The work function (binding energy) is the energy that must be supplied to cause the release of an electron from a photoelectric material. The corresponding photon frequency is the threshold frequency. The higher the energy of the incident light, the more kinetic energy the electrons have in moving away from the surface. The work function for nickel (used in rechargeable batteries) is equivalent to 483.4 kJ/mol photons. Use this information to calculate the energy, wavelength, and velocity of ejected electrons. What is the maximum wavelength (in nm) at which the electron can be removed from nickel? h = 6.626 x 10-34 J·s; C = 2.998 x 108 m/s

The work function (binding energy) is the energy that must be supplied to cause the release of an electron from a photoelectric material. The corresponding photon frequency is the threshold frequency. The higher the energy of the incident light, the more kinetic energy the electrons have in moving away from the surface. The work function for nickel (used in rechargeable batteries) is equivalent to 483.4 kJ/mol photons. Use this information to calculate the energy, wavelength, and velocity of ejected electrons. What is the maximum wavelength (in nm) at which the electron can be removed from nickel? h = 6.626 x 10-34 J·s; C = 2.998 x 108 m/s

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: Three of the known wavelengths of the emission spectrum of helium are 402.6 nm, 447.1 nm and 587.5…

A: Electromagnetic spectrum involves different radiations from the lowest to the highest frequency…

Q: Gamma rays microwaves ultraviolet light X rays radio waves red light infrared light violet light

A: Radio wave>microwave>infrared>red light>violet light>ultraviolet>x-ray>gamma…

Q: When a metal was exposed to photons at a frequency of 1.11 × 1015 s-1, electrons were emitted with a…

A: Given frequency = 1.11×10¹⁵ s-¹ Kinetic energy = 3×10-¹⁹ J We have to find work function

Q: In his explanation of the threshold frequency in the photoelectric effect, Einstein reasoned that…

A: The relationship between the longest wavelength of radiation which can cause the photoelectric…

Q: Calculate the frequency of the light emitted by an atom with a wavelength of 496 nm.

A: We have given that Wavelength of emmited light = 496nm Frequency : Frequency is the number of…

Q: When a metal was exposed to photons at a frequency of 1.10 x 1015 s-, electrons were emitted with a…

Q: The energy of a single photon is 1.005x10-19 J. How many moles of photons would be required to give…

A: Bohr’s theory of atoms was applicable for one electron system. It purposed the energy levels in an…

Q: There are four hydrogen atomic emission lines in the visible region of the electromagnetic spectrum.…

Q: Workshop 6: Introduction to Spectroscopy Part I: Interpreting Visible Emission Spectra Street lights…

Q: Determine the frequency and energy for light with a wavelength of 694.0 nm. V = kJ/mol E = What is…

Q: A retina of a human eye can detect light when radiant energy incident on it is at least 4.0 x 10^-17…

A: Relation between energy and wavelength:

Q: Part A The energy required to dislodge electrons from rubidium metal via the photoelectric effect is…

A: We are given with the Energy required, E = hc/λ = 218 kJ/mol = 218 × 1000 J/mol Where c is velocity…

Q: A foolish man attempted to rob a bank but only brought his red laser pointer, with a wavelength of…

Q: A carbon dioxide laser produces radiation with a wavelength of 1.06 x 104 nm. What is the frequency…

Q: The minimum energy needed to eject electrons from chromium metal via the photoelectric effect is 434…

A: The relation between the energy and wavelength of radiation is as follows, Given: The minimum…

Q: What is the change in energy experienced by an electron in a hydrogen atom that undergoes an n = 2…

A: According to Bohr's model of an atom, electrons, having a negative charge, revolves around the…

Q: If light has a wavelength of 715 nm, what is the energy of this light expressed with units of…

Q: Heated lithium atoms emit photons of light with an energy of . What is the calculated frequency and…

Q: Consider the four scenarios involving visible light. In scenario A, visible light has a wavelength…

Q: When we model light (EM radiation) as a particle, we call it a photon -- a packet of energy. How…

A: The concept used in this question is taken from general chemistry. According to question Light has…

Q: A bank robber forgot his tools, and only brought a red laser pointer, with a wavelength of 650. nm.…

A: We have to calculate the number of photons required.

Q: A photon strikes a hydrogen atom with enough energy to remove an electron in the n=4 energy level…

Q: Red lights has a wavelength of about 6.8 x 102 nm. What

A: ν = C/λ ----(1) Where ν = frequency of light = ? C = light velocity = 3 x 108 m /s λ = wavelenght…

Q: A certain metal is exposed to light with increasing frequency and energy of the photons. Electrons…

A: Please find the attached images for answer

Q: A laser is emitting photons with a wavelength of 624.6 nm. What is the energy for 1 mole of these…

A: The energy of the laser light can be calculated by - E = hv Or E = h c/^ Here - E = energy of the…

Q: A photon has the energy 2.33 × 10–20 J. What is this photon's frequency?

A: We know that , energy of a photon is related to Plank's constant as,…

Q: For light with a wavelength of 6.245 x 10-7 m, determine the following: The frequency of this light…

A: (1) Calculate the frequency of light: Hence, the frequency of light is 4.801×1014 s-1

Q: number of photons

Q: Green light has a wavelength of approximately 5.00 x 102 nm. What is the frequency? Calculate the…

A: CALCULATION Wavelength = 5.00×102 nm= 5.0×10-7 m Speed of light = 3.0×108 m/s Frequency = 3.0×108…

Q: A hydrogen atom absorbs energy and an electron is excited to the n = 2 shell. When the electron…

Q: Consider an atom of hydrogen that absorbs light of a wavelength 384.0 nm. What is the energy, in…

Q: A molecule emits a photon with 6.347x10–19 J of energy. What is the wavelength, in nanometers, does…

A: Given:Energy of photon =6.347 x 10-19 JTo find: Wavelength of photon, λ = ?also we know,speed of…

Q: The work function (ϕ) for the a metal is 7.00 x 10 -19 J. What is the longest wavelength of…

A: Given, work function (ϕ) for metal is 7.00 x 10 -19 J.

Q: Silver has a threshold frequency of 1040 THz, while gold has a threshold frequency of 1330 THz.…

Q: The work function (binding energy) is the energy that must be supplied to cause the release of an…

Q: The energy levels the electron can occupy in the Li2+ ion can be calculated using the energy level…

Concept explainers

Atomic Structure

The basic structure of an atom is defined as the component-level of atomic structure of an atom. Precisely speaking an atom consists of three major subatomic particles which are protons, neutrons, and electrons. Many theories have been stated for explaining the structure of an atom.

Shape of the D Orbital

Shapes of orbitals are an approximate representation of boundaries in space for finding electrons occupied in that respective orbital. D orbitals are known to have a clover leaf shape or dumbbell inside where electrons can be found.

Question

The work function (binding energy) is the energy that
must be supplied to cause the release of an electron
from a photoelectric material. The corresponding
photon frequency is the threshold frequency. The
higher the energy of the incident light, the more
kinetic energy the electrons have in moving away
from the surface. The work function for nickel (used
in rechargeable batteries) is equivalent to 483.4
kJ/mol photons. Use this information to calculate the
energy, wavelength, and velocity of ejected electrons.
80
F3
What is the maximum wavelength (in nm) at which
the electron can be removed from nickel? h = 6.626
x 10-34 J·s; c = 2.998 x 108 m/s
SEP
19
a
F4
F5
tv
♫
c
F6
NIMIZA
&
8
F7
DII
F8
(
|
8
FO

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

When a metal was exposed to photons at a frequency of 1.31 x 105 s-', electrons were emitted with a maximum kinetic energy of 3.80 × 10-19 J. Calculate the work function, D, of this metal. J/photon What is the maximum number of electrons that could be ejected from this metal by a burst of photons (at some other frequency) with a total energy of 8.97 × 10-7 J? number of electrons:
In scenario A, visible light has a wavelength of 690.3 nm. Determine its frequency, energy per photon, and color. frequency: s-1 energy per photon: The visible light in scenario A is J
The figure below provides the approximate frequency and wavelength values for different types of electromagnetic radiation. What is the wavelength and radiation type corresponding to a photon with an energy of 2.23 × 10–16 J? (picture attached) A. 6.69 x 10–8 m, ultraviolet light B. 3.36 x 10–17 m, gamma rays C. 1.12 × 109 m, ultraviolet light D. 8.91 × 10–10 m, X-rays
Use the wave energy equation to calculate the energy or frequency of a photon of light. The frequency of a photon of light is 2.8 x 107 Hz. What is its energy?
An electron in a hydrogen atom goes from the n = 6 to the n = 3 level. What is the wavelength of the photon that is emitted in units of nanometers
The work function (Φ) for a metal is 5.40×10-19 J. What is the longest wavelength of electromagnetic radiation that can eject an electron from the surface of a piece of the metal?
The minimum frequency of light needed to eject electrons from a metal is called the threshold frequency, ?0. Find the minimum energy needed to eject electrons from a metal with a threshold frequency of 3.20×1014 s−1. With what maximum kinetic energy will electrons be ejected when this metal is exposed to light with a wavelength of 285 nm?
Convert between number of photons and energy given a particular wavelength. Low level light therapy (LLLT) using RED light was observed to promote wound healing. The daily dose provided was 24 J/cm. Given the wavelength of 635 nm, how many photons were required to deliver the dose to a 1 cm? area?
The minimum energy required to remove an electron from a certain metal is 3.7 x 10– 19 J. If the metal surface is struck by light having a wavelength of 5.00 x 102 nm, what is the kinetic energy of the electron ejected from the metal?
Radiation in the ultraviolet region of the electromagnetic spectrum is quite energetic. It is this radiation that causes dyes to fade and your skin to develop a sunburn. If you are bombarded with 1.00 mol of photons with a wavelength of 320. nm, what amount of energy, in kilojoules per mole of photons, are you being subjected to? Energy = kJ/mol
When copper is bombarded with high-energy electrons, X rays are emitted. Calculate the energy (in joules) associated with the photons if the wavelength of the X rays is 0.154 nm.
The electron binding energy for copper metal is 1.258 X 10−19 J. Find the longest wavelength of light in nanometers that could eject electrons from copper with a kinetic energy of 5.264 x 10 -21 Jin a photoelectric effect experiment. On your answer sheet, identify the wavelength range in which you expect to find this wavelength.