please answer with a detail explanation III. Draw the hybridized molecular orbital model for CH,CN. Give the formal charges of the atoms, thegeometries of the atoms, the hybridizations, label the bond types (completely), and give the bond angles.II. Rank according to increasing dipole moment. Use the less than (<) inequality symbol and label thestructure with the largest dipole moment.PF3SF4H'ABDE

Answered: Image /qna-images/answer/2c6e5aae-62d4-4b02-8654-63125cd8536d.jpg

Answered: III. Draw the hybridized molecular…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter6: Covalent Bonding

Section: Chapter Questions

Problem 112QRT

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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?
4. Hybridization. Give the best Lewis structure (including formal charge on atoms), VESPR geometry, and hybridization of the indicated atom in the following molecules (sp, sp², sp³ sp³d, sp³d²). Formula: NO Bro PCl, Lewis Structure: sdi al (d VESPR electron group geometry: loh atwollot ses hebiveig od l ntvihsto Hybridization:
The structure of caffeine, present in coffee and many soft drinks, is shown here. How many pi bonds are present in caffeine? How many sigma bonds? Insert the lone pairs in the molecule. Which kinds of orbitals do the lone pairs occupy? CH, H;C.
Use the Lewis dot structure (make sure you show all electron pairs) to predict the electronic geometry_(EG) and the shape of the molecule H2O. O EG - bent; shape - bent O EG - trigonal planar; shape lincar O EG- tetrahedral; shape - bent O EG - tetrahcdral; shape trigonal pyramidal O EG - trigonal bipyramidal; shape - tetrahedral
How Does # of Electron bonding Geometryelectron # of this many lone Molecular. Geometry pairs structure possible have gtructures Steric # Lewis groups resonance? 'exist? Choose... Choose... Choose... Оз Che Cho Cho Choose... Choose... Choose... co32- Cho Ch Cho
7. Fill in the following table. Remember to minimize formal charge for the best Lewis structure!!! Electron pair Molecular Bond Polar? Molecule/lon| 3D Lewis structure geometry geometry angle(s) (Yes or No) so?- SF4 KrBr2
11. Arrange the following compounds in order of increasing bolling polnt. CHO -CHCHO -CHCH CHCHLCH CHo A D hinh >_>_lowest 12. Arrange the following compounds in order of increasing melting point. .. HO CH OH A highest>_>_>_>_lowest 13. For the following molecule: Draw the Lewis Structure, show the molecular geometry around the central atoms, hybridizations, and approximate bond angles Molecular Geometry around Central Atom hybridi- zation bond angle F,CHNCO KFCN = CNC =
VSEPR: Molecular Geometry 1. For the following molecules: 1) draw a Lewis Dot structure, including contributing resonance structures, if present; 2) use VSEPR to draw an appropriate structure; 3) give an appropriate designation for the ideal molecular geometry; 4) describe any deviations to the ideal molecular geometry; *don't worry about corrections for e and h. g. HOCI h.* SO;2 i. NO2*
1. Complete the following table. Molecular Formula Atom a b C C₂H4O 2. Use the Lewis structure below to complete the following table. d H b Lewis Structure H a H H-C-C C-H H-C-O: H Electron Geometry Line-Angle Structure H H :O: H C ||||-- H H C CC H d Hybridization to 3. Identify the functional groups in the Lewis structure from question #2. Approx. Bond Angle
Identify the molecular geometry of the atoms labeled with numbers on the molecule. a. C1 b. 02 c. C3- triangular planar - bent tetrahedral d. C4 triangular planar H H-C H CIC H :O: || C-C-0-H :O: H || | :O-C-C-H H 4
VSEPR: Molecular Geometry 1. For the following molecules: 1) draw a Lewis Dot structure, including contributing resonance structures, if present; 2) use VSEPR to draw an appropriate structure; 3) give an appropriate designation for the ideal molecular geometry; 4) describe any deviations to the ideal molecular geometry; *don't worry about corrections for e and h. a. NH4* b.SOCI2 c. BrFs d. SF4 e.* CH;N f. H¿CO g. HOCI h.* SO;? i. NO,* j. XeF4
Use the References to access important values if needed for this question. Sigma Bonding Ao bond arises from the straight-on overlap of two atomic orbitals. The electron density lies along the axis of the two bonded nuclei. sp3 hybrid orbital Example: Sigma Bonding in methane, CH. 1s orbital What atomic or hybrid orbitals make up the sigma bond between C, and Cl in dichloroethylene, CH,CC1, ? (C, is the second carbon in the structure as written.) orbital on C, + orbital on Cl What is the approximate C1-Cz-Cl bond angle ?

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