How does the number of lines in the emission spectrum for an element compare with the number of lines in the absorption spectrum? There are the same number of lines in the emission spectrum as the absorption spectrum. O There are half as many lines in the emission spectrum as the absorption spectrum. O An element either has an emission spectrum or an absorption spectrum, but not both. There are twice as many lines in the emission spectrum as the absorption spectrum.

How does the number of lines in the emission spectrum for an element compare with the number of lines in the absorption spectrum? There are the same number of lines in the emission spectrum as the absorption spectrum. O There are half as many lines in the emission spectrum as the absorption spectrum. O An element either has an emission spectrum or an absorption spectrum, but not both. There are twice as many lines in the emission spectrum as the absorption spectrum.

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

None
The diagram below shows the wavelengths of four emission lines of the H atom. Using the Bohr model, four of the six transitions listed below each correspond to one of these lines in the spectrum. Which transition is responsible for the line at 410 nm? 410 nm 434 nm Light A85 nm Hatoms Prism 657 nm Emission Spectrum On = 2 to n = 3 On= 3 to n = 2 On-4 to n =2 On= 5 to n = 2 On- 6 to n = 2 On=1 to n = 5
4
The light emitted from one of the following electronic transitions (n=4 to n = 3 or n = 3 to n = 2) in the hydrogen atom causes the photoelectric effect in a particular metal while light from the other transition does not. Which transition causes the photoelectric effect and why?
A photon is emitted during the transition from the n = 7 state to the n = 1 state in the hydrogen atom. Note: Rydberg constant: 2.18x10-18 J Calculate the wavelength of this photon
Which of the following colors from the visible range has the greatest frequency yellow red orange green O blue Which of the following colors from the visible range has the shortest wavelength green red orange O blue O yellow
Using the Bohr model, pick which electronic transition will emit a photon with the shortest wavelength. Group of answer choices n = 1 → n = 3 n = 2 → n = 1 n = 6 → n = 4 n = 3 → n = 2
Electrons in potassium ions (excited by heating in a flame) emit visible light whose wavelength is 409nm. What is the frequency of this light? What is the energy of one quantum of this light? What color light is it?
Q1: The results of a photoelectric experiment comparing two different metals (A and B) are shown below. A B Frequency of light In the experiment, the KE of the photoelectrons is plotted vs. the frequency of the light used for each of the metals. Which metal has the greater p? Group of answer choices: B/cannot be determined/A Photoelectron KE
A mercury atom emits light at many wavelengths, two of which are at (1) 404.7 nm and (2) 435.8 nm. Both of these transitions are to the same final state. Determine the energy of each emitted wavelength (in J). A E1 = 7.908 x 10-19 J and E2 = 6.558 x10-19 J B E1 = 5.908 x 10-19 J and E2 = 5.558 x10-19J E1 = 4.908 x 1019 J and E2 = 4.558 x10-19J D) E1 = 4.628 x 10-19 J and E2 = 4.968 x10-19 J
Calculate the frequency and the energy for one photon of orange light (625 nm) traveling at the speed of light.
1. Complete following table for regions of the visible region of the electromagnetic spectrum: Visible Region Wavelength Range (nm) Visible Region Wavelength Range (nm) purple/violet yellow blue orange green red