The correct MO's generated from side to side overlap of three p orbitals are a good representation of the bonding, location of electron density, and location of charge among the O-C-O atoms in the delocalized anion shown below (as a resonance hybrid). Which orbital correctly shows the location of the nonbonding electrons and negative charge in the anion? -1/2 H3C

The correct MO's generated from side to side overlap of three p orbitals are a good representation of the bonding, location of electron density, and location of charge among the O-C-O atoms in the delocalized anion shown below (as a resonance hybrid). Which orbital correctly shows the location of the nonbonding electrons and negative charge in the anion? -1/2 H3C

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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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.
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 charge would be needed on F2 to generate an ion with a bond order of 2?
Consider the following flat drawing of methane (CH4) . a. What is HCH bond angle implied by this drawing if you assume it is flat? b. Are the electron domains of this flat CH4 spread out as much as possible? c. Use model materials to make a model of CH4 (methane). If you assembled it correctly, thefour bonds (bonding electron domains) of your model will be 109.5° apart. d. In which representation, the drawing above or the model in your hand (circle one) are theH’s of CH4 more spread out around the central carbon? e. Confirm that your model looks like the following drawing. The wedgebond represents a bond coming out of the page, and the dash bondrepresents a bond going into the page f. You will often see methane drawn as if it were flat (like on the previous page). Why is thismisleading, and what is left to the viewer’s imagination when looking at such a drawing?
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?
1. ionization of Cl2 (Cl2 —> Cl2+ + e-) leads to a shortening of the Cl-Cl distance (199 pm in Cl2, 189 pm in Cl2+), why? 2. why the C-O bond distance is nearly identical in CO (113 pm) and CO+ (112 pm)? 3. Derive the MO diagram of a linear C-H (i.e. one carbon atom bonded to one hydrogen atom). Draw out the MOs for orbitals containing electrons Would you expect C-H to behave as a carbocation, carbanion, or radical? Would removal of one electron from C-H to generate C-H+ increase or decrease the bond length between carbon and hydrogen?
Draw an mo diagram for the valence electrons in N2. What is the bond order many sigma and pi bonds are there? What is the HOMO(Highest Occupied Molecular Orbital) and LUMO(Lowest Unoccupied Molecular Orbital)? What is the magnetism of the species?
1. The sigma bond between the Br and F atom in BrF4- is formed from the overlap of which two orbitals?a. 4sp3d-2sb. 4sp3d-2pc. 4sp3d2-2sd.4sp3d2-2p2. Consider the following species F2-, F2, and F2+. Which of these species will be paramagnetic? 3. Which of the following exhibits resonance?a. ClO3-b. BrF3c. OF2d. N2
Sketch the MO diagram of H2. Identify the bonding and non bonding MO’s. Which MO is lower in energy?
One of the molecular orbitals of the H2- ion is sketched below: (a) Is the molecular orbital a σ or π MO? Is it bonding orantibonding? (b) In H2-, how many electrons occupy theMO shown above? (c) What is the bond order in the H2-ion? (d) Compared to the H—H bond in H2, the H—Hbond in H2- is expected to be which of the following:(i) Shorter and stronger, (ii) longer and stronger, (iii) shorterand weaker, (iv) longer and weaker, or (v) the same lengthand strength?
a.) Give the bond order of Li2 ,Be2 ,C2 b.) Give the ground state electron configurations ofCO,NO ,CN- .The gerade and ungerade designation is technically not appropriate for heteronuclear diatomics, but rather use the "*" after S or P to represent antibonding. Still, S would stand for σ. Let P represent a pair of π MO's. Enclose each MO in parenthesis followed by the number of electrons in that MO, e.g., the entry (1S*)2 would represent 1σ* 2.