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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.

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

B. Answer the next two questions about the Lewis structure of XYZ shown below. メー三 -YEz: I. What is the hybridization of the central atom? II. For all covalent bonds, specify the type of bond (o vs. T) and the atomic orbitals that overlap to form the bond. For example, in a molecule of H2, the only bond is o: H(s)-H(s).

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?

Part 1) Select the correct description of the hybrid orbitals that are involved in the sigma bond between C2 and C3 in the structure. choose from answers A through E. Part 2) How many total sigma bonds exist in this structure? Choose from answers F through 1. Part 3) How many total pi bonds exist in this structure? Choose from answers J through M. Cl H C=C=C 2 3 H Cl

What are the angles a and b in the actual molecule of which this is a Lewis structure? H- H a-0° b = 1⁰ C H a b H Note for advanced students: give the ideal angles, and don't worry about small differences from the ideal that might be caused by the fact that different electron groups may have slightly different sizes. X S

What is the atomic orbital and molecular orbital energy diagram for Li2+?

Construct the molecular orbital diagram for SrCl. Would yo u expect the bond length of SrCl+ to be longer or shorter than that of SrCl? Explain and elaborate.

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 B 2 C₂ H₂ stable? O оо yes no yes no yes no diamagnetic or paramagnetic? diamagnetic paramagnetic diamagnetic paramagnetic diamagnetic O paramagnetic bond order 0 0 0 00

2) a) Consider the following molecule . Given what you have learned about hybridization theory, draw an image or images explaining the bonding situation in this molecule. I want you to draw out all of the orbitals, hybrid orbitals and how they overlap to form the bonds in the molecule. Indicate the % s or p character in the given atomic and hybrid orbitals. Which C-C bond or bonds are the longest? In a paragraph or so explain the image or images you just drew. b) Lastly, consider the molecule below. Indicate the Molecular formula, the molar mass, label the hybridization of each atom except for hydrogen, indicate any chiral centers with a *, which bond or bonds are the shortest, identify by name of each functional group with an arrow pointing to the group.

1.) Use the VSEPR model to determine the three-dimensional shapes ofcarbon tetraiodide, CI4, and phosphine, PH3.  Circle the correct answer! Choose only 1. CI4:  Linear trigonal planar      bent tetrahedral trigonal pyramidal trigonal bipyramidal seesaw T-shaped Octahedral square pyramidal square planar Circle the correct answer! Choose only 1. PH3:  Linear trigonal planar      bent tetrahedral trigonal pyramidal trigonal bipyramidal seesaw T-shaped Octahedral square pyramidal square planar   2.) Identify the polarity of carbon dioxide (CO2) and water (H2O) based upon its geometry and the dipole moments of the individual bonds. Circle the correct answer! Choose only 1. carbon dioxide: Polar nonpolar         Circle the correct answer! Choose only 1.water: polar nonpolar