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Consider the H2 ion and respond to the following 2. (a) Sketch the highest occupied MO...
1. Consider the H2+ ion and respond to the following. (a) Sketch the occupied MO of...
1. Consider the H2+ ion and respond to the following. (a) Sketch the occupied MO of H2+. HH (b) Is this a -MO? If not, why? (c) What is the number of molecular orbitals in H2+?
1. Consider the H2* ion and respond to the following questions. (a) Sketch the unoccupied MO...
1. Consider the H2* ion and respond to the following questions. (a) Sketch the unoccupied MO of Hat and tell whether this orbital has a node. If yes, sketch (or describe) the surface. HH (b) How does the energy of the o-bonding MO of H2* compare to that of the 1s orbital of hydrogen? (c) Would you expect Hal to act as an oxidant or as a reducing agent toward the Halon in a chemical reaction? Briefly explain
3. Consider Heat and respond to the following. (a) Sketch the singly occupied MO of Hez*....
3. Consider Heat and respond to the following. (a) Sketch the singly occupied MO of Hez*. He He (b) Decide whether Heation should have a t-MO. Explain. (c) What should happen to Hez upon one-electron reduction? Explain.
10. The MO diagrams of NO and NO+ are similar (see Lecture 15 for the MO...
10. The MO diagrams of NO and NO+ are similar (see Lecture 15 for the MO diagram of NO+). On the basis of this consideration, respond to the following: (a) Sketch the singly-occupied MO of NO. Ν Ο (b) What is the total number of electrons in the anti-bonding MOs of NO? (c) Do the necessary calculations to decide when the NO bond should become stronger: when this compound undergoes one-electron reduction or oxidation? (d) Which atom in NO should...
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?
According to MO theory, which molecule or ion has the highest bond order? Highest bond energy?...
According to MO theory, which molecule or ion has the highest bond order? Highest bond energy? Shortest bond length? (a)O_2, O_2, O_^2- (b) CO and CO^+. (Use the energy ordering of O_2)
The H2 ion is more stable (higher bond order) than H2 since it has an additional...
The H2 ion is more stable (higher bond order) than H2 since it has an additional electron to produce a net lowering of energy. (consider MO theory to answer this.) False O True Question 2 Which best explains the following trend? Element b.p. (K) He 4 Ne 25 Ar 95 Kr 125 Xe 170 O dipole-dipole interaction hydrogen bonding O London dispersion forces O ion-dipole forces
3. MO th eorv for heteronuclear diato mic molecules-II XeF is a stable molecule. The highest...
3. MO th eorv for heteronuclear diato mic molecules-II XeF is a stable molecule. The highest atomic orbital energy of Xe and F atoms are given in the table below The highest MOs that can be constructed with these AOs has the energy order All the lower-lying MOs (coming from lower-lying AOs) are fully occupied. Sketch the highest MOs in the MO-diagram of XeF from the AOs given in the table. What is the bond order of XeF? (5 points)
1.)Construct an MO diagram for the He+2 ion. a.Determine if the He+2 ion is stable or...
1.)Construct an MO diagram for the He+2 ion. a.Determine if the He+2 ion is stable or unstable? b.What is its bond order? 2.) select the correct electron configurations from the list below. You can refer to the periodic table for atomic numbers. The electron configuration of Cu+ is [Ar]4s13d9. The electron configuration of S2− is [Ne]3s23p6. The electron configuration of Fe is [Ar]4s23d6. The electron configuration of Si is [Ne]3s23p2. The electron configuration of Rb is [Kr]5s04d1.
The molecule is 3. (9 points) Sketch the frontier orbitals involved in bonding the H2 to W. a. (3 points) Start by con...
The molecule is
3. (9 points) Sketch the frontier orbitals involved in bonding the H2 to W. a. (3 points) Start by considering the orbitals of the free H2 molecule. Draw the MO diagram for H2 and fill in the electrons. What is the HOMO? LUMO? Draw the shape of these orbitals. b. (4 points) Consider the metal orbitals which would have the appropriate symmetry to interact with each H2 orbital. Draw these interactions. Be sure to indicate the direction...
1. Consider the H2+ ion and respond to the following. (a) Sketch the occupied MO of H2+. HH (b) Is this a -MO? If not, why? (c) What is the number of molecular orbitals in H2+?
1. Consider the H2* ion and respond to the following questions. (a) Sketch the unoccupied MO of Hat and tell whether this orbital has a node. If yes, sketch (or describe) the surface. HH (b) How does the energy of the o-bonding MO of H2* compare to that of the 1s orbital of hydrogen? (c) Would you expect Hal to act as an oxidant or as a reducing agent toward the Halon in a chemical reaction? Briefly explain
3. Consider Heat and respond to the following. (a) Sketch the singly occupied MO of Hez*. He He (b) Decide whether Heation should have a t-MO. Explain. (c) What should happen to Hez upon one-electron reduction? Explain.
10. The MO diagrams of NO and NO+ are similar (see Lecture 15 for the MO diagram of NO+). On the basis of this consideration, respond to the following: (a) Sketch the singly-occupied MO of NO. Ν Ο (b) What is the total number of electrons in the anti-bonding MOs of NO? (c) Do the necessary calculations to decide when the NO bond should become stronger: when this compound undergoes one-electron reduction or oxidation? (d) Which atom in NO should...
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?
According to MO theory, which molecule or ion has the highest bond order? Highest bond energy? Shortest bond length? (a)O_2, O_2, O_^2- (b) CO and CO^+. (Use the energy ordering of O_2)
The H2 ion is more stable (higher bond order) than H2 since it has an additional electron to produce a net lowering of energy. (consider MO theory to answer this.) False O True Question 2 Which best explains the following trend? Element b.p. (K) He 4 Ne 25 Ar 95 Kr 125 Xe 170 O dipole-dipole interaction hydrogen bonding O London dispersion forces O ion-dipole forces
3. MO th eorv for heteronuclear diato mic molecules-II XeF is a stable molecule. The highest atomic orbital energy of Xe and F atoms are given in the table below The highest MOs that can be constructed with these AOs has the energy order All the lower-lying MOs (coming from lower-lying AOs) are fully occupied. Sketch the highest MOs in the MO-diagram of XeF from the AOs given in the table. What is the bond order of XeF? (5 points)
The molecule is
3. (9 points) Sketch the frontier orbitals involved in bonding the H2 to W. a. (3 points) Start by considering the orbitals of the free H2 molecule. Draw the MO diagram for H2 and fill in the electrons. What is the HOMO? LUMO? Draw the shape of these orbitals. b. (4 points) Consider the metal orbitals which would have the appropriate symmetry to interact with each H2 orbital. Draw these interactions. Be sure to indicate the direction...
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