pentachloride N 2 O 4 = dinitrogen tetroxide tetraphosphorus decoxide = P 4 O 10