pg 275 #117-123
117. (use electronegativity values found in textbook, found on pg 194) a) C-O b) C-F c) P-Cl
118. a) C b)N c) S d) O
119. b) Si-O
120. In order of increasing polarity: c, a, b, e, d
121. equal distribution of charge because of symmetry
122. a) Polar, asymmetrical b) nonpolar, symmetrical c)polar, asymmetrical d)nonpolar, symmetrical
123. sulfur difluoride and sulfur tetrafluoride are polar. Sulfur hexafluoride is nonpolar (draw Lewis, check for symmetry, check for polarity)
Test Objectives
- Define and compare ALL vocabulary for chapter 8
- Draw Lewis structures for covalent molecules AND ionic compounds
- Assign formal charge to individual atoms and entire molecules when drawing Lewis structures
- Identify VSEPR geometries and bond angles for a Lewis structure
- Assign bond polarity AND molecule polarity by analyzing electronegativities and symmetry within a molecule
- Name ionic and covalent compounds
- Compare properties of ionic and covalent compounds
- Compare electronegativities to determine the “nature” (polar covalent, non-polar covalent, ionic) of a bond
Test Date: Wednesday 3/18
I told a chemistry joke once…There was no reaction
