Chemistry with Access Code, Hybrid Edition
9th Edition
ISBN: 9781285188492
Author: Steven S. Zumdahl
Publisher: CENGAGE L
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 9, Problem 98CP
Given that the ionization energy of F2− is 290 kJ/mol, do the following:
a. Calculate the bond energy of F2−. You will need to look up the bond energy of F2 and ionization energy of F−.
b. Explain the difference in bond energy between F2− and F2 using MO theory.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
2
НО.
2
NH₂
4
A. 2p-2p
B. sp²-sp²
C. sp-sp³
D. SD-Sp
6
1 3 5
Which bond has the lowest bond dissociation energy?
A. C6-C7
B. C2-C3
7
C. C5-C6
D. C4-C5
What orbitals are used to form the second pi bond between C6 and C7?
The formula for nitryl chloride is CINO2 (in which N is the central atom).
a.Draw the Lewis structure for the molecule, including all resonance structures.
b.What is the N-O bond order?
c.Describe the electron-pair and molecular geometries and give values for all bond angles.
d.What is the most polar bond in the molecule? Is the molecule polar?
e.The computer program used to calculate electrostatic potential surfaces gave the following charges on atoms in the molecule: A =-0.03, B = -0.26, and C = +0.56. Identify the atoms A, B, and C. Are these calculated charges in accord with your predictions?
Chapter 9 Solutions
Chemistry with Access Code, Hybrid Edition
Ch. 9 - Why do we hybtidize atomic orbitals to explain the...Ch. 9 - What hybridization is required for central atoms...Ch. 9 - Describe the bonding in H2S, CH4, H2CO and HCN...Ch. 9 - What hybridization is required for central atoms...Ch. 9 - Electrons in bonding molecular orbitals are most...Ch. 9 - What are molecular orbitals? How do they compare...Ch. 9 - Explain the difference between the and MOs for...Ch. 9 - Compare Figs. 4-47 and 4-49. Why are they...Ch. 9 - Which of the following would you expect to be more...Ch. 9 - Draw the Lewis structure for HCN. Indicate the...
Ch. 9 - Which is the more correct statement: The methane...Ch. 9 - Compare and contrast the MO model with the local...Ch. 9 - What are the relationships among bond order, bond...Ch. 9 - In the hybrid orbital model, compare and contrast ...Ch. 9 - In the molecular orbital mode l, compare and...Ch. 9 - Why are d orbitals sometimes used to form hybrid...Ch. 9 - The atoms in a single bond can rotate about the...Ch. 9 - Compare and contrast bonding molecular orbitals...Ch. 9 - What modification to the molecular orbital model...Ch. 9 - Why does the molecular orbital model do a better...Ch. 9 - The three NO bonds in NO3 are all equivalent in...Ch. 9 - Use the localized electron model to describe the...Ch. 9 - Use the localized electron model to describe the...Ch. 9 - Use the localized electron model to describe the...Ch. 9 - Use the localized electron model to describe the...Ch. 9 - The space-filling models of ethane and ethanol are...Ch. 9 - The space-filling models of hydrogen cyanide and...Ch. 9 - Give the expected hybridization of the central...Ch. 9 - Give the expected hybridization of the central...Ch. 9 - Give the expected hybridization of the central...Ch. 9 - Give the expected hybridization of the central...Ch. 9 - For each of the following molecules, write the...Ch. 9 - For each of the following molecules or ions that...Ch. 9 - Prob. 31ECh. 9 - The allene molecule has the following Lewis...Ch. 9 - Indigo is the dye used in coloring blue jeans. The...Ch. 9 - Urea, a compound formed in the liver, is one of...Ch. 9 - Biacetyl and acetoin are added to margarine to...Ch. 9 - Many important compounds in the chemical industry...Ch. 9 - Two molecules used in the polymer industry are...Ch. 9 - Hot and spicy foods contain molecules that...Ch. 9 - One of the first drugs to be approved for use in...Ch. 9 - The antibiotic thiarubin-A was discovered by...Ch. 9 - Consider the following molecular orbitals formed...Ch. 9 - Sketch the molecular orbital and label its type (...Ch. 9 - Which of the following are predicted by the...Ch. 9 - Which of the following are predicted by the...Ch. 9 - Using the molecular orbital model, write electron...Ch. 9 - Consider the following electron configuration:...Ch. 9 - Using molecular orbital theory, explain why the...Ch. 9 - Using the molecular orbital model to describe the...Ch. 9 - The transport of O2 in the blood is carried out by...Ch. 9 - A Lewis structure obeying the octet rule can be...Ch. 9 - Using the molecular orbital model, write electron...Ch. 9 - Using the molecular orbital model, write electron...Ch. 9 - In which of the following diatomic molecules would...Ch. 9 - In terms of the molecular orbital model, which...Ch. 9 - Show how two 2p atomic orbitals can combine to...Ch. 9 - Show how a hydrogen 1s atomic orbital and a...Ch. 9 - Use Figs. 4-54 and 4-55 to answer the following...Ch. 9 - Acetylene (C2H2) can be produced from the reaction...Ch. 9 - Describe the bonding in NO+, NO, and NO, using...Ch. 9 - Describe the bonding in the O3 molecule and the...Ch. 9 - Describe the bonding in the CO32 ion using the...Ch. 9 - Draw the Lewis structures, predict the molecular...Ch. 9 - FClO2 and F3ClO can both gain a fluoride ion to...Ch. 9 - Two structures can be drawn for cyanuric acid: a....Ch. 9 - Give the expected hybridization for the molecular...Ch. 9 - Vitamin B6 is an organic compound whose deficiency...Ch. 9 - Aspartame is an artificial sweetener marketed...Ch. 9 - Prob. 69AECh. 9 - The three most stable oxides of carbon are carbon...Ch. 9 - Complete the following resonance structures for...Ch. 9 - Prob. 73AECh. 9 - Describe the bonding in the first excited state of...Ch. 9 - Using an MO energy-level diagram, would you expect...Ch. 9 - Show how a dxz. atomic orbital and a pz, atomic...Ch. 9 - What type of molecular orbital would result from...Ch. 9 - Consider three molecules: A, B, and C. Molecule A...Ch. 9 - Draw the Lewis structures for TeCl4, ICl5, PCl5,...Ch. 9 - A variety of chlorine oxide fluorides and related...Ch. 9 - Pelargondin is the molecule responsible for the...Ch. 9 - Complete a Lewis structure for the compound shown...Ch. 9 - Which of the following statements concerning SO2...Ch. 9 - Consider the molecular orbital electron...Ch. 9 - Place the species B2+ , B2, and B2 in order of...Ch. 9 - Consider the following computer-generated model of...Ch. 9 - Cholesterol (C27liu;O) has the following...Ch. 9 - Cyanamide (H2NCN), an important industrial...Ch. 9 - A flask containing gaseous N2 is irradiated with...Ch. 9 - Prob. 92CPCh. 9 - Values of measured bond energies may vary greatly...Ch. 9 - Use the MO model to explain the bonding in BeH2....Ch. 9 - Prob. 95CPCh. 9 - Arrange the following from lowest to highest...Ch. 9 - Use the MO model to determine which of the...Ch. 9 - Given that the ionization energy of F2 is 290...Ch. 9 - Carbon monoxide (CO) forms bonds to a variety of...Ch. 9 - Prob. 100CPCh. 9 - As the bead engineer of your starship in charge of...Ch. 9 - Determine the molecular structure 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
- 6. Which bond is likely to be polar? A. F2 B. HF C. I2 D. H2arrow_forward3. Draw all the possible resonance structures for each of the following molecules. a. SO₂ b. NO3 4. Draw Lewis structures for the following molecules. Describe how the bond angles would be altered based on the Lewis structure. a. CH₂S b. SC1₂ 9arrow_forwardIf we were to compare the SINGLE bond in Fluorine to two people, what would the best comparison be ? A. Two people who work for the same boss but have different working hours? B Two kids in their first relationship,always arguing over the smallest things? C. Two people who happen to have the same father but different mothers? D. Two people in business who are trying to cheat each other out of money?arrow_forward
- 10. How many resonance structures are there for the CO32- ion? A. 3 B. 1 C. 4 D. 2arrow_forwardConsider the following species: NO*, NO,", and NO, a. Draw Lewis structures and, if applicable, resonance structures for each species. b. Rank the species in order of shortest bond length to longest. c. Count the number of sigma and pi bonds in each species.arrow_forward11. Which is a compound? steel water a. b. 12. If the volume of a substance is 98.2 cc and it has a mass 56.12 grams, it should have a density of kg/m³. a. 570 C. 571.5 b. 572 d. Answer is not among the choices 13. When the electronegativities of two atoms are about the same,_______result/s. a. Ionic bonds C. Polar covelent bonds b. Non-polar covalent bonds d. Both a and b 14. 80.45 g of charcoal was combined with 160.18 g of oxygen to produce ash and gases. How much ash, in grams, were left if 220.3 g of gases were produced? a. 20.3 b. 60.1 15. CH4 is the C. oxygen d. Both a and b a. structural b. empirical formula for methane. 16. Which is an element? a. sugar b. alcohol C. d. C. d. C. d. 79.7 Answer is not among the choices molecular Both b and c water None of the choices are elementsarrow_forward
- 3. In a pi bond, A. electron density lies along the internuclear axis. B. electron density lies above and below the internuclear axis. C. electrons are more dense than they are in sigma bonds. D. more than two electrons are involved in the bond.arrow_forwardWhich of the following species is/are not resonance form(s) of the anionic species in the box? II IV Select one: A. Il and IV B. I and II C. I and II D. IIarrow_forwardSulfur dioxide (SO2) and carbon dioxide (CO2) have somewhat different properties, in spite of of the fact that both are triatomic molecules with two terminal oxygen atoms. Explain why they are as different as they are? a. Draw the best Lewis Structure for both molecules in the space below: b. Write the correct formal charge value next to every single atom. c. Identify AND compare each of their following features in the Summary Table below: d. Draw all possible resonance structures (if any) and justify the best ones by citing the “Rule” for best Lewis Structure based on the formal charge distribution.arrow_forward
- Answer the following questions about compound a. Label the shortest C–C single bond. b. Label the longest C–C single bond. c. Considering all the bonds, label the shortest C–C bond. d. Label the weakest C–C bond. e.Label the strongest C–H bond. f.Explain why bond [1] and bond [2] are different in length, even though they are both C–C single bonds.arrow_forwardIf we were to compare the TRIPLE bond in Nitrogen to two people ,what would the best comparison be? A Two people who go swimming but only one can go under water at any particular time? B. Two people whose shoes are always a little too small to fit on their feet properly? C.Two people who have been married for several decades and are totally devoted to each other? D. Two people who are constantly washing their hands out of fear for getting some sickness?arrow_forwardFrom this graph, what are the bond length and bond strengthin the H2 molecule?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
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
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