Ch.7 - Quantum MechanicsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Only certain transitions are allowed from one energy level to another. In one-electron species, the change in ℓ for an allowed transition is ±1. For example, a 3p electron can move to a 2s orbital but

Problem

Only certain transitions are allowed from one energy level to another. In one-electron species, the change in ℓ for an allowed transition is ±1. For example, a 3p electron can move to a 2s orbital but not to a 2p. Thus, in the UV series, where  nfinal = 1, allowed transitions can start in a  p orbital (ℓ = 1) of n = 2 or higher, not in an  s (ℓ = 0) or  d (ℓ = 2) orbital of  n = 2 or higher. From what orbital do each of the allowed transitions start for the first four emission lines in the visible series (nfinal = 2)?