   Chapter 20, Problem 46E

Chapter
Section
Textbook Problem

# Compare the Lewis structures with the molecular orbital view of the bonding in NO, NO+, and NO−. Account for any discrepancies between the two models.

Interpretation Introduction

Interpretation: The comparison of the Lewis structures with the molecular orbital view of the bonding in NO, NO+ and NO- is to be done.  Discrepancies between the two models if present are to be accounted.

Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed.  Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.

Energy of bonding molecular orbitals is less than the nonbonding molecular orbitals.

To determine: The comparison of the Lewis structures with the molecular orbital view of the bonding in NO, NO+ and NO-.

Explanation

Explanation

The bonding in NO+ is explained by lewis structures and molecular orbital model.

The valence electrons in nitrogen is 5. Valence electrons in oxygen is 6.

The cation NO+ is formed when one electron is removed from NO.

The valence electrons in NO is 5+6=11.

Therefore, the valence electrons in NO+ is 11-1=10.

The lewis dot structure for NO+ is

Figure 1

The molecular orbital diagram for NO+ is,

Figure 2.

Bond order is calculated by the formula,

Bondorder=12(Electronsinbondingmolecularorbital-Electronsinantibondingmolecularorbital)

Number of electrons in bonding molecular orbital in NO+ is 8.

Number of electrons in antibonding molecular orbitals is 2.

Substitute the values of electrons in the above formula.

Bondorder=12(8-2)=12×6=3

Therefore, the bond order of NO+ is 3.

The bonding in NO- is explained by lewis structures and molecular orbital model.

The valence electrons in nitrogen is 5. Valence electrons in oxygen is 6.

The anion NO- is formed when one electron is gained by NO.

The valence electrons in NO is 5+6=11.

Therefore, the valence electrons in NO- is 5+6=11.

The lewis dot structure for NO- is

Figure 3

The molecular orbital diagram for NO- is,

Figure 4

Bond order is calculated by the formula,

Bondorder=12(Electronsinbondingmolecularorbital-Electronsinantibondingmolecularorbital)

Number of electrons in bonding molecular orbital in NO- is 8

Number of electrons in antibonding molecular orbitals is 4

Substitute the values of electrons in the above formula

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