COMPOUND Chemical Lewis Dot Electron-pair Molecular Bond Polar Correct Angles bonds? Structure diagram (2D) geometry (3D with lone pairs) Geometry (3D without lone pairs) formula and # of valence (Yes or No) or Model? (Instructor's Initials) available XX Iodine gas Nitrite ion XIX Carbon disulfide Fundamental Chemistry I

COMPOUND Chemical Lewis Dot Electron-pair Molecular Bond Polar Correct Angles bonds? Structure diagram (2D) geometry (3D with lone pairs) Geometry (3D without lone pairs) formula and # of valence (Yes or No) or Model? (Instructor's Initials) available XX Iodine gas Nitrite ion XIX Carbon disulfide Fundamental Chemistry I

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 17P

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Similar questions

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?
How many π molecular orbitals (π-MOs) are formed from the linear combination of atomicorbitals (AOs) contributing to the π-bonding in pentene?
Select one: True or False 1- Besides providing the largest suitable number of valance orbitals for covalent bond formation it can determine the final shape of the molecule for example Sp hybridization leads to a diagonal planner molecule, SP2 hybridization while Sp3 hybridization leads a pyramidal (tetrahydral shape) 2- About the underlying compound ( in the images ) , it it’s a calcium complex of EDTA used to treat metal toxicities like pulmbism in order to avoid hypocalcaemia.
The following is part of a molecular orbital energy-level diagramfor MOs constructed from 1s atomic orbitals. (a) What labels do we use for the two MOs shown? (b) Forwhich of the following molecules or ions could this be theenergy-level diagram:H2, He2, H2+, He2+, or H2-?(c) What is the bond order of the molecule or ion? (d) If anelectron is added to the system, into which of the MOs will itbe added? [
Write simple valence bond wave functions for formationof bonds between C and H atoms. What C-H compounddoes the VB model predict? What geometry does it predictfor the molecules?
For each molecule or molecular ion below, calculate the bond order: N2, N2-, O2 and O2+. In this calculation, show which specifically bonding and anti-bonding molecular orbitals were used in the calculation. Please label molecular orbitals with appropriate “g” (“gerade”) and “u” (“ungerade”) subscripts.
There is persuasive evidence for the brief existence of theunstable molecule OPCl.(a) Draw a Lewis diagram for this molecule in which theoctet rule is satisfied on all atoms and the formalcharges on all atoms are zero .(b) The compound OPCl reacts with oxygen to giveO2PCl. Draw a Lewis diagram of O2PCl for which allformal charges are equal to zero. Draw a Lewis diagram in which the octet rule is satisfied on all atoms.
(a) Using only the valence atomic orbitals of a hydrogenatom and a fluorine atom, and following the model ofFigure 9.46, how many MOs would you expect for the HFmolecule? (b) How many of the MOs from part (a) would beoccupied by electrons? (c) It turns out that the difference inenergies between the valence atomic orbitals of H and F aresufficiently different that we can neglect the interaction ofthe 1s orbital of hydrogen with the 2s orbital of fluorine.The 1s orbital of hydrogen will mix only with one 2p orbitalof fluorine. Draw pictures showing the proper orientationof all three 2p orbitals on F interacting with a 1s orbitalon H. Which of the 2p orbitals can actually make a bondwith a 1s orbital, assuming that the atoms lie on the z-axis?(d) In the most accepted picture of HF, all the other atomicorbitals on fluorine move over at the same energy into themolecular orbital energy-level diagram for HF. These arecalled “nonbonding orbitals.” Sketch the energy-level diagramfor HF using…
a) What is the difference between a localized π bond and adelocalized one? (b) How can you determine whether a moleculeor ion will exhibit delocalized π bonding? (c) Is the πbond in NO2- localized or delocalized?
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 nitrate ion (NO3) . Draw the possible Lewis resonance diagrams for this ion. Use the VSEPR theory to determine the steric number, the hybridization of the central N 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 is predicted by the MO model for the NO bonds in the nitrate ion?
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.