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: Molybdenum metal must absorb radiation with a minimum frequency of 1.09 x 10 15 s-1 before it can eject an electron from its surface via the photoelectric effect. (a) What is the minimum energy needed to eject an electron?

Solution: Molybdenum metal must absorb radiation with a minimum frequency of 1.09 x 10 15 s-1 before it can eject an electron from its surface via the photoelectric effect. (a) What is the minimum energy needed

Problem

Molybdenum metal must absorb radiation with a minimum frequency of 1.09 x 10 15 s-1 before it can eject an electron from its surface via the photoelectric effect. (a) What is the minimum energy needed to eject an electron?

Solution

We’re being asked what is the minimum energy needed to eject an electron from a molybdenum metal. The minimum frequency of radiation that must be absorbed by the metal is 1.09x1015 s-1.

We can calculate the minimum energy from the minimum frequency absorbed using the equation:

E=hν

 E = energy = J
▪ h = Planck's constant = 6.626x10-34 Js
 ν = frequency = Hz or s-1

Solution BlurView Complete Written Solution