Principles of Modern Chemistry
8th Edition
ISBN: 9781305079113
Author: David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher: Cengage Learning
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Textbook Question
Chapter 6, Problem 62P
Discuss the nature of the bonding in the nitrate ion
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Discuss the nature of the bonding in the nitrate ion (NO5).
Draw the possible Lewis resonance diagrams for this ion.
Use the VSEPR theory to determine the steric number, the
hybridization of the central N atom, and the geometry of
the ion. Show how the use of resonance structures can be
avoided by introducing a de-localized 7 MO. What bond
order is predicted by the MO model for the N-O bonds
in the nitrate ion?
Iodine and oxygen form a complex series of ions, among them IO4^- and IO5^3-. Draw the Lewis structures for these ions, and specify their electron-pair geometries and the shapes of the ions. What is the hybridization of the I atom in these ions?
Draw the molecular orbital diagram of the hydroxyl radical, HO•, clearly labeling
the MOs as o, o*, T, T*, or nb. What is the bond order? Given that the most stable electronic
structures are ones in which all of the bonding and non-bonding orbitals are filled, would you
expect HO• to act as an oxidizing or reducing agent? Why?
Chapter 6 Solutions
Principles of Modern Chemistry
Ch. 6 - Determine the number of nodes along the...Ch. 6 - Determine the number of nodes along the...Ch. 6 - Sketch the shape of each of the molecular...Ch. 6 - Sketch the shape of each of the molecular...Ch. 6 - Compare the electron density in the 1g and 1u*...Ch. 6 - Explain why 1g is the ground state for H2+ . By...Ch. 6 - Prob. 7PCh. 6 - Predict the ground electronic state of the He22+...Ch. 6 - Prob. 9PCh. 6 - Prob. 10P
Ch. 6 - Without consulting tables of data, predict which...Ch. 6 - Without consulting tables of data, predict which...Ch. 6 - Without consulting tables of data, on the same...Ch. 6 - Without consulting tables of data, on the same...Ch. 6 - Suppose we supply enough energy to H2 to remove...Ch. 6 - Suppose we supply enough energy to He2+ to remove...Ch. 6 - Prob. 17PCh. 6 - When one electron is added to an oxygen molecule,...Ch. 6 - Predict the valence electron configuration and the...Ch. 6 - Predict the valence electron configuration and the...Ch. 6 - Prob. 21PCh. 6 - For each of the following valence electron...Ch. 6 - For each of the electron configurations in Problem...Ch. 6 - For each of the electron configurations in Problem...Ch. 6 - Following the pattern of Figure 6.21, work out the...Ch. 6 - Following the pattern of Figure 6.21, work out the...Ch. 6 - The bond length of the transient diatomic molecule...Ch. 6 - The compound nitrogen oxide (NO) forms when the...Ch. 6 - What would be the electron configuration for a HeH...Ch. 6 - The molecular ion HeH+ has an equilibrium bond...Ch. 6 - Prob. 31PCh. 6 - Predict the ground state electronic configuration...Ch. 6 - The bond dissociation energies for the species NO,...Ch. 6 - The ionization energy of CO is greater than that...Ch. 6 - Photoelectron spectra were acquired from a sample...Ch. 6 - Photoelectron spectra were acquired from a sample...Ch. 6 - Prob. 37PCh. 6 - From the n=0 peaks in the photoelectron spectrum...Ch. 6 - The photoelectron spectrum of HBr has two main...Ch. 6 - The photoelectron spectrum of CO has four major...Ch. 6 - Write simple valence bond wave functions for the...Ch. 6 - Write simple valence bond wave functions for the...Ch. 6 - Both the simple VB model and the LCAO method...Ch. 6 - Both the simple VB model and the LCAO method...Ch. 6 - Write simple valence bond wave functions for...Ch. 6 - Write simple valence bond wave functions for...Ch. 6 - Write simple valence bond wave functions for the...Ch. 6 - Write simple valence bond wave functions for the...Ch. 6 - Formulate a localized bond picture for the amide...Ch. 6 - Formulate a localized bond picture for the...Ch. 6 - Prob. 51PCh. 6 - Draw a Lewis electron dot diagram for each of the...Ch. 6 - Describe the hybrid orbitals on the chlorine atom...Ch. 6 - Describe the hybrid orbitals on the chlorine atom...Ch. 6 - The sodium salt of the unfamiliar orthonitrate ion...Ch. 6 - Describe the hybrid orbitals used by the carbon...Ch. 6 - Describe the bonding in the bent molecule NF2 ....Ch. 6 - Describe the bonding in the bent molecule OF2 ....Ch. 6 - The azide ion (N3) is a weakly bound molecular...Ch. 6 - Formulate the MO structure of (NO2+) for localized...Ch. 6 - Discuss the nature of the bonding in the nitrite...Ch. 6 - Discuss the nature of the bonding in the nitrate...Ch. 6 - The pyridine molecule (C5H5N) is obtained by...Ch. 6 - For each of the following molecules, construct the...Ch. 6 - (a) Sketch the occupied MOs of the valence shell...Ch. 6 - Calcium carbide (CaC2) is an intermediate in the...Ch. 6 - The B2 molecule is paramagnetic; show how this...Ch. 6 - The Be2 molecule has been detected experimentally....Ch. 6 - Prob. 69APCh. 6 - The molecular ion HeH+ has an equilibrium bond...Ch. 6 - The MO of the ground state of a heteronuclear...Ch. 6 - The stable molecular ion H3+ is triangular, with...Ch. 6 - According to recent spectroscopic results,...Ch. 6 - trans-tetrazene (N4H4) consists of a chain of four...
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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_forwardThe ionization energy of O2 is smaller than the ionization energy of atomic O; the opposite is true for the ionization energies of N2 and atomic N. Explain this behavior in terms of the molecular orbital energy diagrams of O2 and N2.arrow_forwardExplain the Reduction of Polar C—X σ Bonds ?arrow_forward
- Draw the best Lewis dot structure for BrCl₅, being sure to give the electronic geometry, molecular geometry, hybridization of the central element, polarity, and bond angle around the cental element.arrow_forwardWhat is the hybridization of the central atom in the bromine pentafluoride 0 X S (BrFs) molecule?arrow_forwardDraw a Lewis structure for diimide, H-N=N-H, explain how the Lewis structure is drawn. Then, using valence bond theory, describe the bonding in this compound. What orbitals overlap to form the bond between nitrogen atoms in this compound? Explain and elaborate.arrow_forward
- Draw the molecular orbital diagrams for Ne(2), N(2) ^2- and Be(2). Are they stable or unstable?arrow_forwardDraw a Lewis diagram(s) for the ozone molecule (O3). Determine the steric number and hybridization of the central oxygen atom, and identify the molecular geometry. Describe the nature of the p bonds and give the bondorder of the O-O bonds in ozone.arrow_forwardWhat is the hybridization of the central phosphorus atom of PO43− ?arrow_forward
- For a N H 4 + ion, identify its molecular shape, bond angle, and hybrid orbitals.arrow_forwardDescribe how the bond angles in TeF4 and BRF5 deviate from those found in a trigonal bipyramidal and an octahedron, respectively. In TeF4, the lone pair of electrons repels the Te-F bonding pairs, causing the F-Te-F angles to be smaller than v in the ideal trigonal bipyramid. In BrF5, the lone pair is located perpendicular v to the plane of four of the F atoms, giving a square pyramid v geometry to the molecule. The angle between the four E in the plane and the F above the plane will be less than v 90° due to lone pair repulsion. The F-Br-F angles in the plane will remain DEC étv MacBook Air DD F4 F5 F6 F7 F8 F9 F10 F2 F3 @ # 2$ 3 4 6. 8. S LOarrow_forwardTwo useful organic compounds that contain Cl atoms are vinyl chloride(CH2=CHCl) and chloroethane (CH3CH2Cl). Vinyl chloride is the startingmaterial used to prepare poly(vinyl chloride), a plastic in insulation,pipes, and bottles. Chloroethane (ethyl chloride) is a local anesthetic.Why is the C–Cl bond in vinyl chloride stronger than the C–Cl bond inchloroethane?arrow_forward
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