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"Use the MO diagram provided below to answer the following questions: What is the bond order for C^2? [ Select ] [""0.5"", ""1"", ""1.5"", ""3.5"", ""2.5"", ""0"", ""3"", ""2""] Is C^2 paramagnetic or diamagnetic? [ Select ] [""paramagnetic"", ""diamagnetic""] What is the bond order for C^2 -? [ Select ] [""3"", ""0"", ""1.5"", ""3.5"", ""0.5"", ""2.5"", ""2"", ""1""] Is C^2 - paramagnetic or diamagnetic? [ Select ] [""diamagnetic"", ""paramagnetic""] What is the bond order for C^2 +? [ Select ] [""3.5"", ""1"", ""0.5"", ""2"", ""2.5"", ""1.5"", ""0"", ""3""] 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? [ Select ] [""C^2 +"", ""C^2"", ""C^2 -""] "
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Step 1
: Determine the bond order for C^2.

The bond order can be calculated using the formula: From the MO diagram, we see that there are 2 electrons in bonding molecular orbitals and none in antibonding molecular orbitals. Therefore,

Final Answer

Step 2: Determine if C^2 is paramagnetic or diamagnetic. C^2 has no unpaired electrons, so it is diamagnetic. Step 3: Determine the bond order for C^2 -. C^2 - has 3 electrons in bonding molecular orbitals and 1 electron in antibonding molecular orbitals. Therefore,
Bond order=12(3−1)=1 \text{Bond order} = \frac{1}{2} (3 - 1) = 1
Step 4: Determine if C^2 - is paramagnetic or diamagnetic. C^2 - has 1 unpaired electron, so it is paramagnetic. Step 5: Determine the bond order for C^2 +. C^2 + has 2 electrons in bonding molecular orbitals and 2 electrons in antibonding molecular orbitals. Therefore,
Bond order=12(2−2)=0 \text{Bond order} = \frac{1}{2} (2 - 2) = 0
Step 6: Determine if C^2 + is paramagnetic or diamagnetic. C^2 + has no unpaired electrons, so it is diamagnetic. Step 7: Determine which of the three has the longest bond. From the bond order values calculated above, we can see that C^2 + has the lowest bond order (0), followed by C^2 - (1) and C^2 (1). In general, a lower bond order corresponds to a longer bond. Step 8: Determine which of the three has the strongest bond. From the bond order values calculated above, we can see that C^2 has the highest bond order (1), followed by C^2 - (1) and C^2 + (0). In general, a higher bond order corresponds to a stronger bond.

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