Dipole Electron- # Molecule domain Hybridization of Central moment? Yes or Geometry Atom Part F No. 1 CO2 Complete the third row of the table. sp3 yes GaH3 no sp3 trigonal planar O NH3 no Molecule O CH4 5 SF4 BRF3 octahedral no sp2 yes Нао trigonal bipyramidal no 8. Submit Request Answer 9 XeF2 P Pearson Copyright © 2020 Pearson Education Inc. All rights reserved. I Terms of Use Privacy Policy / P 100% earch 2. 4. Electron- Molecule domain Hybridization of Central Dipole moment? Geometry Atom Yes or No. Complete the fourth row of the table. 1 CO2 12 sp3 3. yes О НаСО sp³ O PF3 no Molecule O BH3 trigonal planar no BRF3 5 SF4 PC33 octahedral no 7. sp2 yes Submit Request Answer trigonal bipyramidal no 8. 9 XEF2 Part I P Pearson Copyright © 2020 Pearson Education Inc. All rights reserved. | Terms of Use Privacy Policy / Pe 100% search 4.

Dipole Electron- # Molecule domain Hybridization of Central moment? Yes or Geometry Atom Part F No. 1 CO2 Complete the third row of the table. sp3 yes GaH3 no sp3 trigonal planar O NH3 no Molecule O CH4 5 SF4 BRF3 octahedral no sp2 yes Нао trigonal bipyramidal no 8. Submit Request Answer 9 XeF2 P Pearson Copyright © 2020 Pearson Education Inc. All rights reserved. I Terms of Use Privacy Policy / P 100% earch 2. 4. Electron- Molecule domain Hybridization of Central Dipole moment? Geometry Atom Yes or No. Complete the fourth row of the table. 1 CO2 12 sp3 3. yes О НаСО sp³ O PF3 no Molecule O BH3 trigonal planar no BRF3 5 SF4 PC33 octahedral no 7. sp2 yes Submit Request Answer trigonal bipyramidal no 8. 9 XEF2 Part I P Pearson Copyright © 2020 Pearson Education Inc. All rights reserved. | Terms of Use Privacy Policy / Pe 100% search 4.

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter9: Bonding And Molecular Structure: Orbital Hybridization And Molecular Orbitals

Section: Chapter Questions

Problem 71SCQ: Bromine forms a number of oxides of varying stability. (a) One oxide has 90.90% Br and 9.10% O....

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Antibonding molecular orbitals can be used to make bondsto other atoms in a molecule. For example, metal atomscan use appropriate d orbitals to overlap with the p*2p orbitalsof the carbon monoxide molecule. This is calledd@p backbonding. (a) Draw a coordinate axis system inwhich the y-axis is vertical in the plane of the paper andthe x-axis horizontal. Write “M” at the origin to denote ametal atom. (b) Now, on the x-axis to the right of M, drawthe Lewis structure of a CO molecule, with the carbonnearest the M. The CO bond axis should be on the x-axis.(c) Draw the CO p*2p orbital, with phases (see the “CloserLook” box on phases) in the plane of the paper. Two lobesshould be pointing toward M. (d) Now draw the dxy orbitalof M, with phases. Can you see how they will overlap withthe p*2p orbital of CO? (e) What kind of bond is being madewith the orbitals between M and C, s or p ? (f) Predict whatwill happen to the strength of the CO bond in a metal–COcomplex compared to CO alone.
Antibonding molecular orbitals can be used to make bondsto other atoms in a molecule. For example, metal atomscan use appropriate d orbitals to overlap with the π*2p orbitalsof the carbon monoxide molecule. This is calledd-π backbonding. (a) Draw a coordinate axis system inwhich the y-axis is vertical in the plane of the paper andthe x-axis horizontal. Write “M” at the origin to denote ametal atom. (b) Now, on the x-axis to the right of M, drawthe Lewis structure of a CO molecule, with the carbon nearest the M. The CO bond axis should be on the x-axis.(c) Draw the CO π*2p orbital, with phases (see the “CloserLook” box on phases) in the plane of the paper. Two lobesshould be pointing toward M. (d) Now draw the dxy orbitalof M, with phases. Can you see how they will overlap withthe π*2p orbital of CO? (e) What kind of bond is being madewith the orbitals between M and C, σ or π ? (f) Predict whatwill happen to the strength of the CO bond in a metal–COcomplex compared to CO alone.
How would you explain the experimental observations that the SeF6 unit in Cs2[SeF6] is C2v and looks like six of the seven vertices of a capped trigonal prism are occupied by F, but the SeCl6 unit in Cs2[SeCl6] has Ohsymmetry ?
Bromine forms a number of oxides of varying stability. (a) One oxide has 90.90% Br and 9.10% O. Assuming its empirical and molecular formulas are the same, draw a Lewis structure of the molecule and specify the hybridization of the central atom (O). (b) Another oxide is unstable BrO. Assuming the molecular orbital diagram in Figure 9. 16 applies to BrO, write its electron configuration (where Br uses 45 and 4p orbitals). What is the highest occupied molecular orbital (HOMO) for the molecule?
The molecular orbital diagram of NO shown in Figure 10.47 also applies to OF. Draw the complete molecular orbital diagram for OF. What is the OF bond order? Figure 10.47 Molecular orbital diagram for nitric oxide (NO). The molecular orbital diagram for NO predicts a bond order of 2.5 and predicts that the molecule is paramagnetic with one unpaired electron. These predictions are verified by experimental measurements.
(a) The nitric oxide molecule, NO, readily loses one electronto form the NO+ ion. Which of the following is the best explanationof why this happens: (i) Oxygen is more electronegativethan nitrogen, (ii) The highest energy electron inNO lies in a p2*p molecular orbital, or (iii) The p2*p MO in NOis completely filled. (b) Predict the order of the N¬O bondstrengths in NO, NO+, and NO-, and describe the magneticproperties of each. (c) With what neutral homonuclear diatomicmolecules are the NO+ and NO- ions isoelectronic(same number of electrons)?
Suppose a chloride ion and a sodium ion are separated by a center–centerdistance of 5 Å. Is the interaction energy (the energy required to pull theminfinitely far apart) predicted to be larger if the medium between them iswater, or if it is n-pentane? (as shown)If Ca2+, Na+, and F- each have ionic radii ~1.16. Which ionic bond is stronger: Ca-F or Na-F?If Ca2+ is often bound on the surface of a protein by carboxylic acid functional groups. If the pKa of a particular -COOH group is 4.2, wouldyou predict Ca2+ to be most tightly bound at pH 8, pH 4.2, or pH 3? Explain your answer.
The illustrations below depict differences in orbital hy-bridization of some tellurium (Te) fluorides. (a) Which depictsthe difference, if any, between TeF₆(left) and TeF₅(right)? (b) Which depicts the difference, if any, between TeF₄(left) and TeF₆(right)?
Enter in order the hybridization and coordination number (CN) of the central atom for each substance
Many compounds of the transition-metal elements containdirect bonds between metal atoms. We will assumethat the z-axis is defined as the metal–metal bond axis.(a) Which of the 3d orbitals (Figure 6.23) is most likely tomake a σ bond between metal atoms? (b) Sketch the s3dbonding and σ*3d antibonding MOs. (c) With reference tothe “Closer Look” box on the phases of orbitals, explain whya node is generated in the σ*3d MO. (d) Sketch the energyleveldiagram for the Sc2 molecule, assuming that only the3d orbital from part (a) is important. (e) What is the bondorder in Sc2?
What is the valance configuration for the element in. 3 group 5A. A. 5s2 5p5 B. 5s2 5p1 C. 3s2 3p3 D. 3s2 3p1
Many compounds of the transition-metal elements containdirect bonds between metal atoms. We will assumethat the z-axis is defined as the metal–metal bond axis.(a) Which of the 3d orbitals (Figure 6.23) is most likely tomake a s bond between metal atoms? (b) Sketch the s3dbonding and s*3d antibonding MOs. (c) With reference tothe “Closer Look” box on the phases of orbitals, explain whya node is generated in the s*3d MO. (d) Sketch the energyleveldiagram for the Sc2 molecule, assuming that only the3d orbital from part (a) is important. (e) What is the bondorder in Sc2?