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AP Chemistry Chapter 8 Concepts Details Types of A. Ionic Bonding Chemical Bonds B. Coulomb’s Law C. Bond Length D. Covalent Bonds Electro – A. Electronegativity negativity B. Electronegativity Trends 1 AP Chemistry Chapter 8 C. Characterizing bonds Practice Problem Order the following bonds according to polarity: H-H, O-H, H-Cl, H-S and F-H #1 Bond A. Dipolar Molecules Polarity and Dipole Moments B. Molecules with Polar Bonds but no Dipole Moment Ion A. Bonding and Noble Gas Electron Configurations Electron Configurati on and B. Predicting Formulas of Ionic Compounds Sizes C. Sizes of Ions 2 AP Chemistry Chapter 8 Practice Choose the largest ion in each of the following groups. Explain why it Problem is the largest ion. #2 A) Li+, Na+, K+, Rb+, Cs+ B) Ba2+, Cs+, I-, Te2Formation A. Lattice Energy of Binary Ionic Compounds B. Lattice Energy Calculations Partial A. Calculating Percent Ionic Character Ionic Character of Covalent B. Ionic vs. Covalent Bonds 3 AP Chemistry Chapter 8 The A. Strengths of the Bond Model Chemical covalent bond: A model B. Weaknesses of Bond Model Covalent A. Average Bond Energies Bond Energies and Chemical Reactions B. Multiple Bonds C. Bond Energy and Enthalpy 4 AP Chemistry Chapter 8 Practice Using the bond energies listed in table 8.4, calculate the H for the Problem reaction of methane with chlorine and fluorine gas to give Freon-12 #3 (CF2Cl2). CH4 (g) + 2Cl2 (g) + 2F2 (g) CF2Cl2 (g) + 2 HF (g) + 2HCl (g) The A. Lone Electron Pairs Localized Electron Bonding B. Bonding Electron Pairs Model C. Localized Electron Model D. Derivations of the Localized Model Lewis A. Electrons and Stability Structures B. Writing Lewis Structures Rules 5 AP Chemistry Chapter 8 Practice Give the Lewis structure for each of the following: Problem HF, N2, NH3, CH4, CF4, NO+ #4 Exceptions A. Boron Trifluoride to the octet rule B. Sulfur Hexaflouride C. More about the octet rule 6 AP Chemistry Chapter 8 Practice Write the Lewis structure for each of the following: Problem PCl5, ClF3, XeO3, RnCl2, BeCl2, ICl4- #5 Resonance A. Nitrate Ion Structures B. Resonance Practice Describe the electron arrangement in the in the nitrite anion (NO2-) Problem using the localized electron model. #6 7 AP Chemistry Chapter 8 Molecular A. Valence Shell Electron Pair Repulsion Structure: The VSEPR Model B. Effect of unshared pairs C. VSEPR and Multiple Bonds 8 AP Chemistry Chapter 8 D. Molecules Containing no Single Central Atom E. How well does VSEPR work? Describe the molecular structure of a water molecule. When phosphorous reacts with excess chlorine gas, the compound phosphorous pentachloride (PCl5) is formed. In the gaseous and liquid states, this substance consists of PCl5 molecules, But in the solid state is consists of a 1:1 mixture of PCl4- and PCl6ions. Predict the geometric structures of PCl5, PCl4- and PCl6-. Practice Problem #7 9