First, draw one molecule and add the partial charges where needed - use the AEN to determine the types of bonds. Then, draw the second molecule so thatthe &+ on one molecule lines up across from the 8- on the other. Since we can't draw the molecules here you will answer questions about the drawings that youmade on the homework worksheet.NF3 hasbonds with a AEN =NF3 has 4 REDS and is symmetrical/asymmetrical (answer ismaking it a polar/nonpolar (answer ismolecule.Each F has acharge and the N has acharge.H20 has 2bonds with a AEN =H2O has 4 REDS and is symmetrical/asymmetrical (answer is) making it a polar/nonpolar (answer ismolecule.Each H has acharge and the O has acharge.The strongest possible attractive force between these two molecules isa. nonpolar covalentb. polar covalentC. ionicd. polare. nonpolarf. 0.97g. 0h. 0.01i. 0.94.j. 0.40k. 1.24I. diatomicm. bentn. pyramidalo. planar trigonalp. tetrahedralq. symmetricalr. asymmetricals. London'st. dipole-dipoleu. hydrogen bondv. ion-dipolew. &+Х. 8-y. no partial charge

the structure of NF3 and H2O are as following : electronegativity of F ( 3.98 ) , N ( 3.04 ) , H (…

First, draw one molecule and add the partial charges where needed - use the AEN to determine the types of bonds. Then, draw the second molecule so that the &+ on one molecule lines up across from the 8- on the other. Since we can't draw the molecules here you will answer questions about the drawings that you made on the homework worksheet. NF3 has bonds with a AEN = NF3 has 4 REDS and is symmetrical/asymmetrical (answer is ) making it a polar/nonpolar (answer is molecule. Each F has a charge and the N has a charge. H20 has 2 bonds with a AEN = H20 has 4 REDS and is symmetrical/asymmetrical (answer is ) making it a polar/nonpolar (answer is molecule. Each H has a charge and the O has a charge. The strongest possible attractive force between these two molecules is a. nonpolar covalent b. polar covalent c. ionic d. polar e. nonpolar f. 0.97 g. 0 h. 0.01 i. 0.94. j. 0.40 k. 1.24 I. diatomic m. bent n. pyramidal o. planar trigonal p. tetrahedral

First, draw one molecule and add the partial charges where needed - use the AEN to determine the types of bonds. Then, draw the second molecule so that the &+ on one molecule lines up across from the 8- on the other. Since we can't draw the molecules here you will answer questions about the drawings that you made on the homework worksheet. NF3 has bonds with a AEN = NF3 has 4 REDS and is symmetrical/asymmetrical (answer is ) making it a polar/nonpolar (answer is molecule. Each F has a charge and the N has a charge. H20 has 2 bonds with a AEN = H20 has 4 REDS and is symmetrical/asymmetrical (answer is ) making it a polar/nonpolar (answer is molecule. Each H has a charge and the O has a charge. The strongest possible attractive force between these two molecules is a. nonpolar covalent b. polar covalent c. ionic d. polar e. nonpolar f. 0.97 g. 0 h. 0.01 i. 0.94. j. 0.40 k. 1.24 I. diatomic m. bent n. pyramidal o. planar trigonal p. tetrahedral

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...

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