Skip to main content
Pearson+ LogoPearson+ Logo
Ch.5 - Periodicity & Electronic Structure of Atoms
McMurry - Chemistry 8th Edition
McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook
All textbooksMcMurry 8th EditionCh.5 - Periodicity & Electronic Structure of AtomsProblem 4
Chapter 5, Problem 4

Which type of electromagnetic radiation will cause the greatest number of electrons to be ejected from zinc metal with a work function of 350 kJ/mol? (LO 5.4, 5.5)(a) Dim light with a wavelength of 320 nm (b) Dim light with a wavelength of 360 nm (c) Bright light with a wavelength of 360 nm (d) Bright light with a wavelength of 375 nm

Verified step by step guidance
1
Convert the work function from kJ/mol to Joules per electron by using Avogadro's number. The work function in Joules per electron is calculated by dividing the given work function by Avogadro's number (approximately 6.022 \(\times\) 10^23 mol^-1).
Calculate the energy of the photons for each wavelength using the equation \(E = \frac{hc}{\lambda}\), where \(h\) is Planck's constant (6.626 \(\times\) 10^-34 J s), \(c\) is the speed of light (3.00 \(\times\) 10^8 m/s), and \(\lambda\) is the wavelength in meters.
Convert the wavelengths from nanometers to meters by multiplying by 10^-9.
Compare the photon energy calculated for each wavelength to the work function energy in Joules per electron. Only photons with energy equal to or greater than the work function can eject electrons.
Identify which option(s) have photon energies that meet or exceed the work function energy. The intensity (brightness) of the light does not affect the energy per photon, so it does not influence which type of light ejects more electrons, but rather how many electrons are ejected if the energy condition is met.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
4m
Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Photoelectric Effect

The photoelectric effect is the phenomenon where electrons are emitted from a material when it absorbs light or electromagnetic radiation. The energy of the incoming photons must exceed the work function of the material for electrons to be ejected. This concept is crucial for understanding how light interacts with metals and the conditions necessary for electron emission.
Recommended video:
Guided course
01:26
Photoelectric Effect

Work Function

The work function is the minimum energy required to remove an electron from the surface of a material. It is typically expressed in electron volts (eV) or kilojoules per mole (kJ/mol). In this question, zinc has a work function of 350 kJ/mol, meaning that only photons with energy greater than this value can cause electron ejection.
Recommended video:
Guided course
01:52
Work Function Calculation Example

Photon Energy and Wavelength

The energy of a photon is inversely related to its wavelength, described by the equation E = hc/λ, where E is energy, h is Planck's constant, c is the speed of light, and λ is the wavelength. Shorter wavelengths correspond to higher energy photons. Understanding this relationship is essential for determining which light sources can effectively eject electrons from zinc.
Recommended video:
Guided course
01:40
Photon Energy Formulas
Related Practice
Textbook Question

Which wave corresponds to higher energy radiation? (LO 5.1) (a)

(b)

5
views
Textbook Question
What is the energy (in kJ) of one mole of photons of ultraviolet light with a wavelength of 85 nm? (LO 5.3)(a) 1.4 * 10-6 kJ(b) 1.4 * 103 kJ(c) 2.4 * 1014 kJ(d) 2.4 * 10-15 kJ
3
views
Textbook Question

When a copper salt such as Cu(NO3)2 is burned in a flame, a blue-green color is emitted. Which figure represents the emission spectrum for the element copper? (LO 5.6)? (a)

(b)

(c)

(d)

3
views
Textbook Question
Which arrow in the energy diagram for an atom represents the absorption of light with the shortest wavelength? (LO 5.7)

1
views
1
rank
Textbook Question
Calculate the wavelength in nm of the light emitted when an electron makes a transition from an orbital in n = 5 to an orbital in n = 2 in the hydrogen atom. (LO 5.8)(a) 2.31 * 10-3 nm (b) 4.34 * 10-2 nm (c) 231 nm(d) 434 nm