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Chapter 7: Q67E (page 400)

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

Expert verified

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

01

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.

02

Bond Energy for Hydroxylamine

Observe the structure 鈥�

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 鈥�

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

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

03

Bond Energy for Hydroxylamine

Observe the structure 鈥�

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 鈥�

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

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

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Most popular questions from this chapter

In the Lewis structures listed here, M and X represent various elements in the third period of the periodic table. Write the formula of each compound using the chemical symbols of each element:

Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a two-atom molecule: (a) Adjust the electronegativity value so the bond dipole is pointing toward B. Then determine what the electronegativity values must be to switch the dipole so that it points toward A. (b) With a partial positive charge on A, turn on the electric field and describe what happens. (c) With a small partial negative charge on A, turn on the electric field and describe what happens. (d) Reset all, and then with a large partial negative charge on A, turn on the electric field and describe what happens.

Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a real molecule. You may need to rotate the molecules in three dimensions to see certain dipoles. (a) Sketch the bond dipoles and molecular dipole (if any) for O3. Explain your observations. (b) Look at the bond dipoles for NH3. Use these dipoles to predict whether N or H is more electronegative. (c) Predict whether there should be a molecular dipole for NH3 and, if so, in which direction it will point. Check the molecular dipole box to test your hypothesis.

Sodium nitrite, which has been used to preserve bacon and other meats, is an ionic compound. Write the resonance forms of the nitrite ion, \({\rm{NO}}_{\rm{2}}^{\rm{ - }}\).

Describe the molecular structure around the indicated atom or atoms:

  1. The sulfur atom in sulfuric acid, H2SO4 [ (HO)2 SO2]

  2. The chlorine atom in chloric acid, HClO3 [HOClO2]

  3. The oxygen atom in Hydrogen peroxide, HOOH

  4. The nitrogen atom in nitric acid, HNO3 [HONO2]

  5. The oxygen atom in OH group in nitric acid, HNO3 [HONO2]

  6. The central oxygen atom in the ozone molecule, O3

  7. Each of the carbon atoms in the propyne, CH3 CCH

  8. The carbon atom in Freon, CCl2 F2

  9. each of the carbon atoms in allene H2CCCH2
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