Study Guide for Chemistry: The Central Science
13th Edition
ISBN: 9780321949288
Author: Theodore E. Brown, James C. Hill
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 17.1, Problem 17.1.2PE
The hypochlorite ion, CIO- , is the active ingredient in bleach. The perchlorate ion, CIO4- a main component of rocket propellants. Draw Lewis structures for both ions.
a. What is the formal charge of Cl in the hypochlorite ion?
b. What is the formal charge of Cl in the perchlorate ion, assuming the CI-O bonds are allsingle bonds?
c. What is the oxidation number of Cl in the hypochlorite ion?
d.What is the oxidation number of Cl in the perchlorate ion, assuming the CI-O bonds are all single bonds?
e.In a
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
For NO2-
What is the molecular geometry?
Give the formal charges for each atom.
What is another resonance structure?
1. What is the formal charge on each atom in CH3Cl and the Lewis structure for it?
2. What is the formal charge on each atom in PH4 nd the Lewis structure for it?
3. What is the formal charge on each atom in HNO3 and the Lewis structure for it?
(a) Describe the molecule xenon trioxide, XeO3, using four possible Lewis structures, one each with zero, one, two, or three Xe—O double bonds. (b) Do any of these resonance structures satisfy the octet rule for every atom in the molecule? (c) Do any of the four Lewis structures have multiple resonance structures? If so, how many resonance structures do you find? (d) Which of the Lewis structures in (a) yields the most favorable formal charges for the molecule?
Chapter 17 Solutions
Study Guide for Chemistry: The Central Science
Ch. 17.1 - Calculate the formal charge on the indicated atom...Ch. 17.1 - The hypochlorite ion, CIO- , is the active...Ch. 17.1 - Prob. 17.2.1PECh. 17.1 - a. Triazine, C3 H3N3, is like benzene except that...Ch. 17.2 - Prob. 17.3.1PECh. 17.2 - Prob. 17.3.2PECh. 17.2 - Prob. 17.4.1PECh. 17.2 - Prob. 17.4.2PECh. 17.2 - Prob. 17.5.1PECh. 17.2 - Prob. 17.5.2PE
Ch. 17.2 - Prob. 17.6.1PECh. 17.2 - Prob. 17.6.2PECh. 17.3 - Prob. 17.7.1PECh. 17.3 -
8.103 The compound chloral hydrate, known in...Ch. 17.3 - Barium azide is 62.04% Ba and 37.96% N. Each azide...Ch. 17.3 - Acetylene (C2H2) and nitrogen (N2) both contain a...Ch. 17.3 - Prob. 17.9.1PECh. 17.3 - Prob. 17.9.2PECh. 17.4 - Prob. 17.10.1PECh. 17.4 - Prob. 17.10.2PECh. 17.4 - Prob. 17.11.1PECh. 17.4 - A new compound is made that has a C-C bond length...Ch. 17.4 - A new compound is made that has an N-N bond length...Ch. 17.4 - Prob. 17.12.2PECh. 17.5 - Prob. 17.13.1PECh. 17.5 - An ionic substance of formula MX has a lattice...Ch. 17.5 - Prob. 17.14.1PECh. 17.5 - Prob. 17.14.2PECh. 17.5 - Prob. 17.15.1PECh. 17.5 - Consider the collection of nonmetallic elements 0,...Ch. 17.6 - The substance chlorine monoxide, CIO(g), is...Ch. 17.6 -
[8.87]
a. using the electronegativities of Br...Ch. 17.6 - Prob. 17.17.1PECh. 17.6 - Although I3- is a known ion, F3- is not. a. Draw...Ch. 17 - Prob. 1DECh. 17 -
9.13
a. An AB2 molecule is linear. How...Ch. 17 - Give the electron-domain and molecular geometries...Ch. 17 - Prob. 3ECh. 17 - Prob. 4ECh. 17 - Prob. 5ECh. 17 - Prob. 6ECh. 17 - Prob. 7ECh. 17 - Prob. 8ECh. 17 - Azo dyes are organic dyes that are used for many...Ch. 17 - Prob. 10ECh. 17 - 9.1 A certain AB4, molecule has a "seesaw" shape...Ch. 17 - Prob. 12ECh. 17 - Prob. 13ECh. 17 - Prob. 14ECh. 17 - Prob. 15ECh. 17 - In the hydrocarbon a. What is the hybridization at...Ch. 17 - The drawing below shows the overlap of two hybrid...Ch. 17 - Prob. 18ECh. 17 -
9.10 The following is part of a molecular...Ch. 17 - a. Methane (CH4) and the perchlorate ion (C104-)...Ch. 17 - Prob. 21ECh. 17 - Prob. 22ECh. 17 - Prob. 23ECh. 17 - Prob. 24ECh. 17 - In which of these molecules or ions does the...Ch. 17 - Prob. 26ECh. 17 - How many nonbonding electron pairs are there in...Ch. 17 - Prob. 28ECh. 17 - Prob. 29ECh. 17 - Prob. 30ECh. 17 - Prob. 31ECh. 17 - Prob. 32ECh. 17 - Prob. 33ECh. 17 - Prob. 34ECh. 17 - Ammonia, NH3 reacts with incredibly strong bases...Ch. 17 - In which of the following AFn molecules or ions is...Ch. 17 - a. Explain why BrF4 is square planar, whereas...Ch. 17 -
9.34 Name the proper three-dimensional molecule...Ch. 17 - Prob. 39ECh. 17 - Prob. 40ECh. 17 - a. (a) Is the molecule BF3 polar or nonpolar? b....Ch. 17 - Prob. 42ECh. 17 - Predict whether each of the following molecules is...Ch. 17 - Prob. 44ECh. 17 - Prob. 45ECh. 17 - Prob. 46ECh. 17 - For each statement, irldicate whether it is true...Ch. 17 - Draw sketches illustrating the overlap between the...Ch. 17 - For each statement, indicate whether it is true or...Ch. 17 - Consider the SC12 molecule. a. What IS the...Ch. 17 - Prob. 51ECh. 17 - Prob. 52ECh. 17 - Prob. 53ECh. 17 - Prob. 54ECh. 17 - Prob. 55ECh. 17 - Prob. 56ECh. 17 - a. Draw Lewis structures for ethane (C2He),...Ch. 17 - a. Draw Lewis structures for ethane (C2He),...Ch. 17 - Prob. 59ECh. 17 - Prob. 60ECh. 17 - Prob. 61ECh. 17 - Prob. 62ECh. 17 - In the formate ion, HC02- , the carbon atom is the...Ch. 17 - Prob. 64ECh. 17 - Prob. 65ECh. 17 - Prob. 66ECh. 17 - Prob. 67ECh. 17 - a. If you combine two atomic orbitals on two...Ch. 17 - Prob. 69ECh. 17 - Indicate whether each statement is true or false....Ch. 17 - Prob. 71ECh. 17 - Prob. 72ECh. 17 - Prob. 73ECh. 17 - Prob. 74ECh. 17 - Prob. 75ECh. 17 - Prob. 76ECh. 17 - Determine the electron configurations for CN+, CN,...Ch. 17 - Prob. 78ECh. 17 - Consider the molecular orbitals of the P2...Ch. 17 - Prob. 80ECh. 17 - Consider the following XF4 ions: PF4, BrF4-,...Ch. 17 -
9.88 Consider the molecule PF4Cl....Ch. 17 - Prob. 83AECh. 17 - Fill in the blank spaces in the following chart....Ch. 17 - Prob. 85AECh. 17 - Prob. 86AECh. 17 - Prob. 87AECh. 17 - Prob. 88AECh. 17 - Prob. 89AECh. 17 - Prob. 90AECh. 17 - Prob. 91AECh. 17 - Prob. 92AECh. 17 - In ozone, 03, the two oxygen atoms on the ends Of...Ch. 17 - Butadiene, C4H6, is a planar molecule that has the...Ch. 17 - The structure of borazine, B3N3H6, is a...Ch. 17 - Prob. 96AECh. 17 - Prob. 97AECh. 17 - Prob. 98AECh. 17 - Prob. 99AECh. 17 - Prob. 100AECh. 17 - Prob. 101AECh. 17 - Consider the following AB3 molecules and ions-...Ch. 17 - Prob. 103AECh. 17 - Prob. 104AECh. 17 - Prob. 105AECh. 17 - Prob. 106AECh. 17 - Prob. 107AECh. 17 - Prob. 108AECh. 17 - Determine whether the following molecules are...Ch. 17 - Prob. 110IECh. 17 - Prob. 111IECh. 17 - Prob. 112IECh. 17 - Prob. 113IECh. 17 - Prob. 114IECh. 17 - Prob. 115IECh. 17 - Prob. 116IECh. 17 - Prob. 117IECh. 17 - Prob. 118IECh. 17 - Prob. 119IECh. 17 - Prob. 120IE
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
- Bond Enthalpy When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule: X(g)+X(g)X2(g) a Would you predict that this reaction is exothermic or endothermic? Explain. b Is the bond enthalpy of X2 a positive or a negative quantity? Why? c Suppose H for the reaction is 500 kJ/mol. Estimate the bond enthalpy of the X2 molecule. d Another hypothetical molecular compound, Y2(g), has a bond enthalpy of 750 kJ/mol, and the molecular compound XY(g) has a bond enthalpy of 1500 kJ/mol. Using bond enthalpy information, calculate H for the following reaction. X2(g)+Y2(g)2XY(g) e Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound AX is likely to form. In this compound, A forms the A+ cation, and X forms the X anion. Be sure to justify your answer. Reaction: A(g)+12X2(g)AX(s)The first ionization energy of A(g) is 400 kJ/mol. The electron affinity of X(g) is 525 kJ/mol. The lattice energy of AX(s) is 100 kJ/mol. f If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of AX(s) lattice energy might lead to compound formation?arrow_forwardCompare your answers from parts a and b of Exercise 69 with H values calculated for each reaction using standard enthalpies of formation in Appendix 4. Do enthalpy changes calculated from bond energies give a reasonable estimate of the actual values?arrow_forwardLewis structures can be used to understand why some molecules react in certain ways. Write the Lewis structures for the reactants and products in the reactions described below. a. Nitrogen dioxide dimerizes to produce dinitrogen tetroxide. b. Boron trihydride accepts a pair of electrons from ammonia, forming BH3NH3. Give a possible explanation for why these two reactions occur.arrow_forward
- 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_forwardCompare your answers from parts a and b of Exercise 69 of Chapter 3 with H values calculated for each reaction using standard enthalpies of formation in Appendix 4. Do enthalpy changes calculated from bond energies give a reasonable estimate of the actual values?arrow_forwardPredict die molecular structure and bond angles for each molecule or ion in Exercises 88 and 94. a. POCl3, SO42, XeO4, PO43, ClO4 b. NF3, SO32, PO33, ClO3 c.ClO2, SCl2, PCl2 d. Considering your answers to parts a, b, and c. what conclusions can you draw concerning the structures of species containing the same number of atoms and the same number of valence electrons? (O3), sulfur dioxide, and sulfur trioxide.arrow_forward
- Hydrogenation reactions, which involve the addition of H2 to a molecule, are widely used in industry to transform one compound into another. For example, 1-butene (C4H8) is converted to butane (C4H10) by addition of H2. Use the bond dissociation enthalpies in Table 8.8 to estimate the enthalpy change for this hydrogenation reaction.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_forwardAn important observation supporting the concept of resonance in the localized electron model was that there are only three different structures of dichlorobenzene (C6H4C10). How does this fact support the concept of resonance (see Exercise 89)?arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
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 & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher: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 & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Types of bonds; Author: Edspira;https://www.youtube.com/watch?v=Jj0V01Arebk;License: Standard YouTube License, CC-BY