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4. Tetrachloroethene (CCI2=CCI2) does not have a dipole moment. Explain this fact on the basis of the shape of CCI2=CCI2.

Draw the molecular orbital diagram shown to determine which of the following is most stable. B2, N2^2+, C2^2-, B2^2+, C2^2+

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).

a) Identify atomic orbital #1 and #2. Indicate the number of radial and angular nodes for both b) What type of molecular orbital (σ, π, or no interaction) will be formed when these orbitals approach each other along the x axis? Describe the orbital overlap if applicable. Assume that the atomic orbitals are at appropriate energy levels to mix.

Using the following atomic orbital pictures and radial probability distribution plots: a) Identify atomic orbital #1. Indicate the number of radial and angular nodes. b) Identify atomic orbital #2. Indicate the number of radial and angular nodes. c) What type of molecular orbital (o, T, or no interaction) will be formed when these orbitals approach each other along the x axis? Describe the orbital overlap if applicable. Assume that the atomic orbitals are at appropriate energy levels to mix Atomic Orbital #1 PR 007 0.06 05 004 03 0.02 0.01 10 20 30 r (ao) Atomic Orbital #2 R 012 0.06 04 02 10 15 20 25 r (ao) JSmol

I need the Hybridization, Overlapping orbitals, and Molecular geometry.

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Shown below is the molecular orbital diagram for N2 (with the electrons omitted). Which statement is not correct about N2*? +++ +++ 2p 2p 2s 2s N2 N

The research group has recently focused on identifying the chemical properties of fluorocarbons, such as CF4 and C2F4. These fluorocarbons display a very different reactivity compared to hydrocarbons. Draw the molecular orbital theory diagrams for C-F and C-H bonds. Describe the difference between the C-F and C-H bond.

9) HCCCO₂H, is an organic hydrocarbon. a) Draw a geometrically accurate structure so that the formal charge of each atom is zero identifying the bond angles (Draw it BIG!). b) Identify the hybridization about each atom (not H) forming a bond c) How many o or π bonds are there in this molecule d) The combustion of the hydrocarbon produces carbon dioxide and water in the gaseous state. Use average bond enthalpies to determine enthalpy of reaction

A Moving to another question will save this response. Question 1 Which is the correct molecular orbital diagram for O 2 ion? Oo 2s 1lo 2s t 1 T2p 1 1.t102p tI 2p t o 2s 1ļo 2s 11 m2p 1102p 1 1 72p tt t o 2s 1lo 2s 11 T|2p 1 1. t102p t 2p t1 o 2s 1ļo 2s 1 2p ↑ 1. t L. t I o2p ↑ 1 12p t O o 2s 1io 2s t I 12p ↑ 1 02p ↑ 1 12p t 1.t A Moving to another question will save this response.

Nitric oxide (NO) is an important signaling molecule in biological systems. Two ions based on NO are also known: the nitrosonium cation (NO*) and the nitroxyl anion (NO). Construct the molecular orbital diagram for NO (Note: s-p mixing is significant in NO). To the side, sketch the combinations of AOs that contribute to each MO. b. Explain how your diagram illustrates the difference in electronegativity between N and O. Predict the bond order and number of unpaired electrons in NO. d. Predict the bond order and number of unpaired electrons in the ions NO* and NO". Which of the three species would you predict to have the shortest bond? Explain why. а. С.

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 + N 2 H₂ N₂ stable? O yes O no O yes no yes no diamagnetic or paramagnetic? diamagnetic O paramagnetic diamagnetic paramagnetic diamagnetic paramagnetic OLO OO bond order 0 0 0 00 X

Find the hybrid orbital type for each atom, the carbon-carbon-oxygen bond angle, the molecular geometry of oxygen, and the number of sigma and pi bonds in the molecule.

Help with this please. Use the Molecular Orbital Theory to indicate the bond order, and paramagnetism or diamagnetism of O2, O2+, and O2-.

I wanna help to answer this questions Thanks a lot

Molecule C2H2 SFs- NO3- Lewis structure include lone pairs & formal charges on each atom Resonance structures don't have to include lone pairs; write N/A if there are none Electron Geometry Hybridization on central atom Overlapping orbitals O: O: include value of n in the orbital name (e.g. 1s, not s). Write N/A if that kind T: of bond is not present in T: the molecule Molecular Geometry Bond angle(s) include < as necessary 3D structure and polarity don't have to include lone pairs; draw the dipole arrow on the molecule or write "non- polar"

5.Examine the model and real structures for XeF2. A.What is unusual about the chemical identity of the central atom in this molecule? B.Is this molecule polar or non-polar, explain how you arrived at your decision?

2. Use the molecular orbital diagram shown to find the bond magnetism, and stability of the following. Indicate which is stable. 2+ C₂²+ 2+ N₂²+ B₁₂ C, 2- B₂2+ Bond Order para- or diamagnetic? Atomic orbitals 2p 2s Molecular orbitals $ P2p 52p P2P 524 B2, C₂, N₂ Atomic orbitals 2p order, most