Did this video help you?
Bond Breaking & Bond Forming (Cambridge O Level Chemistry)
Revision Note
Bond Breaking & Bond Forming
- Whether a reaction is endothermic or exothermic depends on the difference between the energy needed to break existing bonds and the energy released when the new bonds are formed
- Bond breaking is always an endothermic process as energy needs to be taken in from the surroundings to break the chemical bonds
- Bond making is always an exothermic process as energy is transferred to the surroundings as the new bond is formed
Exothermic reactions
- If more energy is released than is absorbed, then the reaction is exothermic
- More energy is released when new bonds are formed than energy required to break the bonds in the reactants
- The change in energy is negative since the products have less energy than the reactants
- Therefore an exothermic reaction has a negative ΔH value
Making new chemical bonds releases energy which radiates outwards from the reaction to the surroundings in the form of heat
Endothermic reactions
- If more energy is absorbed to break bonds than is released to form new bonds, this reaction is endothermic overall
- The change in energy is positive since the products have more energy than the reactants
- The symbol ΔH (delta H) is used to show the change in heat energy. H is the symbol for enthaply, which is a measure of the total heat of reaction of a chemical reaction
- Therefore an endothermic reaction has a positive ΔH value, which is shown on the reaction pathway diagrams and in calculations
Breaking chemical bonds requires energy which is taken in from the surroundings in the form of heat
Bond Energy Calculations
Energy of reaction calculations
- Each chemical bond has specific bond energy associated with it
- This is the amount of energy required to break the bond or the amount of energy given out when the bond is formed
- This energy can be used to calculate how much heat would be released or absorbed in a reaction
- To do this it is necessary to know the bonds present in both the reactants and products
Method
- Write a balanced equation if none is present already
- Optional - draw the displayed formula in order to identify the type and number of bonds more easily
- Add together all the bond energies for all the bonds in the reactants – this is the ‘energy in’
- Add together the bond energies for all the bonds in the products – this is the ‘energy out’
- Calculate the enthalpy change:
Enthalpy change (ΔH) = Energy taken in - Energy given out
Worked example
Hydrogen and chlorine react to form hydrogen chloride gas:
H2 + Cl2 ⟶ 2HCl
The table below shows the bond energies.
Calculate the enthalpy change, ΔH, for the reaction and deduce whether it is exothermic or endothermic.
Answer
Worked example
Hydrogen bromide decomposes to form hydrogen and bromine:
2HBr ⟶ H2 + Br2
The table below shows the bond energies.
Calculate the enthalpy change, ΔH, for the reaction and deduce whether it is exothermic or endothermic.
Answer
Examiner Tip
When answering questions to calculate the enthalpy change using bond energies,, it is helpful to write down a displayed formula equation for the reaction before identifying the type and number of bonds, to avoid making mistakes. The reaction thus becomes: H-H + Cl-Cl → H-Cl + H-Cl
You've read 0 of your 5 free revision notes this week
Sign up now. It’s free!
Did this page help you?