CHEM 1211 Lecture 20Outline of Last Lecture I. Covalent bondsII. CH3NH2Outline of Current Lecture I. Covalent BondsA. N2B. CO32-II. Octet Rule ViolatorsA. BCl3B. I3-Current Lecture: I. Covalent BondsA. N21. How many valence electrons are present? 102. How many valence electrons are needed for the outer shell? 163. How many electrons are shared bonds? N-A = 16-10 = 64. How many lone pairs are present? A-S = 10-6 = 45. What is the electron pair geometry? Linear6. What is the molecular geometry? LinearN = NBond Order = 3- Number of electrons bonded between two atoms divided by the number of bonding electrons totalIn this case: 6 – 3 = 3. - The closer two things are together, the greater the bond.B. CO32-1. How many valence electrons are present? 242. How many valence electrons are needed for the outer shell? 323. How many electrons are shared bonds? N-A = 32- 24 = 84. How many lone pairs are present? A-S = 24-8 = 165. What is the electron pair geometry? Trigonal Planar6. What is the molecular geometry? Trigonal Planar7. Average bonding order? 1.33 O = C – O or O – C – O or O – C = O | || | O O OAll structures put together = residence hybridO – C – O | OFormal Charge = NVE – [ LPE + ½ (BE)]II. Octet Rule ViolatorsA. BCl31. How many valence electrons are present? 24- B = very reactive, searching for electrons for p orbital2. Electron Pair geometry? Trigonal Planar3. Molecular Geometry? Trigonal PlanarCl | Cl – B – Cl- Polar Bonds: Cl is more electro-negative than Boron- No Net DipoleB. I3-Valence Electrons: 22Electron Pair Geometry: Trigonal BipyrimidalMolecular Geometry: LinearI – I – I
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