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 2.45P
Select the best choice, and briefly indicate the reason for your choice:
a. Smallest radius: Sc Ti V
b. Greatest volume:
c. Lowest ionization energy: K Rb Cs
d. Highest
e. Most energy necessary to remove an electron:
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Aa.31.
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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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- 3B 4B 5B 68 7B Smalle Ha 68- 18 29 HU Cs+ Rh Pd Ag Co Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Arrange the following ions in order of increasing ionic radius: iodide ion, cesium ion, telluride ion, barium ion. Si P S Cl Ar Ge As Se Br Kr Sb Te I Xe Bi Po At Rn Largest Drag and drop your selection from the following list to complete the answer: Ba2+ Te²- An error has been detected in your answer. Check for typos. miscalculations etc. before submitting your answer. IT Previous Nextarrow_forward2arrow_forwardWhich of the options below provides a reason why the covalent radius of hafnium (1.44 Å) is less than that of zirconium (1.45 Å), even though the element above it in the periodic table? A. Between Zr and Hf lies the 4d10 configuration due to the transition metals. This leads to much greater Z* because the d electrons are so poor at shielding. Thus Hf is smaller than expected for an element in a higher shell than Zr, called the Scandide contraction. B. Hf being below Zr suggests that it will have a smaller atomic radius because the trend shows a decrease going down a group. C. Hf is below Zr and has a smaller ionisation energy, electron affinity and electronegativity compared to Zr. This reduces its atomic radius, thus leading to it having a smaller atomic radius compared to that of Zr. D. Between Zr and Hf lies the 4f14 configuration due to the Lanthanides. This leads to much greater Z* because the f electrons are so poor at shielding. Thus Hf is smaller than expected for an element in…arrow_forward
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