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 5, Problem 5.6P
High-resolution photoelectron spectroscopy has provided information on the energy levelsand bond distance in the ion
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Use the data given below to calculate the bond energies (Do) (in eV) of
'H³°CI and 'H®l Br molecules. Which bond is stronger?
Molecule ve (cm=1) De((cm¯1)
HCI
2991
53194
HBr
2649
34570
The noble gas electron configuration of the ion P2
is
And the Lewis structure of this ion is
Is this ion is paramagnetic or diamagnetic?
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The photoelectron spectrum of CO has four major peakswith ionization energies of 14.5, 17.2, 20.1, and 38.3 eV.Assign these peaks of molecular orbitals of CO, and prepare a quantitative energy level correlation diagram forCO. The ionization energy of carbon atoms is 11.26 eV,and the ionization energy of oxygen atoms is 13.62 eV.
Chapter 5 Solutions
Inorganic Chemistry
Ch. 5.1 - Repeat the process in the preceding example for...Ch. 5.2 - Prob. 5.2ECh. 5.3 - Use a similar approach to the discussion of HF to...Ch. 5.4 - Sketch the energy levels and the molecular...Ch. 5.4 - Using the D2h character table shown, verify that...Ch. 5.4 - Using orbital potential energies, show that group...Ch. 5.4 - Prob. 5.7ECh. 5.4 - Prob. 5.8ECh. 5.4 - Prob. 5.9ECh. 5.4 - Use the projection operator method to derive...
Ch. 5.4 - Determine the types of hybrid orbitals that are...Ch. 5.4 - Determine the reducible representation for all the...Ch. 5 - Expand the list of orbitais considered in Figures...Ch. 5 - On the basis of molecular orbitals, predict the...Ch. 5 - On the basis of molecular orbitals, predict the...Ch. 5 - Compare the bonding in O22,O2 and O2 Include Lewis...Ch. 5 - Although the peroxide ion, O22 and the acetylide...Ch. 5 - High-resolution photoelectron spectroscopy has...Ch. 5 - a. Prepare a molecular orbital energy-level...Ch. 5 - a. Prepare a molecular orbital energy-level...Ch. 5 - NF is a known molecule a. Construct a molecular...Ch. 5 - The hypofluorite ion, OF can be observed only with...Ch. 5 - Prob. 5.11PCh. 5 - Although KrF+ and XeF+ have been studied, KrBr+...Ch. 5 - Prepare a molecular orbital energy level diagram...Ch. 5 - Methylene, CH2 plays an important role in many...Ch. 5 - Beryllium hydride, BeH2 is linear in the gas...Ch. 5 - In the gas phase, BeF2 forms linear monomeric...Ch. 5 - For the compound XeF2 do the following: a. Sketch...Ch. 5 - TaH5 has been predicted to have C4v symmetry, with...Ch. 5 - Describe the bonding in ozone, o3 on the basis of...Ch. 5 - Describe the bonding in SO3 by using group theory...Ch. 5 - The ion H3+ has been observed, but its structure...Ch. 5 - Use molecular orbital arguments to explain the...Ch. 5 - Prob. 5.23PCh. 5 - Prob. 5.24PCh. 5 - The isomenc ions NSO (thiazate) and SNO...Ch. 5 - Apply the projection operator method to derive the...Ch. 5 - Apply the projection operator method to derive the...Ch. 5 - A set of four group orbitals derived from four 3s...Ch. 5 - The projection operator method has applications...Ch. 5 - Although the cl2+ ion has not been isolated, it...Ch. 5 - BF3 is often described as a molecule in which...Ch. 5 - SF4 has C2v symmetry. Predict the possible...Ch. 5 - Consider a square pyramidal AB5 molecule. Using...Ch. 5 - Prob. 5.34PCh. 5 - For the molecule PCl5 : a. Using the character...Ch. 5 - Molecular modeling software is typically capable...Ch. 5 - Prob. 5.39PCh. 5 - Calculate and display the orbitals for the linear...Ch. 5 - Prob. 5.41PCh. 5 - Prob. 5.42PCh. 5 - Prob. 5.43PCh. 5 - Diborane, B2H6 , has the structure shown. a. Using...
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- 8. (a) Define chrömophore. Classify according to the type of electronic transitions, giving examples. the chromophoresarrow_forward5. Explain why lattice enthalpy calculations based on the Bom-Mayer equation reproduce the experimentally detemined values to 99% for LICI but only 91% for AgCl?arrow_forwardWrite the electronic configuration of 3 Li and 26Fe and explain the possible valency they can exhibit.arrow_forward
- Define dr-pn bonding. Why C=N can accept the electron from the dt orbital in metal central?arrow_forward(a) Imagine that a Born-Haber cycle is being constructed by a colleague, to determine the lattice energy of a hypothetical magnesium halide salt, where X is the halide ion. The colleague makes the following list: First and second ionisations of Mg; 737 and 1451 Sublimation energy of Mg; 147 Electron affinity of X; 200 Atomisation enthalpy of X₂; 400 Enthalpy of formation of MgX₂; -450 2+ 2e+ Mg(+2X (8) b 2+ 2e + Mg( + X2 (8) a + Mg(g) + X₂ (8) 1451 Mg(g) + X₂ (8) Mg(s) + X2 (8) f 147 2+ Mg(g) +2X(g) MgX2 (s) d Sadly the colleague becomes discouraged and leaves the document incomplete, simply drawing boxes around unknown quantities. Complete the calculation by writing down the boxed quantities a-f on your answer paper. You may assume that the units are kJ mol-¹.arrow_forward26. The molecular shape of the atoms in PCla*1 is best described as (A) tetrahedral (C) see-saw (B) square planar (D) trigonal bipyramidalarrow_forward
- 2. Using the ionization energy of H 1s and CI 3p electrons of 13.6 eV and 13.1 eV, respectively, calculate the (a) energies and (b) compositions of the bonding and antibonding orbitals of HCI. (Use aH = -13.6 eV and acı = -13.1 eV.) Use B=-1.0 eV and S=0.arrow_forwardEstimate the As¬I bond length from the data in Figure 7.7and compare your value to the experimental As¬I bondlength in arsenic triiodide, AsI3, 2.55 Å.arrow_forwardUsing the molecular orbital method and its qualitative explanations, justify that the bond formation energy in the B2 molecule is equal to -297 kJ mol-1, while in the ionized N2+ molecule it is equal to -842 kJ mol-1. Explain whether these molecules are diamagnetic or paramagnetic.arrow_forward
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