Inorganic Chemistry
5th Edition
ISBN: 9780321811059
Author: Gary L. Miessler, Paul J. Fischer, Donald A. Tarr
Publisher: Prentice Hall
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Textbook Question
Chapter 2, Problem 2.5P
What is the least amount of energy that can be emitted by an excited electron in a hydrogenatom falling from an excited state directly to 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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- What is the difference between an atom’s ground state and an excited state?arrow_forwardInvestigating Energy Levels Consider the hypothetical atom X that has one electron like the H atom but has different energy levels. The energies of an electron in an X atom are described by the equation E=RHn3 where RH is the same as for hydrogen (2.179 1018 J). Answer the following questions, without calculating energy values. a How would the ground-state energy levels of X and H compare? b Would the energy of an electron in the n = 2 level of H be higher or lower than that of an electron in the n = 2 level of X? Explain your answer. c How do the spacings of the energy levels of X and H compare? d Which would involve the emission of a higher frequency of light, the transition of an electron in an H atom from the n = 5 to the n = 3 level or a similar transition in an X atom? e Which atom, X or H, would require more energy to completely remove its electron? f A photon corresponding to a particular frequency of blue light produces a transition from the n = 2 to the n = 5 level of a hydrogen atom. Could this photon produce the same transition (n = 12 to n = 5) in an atom of X? Explain.arrow_forwardAs the weapons officer aboard the Srarship Chemistry, it is your duty to configure a photon torpedo to remove an electron from the outer hull of an enemy vessel. You know that the work function (the binding energy of the electron) of the hull of the enemy ship is 7.52 1019 J. a. What wavelength does your photon torpedo need to be to eject an electron? b. You find an extra photon torpedo with a wavelength of 259 nm and fire it at the enemy vessel. Does this photon torpedo do any damage to the ship (does it eject an electron)? c. If the hull of the enemy vessel is made of the element with an electron configura tion of [Ar]4s13d10, what metal is this?arrow_forward
- What does wave-particle duality mean? What are its implications in our modem view of atomic structure?arrow_forward6.101 Laser welding is a technique in which a tightly focused laser beam is used to deposit enough energy to weld metal parts together. Because the entire process can be automated, it is commonly used in many large-scale industries, including the manufacture of automobiles. In order to achieve the desired weld quality, the steel parts being joined must absorb energy at a rate of about 104 W/mm2. (Recall that 1 W = 1 J/s.) A particular laser welding system employs a Nd:YAG laser operating at a wavelength of 1.06m ; at this wavelength steel will absorb about 80% of the incident photons. If the laser beam is focused to illuminate a circular spot with a diameter of 0.02 inch, what is the minimum power (in watts) that the laser must emit to reach the 104 W/mm2 threshold? How many photons per second does this correspond to? (For simplicity, assume that the energy from the laser does not penetrate into the metal to any significant depth.)arrow_forwardUse the mathematical expression for the 2pz wave function of a one-electron atom (see Table 5.2) to show that the probability of finding an electron in that orbital anywhere in the x-y plane is 0. What are the nodal planes for a dxz orbital and for a dx2y2 orbital?arrow_forward
- 6.17 The laser in most supermarket barcode scanners operates at a wavelength of 632.8 nm. What is the energy of a single photon emitted by such a laser? What is the energy of one mole of these photons?arrow_forwardConsider burning ethane gas, C2H6 in oxygen (combustion) forming CO2 and water. (a) How much energy (in J) is produced in the combustion of one molecule of ethane? (b) What is the energy of a photon of ultraviolet light with a wavelength of 12.6 nm? (c) Compare your answers for (a) and (b).arrow_forwardThe energy needed to ionize an atom of element X when it is in its most stable state is 500kJmol1 . However, if an atom of X is in its lowest excited state, only 120kJmol1 is needed to ionize it. What is the wavelength of the radiation emitted when an atom of X undergoes a transition from the lowest excited state to the ground state?arrow_forward
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