Answer to 1-a:
The antibonding MO means the destructive interference between two waves (from two atomic orbitals of two hydrogens). This decreases in the electron density in the internuclear electron probability density. Thus, a node is created where the elctron density is zero.
Answer to part 1-b:
As it can be seen from the above diagram, the
orbital has lower energy than the energy of the 1S orbital of the
H atom.
Answer to part 1-c:
The electronic configuration according to the MO diagram for
H2+ ion is .
The electronic configuration according to the MO diagram for
H2- ion would be
.
The electron in the antibonding orbital in the
H2- has higher energy than the singly
occupied MO (SOMO) of the H2+. Thus, transfer
of one electron from H2- ion to
the SOMO ofthe H2+ ion is favorable. Thus,
H2+ acts as an oxidizing agent and
H2- acts as an reducing agent in the chemical
reaction between these two ions.
1. Consider the H2* ion and respond to the following questions. (a) Sketch the unoccupied MO...
1. Consider the H2+ ion and respond to the following. (a) Sketch the occupied MO of H2+. HH (b) Is this a -MO? If not, why? (c) What is the number of molecular orbitals in H2+?
Consider the H2 ion and respond to the following 2. (a) Sketch the highest occupied MO of H2 H (b) What is the electron density in this MO at the midpoint of the H-H bond? (c) What is the bond order in H2-?
The following questions are true/false 1. The potential energy associated with London dispersion interactions decreases with intermolecular distance as r-12 (where r is the intermolecular distance). 2. SiH4 is more polarizable than CH4. 3. In H2, the antibonding orbital formed by linear combination of two 1s orbitals has zero nodes. 4. In N2, the π bonding orbital formed by linear combination of two 2p orbitals has one node. 5. CO2 has zero total permanent dipole moment. 6. The kinetic energy...