EBK CHEMISTRY
9th Edition
ISBN: 9780100453807
Author: ZUMDAHL
Publisher: YUZU
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Textbook Question
Chapter 9, Problem 94CP
Use the MO model to explain the bonding in BeH2. When constructing the MO energy-level diagram, assume that the Be’s 1s electrons are not involved in bond formation.
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Chapter 9 Solutions
EBK CHEMISTRY
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- It is possible to write a simple Lewis structure for the SO42- ion, involving only single bonds, which follows the octet rule. However, Linus Pauling and others have suggested an alternative structure, involving double bonds, in which the sulfur atom is surrounded by six electron pairs. (a) Draw the two Lewis structures. (b) What geometries are predicted for the two structures? (c) What is the hybridization of sulfur in each case? (d) What are the formal charges of the atoms in the two structures?arrow_forwardCould the anion Li2 exist? What is the ions bond order?arrow_forwardUsing hybridization and the long method for determining the Lewis Structures, show the most feasible representation of the following compounds: AsCl4+ OClF4- (Cl is the central atom) O3BrF (Br is the central atom)arrow_forward
- The average bond energy (enthalpy) for a C=C double bond is 614 kJ/molkJ/mol and that of a C−C single bond is 348 kJ/molkJ/mol. If it takes 4.42×10−19 J/molecule to break the C=C double bond. What is the longest wavelength λ of light that will provide photons of sufficient energy to break the π bond and cause the isomerization? Express your answer numerically in nanometers.arrow_forwardThe Bond energy of C2(g) is 599 kJ/mol and for F2 is 154 kJ/mol. Use MO theory to justify the difference.arrow_forward2p 2p 2s 2s Given the above MO orbital diagram for N2, indicate number of electrons in the bonding МО, anti-bonding MO. What is bond order? Is it paramagnetic or diamagnetic ENERGYarrow_forward
- Determine the electron geometry (EG) and molecular geometry (MG) of XeF2.arrow_forwardComplete the table below, which lists information about some diatomic molecules or molecular ions. In particular: • Decide whether each molecule is stable or not. • Decide whether each molecule would be diamagnetic or paramagnetic. • Calculate each molecule's bond order. diamagnetic or paramagnetic? molecule stable? bond order O yes O diamagnetic O no O paramagnetic yes O diamagnetic Li, O no O paramagnetic yes O diamagnetic Ne, O no O paramagnetic olo 이0 이0 이arrow_forwardSkethch the molecular orbital diagrams for B2 and F2. The provide the bond order for each molecule, whether they are diamagnetic or paramagnetic, the effect on the bond order and magnetic properties when each molecule is reduced by 1 electron, and the effect on the bond order and magnetic properties when each molecule is reduced by 2 electrons.arrow_forward
- When is a resonance hybrid needed to adequately depict the bonding in a molecule? Using NO2 as an example, explain how a resonance hybrid is consistent with the actual bond length, bond strength, and bond order.arrow_forwardWhat is the valence bond description for H2O, HNNH, and ClF3?arrow_forwardUse the molecular orbital model to fully describe the bonding in O2+, O2, O2-, and O22-.Determine which of the following statements are true and which are false. True or false? : Bond length increases with increasing bond order while bond energy decreases.The number of unpaired electrons in O2- and O2 is, respectively, 1 and 2. The electron configuration of O2 is (σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)1. The electron configuration of O2- is (σ2s)2(σ2s*)2(σ2p)2(π2p)4(π2p*)3. The bond order in O2- and O22- is, respectively, 2.5 and 1. The bond lengths increase in the order: O22- < O2- < O2 < O2+.arrow_forward
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