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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

Many chemical reactions that occur in the atmosphere and stratosphere involve free radicals. Free radical formation occurs when a photon of light is absorbed and the energy of the radiation being absorbed causes a chemical bond in the compound to break. Which of the following bonds requires the most energy (and the most energetic radiation) to be broken?

  1. (a) The oxygen-oxygen bond in O2
  2. (b) The chlorine-carbon bond in CCl2F2
  3. (c) The oxygen-oxygen bond in O3

Interpretation Introduction

Interpretation:

From the given bonds, the bond that requires more energy to break should be determined.

Concept introduction:

To break bond, energy is always required and energy is released when a bond is made. Bond energy is the measure of bond strength in a chemical bond.it is the amount of energy required to break a bond between two atoms in a diatomic molecule.

When a bond is strong there is higher bond energy because it takes more energy to break a strong bond and if the distance between the atoms in a bond is shorter, then more energy will be required to break that bond.

Explanation

Reason for the correct answer:

There exist one double bond between the oxygen atoms in O2 molecule and also its bond length is short compared to the other bond given.

When a bond is strong there is higher bond energy because it takes more energy to break a strong bond and if the distance between the atoms in a bond is shorter, then more energy will be required to break that bond.

Therefore the oxygen-oxygen bond in O2 Option (a) requires more energy to break than the other given bonds

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