Propose a series of chain initiation, propagation, and termination steps for this

Chemistry Notes for Exam 3: Ch. 8­11 on 12/1/15 Corresponding Textbook: Chemistry; The Molecular Nature of Matter and Change Includes: Electron Configuration, Periodic Table Trends, Types of Bonds, Lattice Energy, Lewis Structures, VSEPR, Bond Order, Bond Length, Formal Charge, and Hybridization. Chapter 8: Electron Configuration and Chemical Periodicity 1  Spin quantum number: (m ) s 2 corresponds to direction of electron’s field. For any n value, a lower L value indicates a lower (more stable) sublevel.  Exclusion principle: no two electrons in the same atom can have the same four quantum #’s  Shielding: reduces the full nuclear charge to an effective nuclear charge making it easier to remove an electron.  Electron configuration: nƖ ex. 1s 2s 2p 3s 3p 4s 3d 4p etc…..  Periodic table trends: atomic size←↓(transition elements stay about the same size), ionization energy↑→, electron affinity↑→, metallic behavior ↓←(memorize periodic table trends chart). *Anions are larger than parent atoms.  Paramagnetic vs Diamagnetic: Paramagnetic have an unpaired electron which is attracted to an external magnetic field. Diamagnetic have no unpaired electrons, not attracted (slightly repelled) by magnetic fields. Chapter 9: Models of Chemical Bonding  Ionic bond: between a metal and a non­metal. Large difference in ionization energy. Forms an ionic solid  Covalent bond: usually between two