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: Certain elements emit light of a specific wavelength when they are burned. Historically, chemists used such emission wavelengths to determine whether specific elements were present in a sample. Some characteristic wavelengths for some of the elements are
Ag328.1 nm Fe372.0 nm
Au267.6 nm K404.7 nm
Ba455.4 nm Mg285.2 nm
Ca422.7 nm Na589.6 nm
Cu324.8 nm Ni341.5 nm
Which element emits photons of highest energy?

Solution: Certain elements emit light of a specific wavelength when they are burned. Historically, chemists used such emission wavelengths to determine whether specific elements were present in a sample. Some c

Problem

Certain elements emit light of a specific wavelength when they are burned. Historically, chemists used such emission wavelengths to determine whether specific elements were present in a sample. Some characteristic wavelengths for some of the elements are

Ag328.1 nm
Fe372.0 nm
Au267.6 nm
K404.7 nm
Ba455.4 nm
Mg285.2 nm
Ca422.7 nm
Na589.6 nm
Cu324.8 nm
Ni341.5 nm


Which element emits photons of highest energy?

Solution

We have to determine, which element emits photons of highest energy, using the given wavelengths.


The energy of photon is related to its frequency by this formula:

E = 

Where,

h = Planck's constant (6.626×10–34 J•s)

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