Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 8.10, Problem 3.1ACP
Calculate the difference in electronegativity between hydrogen and chlorine (χCl – χH) in hydrogen chloride using average bond dissociation enthalpy values (Table 8.8). Compare your results with those calculated using electro- negativity values from Figure 8.11.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
The formula of formic acid is HCO2H. One of the carbon-oxygen bond lengths in this molecule is 1.36 A while the other is 1.23 A .Draw the lewis structure of this molecule and label these bonds.
What are the advantages and disadvantages of Allen's electronegativity scale?
Sulfur tetrafluoride reacts slowly with oxygen gas to form sulfur tetrafluoride monoxide.
Write a balanced chemical equation for the reaction.
In the sulfur tetrafluoride monoxide molecule the O atom and the four F atoms are bonded to a central S atom. Write a Lewis structure for this molecule in which the formal charges of all atoms is zero.
Use bond energies to estimate the enthalpy of the above reaction. (S-F bond energy = 327 kJ/mole). Is it endothermic or exothermic?
Determine the electron geometry of the molecule and predict two possible molecular geometries.
Which of the two molecular geometries in part d is more likely to be observed? Explain.
Chapter 8 Solutions
Chemistry & Chemical Reactivity
Ch. 8.2 - Draw Lewis electron dot structures for CH3Cl...Ch. 8.2 - Prob. 8.2CYUCh. 8.2 - Prob. 8.3CYUCh. 8.2 - Prob. 8.4CYUCh. 8.3 - Prob. 8.5CYUCh. 8.4 - Draw resonance structures for the bicarbonate ion,...Ch. 8.5 - Sketch the Lewis structures for CIF2+ and CIF2....Ch. 8.6 - What is the shape of the dichloromethane (CH2C12)...Ch. 8.6 - Give the electron-pair geometry and molecular...Ch. 8.6 - Draw the Lewis structure for lCl2, and then decide...
Ch. 8.7 - For each of the following pairs of bonds, decide...Ch. 8.7 - Draw the resonance structures for SCN. What are...Ch. 8.8 - For each of the following molecules, decide...Ch. 8.8 - The electrostatic potential surface for SOCl2 is...Ch. 8.9 - Using the bond dissociation enthalpies in Table...Ch. 8.10 - Prob. 1.1ACPCh. 8.10 - Do any of the atoms in an ibuprofen molecule have...Ch. 8.10 - What is the most polar bond in the molecule?
Ch. 8.10 - Prob. 1.4ACPCh. 8.10 - Prob. 1.5ACPCh. 8.10 - Prob. 1.6ACPCh. 8.10 - Are there any 120° bond angles in ibuprofen? Any...Ch. 8.10 - Prob. 1.8ACPCh. 8.10 - Prob. 2.2ACPCh. 8.10 - Calculate the difference in electronegativity...Ch. 8.10 - Predict the bond dissociation enthalpy for a...Ch. 8.10 - Prob. 3.3ACPCh. 8 - Give the periodic group number and number of...Ch. 8 - Give the periodic group number and number of...Ch. 8 - For elements in Groups 4A-7A of the periodic...Ch. 8 - Prob. 4PSCh. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Show all possible resonance structures for each of...Ch. 8 - Show all possible resonance structures for each of...Ch. 8 - Prob. 11PSCh. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Determine the formal charge on each atom in the...Ch. 8 - Determine the formal charge on each atom in the...Ch. 8 - Determine the formal charge on each atom in the...Ch. 8 - Determine the formal charge on each atom in the...Ch. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Prob. 18PSCh. 8 - Prob. 19PSCh. 8 - The following molecules or ions all have three...Ch. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Draw a Lewis structure for each of the following...Ch. 8 - Give approximate values for the indicated bond...Ch. 8 - Give approximate values for the indicated bond...Ch. 8 - Phenylalanine is one of the natural amino acids...Ch. 8 - Acetylacetone has the structure shown here....Ch. 8 - For each pair of bonds, indicate the more polar...Ch. 8 - For each of the bonds listed below, tell which...Ch. 8 - Urea, (NH2)2CO, is used in plastics and...Ch. 8 - Considering both formal charges and bond...Ch. 8 - Considering both formal charge and bond...Ch. 8 - Three resonance structures are possible for...Ch. 8 - Three resonance structures are possible for the...Ch. 8 - Compare the electron dot structures of the...Ch. 8 - Compare the electron dot structures of the...Ch. 8 - The chemistry of the nitrite ion and HNO2: (a) Two...Ch. 8 - Draw the resonance structures for the formate ion,...Ch. 8 - Prob. 39PSCh. 8 - Consider the following molecules: (a) CH4 (b)...Ch. 8 - Which of the following molecules is(are) polar?...Ch. 8 - Prob. 42PSCh. 8 - Give the bond order for each bond in the following...Ch. 8 - Prob. 44PSCh. 8 - In each pair of bonds, predict which is shorter....Ch. 8 - In each pair of bonds, predict which is shorter....Ch. 8 - Prob. 47PSCh. 8 - Compare the carbon-oxygen bond lengths in the...Ch. 8 - Consider the carbon-oxygen bond in formaldehyde...Ch. 8 - Compare the nitrogen-nitrogen bond in hydrazine,...Ch. 8 - Ethanol can be made by the reaction of ethylene...Ch. 8 - Methanol can be made by partial oxidation of...Ch. 8 - Hydrogenation reactions, which involve the...Ch. 8 - Phosgene, Cl2CO, is a highly toxic gas that was...Ch. 8 - The compound oxygen difluoride is quite reactive,...Ch. 8 - Oxygen atoms can combine with ozone to form...Ch. 8 - Prob. 57GQCh. 8 - Prob. 58GQCh. 8 - Which of the following compounds or ions do not...Ch. 8 - Prob. 60GQCh. 8 - Draw resonance structures for the formate ion,...Ch. 8 - Prob. 62GQCh. 8 - Prob. 63GQCh. 8 - What is the principle of electroneutrality? Use...Ch. 8 - Prob. 65GQCh. 8 - Draw resonance structures for the SO2 molecule,...Ch. 8 - What are the orders of the NO bonds in NO2 and...Ch. 8 - Which has the greater ONO bond angle, NO2 or NO2+?...Ch. 8 - Compare the FClF angles in CIF2+ and ClF2. Using...Ch. 8 - Draw an electron dot structure for the cyanide...Ch. 8 - Draw the electron dot structure for the sulfite...Ch. 8 - Dinitrogen monoxide, N2O, can decompose to...Ch. 8 - The equation for the combustion of gaseous...Ch. 8 - The cyanate ion, OCN, has the least...Ch. 8 - Vanillin is the flavoring agent in vanilla extract...Ch. 8 - Explain why (a) XeF2 has a linear molecular...Ch. 8 - The formula for nitryl chloride is ClNO2 (in which...Ch. 8 - Hydroxyproline is a less-common amino acid. (a)...Ch. 8 - Amides are an important class of organic...Ch. 8 - Prob. 81GQCh. 8 - The molecule shown here. 2-furylmelhanethiol, is...Ch. 8 - Dihydroxyacetone is a component of quick-tanning...Ch. 8 - It is possible to draw three resonance structures...Ch. 8 - Acrolein is used to make plastics. Suppose this...Ch. 8 - Molecules in space: (a) In addition to molecules...Ch. 8 - 1,2-Dichloroethylene can be synthesized by adding...Ch. 8 - The molecule pictured below is epinephrine, a...Ch. 8 - You are doing an experiment in the laboratory and...Ch. 8 - Prob. 90ILCh. 8 - A paper published in the research Journal Science...Ch. 8 - Uracil is one of the bases in RNA, a close...Ch. 8 - Guanine is present in both DNA and RNA. (a) What...Ch. 8 - Prob. 94ILCh. 8 - Prob. 95SCQCh. 8 - Prob. 96SCQCh. 8 - Bromine-containing species play a role in...Ch. 8 - Acrylamide, H2C=CHCONH2, is a known neurotoxin and...
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
- Sulfuric acid is the industrial chemical produced in greatest quantity worldwide. About 90 billion pounds are produced each year in the United States alone. Write the Lewis structure for sulfuric acid, H2SO4, which has twooxygen atoms and two OH groups bonded to the sulfur.arrow_forwardThe electronegativities of Cl and F are 3.16 and 3.98, respectively. Determine the partial charge of each atom in ClF.arrow_forward18.) Choose all the statements that are correct. (1) Like atomic size, electronegativity decreases going across a period and increases going down a group. (2) The second most electronegative element is chlorine. (3) Electronegativity is directly proportional to atomic number. (4) Like ionization energy, electronegativity increases going across a period and decreases going down a group. (5) Electronegativity is a measure of the ability of an atom to attract electrons and form a negative ion. (6) Electronegativity is a measure of the ability of an atom in a molecule to attract electrons go itself. (7) Electronegativity was first proposed by Linus Pauling. Group of answer choices (2) (1) (4) (3) (5) (7) (6)arrow_forward
- What is electronegativity and what are its periodic trends? What is the general relationship between the size of an atom and its ionization energy?arrow_forward. The Pauling scale of electronegativity is based upon bond dissociation energies, D, and involves using the equation DAB = (DA2 x DB2)1/2 + Δ . For what process does Δ represent the energy? How is Δ related to electronegativities?arrow_forwardExplain the Sanderson's Electronegativity Scale.arrow_forward
- 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_forwardn your own words, what is meant by the term electronegativity? What are the trends across and down the periodic table for electronegativity? Explain them, and describe how they are consistent with trends of ionization energy and atomic radii.arrow_forwardNitrosyl azide, N4O, is a pale yellow solid first synthesized in 1993. Write the Lewis structure for nitrosyl azide.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_forwardWrite 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_forwardChloral, Cl3C—CH=O, reacts with water to form the sedative and hypnotic agent chloral hydrate, Cl3C—CH(OH)2. Draw Lewis structures for these substances, and describe the change in molecular shape, if any, that occurs around each of the carbon atoms during the reaction.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
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