Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Textbook Question
Chapter 9, Problem 104CP
Given that the ionization energy of F2− is 290 kJ/mol, do the following:
a. Calculate the bond energy of F2−. You will need to look up the bond energy of F2 and ionization energy of F−.
b. Explain the difference in bond energy between F2− and F2 using MO theory.
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Chapter 9 Solutions
Chemistry
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
On the left side of Figure 3.6, label the areas shown with a dotted line where... one bond can form. one bond can form.
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Consider the following flat drawing of methane (CH4) . a. What is HCH bond angle implied by this drawing if you assume it is flat? b. Are the electron domains of this flat CH4 spread out as much as possible? c. Use model materials to make a model of CH4 (methane). If you assembled it correctly, thefour bonds (bonding electron domains) of your model will be 109.5° apart. d. In which representation, the drawing above or the model in your hand (circle one) are theH’s of CH4 more spread out around the central carbon? e. Confirm that your model looks like the following drawing. The wedgebond represents a bond coming out of the page, and the dash bondrepresents a bond going into the page f. You will often see methane drawn as if it were flat (like on the previous page). Why is thismisleading, and what is left to the viewer’s imagination when looking at such a drawing?
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Identify the molecules with a dipole moment: (a) SF4 (b) CF4 (c) Cl2CCBr2 (d) CH3Cl (e) H2CO
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Draw the two resonance structures that describe the bonding in SO2. Then describe the bonding in this compound using MO theory. How does MO theory rationalize the bond order of 1.5 for the two SO bonds in this compound?
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When is it desirable to use MO theory rather than valence bond theory?
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When two amino acids react with each other, they form a linkage called an amide group, or a peptide link. (If more linkage. are added, a protein or polypeptide is formed.) (a) What are the hybridizations of the C and N atoms in the peptide linkage? (b) Is the structure illustrated the only resonance structure possible for the peptide linkage? If another resonance structure is possible. compare it with the o ne shown. Decide which is the more important structure. (c) The computer-generated structure shown here, which contains a peptide linkage, shows that this linkage is flat. This is an important feature of proteins. Speculate on reasons that the CONH linkage is planar. What are the sites of positive and negative charge in this dipeptide?
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2. Draw MO energy level diagrams for each of the following diatomic molecules are molecular ions. All contributing atomic orbitals and the resulting molecular orbitals must be labeled properly showing the electrons (as arrows) in the atomic orbitals and in the molecular orbitals. All orbitals should be drawn to show their relative energy relationships. Calculate the bond order for each and label each as either diamagnetic or paramagnetic.
(a) BO‒
(b) CN
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(d) Cl2‒
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can someone explain why this counts as fully conjugated? does the pos charge count as conjugation? I thought conjugation was sigma bond, pi bond, sigma bond, etc...
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Draw an MO energy diagram and predict the bond order of Be2 + and Be2- . Do you expect these molecules to exist in the gas phase?
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