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| 1 | |
The lone pair of electrons on sulfur in the sulfite ion (SO32-) is in |
| | A) | a p orbital. |
| | B) | an s orbital. |
| | C) | an sp2 hybrid orbital. |
| | D) | an sp3 hybrid orbital. |
| | E) | none of the above orbital types. |
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| 2 | |
Which has sp3d hybridization and no dipole moment? |
| | A) | PCl3 |
| | B) | BF3 |
| | C) | SF4 |
| | D) | BrF3 |
| | E) | PCl5 |
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| 3 | |
Which of the following hybridization patterns is associated with octahedral geometry? |
| | A) | sp2 |
| | B) | sp3 |
| | C) | sp3d2 |
| | D) | sp3d |
| | E) | sp |
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| 4 | |
Which hybrid orbitals are associated with bond angles of 90° and 120° at the central atom? |
| | A) | sp3 |
| | B) | sp3d2 |
| | C) | sp |
| | D) | sp2 |
| | E) | sp3d |
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| 5 | |
Which carbon orbitals would be involved in the formation of the hybrid orbitals that are present in ethyne (acetylene), HCCH? |
| | A) | 1s, 2s, 2px |
| | B) | 1s, 2s, 2px, 2py |
| | C) | 2s, 2px |
| | D) | 2s, 2px, 2py |
| | E) | 2s, 2px, 2py, 2pz |
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| 6 | |
For the following molecule, what is the hybridization for each carbon?
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| | A) | sp |
| | B) | sp5 |
| | C) | sd4 |
| | D) | sp2 |
| | E) | sp3 |
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| 7 | |
In H2CNH, which orbitals overlap in forming the NC bond? |
| | A) | 1s overlaps with 2s |
| | B) | sp overlaps with 1s |
| | C) | sp2 overlaps with 1s |
| | D) | sp2 overlaps with sp2 |
| | E) | sp2 overlaps with sp2 and 2p overlaps with 2p |
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| 8 | |
The carbon atoms in ethyne (acetylene, C2H2) are joined by a triple bond. The  Pi
(0.0K)
bonds in this compound consist of: |
| | A) | 6 electrons, 3 orbitals, and 5 lobes |
| | B) | 6 electrons, 3 orbitals, and 4 lobes |
| | C) | 4 electrons, 3 orbitals, and 4 lobes |
| | D) | 4 electrons, 2 orbitals, and 2 lobes |
| | E) | 4 electrons, 2 orbitals, and 4 lobes |
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| 9 | |
Which of the following molecules will not have a Pi
(0.0K)
bond? |
| | A) | C2H2 |
| | B) | C2H6 |
| | C) | N2H2 |
| | D) | None of the above. |
| | E) | All of the above. |
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| 10 | |
Which of the substituted ethylene molecules listed can exist in both cis- and trans- forms? |
| | A) | H2C=CF2 |
| | B) | HFC=CF2 |
| | C) | HFC=CF2 |
| | D) | HFC=CHF |
| | E) | HFC=CH2 |
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| 11 | |
According to molecular orbital theory, in the O2+ ion, how many valence electrons are in antibonding molecular orbitals? |
| | A) | 6 |
| | B) | 5 |
| | C) | 4 |
| | D) | 3 |
| | E) | 2 |
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| 12 | |
Which is the correct order for the oxygen-oxygen bond length? |
| | A) | HOOH>O2->O2+>O2 |
| | B) | HOOH>O2->O2>O2+ |
| | C) | HOOH<O2+<O2-<O2 |
| | D) | HOOH<O2-<O2+<O2 |
| | E) | HOOH>O2->O2+>O2 |
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| 13 | |
Assume that N2 absorbs a photon and an electron is raised to the first excited state. |
| | A) | The excited N2 is less stable than N2 in the ground state |
| | B) | The excited N2 is more stable than N2 in the ground state |
| | C) | The bond length of N2 in the excited state is shorter than the bond length of N2 in the ground state. |
| | D) | The excited state molecule will break up into two nitrogen atoms. |
| | E) | none of the above |
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| 14 | |
The bond order in NO predicted by molecular orbital theory is |
| | A) | 1 |
| | B) | 1.5 |
| | C) | 2 |
| | D) | 2.5 |
| | E) | none of the above. |
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| 15 | |
In the molecular orbital description of bonding in benzene (C6H6), how many electrons occupy delocalized Pi
(0.0K)
MOs? |
| | A) | 2 |
| | B) | 3 |
| | C) | 4 |
| | D) | 5 |
| | E) | 6 |
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