Homework Answers
Q)
A)
a)
b)
There is 12 valance electrons are there .6 from one oxygen and more 6 from another oxygen.
c)
πpy and πpz
orbitals are the degenarate orbitals along with this 
Degenarate orbitals means the orbitals that contain same energy levels..Where as the energy of an orbital is depends on the size and shape .
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7. For molecular oxygen, (a) Define (sketch) your reference system and sketch a * MO. What...
8. For molecular fluorine, F2 (a) Define (sketch) your reference system and sketch the highest occupied...
8. For molecular fluorine, F2 (a) Define (sketch) your reference system and sketch the highest occupied O-MO. What is the number of nodes in this MO? F. F. (b) Name the valence orbitals contributing to the MO you sketched above. (c) What is the number of occupied antibonding molecular orbitals in F2? Are any of these orbitals degenerate?
9. For molecular nitrogen, (a) Sketch the LUMO of N2. Define (sketch) your reference system and...
9. For molecular nitrogen, (a) Sketch the LUMO of N2. Define (sketch) your reference system and name the p orbitals contributing to the MO of your sketch Ν Ν. (b) Name the p orbitals contributing to the HOMO of N2. (c) What is the total number of antibonding orbitals in N2?
5. Consider valence orbitals of oxygen and those of a transition metal M from Period 4. (a) Complete the reference syst...
5. Consider valence orbitals of oxygen and those of a transition metal M from Period 4. (a) Complete the reference system and name the d orbital of M and the orbital of 0 overlapped in the T-bond. M= O (b) Sketch the orbitals you named in 5(a), overlapped in the T-bond. Also, sketch the complete reference system. (c) What is the total number of nodal surfaces in the molecular orbital of your sketch?
4. Consider valence orbitals of oxygen and those of a transition metal M from Period 4....
4. Consider valence orbitals of oxygen and those of a transition metal M from Period 4. (a) Complete the reference system and name the d orbital of M and the p orbital of O overlapping in the o-bond. M= O (b) Sketch the orbitals you named in 4(a), overlapped in the o-bond. Also, sketch the complete reference system. (c) What is the total number of nodal surfaces in the molecular orbital of your sketch?
Write the term symbol for the the ground state of NO and sketch out a molecular...
Write the term symbol for the the ground state of NO and sketch out a molecular orbital energy diagram for NO and place the electrons in the levels appropriate for the ground state. You will need to look up the AO ionization energies for O2s, O2p, N2s, and N2p. The MO energies follow the sequence (from lowest to highest) 1σg, 1σu, 2σg, 2σu, 3σg, 1πu, 1πg, 3σu,. Define the 1σ orbitals as originating primarily from the 1s AOs on N...
4. Consider the atomic orbitals of oxygen and a d-metal M. (a) Complete the reference system...
4. Consider the atomic orbitals of oxygen and a d-metal M. (a) Complete the reference system and name the d orbital of M and the 2p orbital of O overlapping in the o-bond Az M= O (b) Sketch the two overlapping orbitals. (c) What is the total number of nodal surfaces in the overlapping orbitals of your sketch?
13. (14 pts) MO Theory Draw the complete (core and valence) molecular orbital energy level diagram...
13. (14 pts) MO Theory Draw the complete (core and valence) molecular orbital energy level diagram for the homonuclear diatomic molecule Be2. Use standard MO symbols to label the energy levels (That is: o, o, , or n*, as needed, with subscripts indicating which atomic orbitals formed them.) a. Sketch the molecular orbital formed when two 2p orbitals, one each on each Be atom, overlap to form a o antibonding MO b. Using your MO energy level diagram in (a),...
4. On the basis of molecular orbitals and molecular orbital diagrams, predict which molecule in each...
4. On the basis of molecular orbitals and molecular orbital diagrams, predict which molecule in each series will have the longest bond. Be sure to provide a brief explanation a. B2, B2 b. 02*, 0,- c. HHe", Hz 5. Consider the hydroxide ion, OH and do the following: a. Prepare a molecular orbital diagram and fill with electrons given the following atomic orbital potential energies: O(2s) = -32.3 eV, O(2p) = -15.8 eV, H(s) -13.6 eV. Be sure to label...
What is the bond order in O2+
5. What is the bond order in O2+? _______ 6. Draw the molecular orbital diagram for B2. The number of unpaired electrons in the B2 molecule is _______ 7. Which one of the following statements is false? (a) Valence bond theory and molecular orbital theory can be described as two different views of the same thing. (b) When one considers the molecular orbitals resulting from the overlap of any two specific atomic orbitals, the bonding orbitals are always lower in energy than the antibonding orbitals. (c)...
3. The MO diagram below is that of only the n-electron system of the molecule CH2O....
3. The MO diagram below is that of only the n-electron system of the molecule CH2O. The ncc bonding molecular orbital (which has two bonding electrons) shows oxygen bearing more electron density than carbon in the π bond, would you expect the carbonatorn in CH2Oto havemore orless partial positive charge compared to ethene, CH4? Please briefly explain your reasoning (antibonding) 0 0 t (bonding) ช้
8. For molecular fluorine, F2 (a) Define (sketch) your reference system and sketch the highest occupied O-MO. What is the number of nodes in this MO? F. F. (b) Name the valence orbitals contributing to the MO you sketched above. (c) What is the number of occupied antibonding molecular orbitals in F2? Are any of these orbitals degenerate?
9. For molecular nitrogen, (a) Sketch the LUMO of N2. Define (sketch) your reference system and name the p orbitals contributing to the MO of your sketch Ν Ν. (b) Name the p orbitals contributing to the HOMO of N2. (c) What is the total number of antibonding orbitals in N2?
5. Consider valence orbitals of oxygen and those of a transition metal M from Period 4. (a) Complete the reference system and name the d orbital of M and the orbital of 0 overlapped in the T-bond. M= O (b) Sketch the orbitals you named in 5(a), overlapped in the T-bond. Also, sketch the complete reference system. (c) What is the total number of nodal surfaces in the molecular orbital of your sketch?
4. Consider valence orbitals of oxygen and those of a transition metal M from Period 4. (a) Complete the reference system and name the d orbital of M and the p orbital of O overlapping in the o-bond. M= O (b) Sketch the orbitals you named in 4(a), overlapped in the o-bond. Also, sketch the complete reference system. (c) What is the total number of nodal surfaces in the molecular orbital of your sketch?
4. Consider the atomic orbitals of oxygen and a d-metal M. (a) Complete the reference system and name the d orbital of M and the 2p orbital of O overlapping in the o-bond Az M= O (b) Sketch the two overlapping orbitals. (c) What is the total number of nodal surfaces in the overlapping orbitals of your sketch?
13. (14 pts) MO Theory Draw the complete (core and valence) molecular orbital energy level diagram for the homonuclear diatomic molecule Be2. Use standard MO symbols to label the energy levels (That is: o, o, , or n*, as needed, with subscripts indicating which atomic orbitals formed them.) a. Sketch the molecular orbital formed when two 2p orbitals, one each on each Be atom, overlap to form a o antibonding MO b. Using your MO energy level diagram in (a),...
4. On the basis of molecular orbitals and molecular orbital diagrams, predict which molecule in each series will have the longest bond. Be sure to provide a brief explanation a. B2, B2 b. 02*, 0,- c. HHe", Hz 5. Consider the hydroxide ion, OH and do the following: a. Prepare a molecular orbital diagram and fill with electrons given the following atomic orbital potential energies: O(2s) = -32.3 eV, O(2p) = -15.8 eV, H(s) -13.6 eV. Be sure to label...
3. The MO diagram below is that of only the n-electron system of the molecule CH2O. The ncc bonding molecular orbital (which has two bonding electrons) shows oxygen bearing more electron density than carbon in the π bond, would you expect the carbonatorn in CH2Oto havemore orless partial positive charge compared to ethene, CH4? Please briefly explain your reasoning (antibonding) 0 0 t (bonding) ช้
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