How do I fill this out? 1s☐1s8. Would the molecule Li₂+ or Li₂ be likely toexist? Explain.LiMOLiatomLizatom9. Label the MOs drawn below and fill in the electrons. Please note that only MOs for valenceelectrons are shown.N₂N₂+Ne₂Ne22410. Give the bond order for each molecule in e). Which is the least stable (least likely to exist)?

8) Both Li2^2+ and Li2^2- would be unlikely to exist in stable forms under normal conditions.Li2^2+…

Answered: 1s ☐ 1s 8. Would the molecule Li₂+ or…

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter1: Bond Angles And Shape

Section: Chapter Questions

Problem 8CTQ: You hear a student from a nearby group say that “Electron domains repel one another.” Citeevidence...

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Similar questions

You hear a student from a nearby group say that “Electron domains repel one another.” Citeevidence from Figure 1.2 to support or refute this statement.
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.
1. The sigma bond between the Br and F atom in BrF4- is formed from the overlap of which two orbitals?a. 4sp3d-2sb. 4sp3d-2pc. 4sp3d2-2sd.4sp3d2-2p2. Consider the following species F2-, F2, and F2+. Which of these species will be paramagnetic? 3. Which of the following exhibits resonance?a. ClO3-b. BrF3c. OF2d. N2
— Use molecular orbital energy diagrams to determine which of the following is most stable (has highest bond order). (A) C22+ (B). N22+ (C). B2 (D). C22– (E). B22+ —Consider the molecule CH2CF2. A. Draw the best Lewis structure for this molecule. B. Label each bond angle. C. Redraw the shape of the molecule (according to the exacting specifications of your instructor). Draw all dipoles. D. Is the overall molecule polar?
1. lewis structure of Cesium 2-hydroxyacetate, HOCH2CO2Cs 2. assign the VSEPR model of the central atom3. Value of the corresponding theoretical angle4. classify 3 of the different bonds around the central atom as ionic or covalent5. draw the complete 3-D structure with respect to the central atom (s)6. draw the lewis structure for another mnolecule or species with a different atomic arrangement
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. molecule Li₂ + 2 0₂ stable? yes no yes no O yes no diamagnetic or paramagnetic? diamagnetic paramagnetic diamagnetic paramagnetic diamagnetic paramagnetic bond order 0 0 0 00
a) Which orbital is HOMO (Highest occupied)? b) Which orbital is LUMO (lowest unoccupied)? What do those MO look like? c) Paramagentic or diamagnetic d) What is the bond order - Will adding electrons increase or decrease the bond order? 2) Complete the MO for CO2+ 11 2p 1V. 2s 16 TC TV 11 T 1V 72 O 1114 2p 16 2s
1. ionization of Cl2 (Cl2 —> Cl2+ + e-) leads to a shortening of the Cl-Cl distance (199 pm in Cl2, 189 pm in Cl2+), why? 2. why the C-O bond distance is nearly identical in CO (113 pm) and CO+ (112 pm)? 3. Derive the MO diagram of a linear C-H (i.e. one carbon atom bonded to one hydrogen atom). Draw out the MOs for orbitals containing electrons Would you expect C-H to behave as a carbocation, carbanion, or radical? Would removal of one electron from C-H to generate C-H+ increase or decrease the bond length between carbon and hydrogen?
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. ? 000 molecule stable? 2- ○ yes Be2 H₂ no yes no yes no diamagnetic or paramagnetic? diamagnetic paramagnetic O diamagnetic paramagnetic ○ diamagnetic O paramagnetic bond order ☐ Π ㅁㅁ ✗ Ar
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. molecule + Li₂ 0₂ 2 B 2 stable? O yes O O no O yes no O yes O no diamagnetic or paramagnetic? diamagnetic paramagnetic diamagnetic paramagnetic O diamagnetic paramagnetic bond order 0 1 1 00 X S
Using the molecular orbital model, write electron configurations for the 6 points following diatomic species and calculate the bond order. Which ones are paramagnetic? place the species in order of increasing bond energy. ( CO , Co+, CO+2). Assignment questions.
A. Which of the following statements is TRUE about the neutral nitrogen molecule, N2? Select one: . It is paramagnetic. . Its N–N bond length is shorter than that in the cationic nitrogen molecule ion. . Its calculated bond order is 2. . Its molecular orbital diagram shows that each nitrogen atom has two lone pairs. B. What is the correct complete molecular orbital notation for the N2 molecule? Select one: . σ1s² σ*1s² π2p⁴ σ*2p² . σ2s² σ*2s² π2p⁴ σ*2p² . σ1s² σ*1s² σ2s² σ*2s² π2p⁴ σ2p² . σ1s² σ*1s² σ2s² σ*2s² σ*2p² π2p⁴

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