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 5.15P
Beryllium hydride,
a. Construct a molecular orbital energy level diagram for
b. If you have worked Problem 5.14, compare the results of these two problems.
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a. Using the molecular orbital diagram, calculate the bond order of F2+. Show show your work or give a brief explanation of the process.
b. Do you expect this to have a shorter or longer bond length than F2? Explain your answer.
c. Do you expect F2+ to be paramagnetic or diamagnetic? Explain your answer.
Please label your answers a-c and place them on separate lines. Be as specific in your explanation as you can.
In reference to the following figure, which of the following statements is not true?
a. The bond in the hydrogen molecule is formed by the overlap of 1s atomic orbitals.
b. The overlap of electron waves represented by the atomic orbitals may result in constructive (in-phase) or destructive (out-of-phase) interference.
c. In-phase overlap between two 1s orbitals results in a new orbital having higher energy than either of the s orbitals. This new orbital concentrates the electron probability between the two nuclei.
d. Out-of-phase overlap between two 1s orbitals results in a new orbital having higher energy than either of the s orbitals. This new orbital places most of the electron probability to the left and right of the two nuclei.
e. All of the above statements are true.
Consider a NF molecule a. Draw orbitals of each atorn and find possible interactions among them. b. Draw atomic orbitals. using the potential energy information c. Draw molecular orbitals from the atomic orbitals of N and F. d. What is the band order of this molecule? e. Specify the types of molecular orbitals, or (NF,NF? Which of the three has the longest bond length -NF, NF, and NF ? Explain your answer.
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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- The linear molecule FeH2 has been observed in the gas phase. Assume that the iron atom can potentially use s, p, and d orbitals to interact with the hydrogens. If the z axis is collinear with the molecular axis: a. Sketch the group orbitals of the hydrogen atoms that potentially could interact with the iron. b. Show how the group orbitals and the central atom would interact. c. Which interaction would you expect to be the strongest? The weakest? Note that the 1s orbital energy for H is –13.61 eV; the orbital energies of 3p, 3d, and 4s are –30 eV, –11.7 eV, and –7.9 eV, respectively.arrow_forwardConfigurations that is NOT paramagnetic a. 1s2 2s2 2p6 3s2 3p5 b. 1s2 2s2 2p6 3s2 3p6 c. 1s2 2s2 2p6 3s2 3p4 d. 1s2 2s2 2p6 3s7arrow_forwardAccording to the VSEPR theory, the geometry of the SO3 molecule isa. pyramidal b. tetrahedral c. trigonal planar d. distorted tetrahedron (see-saw). e. square planararrow_forward
- Answer numbers 24 & 25arrow_forwardPls help ASAP on botharrow_forward9. Consider the cyclic cation C,H,*. a. How many electrons are in the n system? Circle your answer. [2 pts] 8 9 10 b. Use the appropriate polygon (below) to complete the Hückel analysis of this π system by drawing in the energy levels of the MOs and filling them with the number of electrons you answered in part a. Only one of the four polygons is correct for the analysis in both ring size and- orientation. [6 pts] 8 8 9 9 c. Is the cyclic cation C,H,* aromatic, antiaromatic, or nonaromatic? Circle your answer. [2 pts] aromatic antiaromatic nonaromaticarrow_forward
- The arrangement of electron groups around the Xe atom in XeF4 is A. tetrahedral. B. trigonal bipyramidal. C. square planar. D. octahedral. E. square pyramidal.arrow_forward2021 SCMATH_W- f you remove one of the atoms from Xeo you get a molecule that, with a itle imagination, resembles a sees a shown in the animations on the left. A model for Xeos shown in the chem30 window. Xeo,, has seesaw geometry. This geometry is sometimes caled sanhorse geometry Rotate the molecule until you have a feeling for its three-dimensional shape. Compared to the trigonal bipyramid, what kind of atom is mising? drid de What is the approsimate numerical value of the O-ke-o bond angle? (degrees. What s the approsimate numerical value of the O-ef bond angles? degrees. The two O atoms are in equateriat positions. What is the geometry defned by the Xe atom and the two o atums? for practice, type in the name of the geometry of the moiecule: For practice, type in the name of the positions occupied by the oxypen atume For practice, type in the name of the positions occupied by the fuorine atalnearrow_forwardMolecular orbitals in metals... A. Overlap significantly to allow free electron movement through the system. B. Have a large gap between bonding and valence bands so that electrons cannot easily be promoted to higher energy levels. C. Are so numerous because each atom contributes its atomic orbitals to a large network. D. All of the above. E. Both A and C. O A ОВ OC OE ODarrow_forward
- The molecular orbital (MO) diagram of OF is given below. Answer Questions 15 – 18. 2p, 2p, 2p, 2p. 2p, 2p. 25 25 OF Farrow_forward21. Which of the following does have the lowest polarizability? Z of Br = 35, I = 53, F = 9, S = 16 Group of answer choices a. F b. I- c. S- d. Br-arrow_forwarda. Using the different green coloured atom centres to represent the different halogen atoms (F, light green; Cl, mid-green; Br, dark green), build a model of CHFClBr.b. Build a second model of CHFClBr which corresponds exactly to the mirror image of your first model.c. Try to superimpose the two models over one another – is there any way you can arrange the two models in such a way that all the different atoms in the two models are in the same place? Are they superimposable?d. Using wedge and dash bonds draw the structure of both models.e. Use the Cahn-Ingold-Prelog sequence rules to assign the absolute configuration of each compound.arrow_forward
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