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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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.
— 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. 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
Molecular Orbital Diagrams and Bond Order The blank molecular orbital diagram shown here (Figure 1) applies to the valence of diatomic lithium, beryllium, boron, carbon, or nitrogen. Bonding orbitals are marked with or π and antibonding orbitals with o* or *. Figure 2p CV 2p 1 of 1 What is the bond order of C₂? Express the bond order numerically. ▾ View Available Hint(s) ▶ ▶ Hint 2. Determine the number of valence electrons in C₂ ▸ Hint 3. Determine the number of bonding electrons Hint 4. Determine the number of antibonding electrons ▶ Hint 1. How to approach the problem 2 VE ΑΣΦ ↑ Submit B ? Previous Answers Request Answer * Incorrect; Try Again; 3 attempts remaining Check that you have filled the diagram correctly. Then double-check the numbers of bonding and antibonding electrons. You may want to review Hint 2. Determine the number of valence electrons in C₂_ Review | Ca
Using the molecular orbital model, identify the correct (valence) electron configurations for the following diatomic species. See attached image!! F2CN+ N2
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
Suppose that the following MO-energy-level diagram applies to the the diatomic molecular cation BO+. (See attched image!) Does this diagram display the effect of s-p orbital mixing? YES or NO? Which kind of magnetism would be observed for this cation? paramagnetism or diamagnetism What is the bond order for this cation?
I. Draw the molecular orbital diagram for the valence electrons in the generic, diatomic ion X22+. Each neutral atom of X contains 5 valence electrons. Use the "reversed" energy ordering (for B2, C2, N2) where o2p is higher in energy than n2p. The diagram has been started for you below. Label all molecular orbitals. Energy 2p 2p 2s 2s X atom Molecule X atom II. Calculate the bond order of X2*. III. How would the bond length and bond strength of X22+ compare with neutral X2? Briefly explain why (in about 1 sentence).
None
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.
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
Use the molecular orbital model to fully describe the bonding in 02+, 02, 02, and 022. Determine which of the following statements are true and which are false. The electron configuration of 02+ is (0 25)²(025*)?(02p)²(n2p)*(n2p*)?. O The bond lengths increase in the order: 022- < 02° < 02 < 02+. 2s. The bond order in 02+ and O2 is, respectively, 1.5 and 2. The electron configuration of O2 is (025)²(02s*)²(02p)?(n2p)^(n2p*)*. O Bond length increases with increasing bond order while bond energy decreases. The number of unpaired electrons in O2+ and O22 is, respectively, 1 and 2.

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