CHEM 1211 Lecture 19Outline of Last Lecture I. Ionic BondsA. Lewis Dot Structures 1. RbBr2. Xw3. Al2S3B. Ionic Bond Covalent BondII. Covalent Compounds 1. CCl4I. CHBrCHBrOutline of Current Lecture I. Covalent bondsII. CH3NH2Current Lecture: I. Covalent bondsA. C2H2Br21. How many valence electrons? 242. How many valence electrons are needed to complete the outer shell? 363. How many electrons are shared in bonds? N-A = 124. How many lone pairs? A-S = 12- Geometry Isomers: different chemical and physical properties- Best Value of electro-negativity: halogens (greater pull of electrons)- NO NET DIPOLE: Two polar covalent bonds with dipoles in opposite directionH HC = CBr Br- Vector: magnitude and directionPolar bond- Just because a molecule has polar covalent bonds doesn’t mean the molecule itself is polar!- Mainly between non-metalsII. CH3NH21. How many valence electrons? 142. How many valence electrons needed to complete the outer shell? 263. Electrons shared in bonds? N-A = 124. Lone Pairs? A-S =
View Full Document
Unlocking...