🤓 Based on our data, we think this question is relevant for Professor Mullen's class at UNF.
We’re being asked to compare the H–H bond in H2 and in H2–. For this, we need to determine the bond order for each species. The bond order tells us the strength and length of a bond: a higher bond order means the bond is stronger and shorter.
Step 1: Calculate the total number of valence electrons present.
Step 2: Draw the molecular orbital diagram.
Step 3: Calculate the bond order of the molecule/ion. Recall that the formula for bond order is:
Compared to the H−H bond in H 2, the H−H bond in H 2− is expected to be which of the following?
a. longer and stronger
b. longer and weaker
c. shorter and weaker
d. shorter and stronger
e. the same length and strength
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Bond Order concept. If you need more Bond Order practice, you can also practice Bond Order practice problems.
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Our tutors rated the difficulty ofCompared to the H−H bond in H 2, the H−H bond in H 2− is exp...as medium difficulty.
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Based on our data, we think this problem is relevant for Professor Mullen's class at UNF.