Q. For which of the following diatomic molecules is the bond order equal to 2?
Solution
F2 has a bond order of 1, while C2 has a bond order of 2.
Correct Answer: D — F2
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Q. For which of the following molecules is the bond order equal to 0?
-
A.
He2
-
B.
H2
-
C.
Li2
-
D.
Be2
Solution
He2 has a bond order of 0, as it has equal bonding and antibonding electrons.
Correct Answer: A — He2
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Q. For which of the following molecules is the molecular orbital diagram similar to that of O2?
Solution
The molecular orbital diagram of F2 is similar to that of O2, with the same energy level arrangement.
Correct Answer: B — F2
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Q. For which of the following pairs of molecules is the bond order the same?
-
A.
N2 and C2
-
B.
O2 and F2
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C.
B2 and C2
-
D.
N2 and O2
Solution
O2 and F2 both have a bond order of 2.
Correct Answer: B — O2 and F2
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Q. In molecular orbital theory, which of the following orbitals is filled first?
-
A.
σ2s
-
B.
σ*2s
-
C.
π2p
-
D.
σ2p
Solution
According to the Aufbau principle, the σ2s orbital is filled first before any other orbitals.
Correct Answer: A — σ2s
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Q. In molecular orbital theory, which of the following orbitals is the highest energy in O2?
-
A.
σ2p
-
B.
π2p
-
C.
σ2s
-
D.
π2s
Solution
In O2, the π2p orbitals are the highest energy orbitals.
Correct Answer: B — π2p
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Q. In molecular orbital theory, which of the following statements is correct regarding the energy levels of orbitals?
-
A.
σ orbitals are always lower than π orbitals.
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B.
π orbitals are always lower than σ orbitals.
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C.
σ* orbitals are always higher than π* orbitals.
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D.
Energy levels can vary based on the atoms involved.
Solution
The energy levels of molecular orbitals can vary depending on the specific atoms and their electronegativities.
Correct Answer: D — Energy levels can vary based on the atoms involved.
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Q. In the molecular orbital diagram of diatomic nitrogen (N2), which orbitals are filled first?
-
A.
σ2s, σ*2s
-
B.
σ2p, π2p
-
C.
π2p, σ2p
-
D.
σ*2p, π*2p
Solution
In N2, the 2s orbitals (σ2s and σ*2s) are filled before the 2p orbitals.
Correct Answer: A — σ2s, σ*2s
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Q. In the molecular orbital theory, which of the following is true for the π molecular orbitals?
-
A.
They are formed by end-to-end overlap.
-
B.
They are lower in energy than σ orbitals.
-
C.
They can accommodate a maximum of 2 electrons.
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D.
They are always bonding.
Solution
π molecular orbitals can accommodate a maximum of 2 electrons, similar to all molecular orbitals.
Correct Answer: C — They can accommodate a maximum of 2 electrons.
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Q. In the molecular orbital theory, which of the following orbitals is lower in energy than the 2p orbitals?
Solution
The 2s molecular orbitals are lower in energy than the 2p molecular orbitals.
Correct Answer: A — 2s
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Q. In the molecular orbital theory, which of the following orbitals is lower in energy for homonuclear diatomic molecules?
-
A.
σ2p
-
B.
π2p
-
C.
σ2s
-
D.
π2s
Solution
The σ2s orbital is lower in energy than the π2p and σ2p orbitals in homonuclear diatomic molecules.
Correct Answer: C — σ2s
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Q. In the molecular orbital theory, which of the following orbitals is the highest energy in O2?
-
A.
σ2p
-
B.
π2p
-
C.
σ*2p
-
D.
π*2p
Solution
The highest energy orbital in O2 is σ*2p, which is an antibonding orbital.
Correct Answer: C — σ*2p
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Q. In the molecular orbital theory, which of the following orbitals is the highest occupied molecular orbital (HOMO) in O2?
-
A.
σ2p
-
B.
π2p
-
C.
σ*2p
-
D.
π*2p
Solution
In O2, the highest occupied molecular orbital (HOMO) is π2p.
Correct Answer: B — π2p
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Q. In the molecular orbital theory, which of the following pairs of orbitals can combine to form a sigma bond?
-
A.
s and p
-
B.
p and p
-
C.
s and s
-
D.
d and p
Solution
s and s orbitals can combine to form a sigma bond.
Correct Answer: C — s and s
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Q. In the molecular orbital theory, which orbitals combine to form sigma bonds?
-
A.
s and p orbitals
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B.
p and d orbitals
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C.
s orbitals only
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D.
p orbitals only
Solution
Sigma bonds are formed by the head-on overlap of s and p orbitals.
Correct Answer: A — s and p orbitals
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Q. In which of the following molecules does the molecular orbital configuration lead to paramagnetism?
Solution
O2 is paramagnetic due to the presence of two unpaired electrons in its molecular orbitals.
Correct Answer: B — O2
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Q. In which of the following molecules does the molecular orbital configuration show unpaired electrons?
Solution
O2 has two unpaired electrons in its π* orbitals, making it paramagnetic.
Correct Answer: B — O2
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Q. In which of the following molecules does the molecular orbital diagram show a paramagnetic behavior?
Solution
O2 is paramagnetic due to the presence of two unpaired electrons in its molecular orbitals.
Correct Answer: B — O2
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Q. In which of the following molecules does the molecular orbital theory predict a triple bond?
Solution
N2 has a triple bond, with a bond order of 3 according to molecular orbital theory.
Correct Answer: A — N2
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Q. In which of the following molecules does the molecular orbital theory predict a paramagnetic behavior?
Solution
O2 is paramagnetic due to the presence of two unpaired electrons in its molecular orbitals.
Correct Answer: B — O2
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Q. In which of the following species does the molecular orbital configuration show a paramagnetic behavior?
Solution
O2 has unpaired electrons in its molecular orbital configuration, making it paramagnetic.
Correct Answer: B — O2
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Q. What is the bond order of the CO molecule?
Solution
CO has a bond order of 3, calculated as (10 bonding - 3 antibonding)/2.
Correct Answer: C — 3
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Q. What is the bond order of the ion O2-?
Solution
O2- has a bond order of 1, calculated as (10 bonding electrons - 7 antibonding electrons)/2 = 1.
Correct Answer: B — 2
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Q. What is the bond order of the molecule B2 according to molecular orbital theory?
Solution
B2 has a bond order of 1, calculated as (2 bonding - 0 antibonding)/2.
Correct Answer: B — 1
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Q. What is the bond order of the molecule B2?
Solution
B2 has a bond order of 1, calculated from its molecular orbital configuration.
Correct Answer: A — 1
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Q. What is the bond order of the molecule CO?
Solution
CO has a bond order of 3, calculated as (10 bonding electrons - 2 antibonding electrons)/2 = 3.
Correct Answer: C — 3
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Q. What is the bond order of the molecule He2?
Solution
He2 has a bond order of 0, as it has no net bonding electrons.
Correct Answer: A — 0
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Q. What is the bond order of the N2 molecule?
Solution
N2 has a bond order of 3, calculated as (10 bonding - 0 antibonding)/2 = 3.
Correct Answer: C — 3
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Q. What is the bond order of the O2 molecule according to Molecular Orbital Theory?
Solution
O2 has 12 total electrons, leading to a bond order of (10 bonding - 6 antibonding)/2 = 1.
Correct Answer: B — 2
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Q. What is the molecular geometry of the molecule with the electronic configuration of 1s2 2s2 2p2?
-
A.
Linear
-
B.
Trigonal Planar
-
C.
Tetrahedral
-
D.
Octahedral
Solution
The electronic configuration corresponds to C2, which has a tetrahedral geometry due to sp3 hybridization.
Correct Answer: C — Tetrahedral
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