Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN: 9780618974122
Author: Andrei Straumanis
Publisher: Cengage Learning
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Chapter 2, Problem 19E
Interpretation Introduction
Interpretation:The given Lewis structures should be completed.
Concept introduction:A Lewis structure is diagrammatic view of a molecule, where lone pair of electrons are represented as dots, bonds are represented with lines & formal charge of each atom is mentioned near the atom.
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Describe the difference between a full Lewis structure and bond-line notation. What changes? Why is it easier to write?Dont
Draw the Lewis structures for the following four molecules, being sure to show all steps following the methods covered in class. Structures without work shown will be marked incorrect. Also, one of these molecules has resonance structures – for this compound, make sure to include all resonance structures, indicate formal charges for each atom.
SO2
OF2
IF3
NH4+
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Use the References to access important values if needed for this question.
Draw (on paper) a Lewis structure for SF2 and answer the following questions based on your drawing. Do not draw double bonds unless they are needed for
the central atom to obey the octet rule.
1. For the central sulfur atom:
the number of lone pairs
the number of single bonds
the number of double bonds = Numeric input field
2. The central sulfur atom
A. obeys the octet rule.
B. has an incomplete octet.
C. has an expanded octet.
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Chapter 2 Solutions
Organic Chemistry: A Guided Inquiry
Ch. 2 - Prob. 1CTQCh. 2 - The valence shell of an atom in a legitimate Lewis...Ch. 2 - Prob. 3CTQCh. 2 - Prob. 4CTQCh. 2 - Prob. 5CTQCh. 2 - It is impossible to draw a legitimate Lewis...Ch. 2 - Describe how to calculate the total number of...Ch. 2 - Prob. 8CTQCh. 2 - Prob. 9CTQCh. 2 - Prob. 10CTQ
Ch. 2 - Prob. 11CTQCh. 2 - Prob. 12CTQCh. 2 - A complete Lewis structure must show all nonzero...Ch. 2 - Prob. 14CTQCh. 2 - Prob. 15CTQCh. 2 - Prob. 16CTQCh. 2 - Prob. 17CTQCh. 2 - Prob. 18CTQCh. 2 - Complete the rest of the table for N, O or X by...Ch. 2 - Prob. 20CTQCh. 2 - Prob. 21CTQCh. 2 - Make a checklist that can be used to determine if...Ch. 2 - Prob. 2ECh. 2 - Prob. 3ECh. 2 - Draw the Lewis structure of a neutral molecule...Ch. 2 - Prob. 5ECh. 2 - For each element, predict (and draw a Lewis...Ch. 2 - Predict which of the following species is least...Ch. 2 - The molecules BH3 and SF6 and the ion SO42 exist...Ch. 2 - These are NOTlegitimate Lewisstructures (and...Ch. 2 - Fill in missing formal charges where needed (all...Ch. 2 - Below each structure in the previous question is a...Ch. 2 - Prob. 12ECh. 2 - Carbon monoxide (CO) is an example of an overall...Ch. 2 - Explain why this Lewis structure for CO is not as...Ch. 2 - Prob. 15ECh. 2 - Prob. 16ECh. 2 - Prob. 17ECh. 2 - Prob. 18ECh. 2 - Prob. 19E
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- When drawing a resonance hybrid, how is the relative significance of individual resonance structures represented? O The entire resonance structure will be drawn larger or smaller, depending on its significance. O There is no way to note the significance of a resonance structure in atdrawing. The most significant resonance structure is circled. The partial charges will be written larger or smaller, depending on the significance of the resonance structure. Save for Later Submisarrow_forwardConsider the molecule with the formula below, where X is the only central atom (all other atoms are directly bonded to X). Draw the most important Lewis structure for the molecule that follows the octet rule using the molecular charge and formal charges listed below. Determine the identity of X and the number of single and double bonds in your structure. Molecule formula: HXO2 Molecular charge: -1 Total number of valence electrons: 18 Formal charge on X: 0 The central atom (X) is: Click for List The molecule's number of single bonds is: The molecule's number of double bonds is: Click for List Click for Listarrow_forwardCalculate the formal charge on each of the atoms in the Lewis structure given. Be sure to answer all parts. H: N: O (of OH): O: Nitrous acidarrow_forward
- Give the correct lewis stucturearrow_forwardThe molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six equivalent resonance hybrid Lewis diagrams for this molecular ion. (b) Compute the formal charges on all atoms in the molecular ion in each of the six Lewis diagrams. (c) Determine the charge on each atom in the polyatomic ion, assuming that the true distribution of electrons is the average of the six Lewis diagrams arrived at in parts (a) and (b). (d) An advanced calculation suggests that the actual charge resident on each N atom is 0.375 and on each S atom is +0.041 . Show that this result is consistent with the overall +1 charge on the molecular ion.arrow_forwardWrite Lewis structures for the following: (a) SeF6 (b) XeF4 (c) SeCl3+arrow_forward
- Complete the rest of the table for N, O or X by drawing the number of Lewis structures specified.arrow_forwardIn the Lewis structure for chloromethane, the chlorine atom is sharing _____ electron pair and “owns” _____ of those electrons. Also, the chlorine atom possesses two electrons from each of _____ unshared pairs. The total number of electrons that belong to chlorine is 7 . Chlorine is a Group ____ element. The formal charge on chlorine in chloromethane is ____.arrow_forwardCarbon 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).arrow_forward
- You will not find “hydroxide” in the stockroom, but you will find sodium hydroxide (NaOH) andpotassium hydroxide (KOH). Lithium hydroxide (LiOH) is expensive and used in spacecraft airfilters since hydroxide reacts with carbon dioxide, and lithium is lighter than sodium or potassium.Cesium and francium hydroxides are very expensive and little used. Is this information consistentwith your answer to the previous question?arrow_forwardA complete Lewis structure must show all nonzero formal charges. Complete each of thefollowing Lewis structures by adding any missing formal charges.arrow_forwardA stable triatomic molecule can be formed that contains one atom each of nitrogen, sulfur, and fluorine. Three bonding structures are possible, depending on which is the central atom: NSF, SNF, and SFN. (a) Write a Lewis diagram for each of these molecules, indicating the formal charge on each atom. (b) Often, the structure with the least separation of formal charge is the most stable. Is this statement consistent with the observed structure for this molecule—namely, NSF, which has a central sulfur atom? (c) Does consideration of the electronegativities of N, S, and F from Figure 3.18 help rationalize this observed structure? Explain.arrow_forward
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