1. Chapter 8 Chemistry 1L Cypress Creek High School Unit 8: Ionic Bonds

2. Part 3: Metallic Bonds

3. Metallic Bonds Metallic bonding is collective in nature - all metal cations contribute their valence electrons to form a “sea of electrons” – Examples: Aluminum, Silver, Iron

4. Metallic Bonds The free, mobile electrons are responsible for the unique properties of metals such as malleability, ductility, and conductivity of heat and electricity

5. Ionic vs. Metallic Bonding

6. External forceMetal bends

7. Part 5: Acids & Bases

8. Acids & Bases Naming Binary acids (H + nonmetal element): – hydro ______ic acid – Example: HBr = hydrobromic acid Ternary acids (H + polyatomic ion): – ate ions: _________ic acid – ite ions: _________ous acid – Examples: H 2 SO 3 = sulfurous acid H 3 PO 4 = phosphoric acid Bases (cation + OH): – ________ hydroxide – Example: Ca(OH) 2 = calcium hydroxide

9. Acids & Bases Naming Ions Oxidation Numbers RatioFormulaName Hydrogen & Sulfate H + & SO 4 2- 1:2H 2 SO 4 sulfuric acid Potassium & Hydroxide Hydrogen & Bromine Hydrogen & Phosphite Aluminum & Hydroxide K + & OH - 1:1 KOH potassium hydroxide H + & Br - 1:1 HBr hydrobromic acid H + & PO 3 3- 1:3 H 3 PO 3 phosphorous acid Al 3+ & OH - 3:1 Al(OH) 3 aluminum hydroxide