Inorganic Chemistry
5th Edition
ISBN: 9780321811059
Author: Gary L. Miessler, Paul J. Fischer, Donald A. Tarr
Publisher: Prentice Hall
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Chapter 2, Problem 2.3P
The transition from the
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Chapter 2 Solutions
Inorganic Chemistry
Ch. 2.1 - Determine the energy of the transition from nh=3...Ch. 2.2 - Describe the angular nodal surfaces for a dz2...Ch. 2.2 - Prob. 2.3ECh. 2.2 - A third possible state for the p4 configuration...Ch. 2.2 - A nitrogen atom, with three 2p electrons, could...Ch. 2.2 - Calculate the effective nuclear charge on a 5s,...Ch. 2.2 - Calculate the effective nuclear charge on a 7s,...Ch. 2.3 - Explain why all three graphs in Figure 2.14 have...Ch. 2 - Determine the de Brogue wavelength of a. an...Ch. 2 - Using the equation E=RH(1221nh2) determine the...
Ch. 2 - The transition from the n=7 to the n=2 level of...Ch. 2 - Emissions are observed at wavelengths of 383.65...Ch. 2 - What is the least amount of energy that can be...Ch. 2 - Hydrogen atom emission spectra measured from the...Ch. 2 - The Rydberg constant equation has two terms that...Ch. 2 - For the 3pz and 4dxz hydrogen-like atomic...Ch. 2 - Repeat the exercise in Problem 2.7 for the 4s and...Ch. 2 - Repeat the exercise in Problem 2.7 for the 5s and...Ch. 2 - The 4fz(x2y2) orbital has the angular function...Ch. 2 - Prob. 2.13PCh. 2 - The label for an fz2 orbital, like that for a dz2...Ch. 2 - a. Determine the possible values for the l and ml...Ch. 2 - a. What are the values of quantum numbers I and n...Ch. 2 - a. At most, how many electrons in an atom can have...Ch. 2 - Determine the Coulombic and exchange energies for...Ch. 2 - Prob. 2.19PCh. 2 - Prob. 2.20PCh. 2 - What states are possible for a d3 configuration?...Ch. 2 - Provide explanations of the following phenomena:...Ch. 2 - Give electron configurations for the following:...Ch. 2 - Predict the electron configurations of the...Ch. 2 - Radial probability plots shed insight on issues of...Ch. 2 - Briefly explain the following on the basis of...Ch. 2 - Briefly explain the following on the basis of...Ch. 2 - a. Which 2+ ion has two 3d electrons? Which has...Ch. 2 - A sample calculation in this chapter showed that,...Ch. 2 - Ionization energies should depend on the effective...Ch. 2 - Prepare a diagram such as the one in Figure (a)...Ch. 2 - Why are the ionization energies of the alkali...Ch. 2 - The second ionization of carbon (C+C2++e) and the...Ch. 2 - Prob. 2.35PCh. 2 - Prob. 2.36PCh. 2 - The second ionization energy involves removing an...Ch. 2 - Prob. 2.38PCh. 2 - On the basis of electron configurations, explain...Ch. 2 - a. The graph of ionization energy versus atomic...Ch. 2 - The second ionization energy of He ¡s almost...Ch. 2 - The size of the transition-metal atoms decreases...Ch. 2 - Predict the largest and smallest radius in each...Ch. 2 - Select the best choice, and briefly indicate the...Ch. 2 - Select the best choice, and briefly indicate the...Ch. 2 - There are a number of Web sites that display...Ch. 2 - Prob. 2.47P
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- Calculate the wavelength of the Balmer line of the hydrogen spectrum in which the initial n quantum number is 5 and the final n quantum number is 2.arrow_forwardWarm objects emit electromagnetic radiation in the infrared region. Heat lamps employ this principle to generate infrared radiation. Water absorbs infrared radiation with wavelengths near 2.80 m. Suppose this radiation is absorbed by the water and converted to heat. A 1.00-L sample of water absorbs infrared radiation, and its temperature increases from 20.0C to 30.0C. How many photons of this radiation are used to heat the water?arrow_forwardA hydrogen atom in the ground stale absorbs a photon whose wavelength is 95.0 nm. The resulting excited atom then emits a photon of 1282 nm. What are the regions of the electromagnetic spectrum for the radiations involved in these transitions? What is the principal quantum number of the final state resulting from the emission from the excited atom?arrow_forward
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- The most prominent line in the emission spectrum of aluminum is at 396.15nm. What is the frequency of this line? What is the energy of one photon with this wavelength? Of 1.00 mol of these photons?arrow_forwardAccording to a relationship developed by Niels Bohr, for an atom or ion that has a single electron, the total energy, En, of an electron in a stable orbit of quantum number n is En = [Z2/n2] (2.179 1018 J) where Z is the atomic number. Calculate the ionization energy for the electron in a ground-state He+ ion.arrow_forward6.85 The visible lines in the hydrogen atom emission spectrum arise from transitions with a final state with n = 2. In what spectral region should we expect to find transitions that have a final state of n = 1 ? Explain your reasoning using an energy level diagram similar to the one in Problem 6.26.arrow_forward
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