 11.11.1: Compare the approximations built into valencebond theory and molec...
 11.11.2: Discuss the steps involved in the construction of sp3, sp2, and sp ...
 11.11.3: Distinguish between the Pauling and Mulliken electronegativity scales.
 11.11.4: Discuss the steps involved in the calculation of the energy of a sy...
 11.11.5: Discuss the approximations built into the Hckel method.
 11.11.6: Distinguish between delocalization energy, electron binding energy...
 11.11.7: Use concepts of molecular orbital theory to describe the biochemica...
 11.11.8: Distinguish between semiempirical, ab initio, and density function...
 11.11.1(a): Give the groundstate electron configurations and bond orders of (a...
 11.11.1(b): Give the groundstate electron configurations of (a) H2 , (b) N2, a...
 11.11.2(a): Give the groundstate electron configurations of (a) CO, (b) NO, an...
 11.11.2(b): Give the groundstate electron configurations of (a) ClF, (b) CS, a...
 11.11.3(a): From the groundstate electron configurations of B2 and C2, predict...
 11.11.3(b): Which of the molecules N2, NO, O2, C2, F2, and CN would you expect ...
 11.11.4(a): Sketch the molecular orbital energy level diagram for XeF and deduc...
 11.11.4(b): Sketch the molecular orbital energy level diagrams for BrCl and ded...
 11.11.5(a): Use the electron configurations of NO and N2 to predict which is li...
 11.11.5(b): Arrange the species O2 +, O2, O2 , O2 2 in order of increasing bond...
 11.11.6(a): Show that the sp2 hybrid orbital (s + 21/2p)/31/2 is normalized to ...
 11.11.6(b): Normalize the molecular orbital A +B in terms of the parameter and ...
 11.11.7(a): Confirm that the bonding and antibonding combinations A B are mutua...
 11.11.7(b): Suppose that a molecular orbital has the form N(0.145A + 0.844B). F...
 11.11.8(a): Can the function = x(L x) be used as a trial wavefunction for the n...
 11.11.8(b): Can the function = x2(L 2x) be used as a trial wavefunction for the...
 11.11.9(a): Suppose that the function = Aear2, with A being the normalization c...
 11.11.9(b): Suppose that the function = Aear2, with A being the normalization c...
 11.11.10(a): What is the energy of an electron that has been ejected from an orb...
 11.11.10(b): What is the energy of an electron that has been ejected from an orb...
 11.11.11(a): Construct the molecular orbital energy level diagrams of ethene on ...
 11.11.11(b): Construct the molecular orbital energy level diagrams of ethyne (ac...
 11.11.12(a): Write down the secular determinants for (a) linear H3, (b) cyclic H...
 11.11.12(b): Predict the electronic configurations of (a) the benzene anion, (b)...
 11.11.13(a): Write down the secular determinants (a) anthracene (8), (b) phenant...
 11.11.13(b): Use mathematical software to estimate the electron binding energy ...
 11.11.9: The same data as in 11.8 may be used to calculate the molecular pot...
 11.11.10: J.G. Dojahn, E.C.M. Chen, and W.E. Wentworth (J. Phys. Chem. 100, 9...
 11.11.11: Rydberg molecules are molecules with an electron in an atomic orbit...
 11.11.12: In a particular photoelectron spectrum using 21.21 eV photons, elec...
 11.11.13: Set up and solve the Hckel secular equations for the electrons of N...
 11.11.14: In the free electron molecular orbital (FEMO) theory, the electrons...
 11.11.15: The FEMO theory ( 11.14) of conjugated molecules is rather crude an...
 11.11.16: For monocyclic conjugated polyenes (such as cyclobutadiene and benz...
 11.11.17: If you have access to mathematical software that can perform matrix...
 11.11.18: Molecular orbital calculations based on semiempirical, ab initio, ...
 11.11.19: Electronic excitation of a molecule may weaken or strengthen some b...
 11.11.20: As mentioned in Section 2.8, molecular electronic structure methods...
 11.11.21: An sp2 hybrid orbital that lies in the xyplane and makes an angle ...
 11.11.22: Use the expressions in 11.8 and 11.9 to show that the antibonding o...
 11.11.23: Derive eqns 11.11 and 11.14 by working with the normalized LCAOMOs...
 11.11.24: Take as a trial function for the ground state of the hydrogen atom ...
 11.11.25: We saw in Section 11.5 that, to find the energies of the bonding an...
 11.11.26: In Exercise 11.12a you were invited to set up the Hckel secular det...
 11.11.27: There is some indication that other hydrogen ring compounds and ion...
 11.11.28: Here we develop a molecular orbital theory treatment of the peptide...
 11.11.29: Molecular orbital calculations may be used to predict trends in the...
Solutions for Chapter 11: Molecular structure
Full solutions for Physical Chemistry  8th Edition
ISBN: 9780716787594
Solutions for Chapter 11: Molecular structure
Get Full SolutionsPhysical Chemistry was written by and is associated to the ISBN: 9780716787594. This expansive textbook survival guide covers the following chapters and their solutions. This textbook survival guide was created for the textbook: Physical Chemistry , edition: 8. Since 55 problems in chapter 11: Molecular structure have been answered, more than 57148 students have viewed full stepbystep solutions from this chapter. Chapter 11: Molecular structure includes 55 full stepbystep solutions.

alkaline earth metals
Members of group 2A in the periodic table. (Section 7.7)

Betaine
A neutral molecule with nonadjacent positive and negative charges. An example of a betaine is the intermediate formed by addition of a Wittig reagent to an aldehyde or ketone

Dispersion forces
Very weak intermolecular forces of attraction resulting from the interaction between temporary induced dipoles

displacement reaction
A reaction in which an element reacts with a compound, displacing an element from it. (Section 4.4)

Eclipsed conformation
A conformation about a carboncarbon single bond in which the atoms or groups on one carbon are as close as possible to the atoms or groups on an adjacent carbon.

Gibbs free energy (G)
The ultimate arbiter of the spontaneity of a reaction, where DG = DH  T DS.

Ground state
The lowest energy state of a system.

heterocycle
A cyclic compound containing at least one heteroatom (such as S, N, or O) in the ring.

hydrogen abstraction
In radical reactions, a type of arrowpushing pattern in which a hydrogen atom is abstracted by a radical, generating a new radical.

induction
The withdrawal of electron density that occurs when a bond is shared by two atoms of differing electronegativity.

Lactam
A cyclic amide.

nucleophile
A compound containing an electronrich atom that is capable of donating a pair of electrons.

Oligosaccharide
A carbohydrate containing four to ten monosaccharide units, each joined to the next by a glycosidic bond.

Polyunsaturated triglyceride
A triglyceride having several carboncarbon double bonds in the hydrocarbon chains of its three fatty acids.

Prostaglandin
A member of the family of compounds having the 20carbon skeleton of prostanoic acid

radial probability function
The probability that the electron will be found at a certain distance from the nucleus. (Section 6.6)

reaction order
The power to which the concentration of a reactant is raised in a rate law. (Section 14.3)

solvent
The dissolving medium of a solution; it is normally the component of a solution present in the greater amount. (Section 4.1)

standard atomic weight
The weighted averages for each element, which takes into account isotopic abundance.

Stork enamine synthesis
A Michaelreaction in which an enamine functions as anucleophile.