PART II. MOLECULAR GEOMETRY DBJECTIVE: Illustrate the Lewis dot structure and classify the polarity and molecular geometry. DIRECTIONS: Draw the Lewis dot structure of the species in column A and choose the description column B that best applies. COLUMN A COLUMN B 1. CO2 A. Polar, Bent 2. CH2CI2 B. Nonpolar, Trigonal Planar 3. ХeFz C. Nonpolar, Linear 4. BF3 D. Nonpolar, Trigonal Pyramid 5. NFB12 E. Polar, Tetrahedral F. Polar, Trigonal Pyramid

PART II. MOLECULAR GEOMETRY DBJECTIVE: Illustrate the Lewis dot structure and classify the polarity and molecular geometry. DIRECTIONS: Draw the Lewis dot structure of the species in column A and choose the description column B that best applies. COLUMN A COLUMN B 1. CO2 A. Polar, Bent 2. CH2CI2 B. Nonpolar, Trigonal Planar 3. ХeFz C. Nonpolar, Linear 4. BF3 D. Nonpolar, Trigonal Pyramid 5. NFB12 E. Polar, Tetrahedral F. Polar, Trigonal Pyramid

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 10.118QE

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Similar questions

Identify the hybrid orbitals used by antimony in SbCl5 and in SbCl6, the ion formed from the reaction of SbCl5 and Cl. Explain your choices.
Compare and contrast the molecular orbital and ionic bonding descriptions of LiF.
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Use sketches of orbitals to show how VB theory explains the bonding in the Cl2 molecule. Illustrate with appropriate orbital diagrams as well. Use these to determine the number of orbitals that overlap in the Cl2 molecule. How many orbitals overlap in Cl2? Choose answer that aplies. a. Bonding will be similar to the bonding in F2, because fluorine and chlorine are in the same group of the periodic table. b. One 3p orbital of each chlorine atom will participate in the bonding in the Cl2 molecule. c. One 2p orbital of each chlorine atom will participate in the bonding in the Cl2 molecule. d. Two sp7 molecular orbitals will participate in the bonding in Cl2 molecule. d. Bonding will be similar to the bonding in F2, because fluorine and chlorine are in the same period of the periodic table.
What is the molecular orbital diagram of NO2+? Please label everything and show the steps.
Consider the reaction BF3 + NH3 -> F3B-NH3 (a) Describe the changes in hybridization of the B and N atoms as a result of this reaction. (b) Describe the shapes of all the reactant molecules with their bond angles. (c) Draw the overall shape of the product molecule and identify the bond angles around B and N atoms. (d) What is the name of the bond between B and N. (e)Describe the bonding orbitals that make the B and F, B and N & N and H bonds in the product molecule.
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Consider a NF molecule a. Draw orbitals of each atorn and find possible interactions among them. b. Draw atomic orbitals. using the potential energy information c. Draw molecular orbitals from the atomic orbitals of N and F. d. What is the band order of this molecule? e. Specify the types of molecular orbitals, or (NF,NF? Which of the three has the longest bond length -NF, NF, and NF ? Explain your answer.
a. One of the two known binary compounds of xenon and oxygen is XeO3. A Lewis structure is shown here, which may or may not be complete. How many lone pairs should be present on the central Xe atom? b. What is the electron pair geometry around the Xe? c. What is the molecular geometry of XeO3? d. What hybrid orbitals does the Xe atom use?
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Please fill in the blank ! In part B, the difference is that the molecules have more than one atom with two or more attached neighbors. As molecules become larger and more complex, VSEPR theory does not attempt to create names for the overall geometries that result. Instead, we continue to consider the geometry about one central atom at a time. By giving the arrangement about each such atom in the larger structure, we can generate enough information to develop an overall picture. Thus, in your report for part B, you should determine which atoms have more than one bound neighbor, then repeat the procedure for part A. When deciding whether the molecules in part B are polar or nonpolar, focus on the molecule as a whole, not the geometry about a single atom. If the molecule is polar, draw a dipole arrow on your sketch indicating polarity.
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