Calculate the number of valence electronsDraw the three-dimensional structure of the moleculeMolecule # 7 BrF4Draw the Lewis Structure belowusing the "wedge and dash" notation.The molecular geometry is:This molecule is polar nonpolar (Circle your choice.)Our logic for this choice is:The formal charge on Br isThe formal charge on F isThe hybridization of Br isEstimate F-Br-F bond angleMolecule #3 8 ХеOF4Draw the Lewis Structure belowCalculate the number of valence electronsDraw the three-dimensional structure of the moleculeusing the "wedge and dash" notation.The molecular geometry is:This molecule is polar nonpolar (Circle your choice.)Our logic for this choice is:The formal charge on Xe isThe formal charge on O isThe hybridization of Xe isEstimate F-Xe-F bond angle Calculate the number of valence electronsMolecule # 5 SiF?-Draw the Lewis Structure belowDraw the three-dimensional structure of the moleculeusing the "wedge and dash" notation.The molecular geometry is:This molecule is polar nonpolar (Circle your choice.)Our logic for this choice is:The formal charge on Si isThe formal charge on F isThe hybridization of Si isEstimate F-Si-F bond angleMolecule # 6 CC2F2Draw the Lewis Structure belowCalculate the number of valence electronsDraw the three-dimensional structure of the moleculeusing the "wedge and dash" notation.The molecular geometry is:This molecule is polar nonpolar (Circle your choice.)Our logic for this choice is:The formal charge on C isThe formal charge on Cl/F isThe hybridization of C isEstimate F-C-Cl bond angle

Since you have asked multiple question, we will solve the first question for you.If you want any…

Molecule #7 BrF4* Calculate the number of valence electrons Draw the three-dimensional structure of the molecule using the "wedge and dash" notation. Our logic for this choice is: Draw the Lewis Structure below The molecular geometry is: This molecule is polar nonpolar (Circle your choice.) The formal charge on Br is The hybridization of Br is The formal charge on F is Estimate F-Br-F bond angle

Molecule #7 BrF4* Calculate the number of valence electrons Draw the three-dimensional structure of the molecule using the "wedge and dash" notation. Our logic for this choice is: Draw the Lewis Structure below The molecular geometry is: This molecule is polar nonpolar (Circle your choice.) The formal charge on Br is The hybridization of Br is The formal charge on F is Estimate F-Br-F bond angle

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

Chapter3: Atomic Shells And Classical Models Of Chemical Bonding

Section: Chapter Questions

Problem 94AP: The molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six...

See similar textbooks

Similar questions

A student who missed this class needs to know how to predict the bond angles and shape of amolecule from looking at its bond-line representation. Write a concise but complete explanationfor this student.
Vitamin B6 is an organic compound whose deficiency in the human body can cause apathy, irritability, and an increased susceptibility to infections. Below is an incomplete Lewis structure for vitamin B6. Complete the Lewis structure and answer the following questions. Hint: Vitamin B6 can be classified as an organic compound (a compound based on carbon atoms). The majority of Lewis structures for simple organic compounds have all atoms with a formal charge of zero. Therefore, add lone pairs and multiple bonds to the structure below to give each atom a formal charge of zero. a. How many bonds and bonds exist in vitamin B6? b. Give approximate values for the bond angles marked a through g in the structure. c. How many carbon atoms are sp2 hybridized? d. How many carbon, oxygen, and nitrogen atoms are sp3 hybridized? e. Does vitamin B6 exhibit delocalized bonding? Explain.
Carbon monoxide (CO) is an example of an overall neutral molecule (netcharge=0) that hasnon-zero formal charges. Draw a Lewis structure of carbon monoxide (CO).
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?
For each of the following molecules, complete the Lewis structure and use the VSEPR model to determine the bond angles around each central atom. Note that the drawings are only skeleton structures and may depict the angles incorrectly.
Aspartame is an artificial sweetener marketed under the name Nutra-Sweet. A partial Lewis structure for aspartame is shown below. Aspartame can be classified as an organic compound (a compound based on carbon atoms). The majority of Lewis structures for simple organic compounds have all atoms with a formal charge of zero. Therefore, add lone pairs and multiple bonds to the structure above to give each atom a formal charge of zero when drawing the Lewis structure. Also note that the six-sided ring is shorthand notation for a benzene ring (C6H5). Benzene is discussed in Section 4-7. Complete the Lewis structure for aspartame. How many C and N atoms exhibit sp1 hybridization? How many C and O atoms exhibit sp3 hybridization? How many and bonds are in aspartame?
Q1. Draw the Lewis structure of given compound;a) CH3NH2 (metil amine)b) HCOOH (formic acid)c) HCSNH2d) NH2CONH2Q2. Draw Lewis structure of the following species, indication formal charges andresonance where applicable;a) HOSO3-b) H2NCNc) FCO2-d) HCO3-e) FSO3-Q3. Use the VSEPR theory to predict the shape ofa) The molecule OSF2b) The ion ClO3-c) The ion of S2O32-d) Th ion of BrF4
For the following molecules:I. Draw the best Lewis Dot Structures for each of the following molecules. The best structuretakes into consideration resonance structures, calculations of formal charge for each atom,and tries to minimize the overall formal charge for the structure. II. Draw the 3-D VSEPR structures for the following molecules. You may combine these twodrawings (for I and II) into 1 drawing if you wish. III. Label the bond angles. IV. State the electron geometry (basic VSEPR) and molecular shape (derivative VSEPR) foreach molecule. V. State the hybridization around each central atom in the molecule. VI. State whether the overall molecule is polar or nonpolar. VII. For any two of the following molecules, state the strongest intermolecular force betweenmultiple of the same molecule.a. IF2b. H2CO3c. CH3CH2COOHd. N2O4e. PO4^3-f. CH3COCNg. ClO3^-1h. C4H8
Your assigneed ion is : AlCl4- please give a brief description that includes: (c) the arrangement (or shape) of the electron grouping (includes lone pairs), (e) actual molecular geometry (may be the same or different than answer (c), Please note that your individual assignment may be for an ion (don't forget about charges) or a neutral atom.
A classmate of yours is convinced that he knows everythingabout electronegativity. (a) In the case of atoms X and Y havingdifferent electronegativities, he says, the diatomic moleculeX¬Y must be polar. Is your classmate correct? (b) Yourclassmate says that the farther the two atoms are apart in abond, the larger the dipole moment will be. Is your classmatecorrect?
Given the following molecules and/or ions, characterize them according to the formatshown in the table below. The central atom of the molecule/ion is shown in boldface.The central atom or molecules marked with an asterisk (*) do not obey the octet rule. PCl5* OF2 SF4* A=Bonding electronsB= Sigma-bondsC =Nonbonding electron pairsD= Hybrid orbitals havingnonbonding electron pairsE =Hybrid orbitals usedF= 3-D structure (NAME)G =Polar (P) or nonpolar (NP) MOLECULE OR ION LEWIS STRUCTURE A B C D E F G
1. For the following molecules: I. Draw Lewis Dot Structures and VSEPR structures for the following molecules (you maycombine these two drawings into 1 drawing if you wish). II. Label the bond angles. III. State the electron geometry (basic VSEPR) and molecular shape (derivative VSEPR) for eachmolecule. IV. State the hybridization around each central atom in the molecule. V. State whether the overall molecule is polar or nonpolar. VI. State the number of sigma and pi bonds in the molecule. a. BrF3b. C3H6O