Student Solutions Manual for Zumdahl/Zumdahl/DeCoste?s Chemistry, 10th Edition
10th Edition
ISBN: 9781305957510
Author: ZUMDAHL, Steven S.; Zumdahl, Susan A.; DeCoste, Donald J.
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 8, Problem 7RQ
Define formal charge and explain how to calculate it. What is the purpose of the formal charge? Organic compounds are composed mostly of carbon and hydrogen but also may have oxygen, nitrogen, and/or halogens in the formula. Formal charge arguments work very well for organic compounds when drawing the best Lewis structure. How do C, H, N, O, and Cl satisfy the octet rule in organic compounds so as to have a formula charge of zero?
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Decide whether these proposed Lewis structures are reasonable.
proposed Lewis structure
a=ö]
[[:N_N=N]]
Yes.
Is the proposed Lewis structure reasonable?
No, it has the wrong number of valence electrons.
The correct number is:
No, it has the right number of valence electrons but doesn't satisfy the
octet rule.
The symbols of the problem atoms are:
Yes.
No, it has the wrong number of valence electrons.
The correct number is:
No, it has the right number of valence electrons but doesn't satisfy the
octet rule.
The symbols of the problem atoms are:* ☐
Yes.
No, it has the wrong number of valence electrons.
The correct number is:
No, it has the right number of valence electrons but doesn't satisfy the
octet rule.
The symbols of the problem atoms are:*
*If two or more atoms of the same element don't satisfy the octet rule, just enter the chemical symbol as many
times as necessary. For example, if two oxygen atoms don't satisfy the octet rule, enter "0,0".
The carbonate anion, CO32- , is a resonance hybrid. Draw all of the important resonance structures for this molecule. If an atom has a nonzero formal charge, be sure the formal charge is shown clearly in the structure. Use the resonance structures to calculate the average formal charge on each O atom (which are all equivalent in the "true" structure). [Note: all of the important contributing resonance structures have octets around each atom that desires an octet.]
The azide ion, N, is a symmetrical ion, in which all of the possible Lewis structures have formal charge on one or more atoms. Draw three possible Lewis structures for this ion.
Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all nonbonding electrons. Show the formal charges of all atoms.
Q
NNNITY
¤••
Q
Submit
Q
NENN
N=N-N²
N²NN
с
H O N S P
F Br CI
X
Type the new charge. Press ENTER to finish editing. Press TAB to go through
atoms in the structure.
Previous Answers Request Answer
X Incorrect; Try Again; One attempt remaining
More
Chapter 8 Solutions
Student Solutions Manual for Zumdahl/Zumdahl/DeCoste?s Chemistry, 10th Edition
Ch. 8 - Distinguish between the terms electronegativity...Ch. 8 - When an element forms an anion, what happens to...Ch. 8 - Define the term lattice energy. Why,...Ch. 8 - Explain how bond energies can be used to estimate...Ch. 8 - Prob. 5RQCh. 8 - Explain the terms resonance and delocalized...Ch. 8 - Define formal charge and explain how to calculate...Ch. 8 - Give two requirements that should be satisfied for...Ch. 8 - Consider the following compounds: CO2, SO2, KrF2,...Ch. 8 - Explain the electronegativity trends across a row...
Ch. 8 - The ionic compound AB is formed. The charges on...Ch. 8 - Prob. 3ALQCh. 8 - The bond energy for a CH bond is about 413 kJ/mol...Ch. 8 - Prob. 5ALQCh. 8 - Which has the greater bond lengths: NO2 or NO3?...Ch. 8 - The following ions are best described with...Ch. 8 - The second electron affinity values for both...Ch. 8 - What is meant by a chemical bond? Why do atoms...Ch. 8 - Why are some bonds ionic and some covalent?Ch. 8 - How does a bond between Na and Cl differ from a...Ch. 8 - Arrange the following molecules from most to least...Ch. 8 - Does a Lewis structure tell which electron come...Ch. 8 - True or false? In general, a large atom has a...Ch. 8 - What is the central idea of the VSEPR model?Ch. 8 - In Section 8.13 of the text, the term effective...Ch. 8 - Describe the type of bonding that exists in die...Ch. 8 - Some plant fertilizer compounds are (NH4)2SO4,...Ch. 8 - Some of the important properties of ionic...Ch. 8 - What is the electronegativity trend? Where does...Ch. 8 - Give one example of a compound having a linear...Ch. 8 - When comparing the size of different ions, the...Ch. 8 - In general the higher the charge on the ions in an...Ch. 8 - Combustion reactions of fossil fuels provide most...Ch. 8 - Which of the following statements is/are true?...Ch. 8 - Prob. 29QCh. 8 - The molecules BF3, CF4, CO2, PF5, and SF6 are all...Ch. 8 - Without using Fig. 3-4, predict the order of...Ch. 8 - Without using Fig. 3-4, predict the order of...Ch. 8 - Without using Fig. 3-4, predict which bond in each...Ch. 8 - Without using Fig. 3-4, predict which bond in each...Ch. 8 - Prob. 35ECh. 8 - Prob. 36ECh. 8 - Which of the following incorrectly shows the bond...Ch. 8 - Indicate the bond polarity (show the partial...Ch. 8 - Predict the type of bond (ionic, covalent, or...Ch. 8 - List all the possible bonds that can occur between...Ch. 8 - Hydrogen has an electronegativity value between...Ch. 8 - Rank the following bonds in order of increasing...Ch. 8 - State whether or not each of the following has a...Ch. 8 - The following electrostatic potential diagrams...Ch. 8 - Prob. 45ECh. 8 - Prob. 46ECh. 8 - Predict the empirical formulas of the ionic...Ch. 8 - Predict the empirical formulas of the ionic...Ch. 8 - Write electron configurations for a. the cations...Ch. 8 - Write electron configurations for a. the cations...Ch. 8 - Which of the following ions have noble gas...Ch. 8 - What noble gas has the same electron configuration...Ch. 8 - Give the formula of a negative ion that would have...Ch. 8 - Prob. 54ECh. 8 - Give three ions that are isoelectronic with neon....Ch. 8 - Consider the ions Sc3+, Cl, K+, Ca2+, and S2....Ch. 8 - Prob. 57ECh. 8 - For each of the following groups, place the atoms...Ch. 8 - Which compound in each of the following pairs of...Ch. 8 - Which compound in each of the following pairs of...Ch. 8 - Use the following data for potassium chloride to...Ch. 8 - Use the following data for magnesium fluoride to...Ch. 8 - Consider the following energy changes: E(kJ/mol)...Ch. 8 - Compare the electron affinity of fluorine to the...Ch. 8 - Prob. 65ECh. 8 - Use the following data (in kJ/mol) to estimate E...Ch. 8 - Rationalize the following lattice energy values:...Ch. 8 - The lattice energies of FeCl3, FeCl2, and Fe2O3...Ch. 8 - Use bond energy values (Table 3-3) to estimate E...Ch. 8 - Use bond energy values (Table 3-3) to estimate E...Ch. 8 - Prob. 71ECh. 8 - Acetic acid is responsible for the sour taste of...Ch. 8 - Use bond energies to predict E for the following...Ch. 8 - The major industrial source of hydrogen gas is by...Ch. 8 - Use bond energies to estimate E for the combustion...Ch. 8 - Prob. 76ECh. 8 - Prob. 77ECh. 8 - Consider the following reaction: A2+B22AB E =...Ch. 8 - Compare your answers from parts a and b of...Ch. 8 - Compare your answers from Exercise 72 to the H...Ch. 8 - The standard enthalpies of formation for S(g),...Ch. 8 - Use the following standard enthalpies of formation...Ch. 8 - The standard enthalpy of formation for N2H2(g) is...Ch. 8 - The standard enthalpy of formation for NO(g) is...Ch. 8 - Write Lewis structures that obey the octet rule...Ch. 8 - Write Lewis structures that obey the octet rule...Ch. 8 - Write Lewis structures that obey the octet rule...Ch. 8 - Write Lewis structures that obey the octet rule...Ch. 8 - One type of exception to the octet rule are...Ch. 8 - Lewis structures can be used to understand why...Ch. 8 - The most common exceptions to the octet rule are...Ch. 8 - Prob. 92ECh. 8 - Write Lewis structures for the following. Show all...Ch. 8 - Prob. 94ECh. 8 - Benzene (C6H6) consists of a six-membered ring of...Ch. 8 - Borazine (B3N3H6) has often been called inorganic...Ch. 8 - An important observation supporting the concept of...Ch. 8 - Consider the following bond lengths: CO143pmC9O123...Ch. 8 - A toxic cloud covered Bhopal, India, in December...Ch. 8 - Prob. 103ECh. 8 - Prob. 104ECh. 8 - Write Lewis structures that obey the octet rule...Ch. 8 - Write Lewis structures for the species in Exercise...Ch. 8 - Oxidation of the cyanide ion produces the stable...Ch. 8 - When molten sulfur reacts with chlorine gas, a...Ch. 8 - Carbon and sulfur form compounds with each other...Ch. 8 - Prob. 112ECh. 8 - Predict the molecular structure and bond angles...Ch. 8 - Predict die molecular structure and bond angles...Ch. 8 - There are several molecular structures based on...Ch. 8 - Two variations of the octahedral geometry (see...Ch. 8 - Prob. 117ECh. 8 - Consider the molecular structures illustrated in...Ch. 8 - Predict the molecular structure (including bond...Ch. 8 - Predict the molecular structure (including bond...Ch. 8 - Predict the molecular structure (including bond...Ch. 8 - Predict the molecular structure (including bond...Ch. 8 - Prob. 123ECh. 8 - Which of the molecules in Exercise 120 have net...Ch. 8 - Which of the molecules in Exercise 121 have net...Ch. 8 - Which of the molecules in Exercise 122 have net...Ch. 8 - Write Lewis structures and predict the molecular...Ch. 8 - Write Lewis structures and predict whether each of...Ch. 8 - Consider the following Lewis structure where E is...Ch. 8 - Consider the following Lewis structure where E is...Ch. 8 - Two different compounds exist having the formula...Ch. 8 - Two different compounds have the formula XeF2Cl2....Ch. 8 - Arrange the following in order of increasing...Ch. 8 - For each of the following, write an equation that...Ch. 8 - Use bond energies (table 3-3), values of electron...Ch. 8 - Write Lewis structures for CO32, HCO3, and H2CO3....Ch. 8 - Which member of the following pairs would you...Ch. 8 - What do each of the following sets of...Ch. 8 - Prob. 139AECh. 8 - Although both Br3 and I3 ions are known, the F3...Ch. 8 - Prob. 142AECh. 8 - Which of the following molecules have not dipole...Ch. 8 - Prob. 145AECh. 8 - Look up the energies for the bonds in CO and N2....Ch. 8 - Classify the bonding in each of the following...Ch. 8 - List the bonds PCl, PF, OF, and SiF from least...Ch. 8 - Arrange the atoms and/or ions in the following...Ch. 8 - Use the following data to estimate E for the...Ch. 8 - Use bond energy values to estimate E for the...Ch. 8 - Which of the following compounds or ions exhibit...Ch. 8 - The formulas of several chemical substances are...Ch. 8 - Predict the molecular structure, bond angles, and...Ch. 8 - Use Coulombs Jaw, V=Q1Q240r=2.311019Jnm(Q1Q2r) to...Ch. 8 - Prob. 156CPCh. 8 - Calculate the standard heat of formation of the...Ch. 8 - Given the following information: Energy of...Ch. 8 - Prob. 159CPCh. 8 - Think of forming an ionic compound as three steps...Ch. 8 - The compound NF3 is quite stable, but NCl3, is...Ch. 8 - Three processes that have been used for the...Ch. 8 - The compound hexaazaisowurtzitane is one of the...Ch. 8 - Many times extra stability is characteristic of a...Ch. 8 - The study of carbon-containing compounds and their...Ch. 8 - Draw a Lewis structure for the N,...Ch. 8 - Prob. 167CPCh. 8 - Consider the following computer-generated model of...Ch. 8 - Cholesterol (C27H46O) has the following structure:...Ch. 8 - A compound, XF5, is 42.81% fluorine by mass....Ch. 8 - Identify the following elements based on their...
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
- Consider the pyrosulfate ion, S2O72-. It has no sulfur–sulfur nor oxygen–oxygen bonds. (a) Write a Lewis structure for the pyrosulfate ion using only single bonds. (b) What is the formal charge on the sulfur atoms for the Lewis structure you drew in part (a)? (c) Write another Lewis structure using six bonds and two O—S bonds. (d) What is the formal charge on each atom for the structure you drew in part (c)?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 common trait of simple organic compounds is to have Lewis structures where all atoms have a formal charge of zero. Consider the following incomplete Lewis structure for an organic compound called methyl cyanoacrylate, the main ingredient in Super Glue. Draw a complete Lewis structure for methyl cyanoacrylate in which all atoms have a formal charge of zero.arrow_forward
- Write all resonance structures of chlorobenzene, C6H5Cl, a molecule with the same cyclic structure as benzene. In all structures, keep the CCl bond as a single bond. Which resonance structures are the most important?arrow_forwardWrite the Lewis structure for nitrosyl fluoride, FNO. Using only a periodic table, identify (a) which is the longer bond. (b) which is the stronger bond. (c) which is the more polar bond.arrow_forwardExperimental evidence indicates the existence of HC3N molecules in interstellar clouds. Write a plausible Lewis structure for this molecule.arrow_forward
- An incomplete Lewis structure is shown below. The structure only shows the atoms and how they are connected. The molecule has a net charge of zero. H Н—N—С- -о—с—Н H H Complete the Lewis structure giving all atoms full octets. If there is more than one way to do this, draw resonance structures showing all possibilities. If not, just draw one Lewis structure. Be sure to write in any non-zero formal charges. Click and drag to start drawing a structure.arrow_forwardWhat possible error(s) exist in the Lewis structure (assume we are trying to represent the best possible Lewis structure for the NO₂S ion knowing N is the central atom in this polyatomic ion)? [:ö==S: N= CO :O: The best structure would have double bond and two lone pairs on each oxygen atom and a single bond with three lone pairs on the sulfur. There are no errors. This is the best possible structure. The Lewis structure above does not minimize formal charges, thus is the not the best possible structure. The nitrogen atom has an expanded octet, and this structure is impossible. The Lewis structure contains the wrong number of electrons, thus this structure is impossible.arrow_forwardOxygen gas reacts with sulfur tetrafluoride to slowly form sulfur tetrafluoride monoxide gas. Balance the equation for the formation of sulfur tetrafluoride monoxide. chemical reaction: 0,(g) + SF (g) → OSF,(g) Draw the Lewis structure of OSF, where the formal charge is zero on each atom. The sulfur atom is the central atom in the structure, and it is bonded to the oxygen atom and each of the four fluorine atoms. Select Draw Rings More Erase Use the bond energies in the table to estimate the enthalpy of reaction for the formation of sulfur tetrafluoride monoxide. étv Aaarrow_forward
- An incomplete Lewis structure is shown below. The structure only shows the atoms and how they are connected. The molecule has a net charge of +1. Complete the Lewis structure giving all atoms full octets. If there is more than one way to do this, draw resonance structures showing all possibilities. If not, just draw one Lewis structure. Be sure to write in any non-zero formal charges.arrow_forwardHydrogen azide (HN3) is a shock-sensitive liquid, which means it explodes when subjected to a physical shock. The HN3molecule contains two N-N bonds with bond lengths 113 pm and 124 pm. The H-N-N bond angle is 112°. Draw two Lewis structures of HN3 that obey the octet rule. What is the formal charge of each atom in your structures? Which structure is most consistent with the experimental data?arrow_forward2,2,2-trifluoroethanol, CF₃CH₂OH. is used industrially as a solvent for nylon. Draw the Lewis structure of CF₃CH₂OH. In your final structure, please make sure the elements are in the order they are provided.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
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: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Organic Chemistry: A Guided Inquiry
Chemistry
ISBN:9780618974122
Author:Andrei Straumanis
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