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: What is the wavelength (in nm) of light emitted from a hydrogen atom when an electron falls from the n = 5 to n = 2 energy level?a. 780 b. 656 c. 486 d. 434 e. 308

Problem

What is the wavelength (in nm) of light emitted from a hydrogen atom when an electron falls from the n = 5 to n = 2 energy level?

a. 780
b. 656
c. 486
d. 434
e. 308

Solution

We’re being asked to calculate for the wavelength of light emitted by an electron to transition from n=5 to n = 2.


We’re going to use the Balmer Equation which relates wavelengths to a photon’s electronic transitions.

1λ=RZ21n2final-1n2initial

λ = wavelength, m
R = Rydberg constant = 1.097x107 m-1 
Z = atomic number of the element
ninitial = initial energy level
nfinal = final energy level


Calculate the wavelength of light emitted (λ):


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