QQuestionChemistry
QuestionChemistry
What is the bond order for C^2? [ Select ] [""3"", ""0.5"", ""2"", ""2.5"", ""1"", ""3.5"", ""1.5"", ""0""]
Is C^2 paramagnetic or diamagnetic? [ Select ] [""paramagnetic"", ""diamagnetic""]
What is the bond order for C^2 -? [ Select ] [""3.5"", ""2.5"", ""1.5"", ""0"", ""0.5"", ""3"", ""2"", ""1""]
Is C^2 - paramagnetic or diamagnetic? [ Select ] [""paramagnetic"", ""diamagnetic""]
What is the bond order for C^2 +? [ Select ] [""0.5"", ""2.5"", ""3"", ""0"", ""1.5"", ""2"", ""1"", ""3.5""]
Is C^2 + paramagnetic or diamagnetic? [ Select ] [""paramagnetic"", ""diamagnetic""]
Which of the three has the longest bond? [ Select ] [""C^2 +"", ""C^2 -"", ""C^2""]
Which of the three has the strongest bond?
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Answer
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Step 1:: Determine the molecular orbital configuration for C^2.
The molecular orbital configuration for C^2 can be determined using the Aufbau principle, Pauli exclusion principle, and Hund's rule. The atomic orbitals involved are 2s and 2p from each carbon atom. \begin{align*} &1s^2 2s^2 2p_x^1 2p_y^1 2p_z^0 & \text{(Carbon atom atomic orbital configuration)} \ &\underline{1s^2 2s^2 2p_x^2 2p_y^2 2p_z^0} & \text{(C^2 molecular orbital configuration)} \end{align*}
Step 2:: Calculate the bond order for C^2.
The bond order is calculated as the difference between the number of bonding electrons and the number of antibonding electrons divided by 2. In this case, there are 8 bonding electrons (2p_x^2, 2p_y^2) and 2 antibonding electrons (2p_z^0).
Step 3:: Determine if C^2 is paramagnetic or diamagnetic.
C^2 has no unpaired electrons, so it is diamagnetic.
Step 4:: Calculate the bond order for C^2 -.
For C^2 -, there is an additional electron in the antibonding orbital (2p_z^1). \begin{align*} \end{align*}
Step 5:: Determine if C^2 - is paramagnetic or diamagnetic.
C^2 - has 1 unpaired electron, so it is paramagnetic.
Step 6:: Calculate the bond order for C^2 +.
For C^2 +, there is 1 less electron in the bonding orbital (2p_x^1, 2p_y^1). \begin{align*} \end{align*}
Step 7:: Determine if C^2 + is paramagnetic or diamagnetic.
C^2 + has no unpaired electrons, so it is diamagnetic.
Step 8:: Compare the bond lengths.
The bond length is inversely proportional to the bond order. Therefore, the bond length increases as the bond order decreases.
Step 9:: Compare the bond strengths.
The bond strength is directly proportional to the bond order. Therefore, the bond strength decreases as the bond order decreases.
Final Answer
Bond order for C^2: 3 C^2 is diamagnetic. Bond order for C^2 -: 2.5 C^2 - is paramagnetic. Bond order for C^2 +: 2.5 C^2 + is diamagnetic. The longest bond is in C^2 - with a bond order of 2.5. The strongest bond is in C^2 with a bond order of 3.
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