The molecular orbital description for metal bonding is different from that for diatomic molecules in that ________
A)there are no antibonding orbitals in the metal bonding description.
B)quantum theory no longer applies as the orbitals are continuous.
C)the orbitals are so close in energy that they are referred to as bands.
D)the increased number of electrons results in each bond being stronger.
E)All of the above are true.

Question

Quizplus · Accepted Answer

In the molecular orbital description for metal bonding, the orbitals are so close in energy that they overlap and form bands, rather than distinct molecular orbitals. This is due to the large number of electrons and the delocalized nature of the metal atoms. Therefore, option C is the correct answer. Option A is incorrect because there are antibonding orbitals in the metal bonding description, but they are generally higher in energy and do not play a significant role in bonding. Option B is incorrect because quantum theory still applies to metals, and the continuous nature of the orbitals is a consequence of the delocalization of the electrons. Option D is also incorrect because the increased number of electrons can lead to stronger bonding, but this is not a defining feature of metal bonding.

The Molecular Orbital Description for Metal Bonding Is Different from That