Chapter 6: Problem 9
What are the basic SI units for (a) the wavelength of light, (b) the frequency of light, (c) the speed of light?
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Identify the specific element that corresponds to each of the following electron configurations: (a) \(1 s^{2} 2 s^{2}\), (b) \(1 s^{2} 2 s^{2} 2 p^{4}\), (c) \([\mathrm{Ar}] 4 s^{1} 3 d^{5}\), (d) \([\mathrm{Kr}] 5 s^{2} 4 d^{10} 5 p^{4}\), (e) \(1 s\) ?
Sodium metal requires a photon with a minimum energy of \(4.41 \times 10^{-19} \mathrm{~J}\) to emit electrons. (a) What is the minimum frequency of light necessary to emit electrons from sodium via the photoelectric effect? (b) What is the wavelength of this light? (c) If sodium is irradiated with light of \(439 \mathrm{~nm}\), what is the maximum possible kinetic energy of the emitted electrons? (d) What is the maximum number of electrons that can be freed by a burst of light whose total energy is \(1.00 \mu \mathrm{J} ?\)
The series of emission lines of the hydrogen atom for which \(n_{f}=3\) is called the Paschen series. (a) Determine the region of the electromagnetic spectrum in which the lines of the Paschen series are observed. (b) Calculate the wavelengths of the first three lines in the Paschen series - those for which \(n_{i}=4,5\), and 6 .
Which of the quantum numbers governs (a) the shape of an orbital, (b) the energy of an orbital, (c) the spin properties of the electron, (d) the spatial orientation of the orbital?
Write the condensed electron configurations for the following atoms, and indicate how many unpaired electrons each has: (a) \(\mathrm{Ga},(\mathrm{b}) \mathrm{Ca},(\mathrm{c}) \mathrm{V},(\mathrm{d}) \mathrm{I},(\mathrm{e}) \mathrm{Y}\), (f) \(\mathrm{Pt}\) (g) Lu.
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