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 2.2, Problem 2.6E
Calculate the effective nuclear charge on a 5s, 5p, and 4d electron in a tin atom.
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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 electron configuration of the Ba3+ ion? Suggest a reason why this ion is not normally found in nature.arrow_forwardIn the hydtogen atom, what is the physical significance of the for which n = and E = 0?arrow_forward5. Calculate the effective nuclear charge on a 5s, 5p, and 4d electron in a tin atom.arrow_forward
- 2. (a) What is the smallest atom in group 13?(b) What is the smallest atom of the atoms Te, In, Sr, Po, Sb? Why is that?arrow_forwardBoron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively. (a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Draw the orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons in boron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation for the reaction of solid boron with fluorine gas. (e) ΔHf° for BF3(g) is -1135.6 kj/mol. Calculate the standard enthalpy change in the reaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?arrow_forwardParticles called muons exist in cosmic rays and can be created in particle accelerators. Muons are very similar to electrons, having the same charge and spin, but they have a mass 207 times greater. When muons arecaptured by an atom, they orbit just like an electron but with a smaller radius, since the mass in aB =0.529x 10-10 m is 207 me .(a) Calculate the radius of the n=1 orbit for a muon in a uranium ion( Z=92).(b) Compare this with the 7.5-fm radius of a uranium nucleus. Note that since the muon orbits inside the electron, it falls into a hydrogen-like orbit. Since your answer is less than the radius of the nucleus, you can seethat the photons emitted as the muon falls into its lowest orbit can give information about the nucleus.arrow_forward
- Determine the number of valence electrons and give the electronic confi guration of the valence electrons of each element: (a) nitrogen; (b) potassium.arrow_forward(a) How does the Bohr model differ from the quantum mechanical model of the atom? Describe at least 2 differences.(b) Define each of the 4 quantum numbers (n, l, ml, ms) and what they physically represent about the orbital and/or electron.(d) How many quantum numbers are needed to completely define a specific orbital? Provide the quantum numbers for the 2s orbital.(d) How many quantum numbers are needed to completely define a specific electron? Provide the quantum numbers for the second electron to fill into a 2s orbital.arrow_forwardFor each of the following pairs of hydrogen orbitals, indicate which is higher in energy: (a) 1s, 2s; (b) 2p, 3p; (c) 3dxy , 3dyz ; (d) 3s, 3d; (e) 4f, 5s.arrow_forward
- Which orbital in each of the following pairs is lower in energy in a many-electron atom: (a) 2s, 2p; (b) 3p, 3d; (c) 3s, 4s; (d) 4d, 5f ?arrow_forwardConsider an electron in the N shell. (a) What is the smallest orbital angular momentum it could have? (b) What is the largest orbital angular momentum it could have? Express your answers in terms of h and in SI units. (c) What is the largest orbital angular momentum this electron could have in any chosen direction? Express your answers in terms of h and in SI units. (d) What is the largest spin angular momentum this electron could have in any chosen direction? Express your answers in terms of h and in SI units. (e) For the electron in part (c), what is the ratio of its spin angular momentum in the z-direction to its orbital angular momentum in the z-direction?arrow_forwardThe ionization energy of potassium is 4.34 eV and the electron affinity of Br is 3.36 eV. What is the change in energy in the reaction K(g) + Br(g) → K+(g) + Bl-(g)?arrow_forward
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