Finally, examine the atomic spectrum below. Estimate the wavelength of each spectral line, then use that collection of wavelengths to try and determine the identity of the element using the internet. This is the kind of work a graduate student in chemistry might be assigned to do. 400 450 500 550 600 650 700 750 wavelength (nm) Identity of the element

Finally, examine the atomic spectrum below. Estimate the wavelength of each spectral line, then use that collection of wavelengths to try and determine the identity of the element using the internet. This is the kind of work a graduate student in chemistry might be assigned to do. 400 450 500 550 600 650 700 750 wavelength (nm) Identity of the element

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter5: Electrons In The Atom

Section: Chapter Questions

Problem 118A

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Similar questions

Sketch the major features (number of peaks and relative intensities for the peaks) of the expected photoelectron spectrum for atoms of nitrogen.
Until recently, it was thought that Ca was unstable, and that the Ca atom therefore had a negative electron affinity. Some new experiments have now measured an electron affinity of +2.0kJmol1 for calcium. What is the longest wavelength of light that could remove an electron from Ca ? In which region of the electromagnetic spectrum does this light fall?
When a tube containing hydrogen atoms is energized by passing several thousand volts of electricity into the tube, the hydrogen emits light than when passed through a prism, resolves into the "bright line" spectrum shown in Fig. 11.10. Why do hydrogen atoms emit bright lines of specific wavelengths rather than a continuous spectrum?
Using vertical lines, indicate the transitions from Exercise 58 on an energy-level diagram for the hydrogen atom (see Fig. 2-9).
Using Fig. 2-30, list the elements (ignore the lanthanides and actinides) that have ground-state electron configurations that differ from those we would expect from their positions in the periodic table.
One bit of evidence that the quantum mechanical model is correct lies in the magnetic properties of matter. Atoms with unpaired electrons are attracted by magnetic fields and thus are said to exhibit pararamagnetism. The degree to which this effect is observed is directly related to the number of unpaired electrons present in the atom. Consider the ground-state electron configurations for Li, N, Ni, Te, Ba, and Hg. Which of these atoms would be expected to be paramagnetic, and how many unpaired electrons are present in each paramagnetic atom?
Identify the element that corresponds to each of the simplified photoelectron spectral data given below. (Energy data taken from D. A. Shirley, R. L Martin, S. P. Kowalczyk. F. R. McFeely, and L. Ley: Core-electron binding energies of the first thirty elements, Physical Review B, Vol. 15, pp. 544-552, 1977.) (a) There are peaks at energies of 64.8 and 5.4 eV, corresponding to 2 and 1 electrons, respectively. (b) There are peaks at energies of 3614, 384, 301, 40.9, 24.7, and 4.34 eV, corresponding to 2, 2, 6, 2, 6, and 1 electrons, respectively. (c) There are peaks at energies of 4494, 503, 404, 56.4, 33.6, 8.01, and 6.65 eV, corresponding to 2, 2, 6, 2, 6, 1, and 2 electrons, respectively.
What does wave-particle duality mean? What are its implications in our modem view of atomic structure?
describe trace analysis and explain its role in materials testing.