0Q:#ially Prep3.oeaterial.NuCIF3Total Valence ElectronsASChlorine trifliMoride28STUtUni oLewis Dot Structure:F::FCI:F211Total Electron PairsBonding PairsNonbonding PairsElectron GeometryMolecular GeometryT-Shapedtrigonal bipyramidal4.Total Valence ElectronsSF4

The electronic configurations of chlorine and fluorine are shown below.

Answered: 0 Q: # ially Prep 3. oe aterial .Nu…

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter12: Chemical Bonding

Section: Chapter Questions

Problem 60E

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Predict the molecular structure (including bond angles) for each of the following. (See Exercises 25 and 26.) a. ICl5 b. XeC14 c. SeCl6
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?
7.50 Chemical species are said to be isoelectronic if they have the same Lewis structure (regardless of charge). Consider these ions and write a Lewis structure for a neutral molecule that is isoelectronic with each of them, (a) CN , (b) NH4+ . (c) CO32
The molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six equivalent resonance hybrid Lewis diagrams for this molecular ion. (b) Compute the formal charges on all atoms in the molecular ion in each of the six Lewis diagrams. (c) Determine the charge on each atom in the polyatomic ion, assuming that the true distribution of electrons is the average of the six Lewis diagrams arrived at in parts (a) and (b). (d) An advanced calculation suggests that the actual charge resident on each N atom is 0.375 and on each S atom is +0.041 . Show that this result is consistent with the overall +1 charge on the molecular ion.
Which of the following species (there may be more thanone) is/are likely to have the structure shown here: (a) XeF4,(b) BrF4+, (c) SiF4, (d) TeCl4, (e) HClO4? (The colors do notreflect atom identities.)
what bonds are being broken and formed (include sigma and pi bodns as well)
Calculations (# of valence electrons, # of bonds, etc. CO32-
The VSEPR model was developed before any xenon com-pounds had been prepared. Thus, these compounds provided anexcellent test of the model’s predictive power. What would youhave predicted for the shapes of XeF₂, XeF₄, and XeF₆?
How many unpaired electrons are in [ Fe { C triple bond CSi(CH3)3}64-] please explain completely
The four bonds of carbon tetrachloride (CCl4) are polar, butthe molecule is nonpolar because the bond polarity is canceledby the symmetric tetrahedral shape. When other atoms substitutefor some of the Cl atoms, the symmetry is broken and the mol-ecule becomes polar. Use Figure to rank the fol-lowing molecules from the least polar to the most polar: CH₂Br₂,CF₂Cl₂, CH₂F₂, CH₂Cl₂, CBr₄, CF₂Br
Ketene, CH2=C=O, is an unusual organic molecule that has a singlecarbon atom doubly bonded to two different atoms. Determine thehybridization of both C atoms and the O in ketene. Then, draw a diagramshowing what orbitals are used to form each bond.
(a) Describe the molecule xenon trioxide, XeO3, usingfour possible Lewis structures, one each with zero, one,two, or three Xe¬O double bonds. (b) Do any of theseresonance structures satisfy the octet rule for every atomin the molecule? (c) Do any of the four Lewis structureshave multiple resonance structures? If so, how many resonancestructures do you find? (d) Which of the Lewisstructures in part (a) yields the most favorable formalcharges for the molecule?

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0 Q: # ially Prep 3. oe aterial .Nu CIF3 Total Valence Electrons AS Chlorine trifliMoride 28 STUtUni o Lewis Dot Structure :F: :F CI:F 211 Total Electron Pairs Bonding Pairs Nonbonding Pairs Electron Geometry Molecular Geometry T-Shaped trigonal bipyramidal 4. Total Valence Electrons SF4