We’re being asked to rank the given species in order of increasing bond length and increasing bond energy.
Recall that the bond order tells us the strength and length of a bond: a higher bond order means the bond is stronger and shorter.
higher bond order → higher bond strength → shorter bond length → higher bond energy
We can calculate for the bond order using:
bonding MOs → without an asterisk (e.g., σ1s)
antibonding MOs → those with an asterisk (e.g., σ1s*).
To do so, we need to look at the molecular orbital (MO) diagram of each molecule. Recall that we have two types of MO diagrams:
Place the species B2+, B2, and B2- in order of increasing bond length and increasing bond energy.
Frequently Asked Questions
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 MO Theory: Homonuclear Diatomic Molecules concept. You can view video lessons to learn MO Theory: Homonuclear Diatomic Molecules. Or if you need more MO Theory: Homonuclear Diatomic Molecules practice, you can also practice MO Theory: Homonuclear Diatomic Molecules practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Castaneda's class at UMICH.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.