Part B Predict the molecular geometry for the following molecule: H-O-C-C-O-H O Drag the terms on the left to the appropriate blanks on the right to complete the sentences. Reset Help linear The two central C atoms each have bonding e domains, geometry, sp and hybridization. Each O C O group is planar, whereas the terminal H atoms 3 can rotate out of these planes. sp² 4 sp³ 2 trigonal planar tetrahedral Submit Request Answer MacBook Pro

Part B Predict the molecular geometry for the following molecule: H-O-C-C-O-H O Drag the terms on the left to the appropriate blanks on the right to complete the sentences. Reset Help linear The two central C atoms each have bonding e domains, geometry, sp and hybridization. Each O C O group is planar, whereas the terminal H atoms 3 can rotate out of these planes. sp² 4 sp³ 2 trigonal planar tetrahedral Submit Request Answer MacBook Pro

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter6: Quantum Mechanics And Molecular Structure

Section: Chapter Questions

Problem 74AP: trans-tetrazene (N4H4) consists of a chain of four nitrogen atoms with each of the two end atoms...

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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.
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.
What hybrid orbitals would be expected for the central atom in each of the following molecules or ions?
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.
Compare Figs. 4-47 and 4-49. Why are they different? Because B2 is known to be paramagnetic, the 2p and 2p molecular orbitals must be switched from the first prediction. What is the rationale for this? Why might one expect the 2p to be lower in energy than the 2p? Why cant we use diatomic oxygen to help us decide whether the 2p, or 2p, is lower in energy?
In each of the following molecules, a central atom is surrounded by a total of three atoms or unshared electron pairs: SnCl2, BCl3, SO2. In which of these molecules would you expect the bond angle to be less than 120? Explain your reasoning.