QQuestionChemistry
QuestionChemistry
"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 -""] "
3 months agoReport content
Answer
Full Solution Locked
Sign in to view the complete step-by-step solution and unlock all study resources.
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,
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,
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.
Need Help with Homework?
Stuck on a difficult problem? We've got you covered:
- Post your question or upload an image
- Get instant step-by-step solutions
- Learn from our AI and community of students