Substance a) Draw the best Lewis structure(s), resonances, and structural isomers if any b) In your structure above, indicate polar bonds with dipole arrows toward the more electronegative atom c) Include formal charges if they are not zero Name the electronic around geometry central atom(s) Give hybridization for central atom(s) Name the shape around central atom(s) Show 3-D sketch of the structure and label all bond angles How many sigma bonds? How many pi bonds? Is the substance an ionic compound, a polar molecule, a nonpolar molecule, or a polyatomic ion? Complete the following table for the indicated species: C6H6 (ring) S8 PO43 C3H8O

Substance a) Draw the best Lewis structure(s), resonances, and structural isomers if any b) In your structure above, indicate polar bonds with dipole arrows toward the more electronegative atom c) Include formal charges if they are not zero Name the electronic around geometry central atom(s) Give hybridization for central atom(s) Name the shape around central atom(s) Show 3-D sketch of the structure and label all bond angles How many sigma bonds? How many pi bonds? Is the substance an ionic compound, a polar molecule, a nonpolar molecule, or a polyatomic ion? Complete the following table for the indicated species: C6H6 (ring) S8 PO43 C3H8O

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter9: Bonding And Molecular Structure: Orbital Hybridization And Molecular Orbitals

Section: Chapter Questions

Problem 71SCQ: Bromine forms a number of oxides of varying stability. (a) One oxide has 90.90% Br and 9.10% O....

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The orbital diagram that follows presents the final step in theformation of hybrid orbitals by a silicon atom. (a) Which ofthe following best describes what took place before the steppictured in the diagram: (i) Two 3p electrons became unpaired,(ii) An electron was promoted from the 2p orbital tothe 3s orbital, or (iii) An electron was promoted from the 3sorbital to the 3p orbital? (b) What type of hybrid orbital isproduced in this hybridization? [Section 9.5]
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? [
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.
For the compound CH3CHCH2 draw the hybridization of all the atoms involved, label the type of bonds occurring between carbon atoms. This is all the information I was provided.
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.
Element E forms an oxide of general structure A and a chloride of general structure B, shown at right.For the anion EF5-, what is (a) themolecular shape; (b) the hybridization of E; (c) the O.N. of E?
The molecule 2-butene, C4H8, can undergo a geometricchange called cis-trans isomerization:As discussed in the “Chemistry and Life” box on the chemistryof vision, such transformations can be induced bylight and are the key to human vision. (a) What is the hybridizationat the two central carbon atoms of 2-butene?(b) The isomerization occurs by rotation about the centralC¬C bond. With reference to Figure 9.29, explainwhy the p bond between the two central carbon atoms isdestroyed halfway through the rotation from cis- to trans-2-butene. (c) Based on average bond enthalpies (Table 8.3),how much energy per molecule must be supplied to breakthe C¬C p bond? (d) What is the longest wavelength oflight that will provide photons of sufficient energy to breakthe C¬C p bond and cause the isomerization? (e) Is thewavelength in your answer to part (d) in the visible portionof the electromagnetic spectrum? Comment on the importanceof this result for human vision.
In the formate ion, HCO2-, the carbon atom is the centralatom with the other three atoms attached to it. (a) Draw aLewis structure for the formate ion. (b) What hybridizationis exhibited by the C atom? (c) Are there multiple equivalentresonance structures for the ion? (d) How many electrons arein the π system of the ion?
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.
(a) What are the relationships among bond order, bondlength, and bond energy? (b) According to molecular orbitaltheory, would either Be2 or Be2+ be expected to exist? Explain.
(a) Draw Lewis structures for ethane 1C2H62, ethylene1C2H42, and acetylene 1C2H22. (b) What is the hybridizationof the carbon atoms in each molecule? (c) Predict whichmolecules, if any, are planar. (d) How many s and p bondsare there in each molecule?
Azo dyes are organic dyes that are used for many applications,such as the coloring of fabrics. Many azo dyes arederivatives of the organic substance azobenzene, C12H10N2.A closely related substance is hydrazobenzene, C12H12N2.The Lewis structures of these two substances are(Recall the shorthand notation used for benzene.)(a) What is the hybridization at the N atom in each of thesubstances? (b) How many unhybridized atomic orbitalsare there on the N and the C atoms in each of the substances?(c) Predict the N¬N¬C angles in each of thesubstances. (d) Azobenzene is said to have greater delocalizationof its p electrons than hydrazobenzene. Discussthis statement in light of your answers to (a) and (b). (e) Allthe atoms of azobenzene lie in one plane, whereas thoseof hydrazobenzene do not. Is this observation consistentwith the statement in part (d)? (f) Azobenzene is an intensered-orange color, whereas hydrazobenzene is nearly colorless.Which molecule would be a better one to use in asolar…