Learning objective

Define mean bond enthalpy.

Read the explanation, check the common trap, then practise with flashcards and questions.

Start flashcards Try practice questions Topic hub

At a glance

Flashcards

Questions

Topic

Energetics

Subtopic

Bond enthalpies

AQA A Level ChemistryPhysical chemistry

Study support

Understand this objective

Short explanation

Mean bond enthalpy is defined as the average energy required to break one mole of a specific type of bond in a gaseous molecule, measured in kilojoules per mole (kJ/mol). This value is determined by considering the energy changes associated with breaking bonds in various compounds. It is important to note that mean bond enthalpies are averages and can vary depending on the molecular environment. Therefore, they provide an estimate for the energy changes in chemical reactions involving bond breaking and formation.

Key concepts

mean bond enthalpyenthalpy change

Why it matters

This objective helps connect Bond enthalpies to exam-style questions, flashcards, and revision notes for Energetics.

Common mistakes

1 linked

Mean Bond Enthalpy Confusion: Mean bond enthalpy is an average value for a bond type across different compounds. To define it, state: Mean bond enthalpy is the average energy required to break one mole of a specific type of bond in a gaseous molecule. For example, the mean bond enthalpy for a C-H bond is calculated by averaging the bond energies from various compounds containing C-H bonds.

Revision tools