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. 2.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. 3.Molecular orbitals are generally described as being more delocalized than hybridized atomic orbitals. 4.One of the shortcomings of molecular orbital theory is its inability to account for a triple bond in the N 2 molecule. 5.One of the shortcomings of valence bond theory is its inability to account for the paramagnetism of O 2.

What is the bond order of a species with 7 bonding electrons and 4 antibonding electrons?

zero

zero

What is the bond order for F 2 ?

Which response lists only the molecules given below that are not paramagnetic? B 2, C 2, N 2, O 2, F N 2 and F 2 2.N 2 and O 2 3.B 2 and O 2 4.B 2 and N 2 5.all of these

O 2- and F 2+ 2.O 2 and F 2 3.F 2- and Ne 2+ 4.F 2 and O 2- 5.O 2+ and F 2-

Which response lists all the following diatomic molecules and ions that are paramagnetic? Be 2, B 2, B 2 2+, C 2 2+, C 2 2, O 2 -, O B 2 2+, C 2 2+, and O Be 2 and B 2 3.B 2, C 2 2+, and C B 2, C 2 2+, and O B 2, C 2 2+, and O 2 -

Which of the following statements concerning homonuclear diatomic molecules of the third and subsequent periods is false? The heavier halogens, Cl 2, Br 2, and I 2, which contain only sigma (single) bonds, are the only well-characterized examples at room temperature. 2.Other homonuclear diatomic species (other than the halogens) are neither common nor very stable. 3.The heavier elements are unstable because they cannot form strong pi bonds with each other. 4.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. 5.All of the above statements explain why P 2 is much more stable than N 2.

What is the bond order for NO?