General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN: 9781305580343
Author: Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 10, Problem 10.32QP
What are the bond angles predicted by the VSEPR model about the carbon atom in the formate ion, HCO2−? Considering that the bonds to this atom are not identical, would you expect the experimental values to agree precisely with the VSEPR values? How might they differ?
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Don't used hand raiting don't used Ai solution
Don't used hand raiting and don't used Ai solution
13.84. Chlorine atoms react with methane, forming HCI
and CH3. The rate constant for the reaction is
6.0 × 107 M¹ s¹ at 298 K. When the experiment
was run at three other temperatures, the following data
were collected:
T (K)
k (M-1 s-1)
303
6.5 × 107
308
7.0 × 107
313
7.5 x 107
a. Calculate the values of the activation energy and the
frequency factor for the reaction.
b. What is the value of the rate constant in the lower
stratosphere, where T = 218 K?
Chapter 10 Solutions
General Chemistry - Standalone book (MindTap Course List)
Ch. 10.1 - An atom in a molecule is surrounded by four pairs...Ch. 10.1 - Use the VSEPR method to predict the geometry of...Ch. 10.1 - Prob. 10.2ECh. 10.2 - Bromine trifluoride, BrF3, has a nonzero dipole...Ch. 10.2 - Which of the following would be expected to have a...Ch. 10.2 - Two molecules, each with the general formula AX3,...Ch. 10.3 - Using hybrid orbitals, describe the bonding in NH3...Ch. 10.4 - Describe the bonding on the carbon atom in carbon...Ch. 10.4 - Dinitrogen difluoride (see Example 10.5) exists as...Ch. 10.4 - Prob. 10.3CC
Ch. 10.6 - The C2 molecule exists in the vapor phase over...Ch. 10.6 - Give the orbital diagram and electron...Ch. 10 - Describe the main features of the VSEPR model.Ch. 10 - According to the VSEPR model, what are the...Ch. 10 - Why is a lone pair expected to occupy an...Ch. 10 - Prob. 10.4QPCh. 10 - Explain why nitrogen trifluoride has a small...Ch. 10 - Prob. 10.6QPCh. 10 - What is the angle between two sp3 hybrid orbitals?Ch. 10 - Prob. 10.8QPCh. 10 - Prob. 10.9QPCh. 10 - How does the valence bond description of a...Ch. 10 - Prob. 10.11QPCh. 10 - What factors determine the strength of interaction...Ch. 10 - Prob. 10.13QPCh. 10 - Prob. 10.14QPCh. 10 - Prob. 10.15QPCh. 10 - Describe the bonding in O3, using molecular...Ch. 10 - Prob. 10.17QPCh. 10 - Which of the following molecular geometries does...Ch. 10 - Which of the following would be a polar molecule?...Ch. 10 - Prob. 10.20QPCh. 10 - Best Lewis Formula and Molecular Geometry A...Ch. 10 - Prob. 10.22QPCh. 10 - Prob. 10.23QPCh. 10 - Which of the following molecular models correctly...Ch. 10 - Prob. 10.25QPCh. 10 - Prob. 10.26QPCh. 10 - Indicate what hybrid orbital depicted below is...Ch. 10 - An atom in a molecule has two bonds to other atoms...Ch. 10 - Two compounds have the same molecular formula,...Ch. 10 - A neutral molecule is identified as a...Ch. 10 - Acetic acid, the sour constituent of vinegar, has...Ch. 10 - What are the bond angles predicted by the VSEPR...Ch. 10 - Predict the shape or geometry of the following...Ch. 10 - Use the electron-pair repulsion model to predict...Ch. 10 - Predict the geometry of the following ions, using...Ch. 10 - Use the VSEPR model to predict the geometry of the...Ch. 10 - For each of the following molecules, state the...Ch. 10 - For each of the following molecules, state the...Ch. 10 - Prob. 10.39QPCh. 10 - From the electron-pair repulsion model, predict...Ch. 10 - Predict the geometries of the following ions,...Ch. 10 - Name the geometries expected for the following...Ch. 10 - a The molecule AsF3 has a dipole moment of 2.59 D....Ch. 10 - a The molecule BrF3 has a dipole moment of 1.19 D....Ch. 10 - Which of the following molecules would be expected...Ch. 10 - Which of the following molecules would be expected...Ch. 10 - What hybrid orbitals would be expected for the...Ch. 10 - What hybrid orbitals would be expected for the...Ch. 10 - What hybrid orbitals would be expected for the...Ch. 10 - What hybrid orbitals would be expected for the...Ch. 10 - a Mercury(II) chloride dissolves in water to give...Ch. 10 - a Nitrogen trifluoride, NF3, is a relatively...Ch. 10 - a Carbonyl fluoride, COF2, is an extremely...Ch. 10 - a The molecule HNNH exists as a transient species...Ch. 10 - The hyponitrite ion, ONNO, exists in solid...Ch. 10 - Fumaric acid, C4H4O4, occurs in the metabolism of...Ch. 10 - Describe the electronic structure of each of the...Ch. 10 - Use molecular orbital theory to describe the...Ch. 10 - Prob. 10.59QPCh. 10 - Write the molecular orbital configuration of the...Ch. 10 - Predict the molecular geometry of the following: a...Ch. 10 - Prob. 10.62QPCh. 10 - Which of the following molecules or ions are...Ch. 10 - Which of the following molecules or ions are...Ch. 10 - Describe the hybrid orbitals used by each carbon...Ch. 10 - Prob. 10.66QPCh. 10 - Explain how the dipole moment could be used to...Ch. 10 - Two compounds have the formula Pt(NH3)2Cl2....Ch. 10 - Explain in terms of bonding theory why all four...Ch. 10 - Explain in terms of bonding theory why all atoms...Ch. 10 - What is the molecular orbital configuration of...Ch. 10 - Prob. 10.72QPCh. 10 - Calcium carbide, CaC2, consists of Ca2+ and C22...Ch. 10 - Sodium peroxide, Na2O2, consists of Na+ and O22...Ch. 10 - The oxygen oxygen bond in O2 is 112 pm and in O2...Ch. 10 - The nitrogennitrogen bond distance in N2 is 109...Ch. 10 - Using molecular orbital theory, determine the...Ch. 10 - The ionization energy of O2 is smaller than the...Ch. 10 - Prob. 10.79QPCh. 10 - Prob. 10.80QPCh. 10 - Prob. 10.81QPCh. 10 - Prob. 10.82QPCh. 10 - What is the biological importance of stratospheric...Ch. 10 - Prob. 10.84QPCh. 10 - Prob. 10.85QPCh. 10 - The bond length in C2 is 131 pm. Compare this with...Ch. 10 - Calcium carbide, CaC2, has an ionic structure with...Ch. 10 - Write Lewis formulas for the BF molecule (two with...Ch. 10 - Boron trifluoride, BF3, reacts with ammonia, NH3,...Ch. 10 - Prob. 10.90QPCh. 10 - Allene (1,2-propadicne), a gas, has the following...Ch. 10 - Prob. 10.92QPCh. 10 - The triiodide ion, I3, and the azide ion, N3, have...Ch. 10 - Hydrogen azide (also known as hydrazoic acid),...Ch. 10 - Prob. 10.95QPCh. 10 - A molecule XF6 (having no lone pairs) has a dipole...Ch. 10 - Describe the molecular orbital configurations of...Ch. 10 - Prob. 10.98QPCh. 10 - Three different compounds have the same molecular...Ch. 10 - Prob. 10.100QPCh. 10 - Prob. 10.101QPCh. 10 - Solid sulfur normally consists of crystals of S8...Ch. 10 - Prob. 10.103QPCh. 10 - Consider the bonding in nitrate ion, NO3. First...Ch. 10 - A molecular compound is composed of 52.5% Xe,...Ch. 10 - A molecular compound is composed of 58.8% Xe,...Ch. 10 - A compound of chlorine and fluorine. ClFn, reacts...Ch. 10 - Excess fluorine, F2(g), reacts at 150C with...Ch. 10 - Prob. 10.109QPCh. 10 - One resonance formula of benzene, C6H6, is What is...
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
- My Organic Chemistry textbook says about the formation of cyclic hemiacetals, "Such intramolecular reactions to form five- and six-membered rings are faster than the corresponding intermolecular reactions. The two reacting functional groups, in this case OH and C=O, are held in close proximity, increasing the probability of reaction."According to the book, the formation of cyclic hemiacetals occurs in acidic conditions. So my question is whether the carbonyl group in this reaction reacts first with the end alcohol on the same molecule or with the ethylene glycol. And, given the explanation in the book, if it reacts first with ethylene glycol before its own end alcohol, why would it? I don't need to know the final answer. I need to know WHY it would not undergo an intermolecular reaction prior to reacting with the ethylene glycol if that is the case. Please do not use an AI answer.arrow_forwardDon't used hand raiting and don't used Ai solutionarrow_forwardHighlight in red each acidic location on the organic molecule at left. Highlight in blue each basic location on the organic molecule at right. Note for advanced students: we mean acidic or basic in the Brønsted-Lowry sense only. Cl N شیخ x Garrow_forward
- Q4: Draw the mirror image of the following molecules. Are the molecules chiral? C/ F LL CI CH3 CI CH3 0 CI CH3 CI CH3 CH3arrow_forwardComplete combustion of a 0.6250 g sample of the unknown crystal with excess O2 produced 1.8546 g of CO2 and 0.5243 g of H2O. A separate analysis of a 0.8500 g sample of the blue crystal was found to produce 0.0465 g NH3. The molar mass of the substance was found to be about 310 g/mol. What is the molecular formula of the unknown crystal?arrow_forward4. C6H100 5 I peak 3 2 PPM Integration values: 1.79ppm (2), 4.43ppm (1.33) Ipeakarrow_forward
- Nonearrow_forward3. Consider the compounds below and determine if they are aromatic, antiaromatic, or non-aromatic. In case of aromatic or anti-aromatic, please indicate number of I electrons in the respective systems. (Hint: 1. Not all lone pair electrons were explicitly drawn and you should be able to tell that the bonding electrons and lone pair electrons should reside in which hybridized atomic orbital 2. You should consider ring strain- flexibility and steric repulsion that facilitates adoption of aromaticity or avoidance of anti- aromaticity) H H N N: NH2 N Aromaticity (Circle) Aromatic Aromatic Aromatic Aromatic Aromatic Antiaromatic Antiaromatic Antiaromatic Antiaromatic Antiaromatic nonaromatic nonaromatic nonaromatic nonaromatic nonaromatic aromatic TT electrons Me H Me Aromaticity (Circle) Aromatic Aromatic Aromatic Aromatic Aromatic Antiaromatic Antiaromatic Antiaromatic Antiaromatic Antiaromatic nonaromatic nonaromatic nonaromatic nonaromatic nonaromatic aromatic πT electrons H HH…arrow_forwardA chemistry graduate student is studying the rate of this reaction: 2 HI (g) →H2(g) +12(g) She fills a reaction vessel with HI and measures its concentration as the reaction proceeds: time (minutes) [IH] 0 0.800M 1.0 0.301 M 2.0 0.185 M 3.0 0.134M 4.0 0.105 M Use this data to answer the following questions. Write the rate law for this reaction. rate = 0 Calculate the value of the rate constant k. k = Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher: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
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
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
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
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:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
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