6 3 9 4 2 4 4 5 く 6 V く p orbital sp³ orbital двов a second sp³ orbital S& No bond 3. 3 4. 4 5. Orbital Picture 6. Unused Answer 2 < sp2 orbital

Considering a homonuclear diatomic 2 pis molecule, the parity label "gerade" (or "g") indicates that there is a change in sign of the orbitals when passing through the center of the molecule. * O True O False

SO₂ molecule S Cau z - Determine the projection for the oxygen Px. Orbitals C2U E Ca ov(x2) ou (x2) PA Y b) Determine the a₂ & b, SALC's and the Shape of their LGO's. pz group orbitals for SO3 will reduce to pz = A₂ + B₁ X Oxygen pz group orbitals

An energy level scheme for the orbitals of second row diatomic molecules O, through Ne2 , lists the molecular orbitals in the following order of increasing energy 02 < o'2s < Ozp(z) < T2p(y)- 7T2P(x) < T*2p(y), 7T* 2p(x) < o*2plz) Based on this energy level scheme, how many electrons are there in all of the antibonding molecular orbitals of the F2* ion in its ground state?

Construct the wavefunction of the π MO from the 2pz atomic orbitals perpendicular to the plane of the C atoms.  How many π MO result from the available 2pz A.O.?

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The sp2 orbitals of carbon in ethylene are formed from the H2C=CH2 OA. 2s and one of the 2p orbitals. OB. 2s and three 2p orbitals. OC. 2s and two of the 2p orbitals. O D. three 2p orbitals.

From your knowledge of molecular orbital diagrams, what is the correct set of relationships between the ionization energies of molecular hydrogen to that of atomic hydrogen, and molecular oxygen to that of atomic oxygen? IEĦ, ?IEH;IEo, ?IEo where [? =>, IEo O IEH, > IEH; IE0, IEH; IE0, > IEo O IEH, = IEH; IE0, = IEo

Antibonding molecular orbitals can be used to make bondsto other atoms in a molecule. For example, metal atomscan use appropriate d orbitals to overlap with the p*2p orbitalsof the carbon monoxide molecule. This is calledd@p backbonding. (a) Draw a coordinate axis system inwhich the y-axis is vertical in the plane of the paper andthe x-axis horizontal. Write “M” at the origin to denote ametal atom. (b) Now, on the x-axis to the right of M, drawthe Lewis structure of a CO molecule, with the carbonnearest the M. The CO bond axis should be on the x-axis.(c) Draw the CO p*2p orbital, with phases (see the “CloserLook” box on phases) in the plane of the paper. Two lobesshould be pointing toward M. (d) Now draw the dxy orbitalof M, with phases. Can you see how they will overlap withthe p*2p orbital of CO? (e) What kind of bond is being madewith the orbitals between M and C, s or p ? (f) Predict whatwill happen to the strength of the CO bond in a metal–COcomplex compared to CO alone.

Consider the ring cation, called "cyclopentadienyl cation".... one of five possible resonance structures that can be drawn for it is shown below. In the actual ring cation, what is the charge on any one carbon atom, and what is the bond order of any one C,C bond? ? charge on one C = ? bond order of C,C bond = Select one: O A. +2/5; 4/3 OB. + 1/6; 1.5 O C. + 2/5; 7/5 O D. + 1/5; 6/5 O E. + 1/5; 7/5