Chapter 7, Problem 7.137QP

(a)

Interpretation Introduction

Interpretation: The electronic configuration and bond order of ${\text{P}}_{\text{2}}$ should be found out. Also to found out the magnetic properties of ${\text{P}}_{\text{2}}$.

Concept Introduction:

• In molecular orbital theory, when the bonding takes place the atomic orbitals that take part combine to get a new orbital that has the properties of the whole molecule. The newly formed orbitals are known as molecular orbitals
• The bond order gives an idea about the stability of a molecule. It can be calculated using the molecular orbital theory. The stability of a molecule increase as the bond order increases.
• $\text{Bond}\text{order}\text{=}\frac{\left(\begin{array}{l}\text{number}\text{of}\text{electrons}\text{in}\\ \text{bonding}\text{molecular}\text{orbitals}\end{array}\right)\text{-}\left(\begin{array}{l}\text{number}\text{of}\text{electrons}\text{in}\\ \text{antibonding}\text{molecular}\text{orbitals}\end{array}\right)}{\text{2}}$
• Paramagnetic species contains at least one unpaired electrons and can be attracted towards magnetic fields. In diamagnetic species does have any unpaired electrons. That is spins of all the electrons are paired. It slightly repelled towards the magnetic fields

(b)

Interpretation Introduction

Interpretation: The electronic configuration and bond order of ${\text{P}}_{\text{2}}$ should be found out. Also to found out the magnetic properties of ${\text{P}}_{\text{2}}$.

Concept Introduction:

• In molecular orbital theory, when the bonding takes place the atomic orbitals that take part combine to get a new orbital that has the properties of the whole molecule. The newly formed orbitals are known as molecular orbitals
• The bond order gives an idea about the stability of a molecule. It can be calculated using the molecular orbital theory. The stability of a molecule increase as the bond order increases.
• $\text{Bond}\text{order}\text{=}\frac{\left(\begin{array}{l}\text{number}\text{of}\text{electrons}\text{in}\\ \text{bonding}\text{molecular}\text{orbitals}\end{array}\right)\text{-}\left(\begin{array}{l}\text{number}\text{of}\text{electrons}\text{in}\\ \text{antibonding}\text{molecular}\text{orbitals}\end{array}\right)}{\text{2}}$
• Paramagnetic species contains at least one unpaired electrons and can be attracted towards magnetic fields. In diamagnetic species does have any unpaired electrons. That is spins of all the electrons are paired. It slightly repelled towards the magnetic fields

 (c)

Interpretation Introduction

Interpretation: The electronic configuration and bond order of ${\text{P}}_{\text{2}}$ should be found out. Also to found out the magnetic properties of ${\text{P}}_{\text{2}}$.

Concept Introduction:

• In molecular orbital theory, when the bonding takes place the atomic orbitals that take part combine to get a new orbital that has the properties of the whole molecule. The newly formed orbitals are known as molecular orbitals
• The bond order gives an idea about the stability of a molecule. It can be calculated using the molecular orbital theory. The stability of a molecule increase as the bond order increases.
• $\text{Bond}\text{order}\text{=}\frac{\left(\begin{array}{l}\text{number}\text{of}\text{electrons}\text{in}\\ \text{bonding}\text{molecular}\text{orbitals}\end{array}\right)\text{-}\left(\begin{array}{l}\text{number}\text{of}\text{electrons}\text{in}\\ \text{antibonding}\text{molecular}\text{orbitals}\end{array}\right)}{\text{2}}$
• Paramagnetic species contains at least one unpaired electrons and can be attracted towards magnetic fields. In diamagnetic species does have any unpaired electrons. That is spins of all the electrons are paired. It slightly repelled towards the magnetic fields