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Chapter 8: Q7 E (page 446)

A friend tells you \({{\rm{N}}_{\rm{2}}}\)has three \({\rm{\pi }}\)bonds due to overlap of the three p-orbitals on each N atom. Do you agree?

Short Answer

Expert verified

In the given structure; \({N_2},N \equiv N\), there is one sigma and two pi bonds because one sigma bond is formed by the axial overlapping of two p-orbital of each nitrogen atom. After the formation of one sigma bond; remaining p-orbital overlaps by sidewise and will from two pi bond also.

Step by step solution

01

Definition of Concept

The sigma bond is formed when atomic orbitals involved in the formation of a molecular orbital overlap along the internuclear axis.

The bond formed is known as a pi-bond when p-orbitals involved in bond formation overlap sideways.

02

Explain \({{\rm{N}}_{\rm{2}}}\) has three \({\rm{\pi }}\) bonds due to overlap of the three p-orbitals on each N atom

Considering the given information:

\({N_2},N \equiv N\)

Only a single bond is always a sigma bond, whereas a double bond has one sigma bond and one pi bond, and a triple bond has one sigma bond and two pi bonds.

Therefore, one sigma bond is formed by the axial overlapping of two p-orbitals of each nitrogen atom, the structure \({N_2},N \equiv N\) has one sigma and two pi bonds. Following the formation of one sigma bond, the remaining p-orbital overlaps sideways, resulting in the formation of two pi bonds.

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Most popular questions from this chapter

For the molecule allene, \({{\rm{H}}_{\rm{2}}}{\rm{C = C = C}}{{\rm{H}}_{\rm{2}}}\) , give the hybridization of each carbon atom. Will the hydrogen atoms be in the same plane or perpendicular planes?

If molecular orbitals are created by combining five atomic orbitals from atom A and five atomic orbitals from atom B combine, how many molecular orbitals will result?

Draw a curve that describes the energy of a system with H and CI atoms at varying distances. Then, find the minimum energy of this curve two ways.

(a) Use the bond energy found in Table 8.1 to calculate the energy for one single HCl bond (Hint: How many bonds are in a mole?)

(b) Use the enthalpy of reaction and the bond energies for \({{\rm{H}}_{\rm{2}}}\)and \({\rm{C}}{{\rm{l}}_{\rm{2}}}\)to solve for the energy of one mole of \({\rm{HCl}}\)bonds.

\({{\text{H}}_{\text{2}}}{\text{(g) + C}}{{\text{l}}_{\text{2}}}{\text{(g)}} \rightleftharpoons {\text{2HCl(g)}}\) ΔH°rxn = −184.7 kJ/mol

For the first ionization energy for an \({{\rm{N}}_2}\) molecule, what molecular orbital is the electron removed from?

For each of the following molecules, indicate the hybridization requested and whether or not the electrons will be delocalized: (a) ozone (\({{\rm{O}}_{\rm{3}}}\)) central \({\rm{O}}\) hybridization (b) carbon dioxide (\({\rm{C}}{{\rm{O}}_{\rm{2}}}\)) central \({\rm{C}}\) hybridization (c) nitrogen dioxide (\({\rm{N}}{{\rm{O}}_{\rm{2}}}\)) central \({\rm{N}}\) hybridization (d) phosphate ion (\({\rm{P}}{{\rm{O}}_{\rm{4}}}^{{\rm{3 - }}}\)) central \({\rm{P}}\) hybridization.
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