General Chemistry: Atoms First
2nd Edition
ISBN: 9780321809261
Author: John E. McMurry, Robert C. Fay
Publisher: Prentice Hall
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Chapter 5.6, Problem 5.14P
The B2 and C2 molecules have MO diagrams similar to that of N2 in Figure 5.12a. What MOs are occupied in B2 and C2, and what is the bond order in each? Would you expect either of these substances to be paramagnetic?
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Chapter 5 Solutions
General Chemistry: Atoms First
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- The molecules N2 and CO are isoelectronic but their properties are quite different. Although as a first approximation we often use the same MO diagram for both, suggest how the MOs in N2 and CO might be different.arrow_forwardIn the molecular orbital mode l, compare and contrast bonds with bonds. What orbitals form the bonds and what orbitals form the bonds? Assume the z-axis is the internuclear axis.arrow_forwardWhich of the following molecules or ions are para-magnetic? What is the highest occupied molecular orbital (HOMO) in each one? Assume the molecular orbital diagram in Figure 9.16 applies to all of them. (a) NO (b) OF (c) O22 (d) Ne2+arrow_forward
- The compound sketched below is acetylsalicylic acid, commonly known as aspirin. (a) What are the approximate values of the angles marked A, B, C, and D? (b) What hybrid orbitals are used by carbon atoms 1, 2, and 3ss?arrow_forwardUse valence bond theory to explain the bonding in F2, HF, and CIBr. Sketch the overlap of the atomic orbitals involved in the bonds.arrow_forwardWhat type of molecular orbital would result from the in-phase combination of the two dxz atomic orbitals shown below? Assume the x-axis is the internuclear axis.arrow_forward
- 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?arrow_forwardFor CO draw and label its molecular orbital diagram and assume there are only small s-p interactions. 1. Is the molecule paramagnetic? Give an explanation. 2. What is the bond order for CO?arrow_forwardSketch the molecular orbital diagrams for B2 snd for F2. Using these diagrams, provide the bond order for each of the molecules and state if they are diamagnetic or paramagnetic. Describe the effect on the bond order and on the magnetic properties when B2 and F2 are reduced by 1 electron. Describe the effect on the bond order and on the magnetic properties when B2 and F2 are reduced by 2 electrons.arrow_forward
- Use molecular orbital theory, write a molecular orbital diagram, calculate bond order, and predict whether or not each ion exists in a relatively stable form, for the following two molecular ions for He2^2+arrow_forwardThe molecular orbitals depicted below are derived from 2p atomic orbitals in F₂⁺. (a) Give the orbital designations. (b) Which is occupied by at least one electron in F₂⁺? (c) Which is occupied by only one electron in F₂⁺?arrow_forwardUse MO diagrams and the bond orders you obtain fromthem to answer: (a) Is Be₂⁺ stable? (b) Is Be₂⁺ diamagnetic? (c) What is the outer (valence) electron configuration of Be₂⁺?arrow_forward
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