The number of AOs that three atoms from the second row of the periodic table would contribute in a linear molecule toward the productions of MOs is to be determined. The number of MOs that would be produced by the mixing of these valence shell AOs is to be determined. Concept introduction: According to Molecular Orbital Theory (MO Theory), when two atomic orbitals overlap significantly, they produce two molecular orbitals. One of these molecular orbitals is produced by overlap and mixing of two AOs that have the same phase. This MO is lower in energy than the individual AOs, and is called the bonding atomic orbital. The second MO is produced by the overlap and mixing of the AOs of opposite phases. It is higher in energy than the individual AOs and is called the antibonding MO. In cases where the overlap produces an MO of the same energy, the resulting MO is called a non-bonding MO. Only AOs of similar energies can interact to form MOs. In effect, this means only the AOs from the valence shells of the two atoms can form MOs. For atoms of elements from the second row, this means a total of four AOs, the lone 2s orbital, and the three 2p orbitals can form MOs. The number of MOs formed is the same as the number of AOs that mix.

Question

Want to see the full answer?

Answer 1

Question

Chapter 3, Problem 3.28P

Interpretation Introduction

Interpretation:

The number of AOs that three atoms from the second row of the periodic table would contribute in a linear molecule toward the productions of MOs is to be determined. The number of MOs that would be produced by the mixing of these valence shell AOs is to be determined.

Concept introduction:

According to Molecular Orbital Theory (MO Theory), when two atomic orbitals overlap significantly, they produce two molecular orbitals. One of these molecular orbitals is produced by overlap and mixing of two AOs that have the same phase. This MO is lower in energy than the individual AOs, and is called the bonding atomic orbital. The second MO is produced by the overlap and mixing of the AOs of opposite phases. It is higher in energy than the individual AOs and is called the antibonding MO.

In cases where the overlap produces an MO of the same energy, the resulting MO is called a non-bonding MO.

Only AOs of similar energies can interact to form MOs. In effect, this means only the AOs from the valence shells of the two atoms can form MOs. For atoms of elements from the second row, this means a total of four AOs, the lone 2s orbital, and the three 2p orbitals can form MOs.

The number of MOs formed is the same as the number of AOs that mix.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Suppose a linear molecule were constructed from three atoms, all of which are found in the second row of the periodictable. How many valence shell AOs would these three atoms contribute toward the production of MOs? How manyMOs would be produced by the mixing of these valence shell AOs? Hint: The answer is independent of which orbitalsoverlap.

I am confused why this powerpoint slight says 'sideways overlap... leads to a p-bonding MO AND a p*-antibonding MO.' Isn't it one or the other? Why does it say AND? The orbitals can't have descrutive and constructive interaction at the same time right?

Can you please help me determine the σ framework and π MO Energy Diagram for this molecule?