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 3.23P
Predict the structure of
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(a) Sketch the occupied MOs of the valence shell for the N2
molecule. Label the orbitals as o or ™ orbitals, and
specify which are bonding and which are antibonding.
(b) If one electron is removed from the highest occupied
orbital of N2, will the equilibrium N-N distance
become longer or shorter? Explain briefly.
While O2 is a colorless gas, liquid O2 is blue. Explain this interesting feature of liquid O2. Suggest how liquid O2 can be used to demonstrate the magnetic property of dioxygen molecule.
(a) Construct a molecular orbital energy diagram of N₂.
(b) Use this diagram to explain why the first ionization of N₂ is greater than that of N.
(b) Use this diagram to predict which is more favorable: the first electron affinity of N₂ or that of N.
Chapter 3 Solutions
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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- Predict the magnetic properties and bond orders of (a) theperoxide ion, O22 - ; (b) the acetylide ion, C22 - .arrow_forward3. Sketch the molecular orbital diagrams for O2, O2 (superoxide, 1e reduction of O2) and 02 (peroxide, 2e reduction of O2). Using these diagrams, provide the bond order for each of the molecules and state if they are diamagnetic or paramagneticarrow_forwardClassify O2 and N2 as either paramagnetic or diamagnetic. explain your answer by completing the orbitals in the MO energy level diagrams and referring to the electronic structure of these two moleculesarrow_forward
- .Draw the diatomic molecular orbital for NO* (assume the 2s and 2p orbitals for both N and O are capable of hybridization). State the bond order, magnetic properties and identify the HOMO/LUMO(s). If the compound [Ru(-IV)(NO)]2+ were to be real, explain how NOT would coordinate to the ruthenium center?arrow_forward(a) What does the term diamagnetism mean? (b) How doesa diamagnetic substance respond to a magnetic field?(c) Which of the following ions would you expect to bediamagnetic: N22 -, O22 -, Be22 + , C2-?arrow_forwardWhat is the molecular geometry of the PF4^+ (15P & 9F). Explain your answer brieflyarrow_forward
- Shown below is the molecular orbital diagram for O2. Does O22– have a shorter or longer bond length?arrow_forwardIn which of these two hydrides:NH3or SbH3,would you expect a greater distortion from the normal tetrahedral bond angle of 109°? And give reason for your answerarrow_forwardPredict the structure of I(CF3)Cl2. Do you expect the CF3 group to be in an axial or equatorial position? Why? (See R. Minkwitz, M. Merkei, Inorg. Chem ., 1999 , 38 , 5041.)arrow_forward
- High-resolution photoelectron spectroscopy has provided information on the energy levels and bond distance in the ion. Prepare a molecular orbital energy level diagram for this ion Ar2+. How would you expect the bond distance in to compare with 198.8 pm, the bond distance in Cl2arrow_forwardWhat is the hybridization of As in AsCl3?arrow_forward(1) Show the all shapes of bonding and antibonding molecular orbitals (MOS) by combinations of two p orbitals. (2) Describe the sigma (ơ) and pi (x) bond for ethylene (C2H4). -arrow_forward
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