Hybridizationaround centralMolecularNumber ofLewis StructureSketch 3DMolecularElectronshape ofelectronFormulaValenceGeometryGeometryElectronsatomdomainsaround centralatom (includeall atoms in thesketch)CO2SbClsNH3 MolecularNumber ofLewis StructureSketch 3DMolecularElectronHybridizationshape ofelectronFormulaValenceGeometryGeometryaround centralElectronsatomdomainsaround centralatom (includeall atoms in thesketch)SI2H2CO (C iscentral)BrFs

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Answered: Hybridization around central Molecular…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter9: Covalent Bonding: Orbitals

Section: Chapter Questions

Problem 1RQ: Why do we hybtidize atomic orbitals to explain the bonding in covalent compounds? What type of bonds...

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Why do we hybtidize atomic orbitals to explain the bonding in covalent compounds? What type of bonds form from hybrid orbitals: sigma or pi? Explain.
The molecular orbital diagram of NO shown in Figure 10.47 also applies to the following species. Write the molecular orbital electron configuration of each, indicating the bond order and the number of unpaired electrons. (a) LiBe+ (b) CO+ (c) CN (d) OF 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.
The molecular orbital diagram of NO shown in Figure 10.47 also applies to the following species. Write the molecular orbital electron configuration of each, indicating the bond order and the number of unpaired electrons. (a) CN (b) CO (c) BeB (d) BC+ 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.
The diagram that follows shows the highest-energy occupiedMOs of a neutral molecule CX, where element X is in thesame row of the periodic table as C. (a) Based on the numberof electrons, can you determine the identity of X? (b) Wouldthe molecule be diamagnetic or paramagnetic? (c) Considerthe p2p MOs of the molecule. Would you expect them to havea greater atomic orbital contribution from C, have a greateratomic orbital contribution from X, or be an equal mixtureof atomic orbitals from the two atoms?
Consider the molecule C4H5N, which has the connectivityshown below. (a) After the Lewis structure for the moleculeis completed, how many s and how many p bonds arethere in this molecule? (b) How many atoms in the moleculeexhibit (i) sp hybridization, (ii) sp2 hybridization, and(iii) sp3 hybridization?
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.
Consider the molecule BF3. (a) What is the electron configurationof an isolated B atom? (b) What is the electron configurationof an isolated F atom? (c) What hybrid orbitalsshould be constructed on the B atom to make the B–F bondsin BF3? (d) What valence orbitals, if any, remain unhybridizedon the B atom in BF3?
Which member of each pair has more ioniccharacter in itsbonds: (a) BeF₂ or CaF₂; (b) PbF₂ or PbF₄; (c) GeF₄ or PF₃?
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.
8. What is the hybridization for each of the indicated atoms in the following compound? CH2 Il N: CH3 CH3 | = sp?; II = sp2; III = sp2 1=sp: Il = sp2; Il = sp C) 1= sp?; Il = sp; III = sp3 D) 1= sp?; I| = sp?; III = sp A) %3D B) %3D %3D
7.Answer the questions below regarding the following species: N2, O2, O2', O2 based on the molecular orbital diagram. 2p 2p 25 25 press 1100 the Copyright © 2006 Pearson Prentice Hall, Inc. (a) Which species do not contain any unpaired electrons? -- (b) Which has a bond order of 1? (c) Which has a bond order of 3? -- (d) Which has 3 electrons in the T*2p orbital? --- Energy
What is the hybridization of S in SO32-?

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