2. From the models of SF4, BrF3, and XeF4, deduce whether different atom arrangement, calledgeometrical isomers, are possible; if so, sketch them below. Indicate the preferred geometryfor each case and suggest a reason for your choice. Indicate which structures have dipolemoments and show their direction,PreferredMolecularCompoundElectronDipoleReasonGeometryMoment(Polarity) geometrySF4BRF3XeF43. Using the Lewis structure predict the geometrical structures of the following ions and statethe hybridization of the central atom.IonElectron GeometryMolecularFormal ChargeCentral AtomGeometryof CentralHybridizationAtomCO32-NO3-BF4

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2. From the models of SF4, BrF3, and XEF4, deduce whether different atom arrangement, called geometrical isomers, are possible; if so, sketch them below. Indicate the preferred geometry for each case and suggest a reason for your choice. Indicate which structures have dipole moments and show their direction. Compound Electron Dipole Moment Preferred Reason Geometry Molecular (Polarity) geometry SF4 BrF3 XeF4

2. From the models of SF4, BrF3, and XEF4, deduce whether different atom arrangement, called geometrical isomers, are possible; if so, sketch them below. Indicate the preferred geometry for each case and suggest a reason for your choice. Indicate which structures have dipole moments and show their direction. Compound Electron Dipole Moment Preferred Reason Geometry Molecular (Polarity) geometry SF4 BrF3 XeF4

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter10: Molecular Structure And Bonding Theories

Section: Chapter Questions

Problem 10.100QE: The molecular orbital diagram of NO shown in Figure 10.47 also applies to the following species....

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From models of SF4, BrF3, and XeF4, deduce whether differentatom arrangements, called geometrical isomers, are possible, and,if so, sketch them below.Indicate the preferred geometry foreach case and suggest a reason for your choice.Indicatewhich structures have dipole moments, and show their direction. Molecule Dipole Moment Preferred Geometry SF4 BrF3 XeF4
The figure that follows contains ball-and-stick drawings ofthree possible shapes of an AF4 molecule. (a) For each shape,give the electron-domain geometry on which the moleculargeometry is based. (b) For each shape, how many nonbondingelectron domains are there on atom A? (c) Which of thefollowing elements will lead to an AF4 molecule with theshape in (iii): Be, C, S, Se, Si, Xe? (d) Name an element A thatis expected to lead to the AF4 structure shown in (i).
. For each of the diatomic species listed below, sketch an appropriate molecular orbitaldiagram. In your diagram be sure to show all the contributing atomic orbitals, the molecularorbitals generated, and place all necessary electrons. Be sure to calculate the bond orderand indicate whether the species is diamagnetic or paramagnetic.(a) Br2+(b) BC‒(c) NeO(d) OH‒
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.
2) For each pair of molecules, generate the relevant MO diagram and predict which of the twowill have the highest bond order. (Be sure to include all valenceorbitals, and show the relative positions of the orbitals for each constituent atom.)a) HF vs HF-b) NP vs NP+c) CS vs CS+
What are the bond angles around heteroatoms and non-sp3 hybridised C atoms in C14H23NO ?
Which of these structures is not planar?
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?
Which of the following objects is chiral: (a) a left shoe,(b) a slice of bread, (c) a wood screw, (d) a molecular modelof Zn(en)Cl2, (e) a typical golf club?
Which molecule is non-polar? a) SO2 b) IF3 c) PCl3 d) XeF4
Acetylsalicylic acid, better known as aspirin, has the Lewisstructure (a) What are the approximate values of the bond angles labeled1, 2, and 3? (b) What hybrid orbitals are used about thecentral atom of each of these angles? (c) How many s bondsare in the molecule?
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.