4. How many unpaired electrons doe the cation B have? What's the bond order of the diatomiccation Bz*? Is B2* a stable species? Is it paramagnetic or diamagnetic?5. What is the bonder order of Liz? Is it a stable diatomic molecule? Is it paramagnetic ordiamagnetic?

Two questions based on atomic structure, which is to be accomplished.

Answered: 4. How many unpaired electrons doe the…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter10: Molecular Structure And Bonding Theories

Section: Chapter Questions

Problem 10.97QE

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Similar questions

The molecular orbital diagram of NO shown in Figure 10.47 also applies to OF. Draw the complete molecular orbital diagram for OF. What is the OF bond order? Figure 10.47 Molecular orbital diagram for nitric oxide (NO). The molecular orbital diagram for NO predicts a bond order of 2.5 and predicts that the molecule is paramagnetic with one unpaired electron. These predictions are verified by experimental measurements.
Compare Figs. 4-47 and 4-49. Why are they different? Because B2 is known to be paramagnetic, the 2p and 2p molecular orbitals must be switched from the first prediction. What is the rationale for this? Why might one expect the 2p to be lower in energy than the 2p? Why cant we use diatomic oxygen to help us decide whether the 2p, or 2p, is lower in energy?
Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to explore real molecules. On the Real Molecules tab, select H2O. Switch between the real and model modes. Explain the difference observed.
The molecular orbital diagram of NO shown in Figure 10.47 also applies to the following species. Write the molecular orbital electron configuration of each, indicating the bond order and the number of unpaired electrons. (a) CN (b) CO (c) BeB (d) BC+ Figure 10.47 Molecular orbital diagram for nitric oxide (NO). The molecular orbital diagram for NO predicts a bond order of 2.5 and predicts that the molecule is paramagnetic with one unpaired electron. These predictions are verified by experimental measurements.
Why are d orbitals sometimes used to form hybrid orbitals? Which period of elements does not used orbitals for hybridization? If necessary, which d orbitals (3d, 4d, 5d, or 6d) would sulfur use to form hybrid orbitals requiring d atomic orbitals? Answer the same question for arsenic and for iodine.
How many unpaired electrons doe the cation have? What’s the bond order of the diatomic cation B2+? Is B2+ a stable species? Is it paramagnetic or diamagnetic? 5. What is the bonder order of Li2? Is it a stable diatomic molecule? Is it paramagnetic or diamagnetic?
2. What’s the bond order of the diatomic molecule Ne2? Is your result consistent with the fact that Ne is a monatomic molecule in nature? Explain. 3. How many unpaired electrons doe the ion have? Is your result consistent with the fact that is attracted by magnet? Explain
4, How many unpaired electrons doe the ion B2+have? What’s the bond order of the diatomic cation B2+? Is B2+ a stable species? Is it paramagnetic or diamagnetic? Group of answer choices A, 1 unpaired electron; bond order 1/2; stable; paramagnetic B, 0 unpaired electron; bond order 1/2; stable; paramagnetic C, 2 unpaired electrons; bond order 1; stable; paramagnetic D, 2 unpaired electrons; bond order 1; stable; diamagnetic How many unpaired electrons doe the molecule Li2 have? What’s the bond order of the diatomic molecule Li2? Is Li2 a stable species? Is it paramagnetic or diamagnetic? Group of answer choices A, 2 unpaired electrons; bond order 1; stable; diamagnetic B, 0 unpaired electrons; bond order 1; stable; diamagnetic C, 0 unpaired electrons; bond order 1; stable; paramagnetic D, 2 unpaired electrons; bond order 1; stable; paramagnetic
15. How many hybrid orbitals do we use to describe each molecule? Enter in integer form! -BrCN

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4. How many unpaired electrons doe the cation B* have? What's the bond order of the diatomic cation B2*? Is Bz* a stable species? Is it paramagnetic or diamagnetic? 5. What is the bonder order of Liz? Is it a stable diatomic molecule? Is it paramagnetic or diamagnetic?

4. How many unpaired electrons doe the cation B* have? What's the bond order of the diatomic cation B2? Is Bz a stable species? Is it paramagnetic or diamagnetic? 5. What is the bonder order of Liz? Is it a stable diatomic molecule? Is it paramagnetic or diamagnetic?