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: Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410.1 nm.

Solution: Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410.1 nm.

Problem

Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410.1 nm.

Solution

Violet light is a part of the visible portion of the electromagnetic spectrum.


The energy and frequency of electromagnetic waves are related by this equation.


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Where,

E = energy

h = Planck’s constant

𝜈 = frequency


The relation between the speed of light, it frequency and wavelength is:


null


Where,

c = speed of light

λ = wavelength

𝜈 = frequency


Isolating 𝜈 and placing it in the first equation.


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