Inorganic Chemistry
5th Edition
ISBN: 9780321811059
Author: Gary L. Miessler, Paul J. Fischer, Donald A. Tarr
Publisher: Prentice Hall
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Chapter 3, Problem 3.30P
a. Are the
b. Are the axial or equatorial bonds likely to be longer in
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Inorganic Chemistry
Ch. 3.1 - Use electron-dot diagrams and formal charges to...Ch. 3.2 - Predict the structures of the following ions....Ch. 3.2 - Prob. 3.3ECh. 3.2 - Which molecule has the smallest bond angle in each...Ch. 3.2 - Briefly account for the following observations: a....Ch. 3.2 - Does this approach work for different steric...Ch. 3 - The dimethyldithiocarbamate ion, [S2CN( CH 3 )2]-...Ch. 3 - Several resonance structures are possible for each...Ch. 3 - Draw the resonance structures for the...Ch. 3 - Three isomers having the formula N2CO are known:...
Ch. 3 - Show the possible resonance structures for nitrous...Ch. 3 - Nitric acid, which exists as HNO3 molecules in the...Ch. 3 - L. C. Allen has suggested that a more meaningful...Ch. 3 - Give Lewis dot structures and sketch the shapes of...Ch. 3 - Give Lewis dot structures and sketch the shapes of...Ch. 3 - Give Lewis dot structures and sketch the shapes of...Ch. 3 - Explain the trends in bond angles and bond lengths...Ch. 3 - Select from each set the molecule or ¡on having...Ch. 3 - a. Compare the structures of the azide ion, N3 ,...Ch. 3 - Consider the series OCl2,O( CH3)2 , and O( SiH3)2...Ch. 3 - Two ions isoelectronic with carbon suboxide, C3O2...Ch. 3 - Explain the following: a. Ethylene, C2H4 , is a...Ch. 3 - Explain the following: a. PCI5 is a stable...Ch. 3 - X-ray crystal structures of ClOF3 and BrOF3 have...Ch. 3 - Make the following comparisons about the molecules...Ch. 3 - Prob. 3.20PCh. 3 - A solution containing the lO2F2 ion reacts slowly...Ch. 3 - The XeOF3 anion has been reported recently (D. S....Ch. 3 - Predict the structure of l(CF3)Cl2 . Do you expect...Ch. 3 - a. Which has the longer axial PF distance, PF2(...Ch. 3 - Prob. 3.25PCh. 3 - SeCl62,TeCl62 , and CIF6 are all octahedral, but...Ch. 3 - Prob. 3.27PCh. 3 - The thiazyldichloride ion, NSCl2- , is...Ch. 3 - Sketch the most likely structure of PCl3Br2 and...Ch. 3 - a. Are the CF3 groups in PCl3( CF3)2 more likely...Ch. 3 - Of the molecules C1SO2CH3,C1SO2CF3 , and ClSO2CCl3...Ch. 3 - Prob. 3.32PCh. 3 - Prob. 3.33PCh. 3 - Prob. 3.34PCh. 3 - Prob. 3.35PCh. 3 - Although the CF distances and the FCF bond angles...Ch. 3 - The Cl...Cl distance in CCl4 is 289 pm, and the...Ch. 3 - The FCF angle in F2CO , shown here, is 109.5°; the...Ch. 3 - Compounds in which hydrogen is the outer atom can...Ch. 3 - For each of the following bonds, indicate which...Ch. 3 - Give Lewis dot structures and shapes for the...Ch. 3 - Give Lewis dot structures and sketch the shapes...Ch. 3 - Which of the molecules in Problem 3.41 are polar?Ch. 3 - Which of the molecules in Problem 3.42 are polar?Ch. 3 - Prob. 3.45PCh. 3 - Prob. 3.46P
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- 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?arrow_forwardTwo variations of the octahedral geometry (see Table 4-1) are illustrated below. Which of the compounds/ions Br3, ClF3, XeF4, SF4, PF5, ClF5, and SF6 have these molecular structures?arrow_forwardWhat hybridization is required for central atoms exhibiting trigonal bipyramidal geometry? Octahedral geometry? Describe the bonding of PF5, SF4, SF6, and IF5, using the localized electron model.arrow_forward
- What modification to the molecular orbital model was made from the experimental evidence that B2 is paramagnetic?arrow_forwarda 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_forwardExplain in terms of bonding theory why all atoms of H2CCCCH2 must lie in the same plane.arrow_forward
- The simple valence bond picture of O2 does not agree with the molecular orbital view. Compare these two theories with regard to the peroxide ion, O22. (a) Draw an electron dot structure for O22. What is the bond order of the ion? (b) Write the molecular orbital electron configuration for O22. What is the bond order based on this approach? (c) Do the two theories of bonding lead to the same magnetic character and bond order fo r O22 ss?arrow_forwardIdentify the hybrid orbitals used by boron in BCl3 and in BCl4, the ion formed from the reaction of BCl3 and Cl. Explain your choices.arrow_forwardWhat is the OSO angle and the hybrid orbital set used by sulfur in each of the following molecules or ions? (a) SO2 (b) SO3 (c) SO32 (d) SO42 Do all have the same value for the OSO angle? Does the S atom in all these species use the same hybrid orbitals?arrow_forward
- There are two different molecules with the formula N2F2: Is either molecule polar? Explain.arrow_forwardThe 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_forward
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