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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.

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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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

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.

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

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

2. What is the electron configuration for O2* ion? Show the energy level diagram and label all molecular orbitals. What is the bond order?

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

For a homonuclear diatomic molecule, what type of molecular orbital does the illustration shown below represent? Note: the represents each nuclei. a bonding o orbital formed from two p atomic orbitals. a bonding o orbital formed from two s atomic orbitals. a bonding o orbital formed from one p and one s atomic orbital. a bonding n orbital formed from one s and one p atomic orbital. a bonding n orbital formed from two p atomic orbitals.

The next two questions investigate how Molecular Orbital Theory and Lewis Theory view carbon monoxide. —. Draw a molecular orbital energy diagram (showing all of the bonding and antibonding molecular orbitals and their respective energies) for CO. Use the Molecular Orbital energy levels for B2 , C2 and N 2 for the CO molecule. —. Calculate the bond order for CO from the molecular orbital energy diagram. —. Is CO paramagnetic or diamagnetic? ------------- b. Draw the Lewis structure for CO. —. Calculate the formal charge on each atom in CO. —. Draw the dipole for CO. —. Calculate the oxidation numbers for the carbon and oxygen atoms in CO. —. Formal charges, dipoles, and oxidation numbers are different ways of understanding the charges on covalently-bonded atoms. They tend to agree or be similar. At least in some ways, they disagree for CO. Formal charge guidelines assume that all bonding electrons are shared evenly between the two bonded atoms. Oxidation number guidelines assume that…

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 C₂ Ne ₂ stable? O yes O no yes O no O yes O no 1 H 0 0 diamagnetic or paramagnetic? O diamagnetic paramagnetic diamagnetic paramagnetic O diamagnetic O paramagnetic bond order 2 X