CHEM 1211 Lecture 17Outline of Last Lecture I. Orbital Quantum Number1. Clicker Question One2. Clicker Question Two3. Clicker Question ThreeA. The S OrbitalB. The P OrbitalC. The D Orbital II. Spin Quantum Number1. Clicker Question FourOutline of Current Lecture I. Using a Clicker for SpinsA. Clicker Question OneB. Clicker Question TwoC. Clicker Question ThreeD. Clicker Question FourII. Electron Configurations for HeliumIII. Hund’s RuleCurrent Lecture: I. Using a Clicker for Spins- A: + ½ Spin- V: - ½ Spin- Separating Orbitals: AV_AVA. Clicker Question OneWhat quantum number would be used to determine the number of orbitals in a subshell?A. Angular Momentum Quantum NumberB. Magnetic Quantum NumberC. Principle Quantum NumberD. Spin Quantum NumberB. Clicker Question TwoThe angular momentum quantum number for a subshell is four. How many orbitals would we expect to find?A. 10B. 4C. 6D. 16E. 9C. Clicker Question ThreeWhat type of orbital is this?GD. Clicker Question FourWhen filling three degenerate orbitals with two electrons, you must first?A. Utilize Pauli Exclusion PrincipleB. Throw them in JailC. Understand DE Broglie’s PrincipleD. Apply Hund’s RuleII. Electron Configurations for HeliumZ=2Orbital Box Notation: 1s: Core electron2s: Valence/Outer Shell electronLithium:1s2 2s1 (Valence) [He] 2s1 (Condensed)Number of Valence Electrons: 1III. Hund’s Rule: Nitrogen: Z=71s2s2px2py2pzenergy1s2s2px 2py 2pz1s1s 2s 2pCore
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