LCPO CHEMISTRY W/MODIFIED MASTERING
8th Edition
ISBN: 9780135214756
Author: Robinson
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 7, Problem 7.98SP
Assign formal charges to the atoms in the following structures. Which of the two do you think is the more important contributor to the resonance hybrid?
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Draw three resonance structures for CS,. This species has its three atoms bonded sequentially in the following fashion: S-C-S.
Draw your resonance structures so that the atoms in them are bonded together in this order. Select the most important
resonance structure for this species based on the formal charges on the atoms of the three resonance structures you have
drawn. Select the choices from below which make the statements true about this (most important) resonance structure.
(a) The leftmost bond (between S and C) is a single
v bond.
(b) The rightmost bond (between C and S) is a single
v bond.
(c) The formal charge on the leftmost (S) atom is
-Select-v
(d) The formal charge on the central (C) atom is
-Select---v
(e) The formal charge on the rightmost (S) atom is
Select-v
(f) The number of nonbonding pairs (lone pairs) of electrons in the leftmost (S) atom is
Select-v pairs.
(g) The number of nonbonding (lone) pairs of electrons in the rightmost (S) atom is -Select-- v pairs.
Calculate 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 acid
Describe the difference between a full Lewis structure and bond-line notation. What changes? Why is it easier to write?Dont
Chapter 7 Solutions
LCPO CHEMISTRY W/MODIFIED MASTERING
Ch. 7 - Use the electro negativity values in Figure 7.4...Ch. 7 - Conceptual APPLY 7.2 An electrostatic potential...Ch. 7 - The dipole moment of AgCI in the gas phaseis...Ch. 7 - Predict which bond has greater percent ionic...Ch. 7 - Select the correct electron-dot structure for H2S...Ch. 7 - Use the octet rule to predict the molecular...Ch. 7 - Identify the correct electron-dot structure for...Ch. 7 - Draw an electron-dot structure for each of the...Ch. 7 - Select the correct electron-dot structure for...Ch. 7 - Identify the correct electron-dot structure(s) for...
Ch. 7 - Prob. 7.11PCh. 7 - Which oxygen species do you predict to be most...Ch. 7 - Draw an electron-dot structure for the following...Ch. 7 - There are two molecules with the formula C2H6O...Ch. 7 - The following structure is a representation of...Ch. 7 - Draw two possible electron-dot structures for the...Ch. 7 - Called “laughing gas, nitrous oxide (N2O) is...Ch. 7 - Draw as many resonance structures as possible for...Ch. 7 - Prob. 7.19PCh. 7 - Prob. 7.20ACh. 7 - Calculate the formal charge on each atom in the...Ch. 7 - Start with the electron-dot structure for the...Ch. 7 - Calculate formal charges on the C and O atoms in...Ch. 7 - Three resonance structures for anisole (Problem...Ch. 7 - The toxicity of the organophosphate insecticides...Ch. 7 - Prob. 7.26PCh. 7 - Prob. 7.27PCh. 7 - The following structure is a representation of the...Ch. 7 - The electron-dot structure for the nerve a gentsar...Ch. 7 - Draw the new electron-dot structures indicated by...Ch. 7 - The following diagram shows the potential energy...Ch. 7 - The following diagram shows the potential energy...Ch. 7 - Two electrostatic potential maps are shown, one of...Ch. 7 - Prob. 7.34CPCh. 7 - Which of the following drawings is most likely to...Ch. 7 - The following ball-and-stick molecular model is a...Ch. 7 - The following hall-and-stick molecular model is a...Ch. 7 - Sinapaldehyde, a compound present in the toasted...Ch. 7 - Vitamin C (ascorbic acid) has the following...Ch. 7 - Match the following descriptions with the type of...Ch. 7 - Why do two atoms come together to form a covalent...Ch. 7 - Explain the difference in the bond dissociation...Ch. 7 - Explain the difference in the bond dissociation...Ch. 7 - Predict which of the following bonds should be...Ch. 7 - Prob. 7.45SPCh. 7 - What general trends in electro negativity occur in...Ch. 7 - Predict the electro negativity of the undiscovered...Ch. 7 - Order the following elements according to...Ch. 7 - Order the following elements according to...Ch. 7 - Which of the following substances contain bonds...Ch. 7 - Use the electro negativity data in Figure 7.4 to...Ch. 7 - Show the direction of polarity for each of the...Ch. 7 - Show the direction of polarity for each of the...Ch. 7 - Which of the substances...Ch. 7 - Which of the substances...Ch. 7 - Order the following compounds according to the...Ch. 7 - Order the following compounds according to the...Ch. 7 - Prob. 7.58SPCh. 7 - Using only the elements Ca, Cl, and Si, give...Ch. 7 - The dipole moment of BrCl is 0.518 D, and the...Ch. 7 - Prob. 7.61SPCh. 7 - Prob. 7.62SPCh. 7 - Prob. 7.63SPCh. 7 - Why does the octet rule apply primarily to...Ch. 7 - Which of the following substances contains an atom...Ch. 7 - Draw electron-dot structures for the following...Ch. 7 - Draw electron-dot structures for the following...Ch. 7 - Identify the correct electron-dot structure for...Ch. 7 - Draw an electron.dot structure for the hydronium...Ch. 7 - Oxalic acid, H2C2O4 , is a mildly poisonous...Ch. 7 - Draw an electron-dot structure for carbon...Ch. 7 - Prob. 7.72SPCh. 7 - Identify the fourth-row elements, X, that form the...Ch. 7 - Write electron-dot structures for molecules with...Ch. 7 - Write electron-dot structures for molecules with...Ch. 7 - Which compound do you expect to have the stronger...Ch. 7 - Which compound do you expect to have the stronger...Ch. 7 - Draw an electron-dot structure for each of the...Ch. 7 - Prob. 7.79SPCh. 7 - Methylphenidate (C14H19NO2) , marketed as Ritalin,...Ch. 7 - Pregabalin (C8H17NO2) , marketed as Lyric a, is an...Ch. 7 - The following molecular model is that of...Ch. 7 - Ibuprofen C 13 H 18 O 2 marketed under such brand...Ch. 7 - Draw as many resonance structures as you can that...Ch. 7 - Draw as many resonance structures as you can for...Ch. 7 - Which of the following pairs of structures...Ch. 7 - Which of the following pairs of structures...Ch. 7 - Draw as many resonance structures as you can that...Ch. 7 - Draw as many resonance structures as you can that...Ch. 7 - Benzene has the following structural formula. Use...Ch. 7 - Draw three resonance structures for sulfur...Ch. 7 - Some mothballs used when storing clothes are made...Ch. 7 - Four different structures (a), (b), (c), and (d)...Ch. 7 - Draw an electron-dot structure for carbon...Ch. 7 - Assign formal charges to the atoms in the...Ch. 7 - Assign formal charges to the atoms in the...Ch. 7 - Assign formal charges to the atoms in the...Ch. 7 - Assign formal charges to the atoms in the...Ch. 7 - Calculate formal charges for the C and O atoms in...Ch. 7 - Draw two electron-dot resonance structures that...Ch. 7 - Draw two electron-dot resonance structures that...Ch. 7 - Prob. 7.102SPCh. 7 - Prob. 7.103SPCh. 7 - Boron trifluoride reacts with dimethyl ether to...Ch. 7 - Thiofulminic acid, HCNS, has recently been...Ch. 7 - Draw two rcsonancc strutur for methyl isocyanate,...Ch. 7 - In the cyanatc ion. OCN , carbon is the central...Ch. 7 - Prob. 7.108MPCh. 7 - Prob. 7.109MPCh. 7 - Prob. 7.110MPCh. 7 - The neutral OH molecule has been implicated in...Ch. 7 - Prob. 7.112MPCh. 7 - Prob. 7.113MP
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Assign formal charges to all atoms in the following Lewis diagrams. (a) SO42 (b) S2O32 (c) SbF3 (d) SCNarrow_forwardThe Lewis structure of acetone is Circling the carbonyl carbon, i.e., the carbon atom attached to oxygen, and its octet gives Circling the oxygen atom and its octet gives Thus, atoms share electrons in making bonds, and a pair of electrons may be included in the octet of two different atoms. When computing the formal charge on an atom, the number of electrons that belong to that atom is compared with the number of electrons the atom would have in the unbonded and neutral state. If the two numbers are the same, the formal charge on the atom is zero. In a Lewis structure both electrons in an unshared pair belong to the atom, and one of every pair of shared (bonding) electrons belongs to the atom.arrow_forwardWrite Lewis structures for the following: (a) SeF6 (b) XeF4 (c) SeCl3+arrow_forward
- The 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_forwardGiven the following electro negativities C=2.5N=3.0S=2.6 what is the central atom in CNS-?arrow_forwardOn the basis of the electronegativity values given in Fig. 12.3, indicate whether each of the following bonds would be expected to be covalent, polar covalent, or ionic. msp;a.SSb.SHc.SKarrow_forward
- In 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_forwardWhich of these resonance structures contributes most to the overall structure of the molecule? 0=S=0 :ö-s- =s- ö-s=ö :0-s= :0::ö: :ö: :0:arrow_forwardIn consideration of the overall resonance hybrid OCN(^-), which is the proposed resonance structure that's most important? In lewis Dot Form*arrow_forward
- Consider 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_forwardAssuming acid strength relates directly to electronegativityof the central atom, rank H₃PO₄, HNO₃, and H₃AsO₄ in order of increasing acid strength.arrow_forward. The bond lengths of carbon-carbon, carbon-nitrogen, carbon-oxygen, and nitrogen-nitrogen single, double, and triple bonds are listed in Table 8.4. Plot bond enthalpy versus bond length listed in Table 8.5 for these bonds. (a) Is this statement true: "The longer the bond, the stronger the bond"? (b) Based on your chart, order the relative strengths of C-C, C-N, C-O, and N-N bonds from weakest to strongest.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Stoichiometry - Chemistry for Massive Creatures: Crash Course Chemistry #6; Author: Crash Course;https://www.youtube.com/watch?v=UL1jmJaUkaQ;License: Standard YouTube License, CC-BY
Bonding (Ionic, Covalent & Metallic) - GCSE Chemistry; Author: Science Shorts;https://www.youtube.com/watch?v=p9MA6Od-zBA;License: Standard YouTube License, CC-BY
General Chemistry 1A. Lecture 12. Two Theories of Bonding.; Author: UCI Open;https://www.youtube.com/watch?v=dLTlL9Z1bh0;License: CC-BY