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: The electron in a ground-state H atom absorbs a photon of wavelength 97.20 nm. To what energy level does it move?

Solution: The electron in a ground-state H atom absorbs a photon of wavelength 97.20 nm. To what energy level does it move?

Problem

The electron in a ground-state H atom absorbs a photon of wavelength 97.20 nm. To what energy level does it move?

Solution

Recall: The Balmer equation relates the wavelength of a photon from the transition of an electron in an atom. For an absorption process, the Balmer equation is:

where R = Rydberg constant (1.0974 × 107 m), Z = atomic number, n = energy level.

For an electron in a ground-state H atom (Z = 1), the initial energy level is ninitial = 1. We’re given the wavelength of a photon absorbed by this electron, λ = 97.20 nm. Converting from nm to m:

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