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: One of the emission lines of the hydrogen atom has a wavelength of 93.8 nm. (b) Determine the initial and final values of n associated with this emission.

Solution: One of the emission lines of the hydrogen atom has a wavelength of 93.8 nm. (b) Determine the initial and final values of n associated with this emission.

Problem

One of the emission lines of the hydrogen atom has a wavelength of 93.8 nm. (b) Determine the initial and final values of n associated with this emission.

Solution

The emitted light has a wavelength of 93.8 nm. When you look at the electromagnetic spectrum, this wavelength lies in the UV region. When the emission is within the UV region we call this the Lyman Series.

Lyman series is referred to when an electron goes from higher numbered shell to the 1st shell.

Based on the Lyman Series, we know now that the final energy level is the first shell where:

nf = 1

We can determine ninitial using the Bohr Equation shown below:

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