According to MO theory,?

which of the following ions has the highest bond order?

a) O2

b) O2^-

C)O2^2-

Highest bond energy?

a) O2

b) O2^-

C)O2^2-

Shortest bond length?

a) O2

b) O2^-

C)O2^2-

3 Answers

  • I just did this exact problem on my online homework, masteringchemistry.com. All of the answers are the same, O2.

    a) O2

    b) O2

    c) O2

    A)Bond order = (number of electrons in bonding MOs) - (number of electrons in antibonding MOs) / 2

    Bond order for O2 = (8-4) / 2 = 2

    Bond order for O2- = (8-5) / 2 = 1.5

    Bond order for O2 2- = (8-6) / 2 = 1

    To find the bond order, just draw the molecular orbital energy diagrams and you can find it easily.

    B) The highest bond energy would be O2, because bond order is directly related to bond energy.

    C) The shortest bond length would be O2 also, because the bond order is indirectly related to bond length so O2 would have the shortest bond length.

    Source(s): I just did this exact problem on my online homework, masteringchemistry.com. Just about 5 minutes ago and got them all right.
    Are you in CH 221 benight's class at PSU by any chance? We have the same homework problems and its due at the same time.
  • Highest Bond Order

  • O2 for all

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