EBK CHEMISTRY
9th Edition
ISBN: 9780100453807
Author: ZUMDAHL
Publisher: YUZU
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Chapter 9, Problem 62E
Describe the bonding in the CO32− ion using the localized electron model. How would the molecular orbital model describe the π bonding in this species?
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Chapter 9 Solutions
EBK CHEMISTRY
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...
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- a Nitrogen trifluoride, NF3, is a relatively unreactive, colorless gas. How would you describe the bonding in the NF3 molecule in terms of valence bond theory? Use hybrid orbitals. b Silicon tetrafluoride, SiF4, is a colorless gas formed when hydrofluoric acid attacks silica (SiO2) or glass. Describe the bonding in the SiF4 molecule, using valence bond theory.arrow_forwardDescribe the hybridization around the central atom and the bonding in SCl2 and OCS.arrow_forwardIt is possible to write a simple Lewis structure for the SO42- ion, involving only single bonds, which follows the octet rule. However, Linus Pauling and others have suggested an alternative structure, involving double bonds, in which the sulfur atom is surrounded by six electron pairs. (a) Draw the two Lewis structures. (b) What geometries are predicted for the two structures? (c) What is the hybridization of sulfur in each case? (d) What are the formal charges of the atoms in the two structures?arrow_forward
- The sulfamate ion, H2NSO3, can be thought of as having been formed from the amide ion, NH2, and sulphur trioxide, SO3. (a) What are the electron-pair and molecular geometries or the amide ion and or SO3? What are the hybridizations of the N and S atoms, respectively? (b) Sketch a structure for the sulfamate ion, and estimate the bond angles. (c) What changes in hybridization do you expect for N and S in the course of the reaction NH2 + SO3 H2NSO3? (d) Is SO3 the donor of an electron pair or the acceptor of an electron pair in the reaction with amide ion? Does the electrostatic potential map shown below confirm your prediction?arrow_forwardCould the anion Li2 exist? What is the ions bond order?arrow_forwardWhen considering the Lewis structure for HF, we might mistakenly conclude that HF contains three lone pairs on the F atom which are degenerate. Explain the nature of these three electron pairs by referring to the molecular orbital energy level diagram.arrow_forward
- Draw Lewis structure for OPF, (P is the central atom). Write down all possible resonance structures, including formal charges. Draw the geometry of the ion. Indicate the hybridization of the central atom and type of orbitals involved in x bonding on both bonded atoms.arrow_forwardGive the molecular orbital configuration for the valence electrons in C2 2−. Will this ion be stable?arrow_forwardConstruct the molecular orbital diagram for SrCl. Would yo u expect the bond length of SrCl+ to be longer or shorter than that of SrCl? Explain and elaborate.arrow_forward
- Describe the bonding in formaldehyde (H2CO) in terms of hybrid atomic orbitals and molecular orbitals.arrow_forwardA student claims that if element D is in group 18, then the molecular geometry of DF4(g) is square planar. Do you agree or disagree with the student? Justify your answer in terms of the VSEPR theory.arrow_forwardUse the molecular orbital model to fully describe the bonding in O₂+, O₂, O₂™, and 0₂²- Determine which of the following statements are true and which are false. The electron configuration of O₂ is (025)²(0₂s*)²(02p)²(¹2)4(¹²p*)². 2- The bond order in O₂¯ and O₂²- is, respectively, 2.5 and 1. The number of unpaired electrons in O₂ and O₂ is, respectively, 1 and 0. The electron configuration of O₂¯ is (02)²(02s*)²(0₂p)²(12p)4(¹²µ*)³. The bond energies increase in the order: 0₂²- < 0₂¯ < 0₂ < 0₂¹. Bond length increases with increasing bond order while bond energy decreases.arrow_forward
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