Here are some data collected on a sample of cesium exposed to various energies of light. Electrons are emitted from the surface of a metal Light energy (eV) Electron emitted? Electron KE when it's exposed to light. This is called the photoelectric effect. Each metal has a certain threshold frequency of light, below which nothing happens. Right at this threshold frequency, an electron is emitted. Above this frequency, the electron is emitted and the extra energy is transferred to the electron. (eV) 2.12 no 2.13 no 2.14 yes 2.15 yes 0.01 The equation for this phenomenon is 2.16 yes 0.02 KE= hv – hvo *Note that 1 eV (electron volt) = 1.60 × 10¬19 J. where KEİS the kinetic energy of the emitted electron, h = 6.63 × 10-34 J.s is Planck's constant, v is the frequency of the light, and vo is the threshold frequency of the metal. Part A Also, since E = hv, the equation can also be written as What is the threshold frequency vo of cesium? КЕ-Е-Ф Express your answer numerically in hertz. • View Available Hint(s) where E is the energy of the light and o is the binding energy of the electron in the metal. ? Vo = Hz Submit

Here are some data collected on a sample of cesium exposed to various energies of light. Electrons are emitted from the surface of a metal Light energy (eV) Electron emitted? Electron KE when it's exposed to light. This is called the photoelectric effect. Each metal has a certain threshold frequency of light, below which nothing happens. Right at this threshold frequency, an electron is emitted. Above this frequency, the electron is emitted and the extra energy is transferred to the electron. (eV) 2.12 no 2.13 no 2.14 yes 2.15 yes 0.01 The equation for this phenomenon is 2.16 yes 0.02 KE= hv – hvo *Note that 1 eV (electron volt) = 1.60 × 10¬19 J. where KEİS the kinetic energy of the emitted electron, h = 6.63 × 10-34 J.s is Planck's constant, v is the frequency of the light, and vo is the threshold frequency of the metal. Part A Also, since E = hv, the equation can also be written as What is the threshold frequency vo of cesium? КЕ-Е-Ф Express your answer numerically in hertz. • View Available Hint(s) where E is the energy of the light and o is the binding energy of the electron in the metal. ? Vo = Hz Submit

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

Here are some data collected on a sample of cesium exposed to various energies of light. Light energy(eVeV) Electron emitted? Electron KEKEKE(eVeV) 3.87 no — 3.88 no — 3.89 yes 0 3.90 yes 0.01 3.91 yes 0.02 *Note that 1 eV (electron volt)=1.60×10−19 J1 eV (electron volt)=1.60×10−19 J. Part A What is the threshold frequency ν0ν0nu_0 of cesium? Express your answer numerically in hertz.
You will make a graph of your data from the helium spectrum. What purpose will it serve in the data analysis? O It will allow us to calculate the energies of the lines in the helium spectrum based on their wavelengths. O It will allow us to calculate the energies of the lines in the hydrogen spectrum based on their wavelengths. O It will allow us to calculate the wavelengths of the lines in the helium spectrum based on their positions. O It will allow us to calculate the wavelengths of the lines in the hydrogen spectrum based on their positions. O It will allow us to calculate the colors of the lines in the hydrogen spectrum based on their times.
What happens to an electron in an atom when it absorbs energy? Check all that apply The electron re-emits the energy as light O The electron gets promoted to a higher energy level The extra energy increases the speed of the electron in its orbitals The electron stores energy for later use V The electron falls from the excited state back down to the ground state
7 please
57 Which of the following statements is TRUE? Select one: The maximum number of electrons in the second shell (n=2) is 8. The Heisenberg Uncertainty Principle states that no two electrons can have the same mass and speed. Nitrogen has one unpaired electron. Light is a wave and never behaves as a particle. Infrared light has a higher energy than visible light.
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.
4.Make a prediction using your model. If an electron were to emit a photon and move from the n=3 level to the n=1 level, what wavelength of light would it emit? (Hint: use the Ryberg equation) Would this be a bigger energy What would be the energy change for this transition? change or a smaller energy change that the transition from the n=3 to the n=2 transition? Would you be able to see this energy change (will it be visible light?) What part of the electromagnetic spectrum should you look in to find these photons, the ultraviolet or the infrared?
The energy of an electron is based on its quantum numbers that define which characteristics? color charge number of electrons distance from nucleus orientation in space shape For the fourth level (n = 4), the subshells that you would find include 12
Consider the transition from the energy levels n = 3 to n = 5. What is the wavelength associated with this transition, in nm? nm In what spectral region does this transition occur? this wavelength is in the ultraviolet this wavelength is in the visible this wavelength is in the infrared Is energy absorbed or released for this transition? energy is absorbed energy is released
please solve question 1 and 2, thanks alot sir