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

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Presentation transcript:

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

Part 3: Metallic Bonds

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

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

Ionic vs. Metallic Bonding

External forceMetal bends

Part 5: Acids & Bases

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

Acids & Bases Naming Ions Oxidation Numbers RatioFormulaName Hydrogen & Sulfate H + & SO :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 H 3 PO 3 phosphorous acid Al 3+ & OH - 3:1 Al(OH) 3 aluminum hydroxide

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