Answer the following questions about the Lewis structure for sulfur trioxide, SO3. Draw all resonance structures.There are nvalence electrons. The molecule has dsingle bonds, aaThe central S has eThere areatoms.Each bond hastriple bonds.n. 24REDS, the shape is uand the bond angles are ddresonances structures because the double bond can be drawn between the S and% single bond character andBecause the molecule is symmetrical it is aa. 0b. 1 c. 2d. 3 e. 4m. 200. 26v. linear w. monoatomic ionscc. no bond angles, no central atomii. 33% jj. 67%f. 5p. 30 q. 32g. 8r. 34x. tetrahedraldd. 109.5°h. 11plecule.i. 12Is. 36y. trigonal planaree. polar ff. nonpolar% double bond character.j. 14 k. 16t. diatomic u. pyramidalz. bent aa. 120⁰gg. ionicI. 18bb. 180°hh. 50%double bonds, anddifferent O

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Answer There are n a the following questions about the Lewis structure for sulfur trioxide, SO3. Draw all resonance structures. valence electrons. The molecule has d single bonds, a The central S has e There are atoms. Each bond has n. 24 triple bonds. c. 2 REDS, the shape u , and the bond angles are dd resonances structures because the double bond can be drawn between the S and Because the molecule is symmetrical it is a a. 0 b. 1 d. 3 e. 4 % single bond character and m. 20 0. 26 p. 30 v. linear w. monoatomic ions cc. no bond angles, no central atom ii. 33% jj. 67% f. 5 9. 32 x. tetrahedral molecule. h. 11 i. 12 s. 36 t. diatomic y. trigonal planar z. bent g. 8 r. 34 j. 14 dd. 109.5° ee. polar ff. nonpolar % double bond character. k. 16 u. pyramidal aa. 120° gg. ionic I. 18 bb. 180° hh. 50% double bonds, and different O

Answer There are n a the following questions about the Lewis structure for sulfur trioxide, SO3. Draw all resonance structures. valence electrons. The molecule has d single bonds, a The central S has e There are atoms. Each bond has n. 24 triple bonds. c. 2 REDS, the shape u , and the bond angles are dd resonances structures because the double bond can be drawn between the S and Because the molecule is symmetrical it is a a. 0 b. 1 d. 3 e. 4 % single bond character and m. 20 0. 26 p. 30 v. linear w. monoatomic ions cc. no bond angles, no central atom ii. 33% jj. 67% f. 5 9. 32 x. tetrahedral molecule. h. 11 i. 12 s. 36 t. diatomic y. trigonal planar z. bent g. 8 r. 34 j. 14 dd. 109.5° ee. polar ff. nonpolar % double bond character. k. 16 u. pyramidal aa. 120° gg. ionic I. 18 bb. 180° hh. 50% double bonds, and different O

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter8: Bonding: General Concepts

Section: Chapter Questions

Problem 10RQ: Consider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, IF5, and SCl6....

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7.97 Consider the structure shown below for as well as any other important resonance structures. (a) What is the expected O—N—O bond angle in this structure? (b) The molecule contains N—O bonds of two different lengths. How many sborter N—O bonds would be present?
7.30 The bond in HF is said to be polar, with the hydrogen carrying a partial positive charge. For this to be true, the hydrogen atom must have less than one electron around it. Yet the Lewis dot structure of HF attributes two electrons to hydrogen. Draw a picture of the electron density distribution for HF and use it to describe how the hydrogen atom can carry a partial positive charge. How can these two models of the HF bond (the electron density and the Lewis structure) seem so different and yet describe the same thing?
What is meant by a chemical bond? Why do atoms form bonds with each other? Why do some elements exist as molecules in nature instead of as free atoms?
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Which of the following statements is false concerning bonding? Elements with extremely different electronegativities tend to form ionic bonds with each other. In an N—O bond. electron density is greater near the O atom. An N—O bond is an example of a polar covalent band. In general, chemical bonds form to minimize energy. The bond in KBr is formed by sharing electrons.
Fill in the blanks in each line of the following table that involves characteristics of various bonds between nonmetals. The first line is already completed as an example.
Carbon monoxide (CO) forms bonds to a variety of metals and metal ions. liS ability to bond to iron in hemoglobin is the reason that CO is so toxic. The bond carbon monoxide forms to metals is through the carbon atom: MCO a. On the basis of electronegativities, would you expect the carbon atom or the oxgen atom to form bonds to metals? b. Assign formal charges to the atoms in CO. Which atom would you expect to bond to a metal on this basis? c. In the MO model, bonding MOs place more electron density near the more electronegative atom. (See the HF molecule in Figs. 4-54 and 4-55.) Antibonding MOs place more electron density near the less electronegative atom in the diatomic molecule. Use the MO model to predict which atom of carbon monoxide should form bonds to metals.
Consider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, IF5, and SCl6. These 12 compounds arc all examples of different molecular structures. Draw the Lewis structures for each and predict the molecular structure. Predict the bond angles and the polarity of each. (A polar molecule has a net dipole moment, while a nonpolar molecule docs not.) See Exercises 115 and 116 for the molecular structures based on the trigonal bipyramid and the octahedral geometries.
(a) Use the VSEPR theory to predict the structure of the NNO molecule. (b) The substance NNO has a small dipole moment. Which end of the molecule is more likely to be the positive end, based only on electronegativity?
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.
Predict the molecular structure and bond angles for each molecule or ion in Exercises 81 and 87 from Chapter 3