Which one of the following statements is false ?

1. Which one of the following statements is false? • Valence bond theory and molecular orbital theory can be described as two different views of the same thing. • When one considers the molecular orbitals resulting from the overlap of any two specific atomic orbitals, the bonding orbitals are always lower in energy than the antibonding orbitals. • Molecular orbitals are generally described as being more delocalized than hybridized atomic orbitals. • One of the shortcomings of molecular orbital theory is its inability to account for a triple bond in the N2 molecule. • One of the shortcomings of valence bond theory is its inability to account for the paramagnetism of O2.

2. What is the bond order of a species with 7 bonding electrons and 4 antibonding electrons? • 1 • 1.5 • 2 • 2.5 • 3

3. Draw the molecular orbital diagram for N2. The number of electrons in the {image} molecular orbital is _____. • 1 • 2 • 3 • 4 • zero

4. Draw the molecular orbital diagram for F2. The number of electrons in the {image} molecular orbital is _____. • 1 • 2 • 3 • 4 • zero

5. What is the bond order for F2? • 1 • 2 • 3 • 4.5 • 2.5

6. Which response lists only the molecules given below that are not paramagnetic? B2, C2, N2, O2, F2 • N2 and F2 • N2 and O2 • B2 and O2 • B2 and N2 • all of these

7. What diatomic molecule and/or ion(s) would have the molecular orbital electron configuration given below? {image} • O2- and F2+ • O2and F2 • F2- and Ne2+ • F2 and O2- • O2+ and F2-

8. Which response lists all the following diatomic molecules and ions that are paramagnetic? Be2, B2, B22+, C22+, C22, O2-, O22- • B22+, C22+, and O22- • Be2 and B2 • B2, C22+, and C22- • B2, C22+, and O22- • B2, C22+, and O2-

9. Which of the following statements concerning homonuclear diatomic molecules of the third and subsequent periods is false? • The heavier halogens, Cl2, Br2, and I2, which contain only sigma (single) bonds, are the only well-characterized examples at room temperature. • Other homonuclear diatomic species (other than the halogens) are neither common nor very stable. • The heavier elements are unstable because they cannot form strong pi bonds with each other. • For these larger atoms the sigma bond length is too great to allow the atomic p orbitals on different atoms to overlap side-on-side effectively. • All of the above statements explain why P2 is much more stable than N2.

10. What is the bond order for NO? • 0.5 • 1 • 1.5 • 2 • 2.5