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 cesium (used in IR lamps) is equivalent to 202.6 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 cesium? h = 6.626 x 10-34 J·s; c= 2.998 × 108 m/s³

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 cesium (used in IR lamps) is equivalent to 202.6 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 cesium? h = 6.626 x 10-34 J·s; c= 2.998 × 108 m/s³

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

Similar questions

An electron absorbs a single photon with a wavelength = 127 nm. Calculate the energy of the photon.
Consider an electron in the hydrogen atom that transitions from the n=4 energy level to the n=2 energy level, 1. Calculate the wavelength (in nm) associated with the electron 2. Calculate the frequency (in s-1) associated with the electron 3. Calculate the amount of energy (in joules) of 1 electron that is emitted 4. Calculate the amount of energy (in kilojoules) of 1 mole of electrons that is emitted
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
An energy of 353 kJ/mol is required to cause a magnesium atom on the metal's surface to lose an electron. Calculate the lowest frequency of light that can ionize a magnesium atom.
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
use the bohr equation to find the wavelength of the photon emitted when an H atom undergoes a transition from n=5 to n=2
The photoelectric effect can be used in engineering designs for practical applications. For example, infrared goggles used in night-vision applications have materials that give an electrical signal with exposure to the relatively long wavelength of IR light. If the energy needed for signal generation is 7.6 x 10-40 J, what is the minimum wavelength? What is the frequency of light that can be detected? c = 2.998 × 10° m/s h = 6.626 x 10-34 J s m S -1
The work function (φ) for a metal is the amount of energy needed to eject an electron from the surface of the metal via the photoelectric effect. For nickel φ = 8.25 x 10-19J. Will a photon with a wavelength (λ) of 250.0 nm have enough energy to eject an electron from nickel? If the speed of an electron in the n = 4 energy level of a hydrogen electron is 2.3 x 106 m/s, what is the de Broglie wavelength of this electron in nanometers (the mass of an electron is 9.10938 x 10-31 kg). Note: 1 ? = 1 ?? ∙?2 An F-15 Strike Eagle weighs in at roughly 32,000 kg fully loaded. If an F-15 Eagle is traveling at 3,017 kilometers per hour, what is the de Broglie wavelength associated with the aircraft at this speed in nanometers?
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?
A certain microwave oven delivers 750 watts (J/s) of power to a coffee cup containing 66.6 g of water at 37.5°C. If the wavelength of microwaves in the oven is 9.75 cm, how long does it take, and how many photons must be absorbed, to make the water boil? The specific heat capacity of water is 4.18 J/ °C•g and assume only the water absorbs the energy of the microwaves. S photons
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?
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