General Chemistry: Principles and Modern Applications - With Solutions Manual and Modified MasteringChemistry Code
11th Edition
ISBN: 9780134641003
Author: Petrucci
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Question
Chapter 22, Problem 36E
Interpretation Introduction
Interpretation:
To calculate average bond energy of
Concept introduction:
When a single Lewis structure is insufficient to represent a substance the actual structure is intermediate between two or more substance which is known as resonance structure.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Calculate the lattice energy of magnesium sulfide from the data given below.
Mg(s) → Mg(g)
ΔH° = 148 kJ/mol
Mg(g) → Mg2+(g) + 2e–
ΔH° = 2186 kJ/mol
S8(s) → 8S(g)
ΔH° = 2232 kJ/mol
S(g) + 2e- → S2-(g)
ΔH° = 450 kJ/mol
8Mg(s) + S8(s) → 8MgS(s)
ΔH° = –2744 kJ/mol
MgS(s) → Mg2+(g) + S2-(g)
ΔH°lattice = ?
Calculate the heat of sublimation of PI3[PI3(s)→PI3(g)].
The standard heat of formation of PI3(s) is -24.7 kJ/mol and the PI bond energy in this molecule is 184 kJ/mol. The standard heat of formation of P(g) is 334 kJ/mol and that of I2(g) is 62 kJ/mol. The I2 bond energy is 151 kJ/mol.
Predict the normal boiling point of hydrogen peroxide (H2O2) from the following data:
ΔHºf, kJ/mol
Sº, J/(mol • K)
H2O2(ℓ)
–187.8
110
H2O2(g)
–136.3
233
Tb =
Based on the estimated boiling point, is H2O2 a liquid or a gas at room temperature (25°C)? Why?Choose one:A liquid, because its estimated boiling point is less than 25°C.A gas, because its estimated boiling point is less than 25°C.A liquid, because its estimated boiling point is greater than 25°C.A gas, because its estimated boiling point is greater than 25°C.
Chapter 22 Solutions
General Chemistry: Principles and Modern Applications - With Solutions Manual and Modified MasteringChemistry Code
Ch. 22 - Give the formula of the stable fluride by Li, Be,...Ch. 22 - Fluorine is able to stabilize element’s in very...Ch. 22 - Prob. 3ECh. 22 - Prob. 4ECh. 22 - Prob. 5ECh. 22 - Prob. 6ECh. 22 - Prob. 7ECh. 22 - Use VSEPR theory to predict the probable geometric...Ch. 22 - Prob. 9ECh. 22 - Prob. 10E
Ch. 22 - Prob. 11ECh. 22 - Prob. 12ECh. 22 - Prob. 13ECh. 22 - Prob. 14ECh. 22 - Make a general prediction about which of the...Ch. 22 - The following properties of astatine have been...Ch. 22 - Prob. 17ECh. 22 - Prob. 18ECh. 22 - Prob. 19ECh. 22 - Prob. 20ECh. 22 - Prob. 21ECh. 22 - Prob. 22ECh. 22 - Prob. 23ECh. 22 - Prob. 24ECh. 22 - Each of the following compounds decomposes to...Ch. 22 - Ozone is a power oxidizing agent. Using ozone as...Ch. 22 - Prob. 27ECh. 22 - Prob. 28ECh. 22 - Prob. 29ECh. 22 - Prob. 30ECh. 22 - Prob. 31ECh. 22 - Prob. 32ECh. 22 - Prob. 33ECh. 22 - In water, O2(aq) is a strong base. If 100.0 mg of...Ch. 22 - The conversion of O2(g) to O2(g) can be...Ch. 22 - Prob. 36ECh. 22 - Prob. 37ECh. 22 - Prob. 38ECh. 22 - Prob. 39ECh. 22 - Prob. 40ECh. 22 - Prob. 41ECh. 22 - Joseph Priestley, e British chemist, was credited...Ch. 22 - Give an appropriate name to each of theb following...Ch. 22 - Prob. 44ECh. 22 - Give a specific example of a chemical equation...Ch. 22 - Prob. 46ECh. 22 - Prob. 47ECh. 22 - Prob. 48ECh. 22 - Prob. 49ECh. 22 - Prob. 50ECh. 22 - Prob. 51ECh. 22 - Prob. 52ECh. 22 - Prob. 53ECh. 22 - Prob. 54ECh. 22 - Prob. 55ECh. 22 - Prob. 56ECh. 22 - Prob. 57ECh. 22 - Prob. 58ECh. 22 - Prob. 59ECh. 22 - One reaction that competes with reaction (22.41),...Ch. 22 - Prob. 61ECh. 22 - Prob. 62ECh. 22 - Draw plausible Lewis structures for a....Ch. 22 - Both nitramide and hyponitrous acid have the...Ch. 22 - Prob. 65ECh. 22 - Prob. 66ECh. 22 - Prob. 67ECh. 22 - Prob. 68ECh. 22 - Prob. 69ECh. 22 - Prob. 70ECh. 22 - Use data from Table 7.2 (page 273) to calculate...Ch. 22 - Prob. 72ECh. 22 - Prob. 73ECh. 22 - Prob. 74ECh. 22 - Prob. 75ECh. 22 - What volume of H2(g) at 25C and 752 mmHg is...Ch. 22 - Prob. 77ECh. 22 - How many grams of CaH2(s) are required to generate...Ch. 22 - Prob. 79ECh. 22 - On the basis of molecular orbital theory, would...Ch. 22 - Prob. 81IAECh. 22 - Prob. 82IAECh. 22 - Prob. 83IAECh. 22 - The photograph was taken after a few drops of a...Ch. 22 - Prob. 85IAECh. 22 - Prob. 86IAECh. 22 - Prob. 87IAECh. 22 - Despite the fact that it has the higher molecular...Ch. 22 - The text mentions that ammonium perchlorate is an...Ch. 22 - Prob. 90IAECh. 22 - Prob. 91IAECh. 22 - Prob. 92IAECh. 22 - Refer to Figure 11-25 to arrange the following...Ch. 22 - Prob. 94IAECh. 22 - Prob. 95IAECh. 22 - Estimate the percent dissociation of CI2(g) into...Ch. 22 - Prob. 97IAECh. 22 - The structure of N(SiH2)2 involves a planar...Ch. 22 - Prob. 99IAECh. 22 - Refer to the Integrative Example on page 1082....Ch. 22 - The bond energies of CIz and 159kJmol1 are 243 and...Ch. 22 - Prob. 102IAECh. 22 - Prob. 103IAECh. 22 - Prob. 104IAECh. 22 - Prob. 105IAECh. 22 - The heavier halogens (CI, Br, and I) form...Ch. 22 - Prob. 107IAECh. 22 - Chemists have successfully synthesized the ionic...Ch. 22 - Prob. 109IAECh. 22 - Various thermochemical cycles are being explored...Ch. 22 - The decomposition of aqueous hydrogen peroxide is...Ch. 22 - Both in this chapter and in Chapter 19, we have...Ch. 22 - Prob. 113FPCh. 22 - The so-called pyroanions, X2O7n+ , form a series...Ch. 22 - A description of bonding in XeF2 based on the...Ch. 22 - Prob. 116FPCh. 22 - Prob. 117SAECh. 22 - Prob. 118SAECh. 22 - Prob. 119SAECh. 22 - Which of the following can oxidize Br to Br2 in...Ch. 22 - Prob. 121SAECh. 22 - Prob. 122SAECh. 22 - Prob. 123SAECh. 22 - Prob. 124SAECh. 22 - Prob. 125SAECh. 22 - Prob. 126SAECh. 22 - Prob. 127SAECh. 22 - Give a practical laboratory method that you might...Ch. 22 - Prob. 129SAECh. 22 - Prob. 130SAECh. 22 - Prob. 131SAECh. 22 - Prob. 132SAECh. 22 - Prob. 133SAECh. 22 - Prob. 134SAECh. 22 - Prob. 135SAE
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 data for substance X given in Exercise 117. When the temperature of 1.000 mole of X(g) is lowered from 100.0C to form X(l) at 50.0C. 28.75 kJ of heat is released. Calculate the specific heat capacity of X(g).arrow_forwardWrite Born-Haber cycles showing the relationship between the formation reaction and lattice energy definitions of each of the ionic compounds in exercise 21.49. You may need to review the definition of formation reaction from earlier in the text.arrow_forwardWhat is a driving force? Name two common and important driving forces, and give an example of each. What is entropy? Although the total energy of the universe is constant, is the entropy of the universe constant? What is a spontaneous process?arrow_forward
- Consider the iodine monochloride molecule, ICI. Because chlorine is more electronegative than iodine, this molecule is a dipole. How would you expect iodine monochloride molecules in the gaseous state to orient themselves with respect to each other as the sample is cooled and the molecules begin to aggregate? Sketch the orientation you would expect.arrow_forward9.10 The kinetic energy of molecules is often used to induce chemical reactions. The bond energy in an O1 molecule is 8.221019J . Can an O2 molecule traveling at 780 m/s provide enough energy to break the O = O bond? What is the minimum velocity of an O2 molecule that would give a kinetic energy capable of breaking the bond if it is converted with 100% efficiency?arrow_forwardThe ionic compound CaO crystallizes with the same structureas sodium chloride (Figure 8.3). (a) In this structure,how many O2- are in contact with each Ca2+ ion (Hint: Rememberthe pattern of ions shown in Figure 8.3 repeats overand over again in all three directions.) (b) Would energy beconsumed or released if a crystal of CaO was converted toa collection of widely separated Ca—O ion pairs? (c) Fromthe ionic radii given in Figure 7.8, calculate the potentialenergy of a single Ca—O ion pair that is just touching(the magnitude of electronic charge is given on the insideback cover). (d) Calculate the energy of a mole of such pairs.How does this compare to the lattice energy of CaO? (e)What factor do you think accounts for most of the discrepancybetween the energies in part (d)—the bonding in CaOis more covalent than ionic, or the electrostatic interactionsin a crystal lattice are more complicated than those in a singleion pair?arrow_forward
- Determine Re-face and Si-face?arrow_forwardDraw a simple picture showing one of the possible instantaneous dipoles that could develop in a fluorine molecule due to the shift of one or more electrons?arrow_forwardBased on the thermodynamic properties provided for water, determine the energy change when the temperature of 0.950 kg of water decreased from 111 °C to 25.0 °C. Property Value Units Melting point 0 °C Boiling point 100.0 °C ΔHfus 6.01 kJ/mol ΔHvap 40.67 kJ/mol cp (s) 37.1 J/mol · °C cp (l) 75.3 J/mol · °C cp (g) 33.6 J/mol · °Carrow_forward
- Consider two identical four-atom solids, one having 4 quanta of energy and the other having 10.(a) What observable property differs between these two solids?(b) Allow 3 quanta of energy to be transferred from the solid with 10 quanta to the solid with 4 quanta of energy. Determine whether this energy transfer is likely, explaining your reasoning.arrow_forwardWill the two have the same dipole moment? why or why not? Express in terms of their structure and intermolecular force.arrow_forwardUrea is an organic compound widely used as a fertilizer. its solubility in water allows it to be made into aqueous fertilizer solutions and applied to crops in a spray. what is the maximum number of water molecules that one urea molecule can hydrogen bond with?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
Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Physical Chemistry
Chemistry
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Wadsworth Cengage Learning,
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Calorimetry Concept, Examples and Thermochemistry | How to Pass Chemistry; Author: Melissa Maribel;https://www.youtube.com/watch?v=nSh29lUGj00;License: Standard YouTube License, CC-BY