The basis of the VSEPR model of molecular bonding isregions of electron density on an atom will organize themselves so as to maximize s-characterAregions of electron density in the valence shell of an atom will arrange themselves so as to maximizeBoverlapChybrid orbitals will form as necessary to, as closely as possible, achieve spherical symmetryDelectron domains in the valence shell of an atom will arrange themselves so as to minimize repulsionsatomic orbitals of the bonding atoms must overlap for a bond to form

To solve this problem we have to know about VSEPR Theory

The basis of the VSEPR model of molecular bonding is regions of electron density on an atom will organize themselves so as to maximize s-character regions of electron density in the valence shell of an atom will arrange themselves so as to maximize overlap hybrid orbitals will form as necessary to, as closely as possible, achieve spherical symmetry electron domains in the valence shell of an atom will arrange themselves so as to minimize repulsions atomic orbitals of the bonding atoms must overlap for a bond to form

The basis of the VSEPR model of molecular bonding is regions of electron density on an atom will organize themselves so as to maximize s-character regions of electron density in the valence shell of an atom will arrange themselves so as to maximize overlap hybrid orbitals will form as necessary to, as closely as possible, achieve spherical symmetry electron domains in the valence shell of an atom will arrange themselves so as to minimize repulsions atomic orbitals of the bonding atoms must overlap for a bond to form

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 61P: Discuss the nature of the bonding in the nitrite ion (NO2) . Draw the possible Lewis resonance...

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Similar questions

The Be2 molecule has been detected experimentally. It has a bond length of 2.45 Å and a bond dissociation energy of 9.46kJmol1 . Write the ground-state electron configuration of Be2 and predict its bond order using the theory developed in the text. Compare the experimental bonding data on Be2 with those recorded for B2,C2,N2, and O2 in Table 6.3. Is the prediction that stems from the simple theory significantly incorrect?
For the molecule allene, H2C=C=CH2, give the hybridization of each carbon atom. Will the hydrogen atoms be in the same plane or perpendicular planes?
(a) Sketch the occupied MOs of the valence shell for the N2 molecule. Label the orbitals as or orbitals, and specify which are bonding and which are antibonding. (b) If one electron is removed from the highest occupied orbital of N2 , will the equilibrium NN distance become longer or shorter? Explain briefly.
Explain why 1g is the ground state for H2+ . By combining your answer with the answer to Problem 5, what conclusions can you draw about the molecular orbital description of the bond in H2+ ?
From the n=0 peaks in the photoelectron spectrum for O2 shown in the figure in Connections box, prepare a quantitative energy level diagram for the molecular orbitals of O2 .
Formulate the MO structure of (NO2+) for localized bonds and de-localized bonds. Is it linear or nonlinear? Do you expect it to be paramagnetic? Repeat the analysis for NO2 and for NO2 .
Discuss the nature of the bonding in the nitrite ion (NO2) . Draw the possible Lewis resonance diagrams for this ion. Use the VSEPR theory to determine the steric number, the hybridization of the central nitrogen atom, and the geometry of the ion. Show how the use of resonance structures can be avoided by introducing a de-localized MO. What bond order does the MO model predict for the NO bonds in the nitrite ion?
Predict the valence electron configuration and the total bond order for the molecule S2 , which forms in the gas phase when sulfur is heated to a high temperature. Will S2 be paramagnetic or diamagnetic?
Which of the following statement(s)regarding stable heteronuclear diatomic molecules is(are) CORRECT? a. Their molecular orbital diagram are more symmetrical than those of homonuclear diatomic molecules. b. The greater is the difference in energy between two overlapping atomic orbitals, the more polar the resulting bond is, due to electrons occupying the resulting bonding molecular orbital. c. All have bond orders greater than zero. d. The antibonding molecular orbitals have more of the character of the more electronegative element than the more electropositive element.
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.
Construct the energy level diagrams of molecular orbitals for the π-system of ethylene. Use the model that the molecule is formed from the appropriately hybridized CH2 fragments. Specifically, use the Hückel MO energies which should be expressed in terms of the Coulomb and resonance integrals, and the respective 2x2 secular determinant.
Use molecular orbital theory to explain hydrogen bonding [construct the MO diagram of FHF- from combination of F- and HF instead]