Question

Question: When a molecule can form two different structures, the structure with the stronger bonds is usually the more stable form. Use bond energies to predict the correct structure of the hydroxylamine molecule:

Short answer

Since bond energy of left molecule is \({\rm{B}}{\rm{.E}}{\rm{. = 1444\;kJ}}\), which is more than the bond energy of right molecule i.e., \({\rm{B}}{\rm{.E}}{\rm{. = 1370\;kJ}}\) therefore, left molecule is more stable and is the correct structure.

Step-by-step solution

Concept Introduction

Bond energy, also known as mean bond enthalpy or average bond enthalpy in chemistry, is a measure of the bond strength in a chemical bond.

Bond Energy for Hydroxylamine

Observe the structure –

Bond Energy for\({\rm{N - H}}\)is:\({\rm{390 kJ/mol}}\)

Bond Energy for\({\rm{N - O}}\)is:\({\rm{200 kJ/mol}}\)

Bond Energy for\({\rm{O - H}}\)is:\({\rm{464 kJ/mol}}\)

Calculate the bond energy –

\(\begin{array}{l}{\rm{B}}{\rm{.E}}{\rm{. = 2(390) + 200 + 464}}\\{\rm{B}}{\rm{.E}}{\rm{. = 1444 kJ}}\end{array}\)

Therefore, the bond energy is \({\rm{B}}{\rm{.E}}{\rm{. = 1444\;kJ}}\).

Bond Energy for Hydroxylamine

Observe the structure –

Bond Energy for \({\rm{N - H}}\) is: \({\rm{390 kJ/mol}}\)

Bond Energy for \({\rm{N - O}}\) is: \({\rm{200 kJ/mol}}\)

Calculate the bond energy –

\(\begin{array}{l}{\rm{B}}{\rm{.E}}{\rm{. = 3(390) + 200}}\\{\rm{B}}{\rm{.E}}{\rm{. = 1370 kJ}}\end{array}\)

Therefore, the bond energy is \({\rm{B}}{\rm{.E}}{\rm{. = 1370\;kJ}}\).