4. How many unpaired electrons doe the cation B† have? What's the bond order of the diatomiccation B2*? 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?

To solve these problems, we have first draw Molecular orbital of that molecule.

Answered: 4. How many unpaired electrons doe the…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter6: Quantum Mechanics And Molecular Structure

Section: Chapter Questions

Problem 17P

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Similar questions

What are the relationships among bond order, bond energy, and bond length? Which of these quantities can be measured?
In each of the following molecules, a central atom is surrounded by a total of three atoms or unshared electron pairs: SnCl2, BCl3, SO2. In which of these molecules would you expect the bond angle to be less than 120? Explain your reasoning.
Which of the following statements is/are true? Correct the false statements. a. The molecules SeS3. SeS2, PCl5, TeCl4, ICl3, and XeCl2 all exhibit at least one bond angle which is approximately 120. b. The bond angle in SO2 should be similar to the bond angle in CS2 or SCI2. c. Of the compounds CF4, KrF4, and SeF4, only SeF4 exhibits an overall dipole moment (is polar). d. Central atoms in a molecule adopt a geometry of the bonded atoms and lone pairs about the central atom in order to maximize electron repulsions.
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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.
The diatomic molecule OH exists in the gas phase. The bond length and bond energy have been measured to be 97.06 pm and 424.7 kJ/mol, respectively. Assume that the OH molecule is analogous to the HF molecule discussed in the chapter and that molecular orbitals result from the overlap of a lowerenergy pz, orbital from oxygen with the higher-energy ls orbital of hydrogen (the OH bond lies along the z-axis). a. Which of the two molecular orbitals will have the greater hydrogen 1s character? b. Can the 2px orbital of oxygen form molecular orbitals with the 1s orbital of hydrogen? Explain. c. Knowing that only the 2p orbitals of oxygen will interact significantly with the 1s orbital of hydrogen, complete the molecular orbital energy-level diagram for OH. Place the correct number of electrons in the energy levels. d. Estimate the bond order for OH. e. Predict whether the bond order of OH+ will be greater than, less than, or the same as that of OH. Explain.
4. How many unpaired electrons doe the cation B† have? What's the bond order of the diatomic cation B2*? Is B2* a stable species? Is it paramagnetic or diamagnetic?
4. How many unpaired electrons doe the cation B have? What's the bond order of the diatomic cation 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 or diamagnetic?
4. 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?
Complete 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? 믐 molecule stable? bond order yes O diamagnetic A N2 X. O no paramagnetic yes diamagnetic F paramagnetic yes O'diamagnetic Be, O no paramagnetic O O O
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? O unpaired electron; bond order 1/2; stable; paramagnetic 1 unpaired electron; bond order 1/2; stable; paramagnetic 2 unpaired electrons; bond order 1; stable; diamagnetic 2 unpaired electrons; bond order 1; stable; paramagnetic
How many unpaired electrons doe the molecule Liz have? What's the bond order of the diatomic molecule Li2? Is Liz a stable species? Is it paramagnetic or diamagnetic? 2 unpaired electrons; bond order 1; stable; paramagnetic O 2 unpaired electrons; bond order 1; stable; diamagnetic O unpaired electrons; bond order 1; stable; paramagnetic O unpaired electrons; bond order 1; stable; diamagnetic

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4. How many unpaired electrons doe the cation Bt 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 Liz? Is it a stable diatomic molecule? Is it paramagnetic or diamagnetic?

4. How many unpaired electrons doe the cation Bt 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 Liz? Is it a stable diatomic molecule? Is it paramagnetic or diamagnetic?